Chapter 11: Acids & Bases

Which of the following is a correct statement for a solution with a pH of 8.00? a) The hydroxide ion concentration is greater than the hydronium ion concentration b) The hydronium ion concentration is 8.0 M c) The hydroxide ion concentration is 1.0 x 10-8 M d) None of the above.

a) The hydroxide ion concentration is greater than the hydronium ion concentration

A buffer solution: a) all of the above b) maintains the pH of the solution. c) resists pH changes when an acid or base is added d) contains a weak acid and its salt, or a weak base and its salt.

a) all of the above

A solution with a pH of 12.0 is a) strongly basic b) strongly acidic c) weakly acidic d) weakly basic

a) strongly basic

Lemonade has [H3O+] of 1.0 x 10-4 M. What is the pH of the lemonade? a) 2.00 b) 4.00 c) 10.00 d) 14.00

b) 4.00 Reason: pH= -log[H3O+] = -log(1.0 x 10-4) = 4.00

Which of these solutions will form a buffer? a) KOH and HCl b) H2CO3 and NaHCO3 c) KF and HBr d) HCN and HF

b) H2CO3 and NaHCO3 Reason: Buffers consist of weak acids and their salts, for example, H2CO3 and NaHCO3; or weak bases and their salts, for example, NH3 and NH4Cl.

Which of the following equations represents an acid-base neutralization reaction? a) H2SO4 + Zn → ZnSO4 + H2 b) HNO3 + KOH → KNO3 + H2O c) Ba(OH)2 + Na2SO4 → BaSO4 + 2NaOH d) No correct answer

b) HNO3 + KOH → KNO3 + H2O Reason: In acid and base neutralization reactions, salts and water are produced. The neutralization reaction is also a double replacement reaction.

According to the Bronsted-Lowry theory, a base is a(n) __________. a) proton donor b) proton acceptor c) electron donor d) electron acceptor

b) proton acceptor Reason: Brownsted-Lowry's law states that acids donate protons and bases accept protons.

Which of the following does not describe an acidic solution? a) the pH is less than 7.0 b) the [OH-] is greater than 1.0 x 10-7 c) the [H3O+] is greater than the [OH-] d) the [OH-] is 6.0 x 10-10

b) the [OH-] is greater than 1.0 x 10-7

The pH of a solution for which [OH-] = 1.0 x 10-6 M is ______. a) 6.00 b) 1.00 c) 8.00 d) -6.00

c) 8.00

In which of the following pairs of acids are both members of the pair strong acids? a) H2SO4 and H2SO3 b) HNO3 and HNO2 c) HCl and HNO3 d) no correct answer

c) HCl and HNO3 Reason: The five strong acids are: 1. HCl 2. HNO3 3. HBr 4. HI 5. H2SO4

Which of the following pairs of substances are both members of the pair salts? a) H2SO4 and BaSO4 b) NaCl and NaOH c) NH4Cl and K2CO3 d) HNO3 and KOH

c) NH4Cl and K2CO3

A weak acid a) ionizes completely in water to give only ions b) dissolves in water only as molecules. c) ionizes slightly in water to give mostly molecules and a few ions. d) does not dissolve in water.

c) ionizes slightly in water to give mostly molecules and a few ions.

Which of the following statement is correct for the Bronsted-Lowry acid-base reaction: HCN + HCO3- ↔ CN- + H2CO3 a) HCO3- and CN- are a conjugate acid-base pair. b) HCO3- is the conjugate base of HCN. c) HCN is the conjugate acid of HCO3- d) HCN is the conjugate acid of CN-

d) HCN is the conjugate acid of CN- Reason: HCN and CN- are a conjugate acid-base pair since they differ by one H+. HCN is the conjugate acid of CN-, and CN- is the conjugate base of HCN.

When a strong acid neutralizes a strong base _________. a) a salt is produced. b) water is produced. c) the amount of H3O+ equals the amount of OH-. d) all of the above.

d) all of the above.