Acids and Bases (You may not know it, but they’re everywhere!!)
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Transcript of Acids and Bases (You may not know it, but they’re everywhere!!)
Acids and Bases(You may not know it, but they’re everywhere!!)
Everyday Acids
Acids make food taste sour Lemon and orange juice contains citric acid Vinegar contains acetic acid Milk products (and sore muscles) contain
lactic acid
Stomach acid helps digest food
Car batteries contain sulfuric acid
Everyday Bases
Soaps and cleaners contain basesAmmonia (NH3)
Bleach (NaClO)
Antacids contain bases Milk of magnesia is magnesium
hydroxide
Baking soda is sodium bicarbonate (NaHCO3)
Physical Properties of Acids and Bases
Property Acids BasesColour of Red Litmus Paper No change (red) Blue
Colour of Blue Litmus Paper Red No change (blue)
Colour when Phenolphthaline Indicator is added
No change (clear and colourless)
Bright pink
Colour when Red Cabbage Juice Indicator is added
Red Yellow
Taste Sour Bitter Texture Water-like Slippery Solubility in Water Very good
Form ions Very good Form ions
Electrical Conductivity Very good because acids form ions in water
Very good because bases form ions in water
Chemical Properties of Acids and BasesProperties Acids Bases
Chemical Reactivity
Very corrosive React with some
metals to produce H2 gas
React with carbonates
React with bases to produce a salt and water (neutralization reactions)
Somewhat corrosive
Break down proteins (denaturation reactions)
React with acids to produce a salt and water (neutralization reactions)
Commercial Uses
Used as catalysts Used in refining oil,
making fertilizers, electroplating metals
Used in antacids, cleaners
Acids and Bases “Ionize” in Water
This means that the bonds between ions in acids (or bases) break when they dissolve in water
That leaves the ions free to float around separately
That’s what makes acids and bases good conductors of electricity!
H2O
H2O
H2O
H2O
H2O
H2O
H2O
H2O
H2OH2O
H+ H+
H+
H+
H+H+
H+
H+ Cl-
Cl-
Cl-
Cl-
Cl-
Cl-
Cl-
Cl-
H2O
Acids are Proton (H+ ion) Donors
When dissolved in water, one of the ions that an acid releases is H+ Strong acids are 100% (or nearly so) ionized in water Therefore, they are good H+ donors
HCl H2SO4 HNO3
hydrochloric acid sulfuric acid nitric acid
Weak acids are usually less than 5% ionized in solution
Therefore, they are poor H+ donors
H3PO4 HC2H3O2
phosphoric acid acetic acid
Bases are Proton (H+ ion) acceptors
Bases also ionize in solution
One of the ions released by a base is often an hydroxide ion
(OH-)
NaOH KOH Ca(OH)2
sodium hydroxide potassium hydroxide calcium hydroxide
Bases are also classified as weak or strong based on the
degree of ionization in water The OH- from a base, combines with the H+ from an acid to
form water
H+ + OH- → H2O
Acids and Bases “Neutralize” Each Other
Acids and bases react in “NEUTRALIZATION”
reactions
The reactants are always an acid and a base
The products always include a salt and water
HCl + NaOH → NaCl + H2O
acid base salt water
Measuring Acids and Bases
Acids and bases have a unique scale for measuring their
relative strength
It’s called the pH scale
pH stands for the “power of hydrogen” because the scale is
based on the concentration of H+ ions in solution
The scale goes from 0 to 14
Acids have a pH less than 7 (H+ > OH-)
Bases have a pH greater than 7 (H+ < OH-)
Distilled water has a pH of 7 which is neutral (H+ = OH-)
The pH Scale
0 1 2 3 4 5 6 7 8 9 10 11 12 13 14
NeutralVery Acidic Very Basic
(Alkaline)
more H+ than OH- more OH- than H+
H+ equals OH-
The pH scale is logarithmic That means that the space between successive numbers represents a 10X increase or decrease