17. Acid and Base Equilibrium

A 25.00 mL sample of 0.175 M HCl is being titrated with 0.250 M NaOH. What is the pH when 0 mL of NaOH has been added?

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

What is the concentration of hydronium ions [H3O+] and hydroxide ions [OH−] in a 0.016 mol L−1 solution of HNO3?

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

Calculate the concentration of OH⁻ in a 0.01 M HCl solution 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 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.

Calculate the pH of a 0.012 M solution of HCl, a strong acid.

Calculate the pH of the resulting solution when 22.0 mL of 0.450 M HClO4 is added to 15.0 mL of 0.330 M Ba(OH)₂.

Given the following solutions at 25°C, determine the pH and classify each as acidic, basic, or neutral: Solution 1: [H3O+] = 3.5×10^-3 M Solution 2: [OH−] = 3.8×10^-7 M Solution 3: [H3O+] = 1.8×10^-7 M Which of the following correctly describes the pH and classification for Solution 1?

Consider the titration of a 35.0 mL sample of 0.175 M HBr with 0.200 M KOH. Determine the initial pH of the HBr solution before any KOH is added.