1. 20 mL of 0.1 M NaOH are added to 25 mL of .2 M Acetic acid (K_a = 1.8x10^-5). What is the pH at equilibrium?  

2. In writing the net ionic reaction between KHP and NaOH which of the following would not be included?

a) Na⁺¹ b) K⁺¹ c) PH^-1 d) OH^-1 e) Neither Na⁺¹ nor K⁺¹ would be included.

3. 62.5 mL of 0.10N NaOH is chemically equivalent to __________ meq H₂SO₄  

4. The K_a for HA is 2x10^-5. The K for the reaction

HA + OH^- = H2O + A^-

is a) 5x10^-10 b) 5x10⁴ c) 2x10⁹ d)2x10^-5 e) 1

5-10. In the above titration curve of 0.232 g of an unknown acid with 0.150 N NaOH,

5. This acid is a) monoprotic b) diprotic c) triprotic d) Can not say for sure based on the titration curve.

6. The pK_a of the acid being titrated is

a) 1.8 and 4.2 b) 2.2 and 4.2 c) 4.2 and 9.5

d) 2.2 and 6.5 e) 2.2 and 6.5 and 12.2

7. If methyl orange (pK_a = 4.3) is used as an indicator the EW would be a) 48 b) 96 c) 192 d) 48 e) 145

8. If phenolphthalein (pK_a = 9 )is used as an indicator the EW would be a) 48 b) 96 c) 192 d) 48 e) 145

9. At a volume of 40 mL, what equilibrium constant would you use to calculate the pH?

a) pK_a1 of H₂A b) pK_a2 of H₂A c) pK_b of HA^-

d) none of these

10. What is the pK for the reaction HA^- + H₂O = OH^- + H₂A?

a) 2.2 b) 6.5 c) 4.7 d) 14-2.2 e) 14-6.5

11. What is the pH of a solution that is 0.04 M in NaCN and 0.03 M in HCN?

12. Write down a reaction(s) that describe(s) the following facts:

a) An aqueous solution of sodium carbonate is basic.

b) An aqueous solution of ammonia is basic.

c) A solution of KHP can be titrated with sodium hydroxide.

13. 25 mL of 0.10 M HCl mixed with 10 mL of 0.15 M NaOH; pH = ________.