Chapter 19 Study Guide ANS
1. List the properties of acids and bases.
Acids – taste sour, release hydrogen gas when reacted with active metals, react with bases
to produce salts and water, turn litmus red, are electrolytes (conduct electricity)
Bases – taste bitter, feel slippery, react with acids producing salt and water, turn litmus blue,
are electrolytes (conduct electricity)
2. Define monoprotic, diprotic, and triprotic acids. Give an example of each.
Monoprotic – contains one acidic H (HCl, CH3COOH, HI)
Diprotic – contains two acidic Hs (H2SO4)
3. Define a strong acid.
A substance that is a strong electrolyte and that nearly completely ionizes and produces
H3O+.
4. Define a strong base.
A substance that is a strong electrolyte and that nearly completely ionizes and produces
OH-.
6. Define a Bronsted-Lowry acid and base.
Acid – proton donor
Base – proton acceptor
7. In the equation HCl(g) + H2O(l) ↔ H3O+(aq) + Cl–(aq), identify the acid, base, conjugate
acid, and conjugate base.
Acid, base, conjugate acid, conjugate base
8. In the reaction NH3 + H2O NH4+ + OH–, identify the acid, base, conjugate acid, and
conjugate base.
Base, acid, conjugate acid, conjugate base
9. Define a conjugate acid.
Compound formed after the addition of a proton to a base
10. Define a conjugate base
Compound that remains after the acid has given up a proton
11. Define a conjugate acid-base pair.
Species that appear on opposite sides of an equation and differ by a proton
12. In the reaction HF + H2O H3O+ + F–, identify the conjugate acid-base pairs
HF and F- H2O and H3O+
13. In the reaction HClO3 + NH3 NH4+ + ClO3–, identify the conjugate acid-base pairs
HClO3 and ClO3- NH3 and NH4+
14. In the reaction CH3COOH + H2O H3O+ + CH3COO–, identify the conjugate acid –
base pairs.
CH3COOH and CH3COO- H2O and H3O+
15. Define amphoteric
Species that reacts as acid or a base
16. What is the pH, pOH, [H3O+], and [OH-] for pure water?
pH = 7 pOH = 7 [H3O+] = 1.0 x 10-7 M [OH-] = 1.0 x 10-7 M
17. How do you know if a solution is acidic or basic?
Acid – pH < 7 pOH > 7 [H3O+] > [OH-] [H3O+] > 1.0 x 10-7M
[OH-] < 1.0 x 10-7 M
Base – pH >7 pOH < 7 [H3O+] < [OH-] [H3O+] < 1.0 x 10-7M
[OH-] > 1.0 x 10-7 M
18. What is the pH of a 10-3 M HCl solution?
HCl is a strong acid, dissociates completely so HCl conc=H+ conc
pH = -log(10-3) = 3
19. What is the pH of a 10-4 M KOH solution?
Strong base, pOH = -log(10-4) =4 pH = 14-4 = 10
20. If [H3O+] = 1.7 x 10-5 M, what is the pH of the solution?
pH = -log(1.7 x 10-5)
21. If [H3O+] = 8.26 x 10-3 M, what is the pH of the solution?
pH = -log(8.26 x 10-3)
22. What is the pH of a solution whose hydronium ion concentration is 5.03 x 10-2 M?
pH = -log(5.03 x 10-2)
23. What is the pH of a 0.0056 M KOH solution?
pOH = -log (0.0056) = 2.25
pH = 14 – 2.25 = 11.75
24. What is the pH of a 0.000066 NaOH solution?
pOH = -log (0.000066) = 3.18
pH = 14 – 3.18 = 10.81
25. What is the hydronium ion concentration of a solution whose pH is 8.97?
[H+] = 10^-pH = 10^-8.97 = 1.07 x 10-9 M
26. What is the hydronium ion concentration of a solution whose pH is 3.55?
[H+] = 10^-pH = 10^-3.55
27. What is the hydroxide ion concentration of a solution whose pH is 9.43?
[H+] = 10^-pH = 10^-9.43 = 3.72 x 10-10 M
[OH-] = 1.0 x 10-14/3.72 x 10-10 =
28. Write and balance the neutralization equation for nitric acid and potassium hydroxide. Is
the resulting solution acidic, basic, or neutral?
HNO3 + KOH  KNO3 + H2O
29. When a strong acid and weak base are neutralized the resulting solution is _acidic___.
30. When a strong base and weak acid are neutralized the resulting solution is __basic__.
31. Write all of the ionization equations for phosphoric acid, H3PO4. Write the 3 equilibrium
constant expressions.
32. Write the dissociation equation for barium hydroxide.
Ba(OH)2  Ba+2 + 2OHRemember aqueous symbols
33. Write the dissociation equation for the base methyl amine, CH3NH2. Write the Kb
expression.
CH3NH2 + H2O  CH3NH3+ + OHAll are aqueous except liquid water
34. How many acidic hydrogens does acetic acid, HC2H3O2 have?
1, hydrogens bonded to C are not acidic
35. How many acidic hydrogens does sulfurous acid, H2SO3 have?
2
36. Na2CO3 = basic, NH4Cl = acidic, KBr = neutral