When equal molar amounts of HCl and HOCl are dissolved separately in equal amounts of water, the solution of HCl freezes at a lower temperature. Which compound has the larger equilibrium constant for acid ionization? (a) HCl (b) H+ + Cl–

(b) CaCl2, (c) HNO3, (d) KCN, (e) Mn²+, (f) MnO4 . Calculate the pOH and pH of a 0.0045 M solution of NaOH.

2. Which of the following could be added to 50.0 mL of 0.10 mol L nitric acid solution to change its pH to 3? (A) 450.0 mL of distilled water (B) 450.0 mL of 0.10 mol L-1 nitric acid (C) 4950.0 mL of distilled water (D) 4950.0 mL of 0.10 mol L'nitric acid

In a titration experiment, 40.0 mL of 0.100 M HCI is titrated with 0.100 M NaOH solution. Determine the pH of the solution: (a) before NaOH is added. (b) after 20.0 mL of NaOH is added.

(a) Using the expression Ka=[H+][A−]/[HA], explain how to determine which solution has the lower pH, 0.10MHF(aq) or 0.10MHC2H3O2(aq). Do not perform any numerical calculations. (b) Which solution has a higher percent ionization of the acid, a 0.10M solution of HC2H3O2(aq) or a 0.010M solution of HC2H3O2(aq) ? Justify your answer including the calculation of percent ionization for each solution.

Which of the following will increase the percentage of HF that is converted to the fluoride ion in water? (a) addition of NaOH (b) addition of HCl (c) addition of NaF

The pH of which of the following solutions will decrease by 1.00 pH unit when diluted with water to 10 times its original volume? 0.10 M HCI 0.10 M NAOH 0.10 M CH3COOH 0.10 MCH3COO Na" A mixture of 010 M CH;COOH and 0.10 M CH3COO'Na*

NH3 is a weak base (?b=1.8×10−5Kb=1.8×10−5) and so the salt NH4Cl acts as a weak acid. What is the pH of a solution that is 0.0180.018 M in NH4Cl at 25 °C?

Q7

In the reaction NH3(aq) + H₂O(1)⇒ NH4*(aq)+ OH¯(aq) does water act as a Brønsted-Lowry acid, a Brønsted-Lowry base, or neither, or both? (A) Neither as an acid nor as a base; water is neutral (B) Both an acid and a base. (C) An acid (D) A base (E) Depends temperature