Problem set on Chapter 16, 17

Work as many of these problems in class as you can. You may use your textbook to find the necessary constants. These constants will be provided on the exam. The whole idea of this worksheet is to practice recognition of the type of equilibrium problem presented.The problem set and answers will be posted on Blackboard.

1. What is the pH of a 0.020 M solution of Ba(OH)2?

2. What are the concentration of all species in solution for a solution that is 0.30M in HCN and 0.40M in NaCN?

3. Find the concentration of all species in solution for a 0.45M solution of HNO3.

4. Find the concentration of all species in solution for a 0.45M solution of HNO2.

5. Find the concentration of all species in solution for a 0.45M solution of NaNO3.

6. Find the concentration of all species in solution for a 0.45M solution of KNO2.

7. What is the pH of a 0.35M solution of CH3NH2?

8. Find the concentration of all species in solution for a 0.45M solution of CH3NH2 and 0.30 M in CH3NH3Br?

9. What is the molar solubility of chromium(III) hydroxide?

10. If a solution contains 0.0050 M SO42-, what concentration of barium ions will remain

in solution?

11. If 200. mL of 0.0040 M calcium nitrate is mixed with 400. mL of 0.00033 M sodium carbonate, will a precipitate form?

12. A 100. mL volume of solution initially contains 0.50 M of CN ˉ and 0.10 M Cu2+ and can form a complex ion. What concentration of Cu2+ ions will remain in solution at equilibrium? The equilibrium is shown below:

Cu2+(aq) + 4 CN ˉ(aq) ↔ Cu(CN)42-(aq)