28. Consider 0.10M HCI, 0.10 M NAOH, 0.10 M NH3, 0.1 M acetic acid, and 0.10 M NaCl, This solution has the highest pH. A. HCI В. NaOH С. NH D. Acetic acid E. Nacl

10. Which solution would be expected to have the highest pH? (No calculation needed.) A. 0.50 M NaOH B. 0.05 M HC1 C. 0.05 M CH3NH₂ D. 0.60 M CH3COOH

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What happens when an acid is added to a buffer? a. The OH- reacts with the acid in the buffer b. The OH- reacts with the conjugate base in the buffer c. The H+ reacts with the base in the buffer d. The H+ reacts with the conjugate acid in the buffer

Explain why the pH does not change significantly when a small amount of an acid or a base is added to a solution that contains equal amounts of the acid H,CO, and a salt of its conjugate base NaHCO3 O Excess acid is removed by reacting with NaHCO3; excess base is removed by reacting with H,O O Excess base is removed by reacting with NaHCO3; excess acid is removed by reacting with H2CO3 O Excess H,O is removed by reacting with NaHCO3; excess base is removed by reacting with H,CO

Based on the ion-product constant, calculate the concentration of OH- ions if the concentration of H+ ions in a given solution is 2.67 x 10^(-5) M.  A. 2.67x10-5 B. 2.67x109 C.3.74x10-10 D. none

18.   A. Calculate [OH−] for this strong base solution: 7.3×10−2 M KOH and then it's pH   B. Calculate [OH−] for this strong base solution: 10.0 mL of 1.00×10−2 M Ca(OH)2 diluted to 500.0 mL and it's pH   C. Calculate [OH−] for the strong base solution formed by mixing 10.0 mL of 1.50×10−2 M Ba(OH)2 with 34.0 mL of 6.0×10−3 M NaOH and it's pH

1. Acetic acid is a weak monoprotic acid with Ka = 1.77 x 10¯5. NaOH(s) was gradually added to 1.00 L of 0.0179 M acetic acid. (Assume no volume change occurs.) Calculate the pH of the solution after the addition of 0.0286 mol of NaOH(s).    A.  8.502  B.  1.971  C.  12.029  D.  7.000 2.What is the ratio of [A-] / [HA] for a buffer solution of HA with a pH of 7 if the pKa = 5 for HA?      A.  100  B.  0.01  C.  10  D.  0.1 3.  Titrate 50.0 ml 0.1 M HCN (Ka = 6.2 x 10-10) with 0.10 M NaOH. Calculate the pH at the half-way or midpoint.    A.  9.2  B.  7.0  C.  4.8  D.  0.0