Toyota Chapter 17 Review 5

1.  Next to the acids listed below, circle all the applicable descriptions:

  1. HCl Arr. acid B/L acid Lewis acid Strong Polyprotic
  2. NH4+ Arr. acid B/L acid Lewis acid Strong Polyprotic
  3. Acetate Arr. acid B/L acid Lewis acid Strong Polyprotic
  4. HF Arr. acid B/L acid Lewis acid Strong Polyprotic
  5. H2SO4 Arr. acid B/L acid Lewis acid Strong Polyprotic
  6. Fe3+ Arr. acid B/L acid Lewis acid Strong Polyprotic
  7. BH3 Arr. acid B/L acid Lewis acid Strong Polyprotic
  8. Chloride Arr. acid B/L acid Lewis acid Strong Polyprotic

2.  Calculate the following:

  1. The pH of a 0.75 M solution of NaOH
  1. The pOH of a solution that is 1.3 x 10-4 M in hydronium
  1. The [H3O+] of a solution with pH 8.5

3.  Indicate whether the salts below are expected to be acidic, basic, or neutral:

  1. NaCl acidic neutral basic
  2. NaHSO4 acidic neutral basic
  3. NH4Cl acidic neutral basic
  4. KCH3CO2 acidic neutral basic
  5. Al(H2O)6+3 acidic neutral basic
  6. Fe(H2O)5(OH)+2 acidic neutral basic
  7. NaCO3 acidic neutral basic
  8. KSO4 acidic neutral basic
  9. NH4HCO3 acidic neutral basic

4.  Write the reaction that occurs when chili-eating-champion Bill “Smokehouse” Stevenson treats his heartburn with Tums. Bill’s stomach acid is primarily HCl and the active ingredient in Tums is CaCO3. Be sure to show why Bill gets a little gassy (from the Tums, not the chili—that’s another story).

5.  Consider a 125 mM NaF solution. Identify ALL species in solution and calculate the concentration of each.

6.  Estimate product concentrations when the following come to equilibrium. Also determine the pH values for a and c. You shouldn’t need a calculator.

  1. 0.010 M solution of HNO3
  1. 0.10 M solution of acetic acid
  1. 0.005 M solution of Ca(OH)2

7.  Calculate the pH of a 25.0 mL solution that is 0.025 M in NH3.

  1. What is the pH if 5.0 mL of 0.1 M H2SO4 are added?
  1. What is the pH if the 25.0 mL solution (0.025 M in NH3) also contains 0.013 NH4Cl?

8.  A concentrated solution of salicylic acid, C6H4OHCOOH, used to synthesize acetyl salicylic acid, a.k.a. aspirin, contains 2.2 g per L of solution. If the solution has a pH of 2.43 what is the value of Ka for salicylic acid?

9.  A delicious fruit drink contains 11.0 g of tartaric acid, H2C4H4O6, and 20.0 g of its potassium salt per L. What is the pH of the drink? Ka1 = 1.0 x 10-3.

10.  What is the pH of the solution when 25 mL of 0.065 M benzylamine, C7H7NH2, is titrated to the equivalence point with 0.050 M hydrochloric acid? Kb for benzylamine is 4.7 x 10-10.

11.  The following are dissolved in water. List them in order of most acidic solution to the most basic.

NaF HClO4 NaCH3COO NH4Cl NaCN NaHCO3

KH2PO Sr(OH)2 NaCl

most acidic most basic

12.  One of the important buffers in the blood comprises hydrogen carbonate and carbonate. What is the ratio of CO3-2 to HCO3- if the pH is 7.45?

13.  In the following pairs, choose the stronger acid:

  1. HClO3 and HClO2
  1. CH3CH2CCl2OH and CH3CH2CI2OH

c.  Fe(H2O)6+3 or Fe(H2O)6+2

14.  Draw the Lewis structure for propionic acid (CH3CH2COOH) and explain why it has a pKa of 4.7 and propanol (CH3CH2CH2OH) has a pKa of about 16.

15.  What is the pH of a 2.0 M solution of HNO3?

16.  If the pKa of HCN is 9.31, what is the Kb for CN-?

17.  The pH of a solution is 4.3, what is the pOH?

18.  Morphine, a naturally occurring alkaloid base, helps with my chronic pain in the ass. What is the pH of a 7.5 mM solution of morphine? The Kb is 1.6 x 10-6.

19.  A 0.325 g tablet of aspirin (C6H4OHCOOH, remember) is dissolved in 0.500 L of water. What is the pH of the solution? Ka is 3.3 x 10-4.