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Chemistry Exercise: Identifying Substances and Calculating pH and Equilibria, Exercises of Chemistry

Alliance UniversityChemistry

A chemistry exercise that involves identifying the properties of various substances as strong acids, weak acids, strong bases, weak bases, acidic salts, basic salts, or neutral salts. It also includes questions on calculating the ph of solutions of different concentrations of acids and bases, and determining the concentrations of solutes in complex solutions. The exercise includes equations for the ionization of acetic acid and ammonia, and questions on the solubility of silver bromide and silver chromate.

Typology: Exercises

2011/2012

Uploaded on 12/23/2012

saiba
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1. 20 pts. Consider aqueous solutions of each of the following substances and fill in the
blanks with one of these descriptors: (strong acid, weak acid, strong base, weak base,
acidic salt, basic salt, neutral salt):
a. KOH ______________________________
b. KNO3 ______________________________
c. KNO2 ______________________________
d. HCN ______________________________
e. NH4Cl ______________________________
f. (CH3)3N ______________________________
g. Ni(NO3)2 ______________________________
h. HF ______________________________
i. NaF ______________________________
j. HBr ______________________________
2. 4 pts. Do you think that an aqueous solution of ammonium fluoride (NH4F) will be
acidic, basic, or neutral? Explain how you obtained your answer.
Questions 3-14 are each worth 5 points:
3. What is the pH of a 0.28 M HNO3(aq) solution?
a) -0.55 b) 0.28 c) 0.55 d) 1.27
4. What is the pH of a 2.1 × 10-5 M NaOH(aq) solution?
a) -4.68 b) 4.68 c) 3.23 d) 9.32
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  1. 20 pts. Consider aqueous solutions of each of the following substances and fill in the blanks with one of these descriptors: (strong acid, weak acid, strong base, weak base, acidic salt, basic salt, neutral salt):

a. KOH ______________________________

b. KNO 3 ______________________________

c. KNO 2 ______________________________

d. HCN ______________________________

e. NH 4 Cl ______________________________

f. (CH 3 ) 3 N ______________________________

g. Ni(NO 3 ) 2 ______________________________

h. HF ______________________________

i. NaF ______________________________

j. HBr ______________________________

  1. 4 pts. Do you think that an aqueous solution of ammonium fluoride (NH 4 F) will be acidic, basic, or neutral? Explain how you obtained your answer.

Questions 3-14 are each worth 5 points:

  1. What is the pH of a 0.28 M HNO 3 (aq) solution? a) -0.55 b) 0.28 c) 0.55 d) 1.
  2. What is the pH of a 2.1 × 10 -5^ M NaOH(aq) solution? a) -4.68 b) 4.68 c) 3.23 d) 9.
  1. What is the H 3 O+^ concentration of an aqueous solution with a pH of 12.17? a) 6.8 × 10 -13^ M b) 1.9 × 10 -9^ M c) 5.2 × 10 -6^ M d) 1.5 × 10 -2^ M
  2. What is the OH-^ concentration of an aqueous solution with a pH of 11.45? a) 3.5 × 10 -12^ M b) 9.4 × 10 -10^ M c) 1.1 × 10 -5^ M d) 2.8 × 10 -3^ M
  3. Write a chemical equation showing how acetic acid (CH 3 COOH) behaves as a weak acid. Label the acid, the base, the conjugate acid, and the conjugate base in this equation:
  4. Write a chemical equation showing how ammonia (NH 3 ) behaves as a weak base. Label the acid, the base, the conjugate acid, and the conjugate base in this equation:
  5. What is the pH of 0.015 M aqueous benzoic acid? a) 1.82 b) 3.03 c) 4.20 d) 6.
  6. The pH of a 0.050 M solution of weak base is 11.24. What is the K b of this unknown? a) 6.6 × 10 -22^ b) 10 -125.8^ ×c) 10 -5^ 6.3 × d) 10 -3 1.7 ×
  7. What is the pH of an aqueous solution of 0.30 M HF and 0.15 M F-? a) 1.83 b) 2.86 c) 3.14 d) 3.
  8. A volume of 25.0 mL of 0.100 M HCOOH(aq) is titrated with 0.100 M NaOH(aq). What is the pH after the addition of 12.5 mL of NaOH? a) 2.52 b) 3.73 c) 4.74 d) 7.
  9. The K sp of AgBr is 5.40 × 10 -13^ at 25 °C. Calculate the molar solubility of AgBr at this temperature. a) 8.11 × 10 -15^ mol/L b) 3.60 × 10 -11^ mol/L c) 1.12 × 10 -8^ mol/L d) 7.35 × 10 -7^ mol/L

Extra Credit. 10 pts. A certain weak base with Kb equal to 5.41 x 10 -6^ is titrated with a 0.100 M HNO 3 solution. If we begin with 50.00 mL of a 0.100 M solution of the weak base, calculate the pH at the following points during the titration and make a sketch of the titration curve. Circle your answers for each part.

mL of HNO 3 : a. 0.00 b. 25.00 c. 48.00 d. 50.00 e. 52.