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ch16_acid-base equilibrium
Course: CHM 116, Spring 2008School: Santa Monica
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Chapter 16: Acid-Base Equilibrium 1. Designate the Bronsted-Lowry acid and base on the left side of each equation, and also designate the conjugate acid and conjugate base on the right side. a. NH3(aq) + H2O(l) NH4+(aq) + OH (aq) - b. H3PO4(aq) + H2O(l) H2PO4 (aq) + H3O+(aq) - 2. Write the conjugate base of each of the following acids: a. HCN b. HCO3 - 3. Write the conjugate acid of each of the following bases: a....
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Chapter 16: Acid-Base Equilibrium 1. Designate the Bronsted-Lowry acid and base on the left side of each equation, and also designate the conjugate acid and conjugate base on the right side. a. NH3(aq) + H2O(l) NH4+(aq) + OH (aq) - b. H3PO4(aq) + H2O(l) H2PO4 (aq) + H3O+(aq) - 2. Write the conjugate base of each of the following acids: a. HCN b. HCO3 - 3. Write the conjugate acid of each of the following bases: a. HS - b. HPO42- 4. Describe the difference between strong acids and bases, and weak acids and bases when mixed with water. 5. Which of the following are acids are strong acids? HCl HNO3 H3PO4 H2S HF HBr 6. Which of the following are bases are weak bases? NaOH NH3 H2CO3 CO32 KOH Ba(OH)2 - 7. The concentration of <a href="/keyword/hydroxide-ion/" >hydroxide ion</a> , [OH ], in a solution was measured as 7.50 x 10-10 M. a. What is the concentration of hydronium ion, [H3O+], in this solution? b. What is the pH of this solution? c. Is this solution acidic or basic? 8. The pH of a solution was measured to be 2.84. a. What is the hydronium ion concentration, [H3O+]? - b. What is the <a href="/keyword/hydroxide-ion/" >hydroxide ion</a> concentration, [OH ]? c. What is the pOH? d. Is this solution acidic or basic? 9. What is the pH of 0.015 M KOH solution? 10. Order the compounds in each of the following groups from least acidic to most acidic. Explain why. a. H2O, NH3, HF b. HBrO3, HBrO, HBrO2 c. H2O, H2S, H2Se 11. A study of phenylacetic acid (abbreviated HPAc) shows that the pH of a 0.12 M HPAc solution is 2.60 at a specific temperature. What is the Ka of the phenylacetic acid at that temperature? (Hint: Write a balanced equation for the ionization HPAc in water and then fill in an "ICE" table) 12. Propanoic acid (CH3CH2COOH, abbreviated as HPr) has a Ka of 1.3x10-5. What is the pH of a 0.10 M HPr solution? (Hint: first determine [H3O+]) 13. Predict whether aqueous solutions of the following acids will be acidic, basic, or neutral. NaCl NaF NH4NO3 CaCl2 NH4Cl FeCl3 Cu(NO3)2 14. Complete the following table by calculating the missing entries. [H+] 3.5 x 10-3 M [OH-] 5.6 x 10-4 M 6.21 10.13 15. What is the pOH of 0.015 M KOH solution? pH pOH acidic or basic? 16. A solution is labeled 0.0075 M Sr(OH)2. What is the pH of the solution? 17. What is the Kb for F- if the Ka for HF is 6.8 x 10-4? 18. A 0.20 M solution of HC6H5O has a pH of 4.2. Calculate Ka. 19. The Ka for is HF 6.8 x 10-4. Calculate [OH-] for a solution containing 0.32M NaF. 20. The [H3O+] in a solution was measured as 6.87 x 10-12 M. a. What is the [OH-] in this solution? b. What is the pH of this solution? c. Is this solution acidic or basic? 21. The pH of a solution was measured to be 11.67. a. What is the hydronium ion concentration, [H3O+]? b. What is the <a href="/keyword/hydroxide-ion/" >hydroxide ion</a> concentration, [OH-]? c. What is the pOH? d. Is this solution acidic or basic? 22. A study of phenylacetic acid (abbreviated HPAc) shows that the pH of a 0.34 M HPAc solution is 1.89 at a specific temperature. What is the Ka of the phenylacetic acid at that temperature? 23. Propanoic acid (CH3CH2COOH, abbreviated as HPr) has a Ka of 1.3x10-5. What is the pH of a 0.25 M HPr solution?
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