11) A 520 ml solution contains 0.130 M formic acid (K, = 1.80 x 10) and 0.130 M sodium formate. First determine the pH of this initial solution. Next, determine the pH if 1 mL of 5.5 M of HCI was added to this solution. Finally, determine if rather than HCI, 1 mL of 5.5 M NaOH was added to the solution.

You add 7.50 mL of 0.0500 M NaOH to 25.00 mL of pure water, and to this mixture you then add 1.50 mL of 0.200 M HCl. What will be the pH of the resulting solution?

8. Determine the pH at the equivalence point when 65.0 mL of 0.429 M HBrO is mixed with 0.371 M NaOH. Ka = 2.8 x 10 ⁹ Your answer must include an ICE box showing the new equilibrium formed.

Aspirin, or acetylsalicylic acid (CH3COC6H4CO2H; molar mass = 164.15 g/mol) has Ka= 3.0 x 10–4. If saturated solution of aspirin has pH = 2.68. Determine the solubility of aspirin in mol/L and in g/L

You add 7.00 mL of 0.100 M NaOH to 50.00 mL of pure water, and to this mixture you then add 12.00 mL of 0.800 M HCl. What will be the pH of the resulting solution?

You make 0.1 L of a buffered solution (pH=9.1) by mixing acetic acid and sodium acetate. You have 1.00 M solutions of each component of the buffered solution. What volume of each solution do you mix to make such a buffered solution? Note that the total ion concentration must be 0.170M.

A chemist titrates 100.0 mL of a 0.0621 M hydrobromic acid (HBr) solution with 0.6950M KOH solution at 25 °C. Calculate the pH at equivalence. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of KOH solution added. pH = 0 X 5

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A 1.50 L buffer solution consists of 0.280 M propanoic acid and 0.139 M sodium propanoate. Calculate the pH of the solution following the addition of 0.065 mol HCl. Assume that any contribution of the HCl to the volume of the solution is negligible. The Ka of propanoic acid is 1.34×10^−5.

A small amount of a strong base is added to a buffer solution made up of a weak acid (HA) and the sodium salt of its conjugate base (NaA).  What happens to the pH of the system? Be sure you can explain your answer.   The pH will increase significantly.         The pH will decrease significantly.         The pH will decrease, but not appreciably.       The pH will increase, but not appreciably.