C. Johannesson III. Titration/Neutralization 18.4 Ch. 18- Acids & Bases.
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Transcript of C. Johannesson III. Titration/Neutralization 18.4 Ch. 18- Acids & Bases.
C. Johannesson
III. Titration/Neutralization18.4
III. Titration/Neutralization18.4
Ch. 18- Acids & BasesCh. 18- Acids & Bases
C. Johannesson
A. NeutralizationA. Neutralization
ACID + BASE ACID + BASE SALT + WATER SALT + WATER
HCl + NaOH HCl + NaOH NaCl + H NaCl + H22OO
HCHC22HH33OO22 + NaOH + NaOH NaC NaC22HH33OO22 + H + H22OO
• Salts can be neutral, acidic, or basic.
• Neutralization does not mean pH = 7.
weak
strong strong
strong
neutral
basic
C. Johannesson
B. TitrationB. Titration
TitrationTitration• Analytical method
in which a standard solution is used to determine the concentration of an unknown solution.
standard solution
unknown solution
C. Johannesson
Equivalence pointEquivalence point• Point at which equal amounts of
H3O+ and OH- have been added.
B. TitrationB. Titration
C. Johannesson
Equivalence pointEquivalence point• Determined by…
• indicator color change–phenolpthalein turns hot pink in a base
B. TitrationB. Titration
C. Johannesson
Equivalence point Equivalence point • Determined by…
• dramatic change in pH
B. TitrationB. Titration
B. Titration and NeutralizationB. Titration and Neutralization
The solution of known concentration is called the standard solution
• added by using a buret Continue adding until the
indicator changes color
• called the “end point” of the titration
• end points are different for different indicators
B. Titration StepsB. Titration Steps
1. A measured volume of acid of known concentration is added to a flask
2. Several drops of an indicator are added
3. A base of unknown concentration is slowly added and swirled until the indicator changes color; measure the volume delivered by the buret
B. Titration ProcessB. Titration Process
C. Johannesson
C. Johannesson
B. TitrationB. Titration
moles H3O+ = moles OH-
MV n = MV n
M: MolarityV: volumen: # of H+ ions in the acid
or OH- ions in the base
C. Johannesson
B. TitrationB. Titration
42.5 mL of 1.3M KOH are required to neutralize 50.0 mL of H2SO4. Find the molarity of H2SO4.
H3O+
M = ?V = 50.0 mLn = 2
OH-
M = 1.3MV = 42.5 mLn = 1
MV# = MV#M(50.0mL)(2)
=(1.3M)(42.5mL)(1)
M = 0.55M H2SO4
WorksheetWorksheet
Complete the worksheets on titration
C. Johannesson