CHEM 1403                                                                            ________________________

COOP 5                                                                                                           (name)

Dr. Robert E. Belford           

 

 

 

1. (25 pts) What is the pH of a solution which is 1.0 x 10-4M in HNO3?

 

 

 

 

 

2. (25 pts) What is the hydonium ion concentration of a solution which is 3 M in hydrocyanic acid (HCN),  Ka (HCN) =  4.9 x 10-10?

 

 

 

 

 

 

3.  Consider a solution which is 3M in sodium cyanide (NaCN), Ka (HCN) =  4.9 x 10-10 .

 

 

 

a. (20 pts) What is the hydroxide ion concentration?

 

 

 

 

 

 

b.  (5 pts) What is the pOH?

 

 

 

 

 

 

c.  (5 pts)What is the pH?

 

 

 

 

 

                                   

 

4.  Determine via chemical equation whether aqueous solutions of the following salts are neutral,  acidic or basic.(20 pts)

 

a.  NaCl

 

 

 

 

 

b. NH4Cl        

 

 

 

 

 

 

5.  Consider the titration of 50.00 mL of 0.100M acetic acid (CH3COOH) with 0.200 M Soidum Hydroxide (NaOH).  What is the pH when the following amounts of base have been added?  You may check your work with the Acic/Base virtual lab.

a.  0.00 mL

 

 

b.  10.00 mL

 

 

c.  12.50 mL

 

 

d.  15.00 mL

 

 

e.  24.00 mL

 

 

 

f.   25.00 mL

 

 

 

g.  26.00 mL

 

 

 

h.  30.0 mL

 

 

6.  A buffer is prepared by mixing 17.5 g of acetic acid (fw = 60.02 g/mol) with 15.8 g sodium acetate (fw = 82.02g/mol), and diluting to 500.0 mL.  What is the pH of the buffer?

 

 

 

 

 

 

 

 

 

 

 

7. What must be the ratio of acetic acid to sodium acetate to prepare a buffer whose pH = 4.81?

 

 

 

 

8.  The solubility of gold chloride (AuCl3(s) <=> Au3+ + 3Cl- ) in water is 1.04 x 10-6 mol/L. Calculate the value of the solubility-product constant, Ksp, for gold chloride.

 

 

 

9.  The solubility-product constant for lead iodide (PbI2 <=> Pb2+ + 2I- ) is                                Ksp = 7.1 x 10-9. Calculate the molar solubility of lead iodide in otherwise pure water.

 

 

 

10.  Calculate the molar solubility of lead iodide (PbI2 <=> Pb2+ + 2I- , Ksp = 7.1 x 10-9) in a solution containing 0.10 M potassium iodide (KI), a very soluble salt.