17. Acid and Base Equilibrium

What is the pH of a $0.000100$ M solution of hydrobromic acid, HBr, assuming it behaves as a strong acid and water autoionization is negligible?

What is the pH of a 2.8 M solution of HClO_4, assuming complete dissociation?

Determine the pH of a 7.8×10⁻⁴ M Ba(OH)₂ solution.

Pyridinium bromide (C5H5NHBr) is a strong electrolyte that dissociates completely into C5H5NH+ and Br-. A solution of pyridinium bromide has a pH of 2.92. Kb for pyridine is 1.7×10^-9. What is the molarity of the solution?

What is the pH of an aqueous $8.5\times {10}^{-3}$ M HI solution at 25 °C? (Assume HI is a strong acid.)

Rank the following 0.100 M aqueous solutions in order of increasing pH (lowest to highest): NaOH, CH3COOH, HNO3, HClO2, CH3NH2.

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

An aqueous solution has a pH of 3.0. Calculate the pOH. Be sure your answer has the correct number of significant digits.

Calculate the concentration of H3O+ in a 0.01 M solution of HCl at 25°C, and classify the solution as acidic or basic.

Given the following hydronium ion concentrations at 25°C, calculate the hydroxide ion concentration and classify each solution as acidic or basic: a. [H₃O⁺] = 1.5 × 10⁻³ M, b. [H₃O⁺] = 3.5 × 10⁻⁹ M, c. [H₃O⁺] = 8.3 × 10⁻¹¹ M. Which of the following correctly classifies solution b?

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.

Calculate the concentration of a NaOH solution that has a pH of 11.3.

Calculate the pH of a 0.10 M solution of barium hydroxide, Ba(OH)₂.

What is the pH and [OH-] concentration of a solution if the [H3O+] is 4.0 x 10^-9 M?