Acids and Bases Homework Name ______
I. Conjugate Acid Base Pairs
Use the Bronsted-Lowry definitions of acids and bases to identify the acid, base, conjugate acid, and conjugate base in each of the following reactions. Fill in the arrows for each reaction.
Acid / Base / Conj. Acid / Conj. Basea. HF (aq) + H2O (l) H3O+ (aq) + F- (aq)
b. HCl (aq) + H2O (l) H3O+ (aq) + Cl- (aq)
c. HC2H3O2 (aq) + H2O (l) H3O+ (aq) + C2H3O2- (aq)
d. HNO3 (aq) + H2O (l) H3O+ (aq) + NO3 (aq)
e. NH3 (aq) + H2O (l) OH- (aq) + NH4+ (aq)
f. CH3COO- (aq) + H2O (l) CH3COOH (aq) + OH-
II. Acid Dissociation Constant Expressions
Complete the following reactions and write the acid dissociation constant expression.
1. HNO3 (aq) + H2O (l) ______+ ______2. H3BO3 (aq) + H2O (l) ______+ ______
3. H2SO3 (aq) + H2O (l) ______+ ______
4. HClO4 (aq) + H2O (l) ______+ ______
5. HC2H3O2 (aq) + H2O (l) ______+ ______
6. HF (aq) + H2O (l) ______+ ______
III. Base Dissociation Constant Expressions
Complete the following reactions and write the base dissociation constant expression.
1. C5H5N (aq) + H2O (l) ______+ ______2. C6H5NH2 + H2O (l) ______+ ______
3. (CH3)2NH (aq) + H2O (l) ______+ ______
4. N2H4 (aq) + H2O (l) ______+ ______
5. PO4-3 (aq) + H2O (l) ______+ ______
6. F- (aq) + H2O (l) ______+ ______
IV. Dissociation Constant Calculations
1. Acetic acid is a weak acid. It is the active ingredient in vinegar. If the initial concentration of acetic acid is 0.200M and the equilibrium concentration of H3O+ is 0.0019M, calculate Ka for acetic acid.
2. Ammonia is a weak base. If the initial concentration of ammonia is 0.150M and the equilibrium concentration of OH- is 1.6 x 10-3M, calculate Kb for ammonia.
3. Formic acid is a weak monoprotic acid. If the initial concentration of formic acid is 0.10M and the equilibrium concentration of H3O+ is 4.2 x 10-3M, calculate Ka for formic acid.
4. Cyanic acid is a weak monoprotic acid. If the initial concentration of cyanic acid is 0.150M and the equilibrium concentration of H3O+ is 4.8 x 10-2M, calculate the Ka for formic acid.
5. Isobutylamine is a weak base. If the initial concentration of isobutylamine is 0.055M and the equilibrium concentration of H3O+ is 4.8 x 10-2M, calculate Ka for isobutylamine.
6. Gallic acid is a weak monoprotic acid. If the initial concentration of gallic acid is 0.280M and the equilibrium concentration of H3O+ is 3.3 x 10-3M, calculate the Ka for gallic acid.
7. Trimethylamine is a weak base. If the initial concentration of trimethylamine is 0.390M and the equilibrium concentration of OH- is 4.4 x 10-3M, calculate Kb for trimethylamine.
8. Dipropylamine is a weak base. If the initial concentration of dipropylamine is 0.160M and the equilibrium concentration of OH- is 0.012M, calculate Kb for dipropylamine.
9. Uric acid is a weak acid. If the initial concentration of uric acid is 0.110M and the equilibrium concentration of H3O+ is 3.4 x 10-2M, calculate Ka for uric acid.
10. Butylamine is a weak base. If the initial concentration of butylamine is 0.230M and the equilibrium concentration of OH- is 8.6 x 10-6M, calculate Kb for butylamine.
V. Self-Ionization, pH & pOH Calculations
1. What is the concentration of hydroxide ions in saturated limewater if the hydronium ion concentration is 3.98 x 10-11M? Is the limewater acidic, basic, or neutral?
2. What is the concentration of hydronium ions in a wheat flour and water solution if the hydroxide ion concentration is 1.00 x 10-8M? Is wheat flour and water acidic, basic, or neutral?
3. What is the concentration of hydroxide ions in a potato and water solution if the hydronium ion concentration is 1.60 x 10-6M? Are potatoes and water acidic, basic, or neutral?
4. What is the concentration of hydronium ions in 0.1M ammonia is the hydroxide ion concentration is 1.68 x 10-3M? Is ammonia acidic, basic, or neutral?
5. What is the concentration of hydroxide ions in butter if the hydronium ion concentration is 6.750 x 10-7M? Is butter acidic, basic, or neutral?
You must solve the next five using the Kw formula and the next set of five using the pH + pOH formula, and the final five using any method you wish.
6. Analysis of a sample of maple syrup reveals that the concentration of the hydroxide ions is 5.0 x 1-8M. What is the pH of this syrup? Is it acidic, basic, or neutral?
7. In a sample of bananas and water, it is found that the hydronium ion concentration is 2.51 x 10-5M. What is the corresponding pOH value, and are the bananas and water acidic, basic, or neutral?
8. The hydroxide ion concentration in a sample of vinegar is 7.945 x 10-12M. What is the pH of the vinegar, and is it acidic, basic, or neutral?
9. A sample of human blood plasma is found to have a concentration of the hydronium ions of 3.72 x 10-8M. What is the pOH of this sample? Is it an acid, base, or neutral?
10. In a sample of saturated magnesia, it is found that the hydroxide ion concentration is 3.22 x 10-4M. What is the pH of this sample, and is it acidic, basic, or neutral?
11. Tomatoes are found to have a hydronium ion concentration of 6.2 x 10-5M. What is the pOH of these tomatoes, and are they acidic, basic, or neutral?
12. A saturated solution of calcium carbonate has a hydroxide concentration of 2.44 x 10-4M. What is the pH of this solution, and is it acidic, basic, or neutral?
13. The hydronium concentration in a urine specimen is measured to be 6.3 x 10-6M. What is the pOH of this sample, and is it acidic, basic, or neutral?
14. What is the pH of sour pickles if the hydroxide ion concentration is 1.6 x 10-10M? Are the pickles acidic, basic, or neutral?
15. The hydroxide content of a popular soft drink is measured and found to be 4.11 x 10-9M. What is the pH of this soft drink, and is it acidic, basic, or neutral?
16. Determine the hydroxide ion concentration of a solution with a pH of 4.35.
17. Determine the hydronium ion concentration of a solution with a pOH of 11.28.
18. Students found that a yogurt sample had a pH of 2.85. What are the hydronium and hydroxide ion concentrations?
19. Find the hydronium and hydroxide ion concentration for lemon juice with a pOH of 11.10.
20. A solution has a pH of 10.81.
a. Find the hydroxide ion concentration for this solution.
b. Verify your answer using a different method.
VI. Titration
1. A volume of 30.mL of 0.25M hydrochloric acid neutralizes a 50.0mL sample of potassium hydroxide solution. What is the concentration of the potassium hydroxide solution?
2. How many milliliters of 0.0947M sodium hydroxide are needed to neutralize 21.4mL of 0.106M perchloric acid?
3. A volume of 9.0mL of 0.70M ammonium hydroxide neutralizes a 35mL sample of selenic acid. What is the concentration of the selenic acid?
4. How many milliliters of 0.200M potassium hydroxide will exactly neutralize 15.0mL of 0.400M sulfuric acid?
5. A volume of 90mL of 0.2M hydrobromic acid neutralizes a 60mL sample of calcium hydroxide solution. What is the concentration of the calcium hydroxide?
6. What volume of 0.126M lithium hydroxide is required to neutralize 25.0mL of 0.413M sulfuric acid?
7. What volume of 0.522M hydroiodic acid is required to titrate 25.0mL of 0.50M strontium hydroxide?
8. A volume of 37mL of 0.36M potassium cyanide neutralizes a 75mL sample of hypochlorous acid. What is the concentration of hypochlorous acid?
9. Calculate how many milliliters of 0.300M sulfuric acid must be added to titrate 75mL of 0.10M ammonium hydroxide.
10. A volume of 46mL of 0.40M rubidium hydroxide neutralizes an 80.mL sample of cyanic acid solution. What is the concentration of the cyanic acid?