Sodium is prepared by adding 10 mL of 0.1 M acetic acid to 20 mL of 0.1 M sodium acetate. Calculate the pH of sodium. [pKa (acetic acid) = 4.67]. a. 5.04 b. 5.06                   c. 4.48                   d. None of these              e. 4.74

Choose the letter of the correct answer: 1. Which of the following salts will produce a basic solution upon hydrolysis?a. NH4NO3b. K2SO4c. NaC6H5COOd. NH4ClO4 2. What buffer pH can be prepared from an arbitrary weak acid whose pKa is 7.20?a. pH 8.30b. pH 6.40c. pH 2.80d. pH 5.80 3. All salts are products of neutralization reactions between an acid and a base. Thus, all salts form a neutral solution when dissolved.a. Trueb. False 4. Which source of error will cause an increase in buffer capacity during determination?a. Higher volume of the buffer was usedb. pH meter was read prematurely, resulting to a larger pH changec. Large amounts of the NaOH was added to the buffer with minimal pH changed. Large amounts of water was accidentally spilled into the buffer 5. Ions that are derived from strong acids and bases, which neither has acid nor base propertiesa. Hydrolyzable ionsb. Acidic/Basic ionsc. Spectator ionsd. Neutralizer ions

You are titrating 20.00 ml of 0.200 M HOAc with 0.200 M NaOH. What is the pH at the equivalence point of the titration?   (ka of HOAc = 1.80 x 10-5)              HOAc   +  NaOH  -------- NaOAc  +  H2O     A. pH 7.92   B. pH 7.00   C. pH 7.82   D. pH 8.87   E. pH 4.74

17. What is the pH of the solution produced when 50 mL of 0.25 M HCl is added to 250.0 mL of 0.1 M ammonia? [Given pKa of NH4 is 9.245] a. 4.755 b. 8.944 C. 9.245 d. 9.546