Ch4.1 – Types of Chemical Reactions and Solutions.
-
Upload
thomas-dixon -
Category
Documents
-
view
235 -
download
0
Transcript of Ch4.1 – Types of Chemical Reactions and Solutions.
![Page 1: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/1.jpg)
![Page 2: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/2.jpg)
Ch4.1 – Types of Chemical Reactions and Solutions
![Page 3: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/3.jpg)
This is the process of hydration.
Dissociation equation: NaCl(s) Na+(aq) + Cl–(ag)
H2O
![Page 4: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/4.jpg)
Solubility varies greatly. For ions - depends on who has the greater attraction.For molecules – depends on polarity
Solvent – the substance doing the dissolving (water)Solute – the substance that gets dissolved (salt)
![Page 5: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/5.jpg)
ElectrolytesStrong electrolytes
- conduct current very efficiently- soluble salts, acids, bases
![Page 6: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/6.jpg)
ElectrolytesStrong electrolytes
- conduct current very efficiently- soluble salts, acids, bases
Arrhenius Theory of Acids- produces H+ ions (protons) in water
HCl H2O H+(aq) + Cl–(aq)
- strong acid – vitrually every H ionizes
H2SO4 H2O H+(aq) + HSO4
–(aq)
![Page 7: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/7.jpg)
Weak electrolytes – only a small degree of ionization Weak Acid Weak Base
HC2H3O2 H2O H+(aq) + C2H3O2
–(aq) NH3 H2O NH4
+(aq) + OH–
(aq)
Only about 1 in 100 H’s ionize. The rest stay in their molecules.Nonelectrolytes – dissolve in water, but don’t produce ions.
- like sugar (nonpolar substances)
![Page 8: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/8.jpg)
Molarity
Units: Molar or M
Ex1) Calc the molarity of a solution prepared by dissolving 11.5g NaOH in enough water to make 1.50L soln.
soln of liters
solute of molesM
![Page 9: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/9.jpg)
Concentration of Ions
Ex2) Give the concentration of ions in a 0.50M Co(NO3)2 soln.
![Page 10: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/10.jpg)
Ex3) Calculate the number of moles of Cl– ions in
1.75L of 1.0x10-3M ZnCl2 soln.
Ch4 HW#1 p180+ 11(d-g),13,15(a,b),17(a,b)
![Page 11: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/11.jpg)
Ch4 HW#1 p180+ 11(d-g),13,15(a,b),17(a,b)11. Show how each of the following strong electrolytes “ breaks up” into its
component ions dissolving in water.
d. (NH4)2SO4
e. HI f. FeSO4
g. KMnO4
h. HClO4
13. Calcium chloride is a strong electrolyte and is used to “salt” streets in the winter to melt ice and snow. Write a reaction to show how this substance breaks apart when it dissolves in water.
![Page 12: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/12.jpg)
Ch4 HW#1 p180+ 11(d-g),13,15(a,b),17(a,b)11. Show how each of the following strong electrolytes “ breaks up” into its
component ions dissolving in water.
d. (NH4)2SO4 H2O 2NH4+ + SO4
-2
e. HI H2O H+ + I-
f. FeSO4 H2O Fe+ + SO4
-
g. KMnO4 H2O K+ + MnO4
-
h. HClO4 H2O H+ + ClO4
-
13. Calcium chloride is a strong electrolyte and is used to “salt” streets in the winter to melt ice and snow. Write a reaction to show how this substance breaks apart when it dissolves in water.
![Page 13: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/13.jpg)
Ch4 HW#1 p180+ 11(d-g),13,15(a,b),17(a,b)11. Show how each of the following strong electrolytes “ breaks up” into its
component ions dissolving in water.
d. (NH4)2SO4 H2O 2NH4+ + SO4
-2
e. HI H2O H+ + I-
f. FeSO4 H2O Fe+ + SO4
-
g. KMnO4 H2O K+ + MnO4
-
h. HClO4 H2O H+ + ClO4
-
13. Calcium chloride is a strong electrolyte and is used to “salt” streets in the winter to melt ice and snow. Write a reaction to show how this substance breaks apart when it dissolves in water.
CaCl2 H2O Ca2+ + 2Cl-
![Page 14: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/14.jpg)
15.Calculate the molarity of each of these solutions. a. A 5.623g sample of NaHCO3 is dissolved in enough water
to make 250 ml of solution.
b. A 184.6mg sample of K2Cr2O7 is dissolved in enough water to make 500 ml of solution.
![Page 15: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/15.jpg)
15.Calculate the molarity of each of these solutions. a. A 5.623g sample of NaHCO3 is dissolved in enough water
to make 250 ml of solution.
b. A 184.6mg sample of K2Cr2O7 is dissolved in enough water to make 500 ml of solution.
M268.0NaHCO 84.0g soln 0.250L
NaHCO 1mol NaHCO 5.623g
3
33
![Page 16: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/16.jpg)
15.Calculate the molarity of each of these solutions. a. A 5.623g sample of NaHCO3 is dissolved in enough water
to make 250 ml of solution.
b. A 184.6mg sample of K2Cr2O7 is dissolved in enough water to make 500 ml of solution.
M268.0NaHCO 84.0g soln 0.250L
NaHCO 1mol NaHCO 5.623g
3
33
M001255.0OCrK 294.2g soln 0.500L
OCrK 1mol OCrK 0.1846g
722
722722
![Page 17: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/17.jpg)
17. Calculate the concentration of all ions present in each of the following solutions of strong electrolyte
a. 0.15M CaCl2
b. 0.26M Al(NO3)3
![Page 18: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/18.jpg)
17. Calculate the concentration of all ions present in each of the following solutions of strong electrolyte
a. 0.15M CaCl2
0.15M Ca+ ions
0.30M Cl- ions
b. 0.26M Al(NO3)3
![Page 19: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/19.jpg)
17. Calculate the concentration of all ions present in each of the following solutions of strong electrolyte
a. 0.15M CaCl2
0.15M Ca+ ions
0.30M Cl- ions
b. 0.26M Al(NO3)3
0.26M Al+3 ions
0.78M NO3- ions
![Page 20: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/20.jpg)
Ch4.2 More Concentration CalculationsEx1) Blood serum is 0.14M NaCl. What volume of blood contains
1.0mg NaCl?
![Page 21: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/21.jpg)
Ex2) How would I prepare 500 mls of a 0.100M ______ solution,given solid solute?
![Page 22: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/22.jpg)
Dilutions
Ex3) How would I prepare 500 mls of a 0.100M H2SO4 solution,
given concentrated stock solution of 18M?
Ch4 HW#2 p181 21,23(a,b),25
![Page 23: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/23.jpg)
Ch4 HW#2 p181 21,23(a,b),2521. What volume of a 0.100 M solution of NaHCO3 contains
0.350 g of NaHCO3?
![Page 24: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/24.jpg)
Ch4 HW#2 p181 21,23(a,b),2521. What volume of a 0.100 M solution of NaHCO3 contains
0.350 g of NaHCO3?
soln L0417.0
NaHCO 0.100mol NaHCO 84.0g
soln 1L NaHCO 1mol NaHCO 0.350g
33
33
![Page 25: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/25.jpg)
23. Describe how you would prepare 2.00 L of each of the following solutions.a. 0.250M NaOH from solid NaOHb. 0.250M NaOH from 1.00M NaOH stock solution
![Page 26: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/26.jpg)
23. Describe how you would prepare 2.00 L of each of the following solutions.a. 0.250M NaOH from solid NaOHb. 0.250M NaOH from 1.00M NaOH stock solution
soln 0.20 NaOH 1mol soln 1L
NaOH 40.0g NaOH 0.250molsoln 2Lg
![Page 27: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/27.jpg)
23. Describe how you would prepare 2.00 L of each of the following solutions.a. 0.250M NaOH from solid NaOHb. 0.250M NaOH from 1.00M NaOH stock solution
b. M1.V1 = M2
.V2
soln 0.20 NaOH 1mol soln 1L
NaOH 40.0g NaOH 0.250molsoln 2Lg
waterdistilled 1.5L wmixedsoln stock of 0.5LV
Vsoln 1L
1.00mol
1
soln 2L
soln 1L
0.250mol
1
2
![Page 28: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/28.jpg)
25. A solution is prepared by dissolving 10.8 g ammonium sulfate in enough water to make 200.0 mL of stock solution.
A 10.0 mL sample of this stock solution is added to 50.0 mL of water. Calculate the concentration of ammonium ions and sulfate ions in the final
solution.
soln M391.0 SO)(NH 138.1g soln 0.200L
SO)(NH 1mol SO)(NH 10.8g
424
424424
![Page 29: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/29.jpg)
25. A solution is prepared by dissolving 10.8 g ammonium sulfate in enough water to make 200.0 mL of stock solution.
A 10.0 mL sample of this stock solution is added to 50.0 mL of water. Calculate the concentration of ammonium ions and sulfate ions in the final
solution.
soln M391.0 SO)(NH 138.1g soln 0.200L
SO)(NH 1mol SO)(NH 10.8g
424
424424
0.0782MM 1
50ml
1
soln 10mL
soln 1L
0.391mol
2
2
M
![Page 30: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/30.jpg)
Ch4.3 Types of Solution Reactions
1. Precipitation Reactions2. Acid-base Reactions3. Oxidation-Reduction Reactions (Redox)
![Page 31: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/31.jpg)
1. Precipitation Reactions solns mixed and an insoluble substance forms, and separates,
called a precipitate.
AgNO3(aq) and NaCl(ag)
![Page 32: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/32.jpg)
1. Precipitation Reactions solns mixed and an insoluble substance forms, and separates,
called a precipitate.
K2CrO4(aq) + Ba(NO3)2(aq)
![Page 33: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/33.jpg)
Simple solubility rules for salts in water:
1. Most nitrates NO3-1 are soluble.
2. Most salts of alkali metals (Li+, Na+, K+, Cs+, Rb+ )are soluble. Same for ammonium, NH4
+ .
3. Most chloride, bromide, and iodide salts are soluble,
but not when with Ag+, Pb2+, Hg22+.
4. Most sulfates are soluble,
except BaSO4, PbSO4, Hg2SO4, CaSO4.
5. Most hydroxides are only slightly soluble,
except NaOH and KOH very soluble.
Ba(OH)2, Ca(OH)2, Sr(OH)2 only slightly soluble.
6. Most sulfides (S2–), carbonates (CO32–),
phosphates (PO43–), and chromtes (CrO4
2–)
are only slightly soluble.
![Page 34: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/34.jpg)
Ex1) Use rules to predict what will happen if following solutions are mixed:
a) KNO3(aq) and BaCl2(aq) b) Na2SO4(aq) and Pb(NO3)2(aq) c) KOH(aq) and Fe(NO3)3(aq)
![Page 35: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/35.jpg)
3 types of equations are used to describe reactions in solution:1. molecular eqn – great for doing stoichiometry.2. complete ionic eqn – all ions listed,
great for seeing strong electrolytes.3. net ionic eqn – only those soln components
that undergo change. Spectators not included.
Ex2) Aqueous potassium hydroxide is mixed with aqueous iron(III) nitrate to form a ppt of iron(III) hydroxide and aqueous potassium nitrate.Write all 3 eqns.
Ch4 HW#3 p181+ 29,31,33,35(a,b)
![Page 36: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/36.jpg)
Ch4 HW#3 p181+ 29,31,33,35(a,b)29. When the following solutions are mixed together,
what precipitation (if any) will form?
a. BaCl2(aq) + Na2SO4(aq)
b. Pb(NO3)2(aq) + KCl(aq)
c. AgNO3(aq) + Na3PO4(aq)
d. NaOH(aq) + Fe(NO3)3(aq)
31. For the reactions in Exercise 29, write the balanced molecular equation, complete ionic equation, and net ionic equation. If no precipitate forms, write “No reaction.”
![Page 37: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/37.jpg)
Ch4 HW#3 p181+ 29,31,33,35(a,b)29. When the following solutions are mixed together,
what precipitation (if any) will form?
a. BaCl2(aq) + Na2SO4(aq) BaSO4(s)
b. Pb(NO3)2(aq) + KCl(aq) PbCl2(c)
c. AgNO3(aq) + Na3PO4(aq) Ag3PO4(s)
d. NaOH(aq) + Fe(NO3)3(aq) Fe(OH)3(s)
31. For the reactions in Exercise 29, write the balanced molecular equation, complete ionic equation, and net ionic equation. If no precipitate forms, write “No reaction.”
![Page 38: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/38.jpg)
Ch4 HW#3 p181+ 29,31,33,35(a,b)29. When the following solutions are mixed together,
what precipitation (if any) will form?
NIE: a. BaCl2(aq) + Na2SO4(aq) BaSO4(s)
NIE: b. Pb(NO3)2(aq) + KCl(aq) PbCl2(c)
NIE: c. AgNO3(aq) + Na3PO4(aq) Ag3PO4(s)
NIE: d. NaOH(aq) + Fe(NO3)3(aq) Fe(OH)3(s)
31. For the reactions in Exercise 29, write the balanced molecular equation, complete ionic equation, and net ionic equation. If no precipitate forms, write “No reaction.”
BME: a. BaCl2(aq) + Na2SO4(aq) 2Cl-(aq)+2Na+
(aq)+ BaSO4(s)
b. Pb(NO3)2(aq) + 2KCl(aq) 2NO3-(aq)+2K+
(aq)+ PbCl2(c)
c. 3AgNO3(aq)+Na3PO4(aq) 3NO3-(aq)+3Na+
(aq)+Ag3PO4(s)
d. 3NaOH(aq)+Fe(NO3)3(aq) 3NO3-(aq)+3Na+
(aq)+ Fe(OH)3(s)
![Page 39: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/39.jpg)
33. Write net ionic equations for each of the following.
a. AgNO3(aq) + KI(aq)
b. CuSO4(aq) + Na2S(aq)
c. CoCl2(aq) + NaOH(aq)
d. NiCI2(aq) + KNO3(aq)
![Page 40: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/40.jpg)
33. Write net ionic equations for each of the following.
a. AgNO3(aq) + KI(aq)
Ag+(aq) + I-
(aq) AgI(s)
b. CuSO4(aq) + Na2S(aq)
Cu2+(aq) + S2-
(aq) CuS(s) (only slightly)
c. CoCl2(aq) + NaOH(aq)
Co2+
(aq) + 2OH-(aq) Co(OH)2(aq) (only slightly)
d. NiCI2(aq) + KNO3(aq) No ppt
![Page 41: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/41.jpg)
35. Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed.
a. Ammonium sulfate and barium nitrate
(NH4)2(SO4)(aq) + Ba(NO3)2(aq)
b. Lead(II) nitrate and sodium chloride
Pb(NO3)2(aq) + NaCl(aq)
![Page 42: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/42.jpg)
35. Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed.
a. Ammonium sulfate and barium nitrate
SO42-
(aq) + Ba2+(aq) BaSO4(s)
b. Lead(II) nitrate and sodium chloride
Pb+2(aq) + 2Cl-(aq) PbCl2(s)
![Page 43: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/43.jpg)
Ch4.4 Mass of Precipitate
Ex1) Calculate the mass of solid NaCl that must be added to 1.50L of a 0.100M AgNO3 solution to precipitate all the Ag+ ions.
![Page 44: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/44.jpg)
Ex2) What mass of PbSO4 precipitates when 2.00L of 0.025M aqueous Na2SO4 and 1.25L of 0.0500M aqueous Pb(NO3)2 are mixed?
Ch4 HW#4 p182 39,41,43
![Page 45: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/45.jpg)
Ch4 HW#4 p182 39,41,4339. What mass of NaCl is required to precipitate all the silver ions from 50.0 mL of a 0.0500 M solution of AgNO3?
NaCl + AgNO3 ?g 0.0500M
50.0ml
![Page 46: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/46.jpg)
Ch4 HW#4 p182 39,41,4339. What mass of NaCl is required to precipitate all the silver ions from 50.0 mL of a 0.0500 M solution of AgNO3?
NaCl + AgNO3 ?g 0.0500M
50.0ml
Cl- + Ag+ AgCl(s)
NaCl 146.0 NaCl 1mol Ag 1mol soln 1L
NaCl 58.5g NaCl 1mol Ag 0.050molsoln 0.050Lg
![Page 47: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/47.jpg)
41. What mass of solid aluminum hydroxide is produced when 50.0 mL of 0.200 M Al(NO3)3 is added to 200.0 mL of 0.100M KOH?
Al(NO3)3 + 3KOH 0.200M 0.100M 50.0ml 200.0ml
![Page 48: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/48.jpg)
41. What mass of solid aluminum hydroxide is produced when 50.0 mL of 0.200 M Al(NO3)3 is added to 200.0 mL of 0.100M KOH?
Al(NO3)3 + 3KOH K+(aq) + NO3
-(aq) + Al(OH)3(s)
0.200M 0.100M ?g 50.0ml 200.0ml
Al is L.R.
x 3 = 0.06 mol
33
Al mol 010.0 soln 1L
A1 0.200molsoln 0.050L
-OH mol 020.0 soln 1L
OH 0.100molsoln 0.200L
![Page 49: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/49.jpg)
41. Al(NO3)3 + 3KOH K+(aq) + NO3
-(aq) + Al(OH)3(s)
0.200M 0.100M ?g 50.0ml 200.0ml
Al is L.R.
x 3 = 0.06 mol
33
Al mol 010.0 soln 1L
A1 0.200molsoln 0.050L
-OH mol 020.0 soln 1L
OH 0.100molsoln 0.200L
33
333
3
Al(OH) 780.0 Al(OH) 1mol Al 1mol soln 1L
Al(OH) 78.0 Al(OH) 1mol Al 0.200molsoln 0.050Lg
![Page 50: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/50.jpg)
43. A 100.0-mL aliquot of 0.200 M aqueous potassium hydroxide is mixed with 100.0 mL of 0.200 M aqueous magnesium nitrate.a. Write a balanced chemical equation for any reaction that occurs.b. What precipitate forms?c. What mass of precipitate is produced?d. Calculate the concentration of each ion remaining in solution
after precipitation is complete.
![Page 51: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/51.jpg)
43. A 100.0mL aliquot of 0.200 M aqueous potassium hydroxide is mixed with 100.0 mL of 0.200 M aqueous magnesium nitrate. a. Write a balanced chemical equation for any reaction that occurs. b. What precipitate forms? c. What mass of precipitate is produced? d. Calculate the concentration of each ion remaining in solution
after precipitation is complete.
2KOH + Mg(NO3)2 2K+ + 2NO3- + Mg2+ + 2OH-
2KOH + Mg(NO3)2 Mg(OH)2(s) 0.200M 0.200M100ml 100ml
LR
22
222
2
Mg(OH) 17.1 Mg(OH) 1mol Mg 1mol soln 1L
Mg(OH) 58.3 Mg(OH) 1mol Mg 0.200molsoln 0.100Lg
![Page 52: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/52.jpg)
43. A 100.0mL aliquot of 0.200 M aqueous potassium hydroxide is mixed with 100.0 mL of 0.200 M aqueous magnesium nitrate. d. Calculate the concentration of each ion remaining in solution
after precipitation is complete.
2KOH + Mg(NO3)2 2K+ + 2NO3- + Mg(OH)2(s)
start:end:
![Page 53: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/53.jpg)
Ch4.4B – Ion ConcentrationEx1) A 100.0mL aliquot of 0.100 M aqueous barium chloride is mixed with 100.0 mL of 0.300 M aqueous sodium sulfate. Barium sulfate precipitates out. a. Write a balanced chemical equation for any reaction that occurs. b. What mass of precipitate is produced? c. Calculate the concentration of each ion remaining in solution
after precipitation is complete.
![Page 54: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/54.jpg)
c. Calculate the concentration of each ion remaining in solution after precipitation is complete.
BaCl2 + Na3SO4 3Na+ + 2Cl- + BaSO4(s)
Ch4 HW#5 p182 44
![Page 55: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/55.jpg)
Ch4 HW#5 p182 44 44. How many grams of silver chloride can be prepared by the reaction of 100.0mL of 0.20M silver nitrate with 100.0mL of 0.15M calcium chloride? Calculate the concentration of each ion remaining in solution after precipitation is complete.
AgNO3 + CaCl2 Ca+2 + NO3-1 + AgCl(s)
![Page 56: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/56.jpg)
44. How many grams of silver chloride can be prepared by the reaction of 100.0ml of 0.20M silver nitrate with 100.0ml of 0.15M calcium chloride.How much leftover of each ion? Unbalanced:
AgNO3(aq) + CaCl2(aq) AgCl(s) + Ca+2(aq) + NO3
-(aq)
0.20M 0.15M ?g0.1000L 0.1000L
ions: Ag+ NO3- Ca+2
Cl- start:end:
![Page 57: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/57.jpg)
44. How many grams of silver chloride can be prepared by the reaction of 100.0ml of 0.20M silver nitrate with 100.0ml of 0.15M calcium chloride.How much leftover of each ion? Balanced Molecular Equation:
2AgNO3(aq) + CaCl2(aq) 2AgCl(s) + Ca+2(aq) + 2NO3
-(aq)
0.20M 0.15M ?g 0.1000L 0.1000L
ions: Ag+ NO3- Ca+2
Cl- start:end:
![Page 58: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/58.jpg)
44. How many grams of silver chloride can be prepared by the reaction of 100.0ml of 0.20M silver nitrate with 100.0ml of 0.15M calcium chloride.How much leftover of each ion? Balanced Molecular Equation:
2AgNO3(aq) + CaCl2(aq) 2AgCl(s) + Ca+2(aq) + 2NO3
-(aq)
0.20M 0.15M ?g 0.1000L 0.1000L
ions: Ag+ NO3- Ca+2
Cl- start:end:
AgCl 87.2 AgCl 1mol AgNO 2mol soln 1L
AgCl 143.4 AgCl 2mol AgNO 0.2molsoln 0.100L
3
3 g
AgCl 30.4 AgCl 1mol CaCl 1mol soln 1L
AgCl 143.4 AgCl 2mol CaCl 0.15molsoln 0.100L
2
2 g
![Page 59: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/59.jpg)
44. How many grams of silver chloride can be prepared by the reaction of 100.0ml of 0.20M silver nitrate with 100.0ml of 0.15M calcium chloride.How much leftover of each ion? Balanced Molecular Equation:
2AgNO3(aq) + CaCl2(aq) 2AgCl(s) + Ca+2(aq) + 2NO3
-(aq)
0.20M 0.15M ?g 0.1000L 0.1000L
ions: Ag+ NO3- Ca+2
Cl- start:end:
The AgNO3 limits the reaction to produce 2.87g AgCl
But what about the ions leftover? Might consider solving this differently…
AgCl 87.2 AgCl 1mol AgNO 2mol soln 1L
AgCl 143.4 AgCl 2mol AgNO 0.2molsoln 0.100L
3
3 g
AgCl 30.4 AgCl 1mol CaCl 1mol soln 1L
AgCl 143.4 AgCl 2mol CaCl 0.15molsoln 0.100L
2
2 g
![Page 60: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/60.jpg)
44. How many grams of silver chloride can be prepared by the reaction of 100.0ml of 0.20M silver nitrate with 100.0ml of 0.15M calcium chloride.How much leftover of each ion? Complete Ionic Equation: Look at the CIE, not the molecular equation:
2Ag+(aq)+ NO3
–(aq)+Ca2++2Cl–(aq)2AgCl(s)+Ca+2
(aq)+2NO3-(aq)
0.20M 0.20M 0.15M 0.30M 2.87g 0.1000L 0.1000L 0.1000L 0.1000L
ions: Ag+ NO3- Ca+2
Cl- start: 0.02mol 0.02mol 0.015mol 0.030molend:
![Page 61: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/61.jpg)
44. How many grams of silver chloride can be prepared by the reaction of 100.0ml of 0.20M silver nitrate with 100.0ml of 0.15M calcium chloride.How much leftover of each ion? Complete Ionic Equation:
2Ag+(aq)+NO3
–(aq)+Ca2++2Cl–(aq)2AgCl(s)+Ca+2
(aq)+2NO3–
(aq)
0.20M 0.20M 0.15M 0.30M 2.87g 0.1000L 0.1000L 0.1000L 0.1000L
ions: Ag+ NO3- Ca+2
Cl- start: 0.02mol 0.02mol 0.015mol 0.030molend: 0mol 0.02mol 0.015mol ?mol
All the silver ions get used up. Ag+: 0MNo NO3
- are used, only spectator ions: NO3-: 0.02mol/.200L = 0.1M
No Ca2+ are used, only spectator ions: Ca2+:0.015mol/.20L=0.075MBut what about the chloride ions?
![Page 62: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/62.jpg)
44. How many grams of silver chloride can be prepared by the reaction of 100.0ml of 0.20M silver nitrate with 100.0ml of 0.15M calcium chloride.How much leftover of each ion? Net Ionic Equation:
Ag+(aq) + Cl–(aq) AgCl(s)
ions: Ag+ NO3- Ca+2
Cl- start: 0.02mol 0.02mol 0.015mol 0.030molend: 0mol 0.02mol 0.015mol 0.010mol
All the silver ions get used up. Ag+: 0MNo NO3
- are used, only spectator ions: NO3-: 0.02mol/.200L = 0.1M
No Ca2+ are used, only spectator ions: Ca2+:0.015mol/.20L=0.075MBut what about the chloride ions?
They were consumed at a rate of one-to-one with Ag+.So if 0.02mol Ag+ is consumed, same with Cl-.That leaves 0.01 moles leftover.
Cl–: 0.010mol/.20L=0.050M
![Page 63: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/63.jpg)
Ch4.5 – Acid-Base ReactionsBronsted-Lowry Theory of acids and bases:
Acid – proton donorBase – proton acceptor
HCl(aq) + NaOH(aq)
HC2H3O2(aq) + KOH(aq)
![Page 64: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/64.jpg)
Ex1) What volume of a 0.100M HCl solution is needed to neutralize
25.0mL of 0.350M NaOH?
HCl(aq) + NaOH(aq)
![Page 65: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/65.jpg)
Ex2) In a certain experiment, 28.0ml of 0.250M HNO3 and 53.0ml of 0.320M KOH are mixed.
Calculate the amount of water formed and the amount
of excess H+ or OH-.
![Page 66: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/66.jpg)
Acid-Base Titrations - delivery of a measured volume of soln (usually from a buret)
of know concentration into a soln being analyzed (the analyte). The point where enough titrant has been added to react
exactly is called the equivalence point, often indicated by an indicator (substance that changes color.)This point is often called the endpoint.
Ex3) Benzoic acid, HC7H5O2, is a component of waste effluent released
in some industrial processes. If 10.59 ml of 0.1546M NaOH is required to neutralize it, what volume of benzoic acid was present?
(next slide)
![Page 67: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/67.jpg)
Ex3) Benzoic acid, HC7H5O2, is a component of waste effluent released
in some industrial processes. If 10.59 ml of 0.1546M NaOH is required to neutralize it, what volume of benzoic acid was present?
H+ + C7H5O2- + Na+ + OH-
Ch4 HW#5 p182 45(a,b),47(a,b),49(a,b)
![Page 68: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/68.jpg)
Ch4 HW#6 p182 45(a,b),47(a,b),49(a,b)45. Write the balanced molecular, complete ionic, and net ionic equations for each of the following acid-base reactions.
a. HClO4(aq) + Mg(OH)2(s) →
2H+(aq) +2ClO4
-(aq)+Mg+2
(aq) + 2(OH)-(aq)→
b. HCN(aq) + NaOH(aq) →
H+(aq) +CN-
(aq)+Na+(aq) + (OH)-
(aq)→
![Page 69: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/69.jpg)
45. Write the balanced molecular, complete ionic, and net ionic equations for each of the following acid-base reactions.
a. HClO4(aq) + Mg(OH)2(s) →
2H+(aq) +2ClO4
-(aq)+Mg+2
(aq) + 2(OH)-(aq)→H(OH)(l) +Mg+2
(aq)+ ClO4-(aq)
H+(aq) + (OH)-
(aq)→H(OH)(l)
b. HCN(aq) + NaOH(aq) →
H+(aq) +CN-
(aq)+Na+(aq) + (OH)-
(aq)→
![Page 70: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/70.jpg)
45. Write the balanced molecular, complete ionic, and net ionic equations for each of the following acid-base reactions.
a. HClO4(aq) + Mg(OH)2(s) →
2H+(aq) +2ClO4
-(aq)+Mg+2
(aq) + 2(OH)-(aq)→H(OH)(l) +Mg+2
(aq)+ ClO4-(aq)
H+(aq) + (OH)-
(aq)→H(OH)(l)
b. HCN(aq) + NaOH(aq) →
H+(aq) +CN-
(aq)+Na+(aq) + (OH)-
(aq)→H(OH)(l) +Na+(aq)+ CN-
(aq)
H+(aq) + (OH)-
(aq)→H(OH)(l)
![Page 71: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/71.jpg)
47. Write the balanced molecular, complete ionic, and net ionic equations for the reactions that occur when the following are mixed.
a. potassium hydroxide (aqueous) and nitric acid
KOH(aq) + HNO3(aq)
b. barium hydroxide (aqueous) and hydrochloric acid
Ba(OH)2(aq) + HCl(aq)
![Page 72: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/72.jpg)
47. Write the balanced molecular, complete ionic, and net ionic equations for the reactions that occur when the following are mixed.
a. potassium hydroxide (aqueous) and nitric acid
K+(aq)+OH-
(aq)+H+(aq)+NO3
-(aq)H+
(aq)+OH-(aq)+K+
(aq)+NO3-(aq)
H+(aq)+ OH-
(aq) H(OH)(l)
b. barium hydroxide (aqueous) and hydrochloric acid
Ba2+(aq)+2(OH)-
(aq)+2H+(aq)+2Cl-(aq) 2H+
(aq)+2(OH)-(aq)+ Ba2+
(aq)+ 2Cl-
H+(aq)+ OH-
(aq) H(OH)(l)
![Page 73: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/73.jpg)
49. What volume of each of the following acids will react completely with 50.00 mL of 0.200 M NaOH?a. 0.100 M HCl
HCl(aq) + NaOH(aq)→H(OH)(l) +Na+(aq)+ Cl-(aq)
0.100M 0.200M ?L 0.05000L
b. 0.150 M HNO3
![Page 74: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/74.jpg)
49. What volume of each of the following acids will react completely with 50.00 mL of 0.200 M NaOH?a. 0.100 M HCl
HCl(aq) + NaOH(aq)→H(OH)(l) +Na+(aq)+ Cl-(aq)
0.100M 0.200M ?L 0.05000L
b. 0.150 M HNO3
HNO3(aq) + NaOH(aq)→H(OH)(l) +Na+(aq)+ NO3
-(aq)
0.150M 0.200M ?L 0.05000L
HCl 0.100L HCl 0.100mol NaOH 1mol soln 1L
HCl 1L HCl 1mol NaOH 0.200molsoln 0.0500L
![Page 75: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/75.jpg)
49. What volume of each of the following acids will react completely with 50.00 mL of 0.200 M NaOH?a. 0.100 M HCl
HCl(aq) + NaOH(aq)→H(OH)(l) +Na+(aq)+ Cl-(aq)
0.100M 0.200M ?L 0.05000L
b. 0.150 M HNO3
HNO3(aq) + NaOH(aq)→H(OH)(l) +Na+(aq)+ NO3
-(aq)
0.150M 0.200M ?L 0.05000L
HCl 0.100L HCl 0.100mol NaOH 1mol soln 1L
HCl 1L HCl 1mol NaOH 0.200molsoln 0.0500L
HCl 0.0667L HCl 0.150mol NaOH 1mol soln 1L
HCl 1L HCl 1mol NaOH 0.200molsoln 0.0500L
![Page 76: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/76.jpg)
Lab 4.2 Pre-lab QuestionsThe following data was obtained from a regular chemistry lab group
conducting this lab:
Trial 1 NaOH Initial Volume
Final Volume
Volume Used
Molarity 0.100M 1mL 12mL 11mL
HCl Initial Volume
Final Volume
Volume Used
Molarity 0.0157M0.016M0.02M
2mL 9mL 7mL
![Page 77: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/77.jpg)
3. Knowing my regular chem classes, this trial may have lacked accuracy, but it definitely lacked precision. Please list the obvious non-precise measurements.4. Look at your calculator answer. Round the answer to the correct number of significant digits. If you look at the first 3 digits on your calculator screen, how different do your 2 answers look?
Trial 1 NaOH Initial Volume
Final Volume
Volume Used
Molarity 0.100M 1mL 12mL 11mL
HCl Initial Volume
Final Volume
Volume Used
Molarity 0.0157M0.016M0.02M
2mL 9mL 7mL
![Page 78: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/78.jpg)
5. If the actual molarity of HCl was 0.150M, please find the % error for the answer with the correct sig digs.6. Can you see how precise measuring can be as important as accurate measuring?
Trial 1 NaOH Initial Volume
Final Volume
Volume Used
Molarity 0.100M 1mL 12mL 11mL
HCl Initial Volume
Final Volume
Volume Used
Molarity 0.0157M0.016M0.02M
2mL 9mL 7mL
![Page 79: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/79.jpg)
Ch4 HW#7 Mid Chapter Review p180+16c,18c,24b,54
Lab4.2 NeutralizationVolume of NaOH: ____ (measured)Molarity of NaOH: 0.200Volume of HCl: ____ (measured)Molarity of HCl: ?
HClMHClLNaOHmol
HClmol
NaOHL
NaOHmolNaOHL ____
____ 1
1
1
2.0 ___
![Page 80: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/80.jpg)
Ch4 HW#7 Mid Chapter Review p180+ 16c,18c,24b,5416c. A 0.4508-g sample of iron is dissolved in a small amount of concentrated nitric acid forming Fe3+ ions in solution and is diluted to a total volume of 500.0ml. Calculate the molarity of Fe3+.
![Page 81: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/81.jpg)
16c. A 0.4508-g sample of iron is dissolved in a small amount of concentrated nitric acid forming Fe3+ ions in solution and is diluted to a total volume of 500.0ml. Calculate the molarity of Fe3+.
Fe(s) + HNO3(aq) Fe3+ (aq) + NO3-(aq) + H2(g)
M016.0Fe 55.8gsoln 0.500L
Fe 1mol Fe 0.4508g
![Page 82: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/82.jpg)
18c.Calculate the concentration of all ions present in 5.00g of NH4Cl in 500.0mL of solution.
NH4Cl H2O NH4+ + Cl-
![Page 83: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/83.jpg)
18c.Calculate the concentration of all ions present in 5.00g of NH4Cl in 500.0mL of solution.
NH4Cl H2O NH4+ + Cl-
ClNH 0.187MClNH 53.5gsoln 0.500L
ClNH 1mol ClNH 5.00g4
4
44
![Page 84: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/84.jpg)
24b. How would you prepare 1.00 L of a 0.50M HCl soln from “concentrated” (12M) reagent?
![Page 85: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/85.jpg)
24b. How would you prepare 1.00 L of a 0.50M HCl soln from “concentrated” (12M) reagent?
L. 1 water todistilled wmixedsoln stock of 0.04LV
Vsoln 1L
12.00mol
1
soln 1L
soln 1L
0.500mol
1
2
![Page 86: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/86.jpg)
54. What volume of 0.0200 M calcium hydroxide is required to neutralize 35.00 mL of 0.0500 M nitric acid?
2HNO3(aq) + Ca(OH)2(aq)→ 2H(OH)(l) +Na2+(aq)+ NO3
-(aq)
0.050M 0.200M 0.03500L ?L
![Page 87: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/87.jpg)
54. What volume of 0.0200 M calcium hydroxide is required to neutralize 35.00 mL of 0.0500 M nitric acid?
2HNO3(aq) + Ca(OH)2(aq)→ 2H(OH)(l) +Na2+(aq)+ NO3
-(aq)
0.050M 0.200M 0.03500L ?L
2
23
223
Ca(OH) 0.00438L
Ca(OH) 0.200mol HNO 2mol soln 1L
Ca(OH) 1L Ca(OH) 1mol HNO 0.050molsoln 0.03500L
![Page 88: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/88.jpg)
Ch4.6 Oxidation-Reduction Reactions (Redox)Redox reactions involve the transfer of electrons.
Ex1) Na(s) + Cl2(g)
![Page 89: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/89.jpg)
In redox reactions, one element is oxidized (loses electrons),one element is reduced (gains electrons).
OIL RIG
(Oxidation Is Losing, Reducing Is Gaining)
(reduced in charge)
Oxidation numbers – in covalent bonds, where electrons are shared,they are rarely shared equally. So we assign a charge to each.
Here’s the rules:
![Page 90: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/90.jpg)
Oxidation numbers – in covalent bonds, where electrons are shared,they are rarely shared equally. So we assign a charge to each.
Here’s the rules:
1. Free elements are 0. Exs: Na(s), O2(g) 2. Monatomic ions take ox #’s
based on their column: Exs: Na: +1, Cl: -13. Fluorine is always -1.
4. Oxygen is usually -2. Exs: CO, CO2, SO2, SO3
Exceptions: the O22- group is -1, like in H2O2
when bonded to fluorine it +2, OF2.
5. With nonmetals, H is +1 Exs: HCl, NH3, H2O, CH4
6. Sum in a compound adds up to 0, oradds up to the sum of the whole polyatomic ion charge.
Exs: NH4+
![Page 91: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/91.jpg)
Ex2) Assign oxidation states to all the atoms:
a) CO2 b) SF6
c) NO3- d) Fe2O3
![Page 92: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/92.jpg)
Ex3) In the following reaction, identify which element is oxidizedand which is reduced:
2Al(s) + 3I2(s) 2AlI3(s) 0 0 +3 -1
Al: oxidized
I2: reduced
I2 is referred to as the oxidizing agent (takes electrons).
Al is the reducing agent (furnishes electrons).
![Page 93: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/93.jpg)
Ex4) In the following reaction, identify which element is oxidizedand which is reduced:
2PbS(s) + 3O2(g) 2PbO(s) + 2SO2(g)
Ch4 HW#8 p182+ 57,59,61(a,b)
![Page 94: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/94.jpg)
Ch4 HW#8 p182+ 57,59,61(a,b)57. Assign oxidation states for all atoms in each of the following compounds.
a. KMnO4 b. NiO2
c. K4Fe(CN)6 (Fe only) d. (NH4)2HPO4
e. P4O6 f. Fe3O4
g. XeOF4 h. SF4
i. CO j. Na2C2O4
![Page 95: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/95.jpg)
57. Assign oxidation states for all atoms in each of the following compounds.
a. KMnO4 b. NiO2
(+1)___(-8) ___(-4)
c. K4Fe(CN)6 (Fe only) d. (NH4)2HPO4
(+4)___(-6) (+2)(+1)___(-8)
e. P4O6 f. Fe3O4
___(-12) ___(-8)
g. XeOF4 h. SF4
___(-2)(-4) ___(-4)
i. CO j. Na2C2O4
___(-2) (+2)___(-8)
![Page 96: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/96.jpg)
57. Assign oxidation states for all atoms in each of the following compounds.
a. KMnO4 b. NiO2
(+1)+7(-8) +4(-4)
c. K4Fe(CN)6 (Fe only) d. (NH4)2HPO4
(+4)+2(-6) (+2)(+1)+5(-8)
e. P4O6 f. Fe3O4
+3each(-12) +8/3each(-8)
g. XeOF4 h. SF4
+6(-2)(-4) +4(-4)
i. CO j. Na2C2O4
+2(-2) (+2)+6(-8)
![Page 97: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/97.jpg)
59. Assign the oxidation for chlorine in each of the following anion:
OCl-
ClO2-
CLO3-
CLO4-
![Page 98: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/98.jpg)
59. Assign the oxidation for chlorine in each of the following anion:
OCl- [(-2)___](-1)
ClO2-
[___ (-4)](-1)
ClO3-
[___(-6)](-1)
ClO4-
[___(-8)](-1)
![Page 99: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/99.jpg)
59. Assign the oxidation for chlorine in each of the following anion:
OCl- [(-2)+1](-1)
ClO2-
[+3 (-4)](-1)
ClO3-
[+5(-6)](-1)
ClO4-
[+7(-8)](-1)
![Page 100: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/100.jpg)
61(a,b). Specify which of the following are oxidation-reduction reactions, and identify the oxidizing agent, the reducing agent, the substance being oxidized, and the substance being reduced.
a. CH4(g) + 2O2(g) CO2(g) + 2H2O(g)
b. Zn(s) + 2HCI(aq) ZnCI2(aq) + H2(g)
![Page 101: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/101.jpg)
61(a,b). Specify which of the following are oxidation-reduction reactions, and identify the oxidizing agent, the reducing agent, the substance being oxidized, and the substance being reduced.
a. CH4(g) + 2O2(g) CO2(g) + 2H2O(g) [+4(-4) ] (0) [+4(-4)] [+2(-2)]
-1each -2each +1eachOIL: H lost 2e- so is oxidized, making it the reducing agent.RIG: O gained 2e- so is reduced, making it the ox agent.
b. Zn(s) + 2HCI(aq) ZnCI2(aq) + H2(g) (0) [+1(-1)] [+2(-1each)] (0)
![Page 102: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/102.jpg)
61(a,b). Specify which of the following are oxidation-reduction reactions, and identify the oxidizing agent, the reducing agent, the substance being oxidized, and the substance being reduced.
a. CH4(g) + 2O2(g) CO2(g) + 2H2O(g) [+4(-4) ] (0) [+4(-4)] [+2(-2)]
-1each -2each +1eachOIL: H lost 2e- so is oxidized, making it the reducing agent.RIG: O gained 2e- so is reduced, making it the ox agent.
b. Zn(s) + 2HCI(aq) ZnCI2(aq) + H2(g) (0) [+1(-1)] [+2(-1each)] (0)
OIL: Zn lost 2e- so is oxidized, making it the reducing agent.RIG: H gained 1e- each so is reduced, making it the ox agent.
![Page 103: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/103.jpg)
Ch4.7 - Balancing Redox EquationsHalf reactions: break up a redox reaction into 2 parts,
one involving oxidation, one involving reduction. Slightly different methods if the solution is acidic or basic,
so determine that first.Ex1) Potassium dichromate, K2Cr2O7, reacts with ethyl alcohol, C2H5OH, in the following reaction:
H+(aq) + Cr2O7
2-(aq) + C2H5OH Cr+3
(aq) + CO2(aq) + H2O(l) (yellow) (violet)
![Page 104: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/104.jpg)
Ex1) Potassium dichromate, K2Cr2O7, reacts with ethyl alcohol, C2H5OH, in the following reaction: (Acidic)
H+(aq) + Cr2O7
2-(aq) + C2H5OH(l) Cr+3
(aq) + CO2(aq) + H2O(l) (yellow) (violet)
Step1: Write ½ rxns.Step2:
a.b.c.d.
Step3:Step4:Step5:Reduction ½ rxn:
Oxidation ½ rxn:
![Page 105: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/105.jpg)
H+(aq) + Cr2O7
2-(aq) + C2H5OH(l) Cr+3
(aq) + CO2(aq) + H2O(l) Step1: Write ½ rxns.Step2: Balance ½ rxns. (Start with 1st.)
a. Balance all except H n O.b. c. d.
Step3:Step4:Step5:
Reduction ½ rxn: Cr2O72-
(aq) Cr+3(aq)
Oxidation ½ rxn: C2H5OH(l) CO2(aq)
(+6) (+3) (–2) (+4)
![Page 106: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/106.jpg)
H+(aq) + Cr2O7
2-(aq) + C2H5OH(l) Cr+3
(aq) + CO2(aq) + H2O(l) Step1: Write ½ rxns.Step2: Balance ½ rxns. (Start with 1st.)
a. Balance all except H n O.b. Balance O using H2O.c. d.
Step3:Step4:Step5:
Reduction ½ rxn: Cr2O72-
(aq) 2Cr+3(aq)
Oxidation ½ rxn: C2H5OH(l) CO2(aq)
(+6) (+3) (–2) (+4)
![Page 107: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/107.jpg)
H+(aq) + Cr2O7
2-(aq) + C2H5OH(l) Cr+3
(aq) + CO2(aq) + H2O(l) Step1: Write ½ rxns.Step2: Balance ½ rxns. (Start with 1st.)
a. Balance all except H n O.b. Balance O using H2O.c. Balance H using H+.d.
Step3:Step4:Step5:
Reduction ½ rxn: Cr2O72-
(aq) 2Cr+3(aq) + 7H2O(l)
Oxidation ½ rxn: C2H5OH(l) CO2(aq)
(+6) (+3) (–2) (+4)
![Page 108: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/108.jpg)
H+(aq) + Cr2O7
2-(aq) + C2H5OH(l) Cr+3
(aq) + CO2(aq) + H2O(l) Step1: Write ½ rxns.Step2: Balance ½ rxns. (Start with 1st.)
a. Balance all except H n O.b. Balance O using H2O.c. Balance H using H+.d. Balance charge using electrons.
Step3:Step4:Step5:
Reduction ½ rxn: 14H+(aq) + Cr2O7
2-(aq) 2Cr+3
(aq) + 7H2O(l)
Oxidation ½ rxn: C2H5OH(l) CO2(aq)
(+6) (+3) (–2) (+4)
![Page 109: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/109.jpg)
H+(aq) + Cr2O7
2-(aq) + C2H5OH(l) Cr+3
(aq) + CO2(aq) + H2O(l) Step1: Write ½ rxns.Step2: Balance ½ rxns. (Start with 1st.) (Repeat w 2nd.)
a. Balance all except H n O.b. Balance O using H2O.c. Balance H using H+.d. Balance charge using electrons.
Step3:Step4:Step5:
Reduction ½ rxn: 6e- + 14H+(aq) + Cr2O7
2-(aq) 2Cr+3
(aq) + 7H2O(l)
Oxidation ½ rxn: C2H5OH(l) CO2(aq)
(+6) (+3) (–2) (+4)
![Page 110: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/110.jpg)
H+(aq) + Cr2O7
2-(aq) + C2H5OH(l) Cr+3
(aq) + CO2(aq) + H2O(l) Step1: Write ½ rxns.Step2: Balance ½ rxns. (Start with 1st.) (Repeat w 2nd.)
a. Balance all except H n O.b. Balance O using H2O.c. Balance H using H+.d. Balance charge using electrons.
Step3: Equalize electronsStep4:Step5:
Reduction ½ rxn: 6e- + 14H+(aq) + Cr2O7
2-(aq) 2Cr+3
(aq) + 7H2O(l)
Oxidation ½ rxn: C2H5OH(l) + 3H2O(l) 2CO2(aq) + 12H+(aq)+12e-
(+6) (+3) (–2) (+4)
![Page 111: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/111.jpg)
H+(aq) + Cr2O7
2-(aq) + C2H5OH(l) Cr+3
(aq) + CO2(aq) + H2O(l) Step1: Write ½ rxns.Step2: Balance ½ rxns. (Start with 1st.) (Repeat w 2nd.)
a. Balance all except H n O.b. Balance O using H2O.c. Balance H using H+.d. Balance charge using electrons.
Step3: Equalize electronsStep4: Add the ½ reactions togetherStep5:
Reduction ½ rxn:2(6e- +14H+(aq) +Cr2O7
2-(aq) 2Cr+3
(aq) + 7H2O(l)) 12 28 2 4 14
Oxidation ½ rxn: C2H5OH(l) + 3H2O(l) 2CO2(aq) + 12H+(aq)+12e-
(+6) (+3) (–2) (+4)
![Page 112: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/112.jpg)
H+(aq) + Cr2O7
2-(aq) + C2H5OH(l) Cr+3
(aq) + CO2(aq) + H2O(l) Step1: Write ½ rxns.Step2: Balance ½ rxns. (Start with 1st.) (Repeat w 2nd.)
a. Balance all except H n O.b. Balance O using H2O.c. Balance H using H+.d. Balance charge using electrons.
Step3: Equalize electrons.Step4: Add the ½ rxns and cancel identical items.Step5: Check that elements and charges balance.
Reduction ½ rxn:12e- +28H+(aq)+2Cr2O7
2-(aq) 4Cr+3
(aq) +14H2O(l)
Oxidation ½ rxn: C2H5OH(l) + 3H2O(l) 2CO2(aq) + 12H+(aq)+12e-
C2H5OH(l)+16H+(aq)+2Cr2O7
2-(aq) 2CO2(aq)+4Cr+3
(aq)+11H2O(l)
(+6) (+3) (–2) (+4)
![Page 113: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/113.jpg)
Ex2) An aqueous soln of cyanide ion is often used to extract silver from ore. It occurs in a basic soln in the following reaction:
Ag(s) + CN-(aq) + O2(g) Ag(CN)2
-(aq)
Balance using ½ rxn method.
![Page 114: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/114.jpg)
HW#63b) Balance using ½ rxn method:
I-(aq) + ClO-
(aq) I3-(aq) + Cl-(aq)
Ch4 HW#9 p183 63(a,b), 65(a,b)
![Page 115: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/115.jpg)
Ch4 HW#9 p183 63(a,b), 65(a,b)63. Balance the following oxidation-reduction reactions that occur in acidic solutions.
a. Zn(s) + HCl(aq) Zn2+(aq) + H2(g)
![Page 116: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/116.jpg)
63. Balance the following oxidation-reduction reactions that occur in acidic solutions.
b. I-(aq) + ClO-(aq) I3-(aq) + Cl-(aq)
![Page 117: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/117.jpg)
65. Balance the following oxidation-reductions reactions that occur in basic solutions.
a. Al(s) + MnO4-(aq) MnO2(s) + Al(OH)4
-(aq)
![Page 118: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/118.jpg)
65. Balance the following oxidation-reductions reactions that occur in basic solutions.
b. Cl2(g) Cl-(aq) + OCl-(aq)
![Page 119: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/119.jpg)
Ch4 HW#10 p183 64(a,b),66(a,b)64. Balance the following oxidation-reduction reactions that occur in acid solution using the half-reactions method.
a. Cu(s) + NO3-(aq) Cu2+(aq) + NO(aq)
![Page 120: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/120.jpg)
64. Balance the following oxidation-reduction reactions that occur in acid solution using the half-reactions method.
b. Cr2O72-(aq) + Cl-(aq) Cr3+(aq) + Cl2(g)
![Page 121: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/121.jpg)
66. Balance the following oxidation-reduction reactions the occur in basic solution.
a. Cr(s) + CrO42(aq) Cr(OH)3(s)
![Page 122: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/122.jpg)
66. Balance the following oxidation-reduction reactions the occur in basic solution.
b. MnO4-(aq) + S2-(aq) MnS(s) + S(s)
![Page 123: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/123.jpg)
Ch4 Rev#1 p180+ 12c,16b,18d, 22,24e, 36(a,b)
12c. Show how Ca(OH)2 “breaks up” into its component ions
dissolving in water.
![Page 124: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/124.jpg)
16b. An 853.5-mg sample of KIO3 is dissolving in enough water
to make 250.0 mL of solution. Calculate the molarity.
![Page 125: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/125.jpg)
18d. Calculate the concentration of all ions present of 1.00 g K3PO4
in 250.0 mL of solution.
![Page 126: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/126.jpg)
22. How many grams of NaOH are contained in 250.0 mL of a 0.400 M sodium hydroxide solution.
![Page 127: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/127.jpg)
24e. How would you prepare 1.00 L of a 0.50 solution of sodium carbonate from the pure solid.
![Page 128: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/128.jpg)
36. Write net ionic equations for the reaction, if any, when aqueous solutions of the following are mixed.
a) Cobalt(III) chloride and sodium hydroxide.
b)Silver nitrate and ammonium carbonate.
Ch4 Rev#2 p180+ 42, 53, 62a, 67
![Page 129: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/129.jpg)
Ch4 Rev#2 p180+ 42, 53, 62a, 6742. What mass of barium sulfate is produced when 100.0 mL
of a 0.100M solution of barium chloride is mixed with 100.0 mL of a 0.100M solution of iron(III) sulfate?
Before After
FeBa
ClSO4
Cl
SO4 SO4
![Page 130: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/130.jpg)
53. A 25.00 mL sample of hydrochloric acid solution requires 24.16 mL of 0.106 M sodium hydroxide for complete neutralization. What is the concentration of the original hydrochloric acid solution?
![Page 131: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/131.jpg)
62a. Specify if Cu(s) + 2Ag+(aq) 2Ag(s) +Cu2+(aq) is a oxidation-reduction reaction, and identify the oxidizing agent, the reducing agent, the substance being oxidized, and the substance being reduced.
![Page 132: Ch4.1 – Types of Chemical Reactions and Solutions.](https://reader036.fdocuments.net/reader036/viewer/2022081420/56649ddf5503460f94ad8dad/html5/thumbnails/132.jpg)
67. Chlorine gas was first prepared in 1774 by C.W. Scheele by oxidizing sodium chlorine with manganese(IV) oxide. The reaction is:
NaCl(aq) + H2SO4(aq) + MnO2(s) Na2SO4(aq) + MnCl2(aq) + H2O(l) + Cl2(g)