17. Acid and Base Equilibrium

What is the pH of a neutral solution at a temperature where Kw = 1.8 × 10^-14?

What is the pH of a solution made by mixing 25.00 mL of 0.100 M HCl with 40.00 mL of 0.100 M KOH? Assume that the volumes of the solutions are additive.

What is the pH of the solution formed when 50 mL of 0.250 M NaOH is added to 50 mL of 0.120 M HCl?

What is the pOH of a solution that has a hydroxide ion concentration of 1.0 x 10^-13 M, which corresponds to a 0.10 M HCl solution? Express your answer to two significant figures.

What volume of 0.855 M KOH solution is required to make 3.55 L of a solution with a pH of 12.4?

Calculate the pH of a mixture of 150.0 mL of 0.0150 M HNO3 (aq) and 100.0 mL of 0.0100 M HBr (aq), assuming volumes are additive.

Calculate the pH of a 0.10 M HNO3 solution and a 5.0 × 10^-2 M NaOH solution.

Calculate the pH of a solution that is 0.075 M in HNO₃ and 0.170 M in HC₇H₅O₂, given that HNO₃ is a strong acid and HC₇H₅O₂ is a weak acid.