1. Acids, Bases and Salts
Acids give up hydrogen ions (H+) in a water solution.
Bases give up hydroxide ions (OH-) in a water solution.
Mullis

2. Properties of Bases Bitter taste Feel slippery if you touch them
pH > 7.0
Strong bases:
Sodium hydroxide (NaOH)
Potassium hydroxide (KOH)
Weak bases:
Sodium bicarbonate (NaHCO3)
Mullis

3. Properties of Acids Sour taste pH < 7.0
React with metals to form H2 gas
Strong acids:
Sulfuric acid (H2SO4)
Hydrochloric acid (HCl)
Weak acids:
Acetic acid (vinegar – CH3COOH))
Citric acid (in fruits)
Ascorbic acid (Vitamin C)
Mullis

4. Naming Acids Binary Acid = 2 elements (HCl)
Begin with hydro-.
Use name of 2nd element and end with –ic.
HCl is hydrochloric acid.
Oxyacid = H + O + 3rd element (H2SO4)
Usually incorporates the polyatomic ion name into the acid name.
Written with H first, then the polyatomic ion.
H2SO4 is sulfuric acid.
Mullis

5. Acid Strength Strong acids ionize completely in water.
Many H3O+ ions
Strong electrolyte
Weak acids do not ionize completely in water.
Some H3O+ ions
Weak electrolyte
The ionized H3O+ ions are being bonded back to the negative species (reverse reaction) at the same time some acid molecules are being ionized to form H3O+ ions .
Strong and weak bases are similar, except ion involved is OH- instead of H3O+ .
Mullis

6. Acid-Base Systems Type Acid Base Examples Arrhenius
H+ or H3O+ producer
OH- producer
HNO3 + H2O H3O+ + NO3-
NH3 + H2O NH4+ + OH-
Brønsted-Lowry
proton (H+) donor
proton (H+) acceptor
HCl + NH NH4+ + Cl-
Lewis
electron pair acceptor
electron pair donor
BF3 + F BF4-
BF3 is Lewis acid,
F- is Lewis base
Mullis

7. Brønsted-Lowry Acids Brønsted-Lowry acids donate a proton.
A monoprotic acid donates one proton per molecule, such as HCl and HClO4.
A polyprotic acid donates more than one proton per molecule, such as H2SO4 and H3PO4.
H2SO4 is a diprotic acid.
H3PO4 is a triprotic acid.
Mullis

8. Conjugate acids and bases
The species remaining after a Brønsted-Lowry acid gives up its proton is the conjugate base of that acid: Take off one H from the acid.
The species remaining after a Brønsted-Lowry base accepts its proton is the conjugate acid of that base: Take off one H. Add an H to the base.
CH3COOH(aq) + H2O(l) H3O+(aq) + CH3COO- (aq)
acid base conjugate conjugate
(proton donor) acid base
Mullis

9. Examples of conjugate acids and bases
HCO3- (aq) + H2O(l) H2CO3 (aq) + OH- (aq)
base acid conjugate conjugate
(proton acid base
acceptor)
HF(aq) + H2O(l) H3O+(aq) + F- (aq)
acid base conjugate conjugate
(proton acid base
donor)
Mullis

10. Measuring Strength of Acids and Bases
pH is a measurement which indicates acidic or basic strength, measuring the concentration of H+ ions.
More H+ ions = lower pH = acid.
An indicator changes color depending on pH of a solution.
pH paper is treated with indicators to change color when dipped in a solution.
1: acid
7: neutral
14: base
Mullis

11. The Hydronium Ion
Ionization is the creation of ions from a molecular compound.
If the force of attraction between solvent molecules and parts of the solute are stronger than the covalent bonds of the solute, the solute breaks into ions.
In water, HYDRATION produces heat, which provides energy to break more covalent bonds.
H + attracts other molecules or ions
In water, H+ becomes a proton bonded to the oxygen of a water molecule.
The hydronium ion is H3O+. + H - Cl Cl H H + O H O + H H
Mullis

12. Salts
An acid and base combined together react to neutralize each other.
Neutralization is a process which produces produces that are not acids or bases.
H+ and OH- make water.
The remaining reactants combine to make a salt.
A salt is an ionic compound made of a metal and a nonmetal.
Soap and detergent are organic salts.
Mullis

13. Neutralization HCl + NaOH NaCl + H2O HNO3 + KOH KNO3 + H2O
ACID + BASE YIELDS SALT + WATER
acid
base
salt
water
Mullis

14. Neutralization
The reaction between an acid and a base which produces a salt and water.
Recall: A salt is an ionic compound: metal + nonmetal which is likely to dissociate in water.
Ex: You take a dose of the antacid magnesium hydroxide, Mg(OH)2, to relieve excess stomach acid, HCl.
What is the chemical equation for this neutralization reaction?
HCl + Mg(OH)2 MgCl2 + H2O
These products are magnesium chloride and water.
Mullis

15. pH and acidity
pH is related to the concept of concentration of hydronium ions found in water.
Water and all its solutions contain hydronium ions and hydroxide ions.
Acidic solutions: More H3O+ ions.
Basic solutions: Fewer H3O+ ions / more OH- ions.
If pH = 2:
H3O+ ion concentration = 0.01 M
OH- ion concentration = M
If pH = 12:
H3O+ ion concentration = M
OH- ion concentration = 0.01 M
Mullis

16. The pH scale pH = -log [H3O+] pH stands for “power of hydronium ion.”
pH value is the exponent on the power of 10 with its sign changed.
Mullis

17. pH examples Example 1: Example 2: 0.001 mol H3O+ = 1 x 10-3 mol H3O+
Concentration is 0.001M
pH = -log [H3O+] = -log (1x 10-3 ) = -(-3.0) = 3.0
pH is This is an acid.
Example 2:
mol H3O+ = 1 x 10-8 mol H3O+
Concentration is M
pH = -log [H3O+] = -log (1x 10-8 ) = -(-8.0) = 8.0
pH is This is a base.
Mullis

18. pOH pOH = -log [OH-] pH + pOH = 14.0
pOH is the negative of the logarithm of the hydroxide ion (OH-) concentration.
pOH = -log [OH-]
pH + pOH = 14.0
at 25 deg. C
Mullis

19. Buffers
Why is the pH of some lakes unaffected by acid rain even when they are downwind of big polluters?
The lakes are surrounded by soils which neutralize the acidic precipitation.
One way to neutralize acid is to add a base. Limestone (CaCO3) is a weak base.
Another way to neutralize either an acid or a base is to add a buffer.
A buffer is a substance or combination of substances capable of neutralizing limited quantities of either acids or bases.
Mullis

20. Buffers
Calcium carbonate around a lake contaminated with acid rain would react this way:
CaCO H3O Ca HCO3- + H2O
The polyatomic ion HCO3- acts as a buffer:
HCO H3O H2O CO2
HCO OH- H2O CO32-
Another buffer is the hydrogen phosphate ion. Possible sources of this ion are Na2HPO4 and NaH2PO4.
H3O+ + H2PO H2PO H2O
Mullis