17. Acid and Base Equilibrium

Which of the following solutions will have the lowest concentration of hydronium ions?

Which of the following statements about aqueous solutions is/are true?

What is the Kw of pure water at 20.0°C, if the pH is 7.083?

Calculate the pH of 50.00 mL of 4.3 x 10^-7 M H₂SO₄.

Determine the pH of a solution made by dissolving 6.1 g of sodium cyanide, NaCN, in enough water to make a 500.0 mL of solution. (MW of NaCN = 49.01 g/mol). The Ka value of HCN is 4.9 x 10^-10.

OI⁻      OCl⁻      OBr⁻

A solution of NaOH was prepared in a chemistry lab and the pOH was determined to be 9.3. What is the concentration of OH⁻ ions of this basic solution?

Calculate [OH⁻] of a lemon juice solution at 25°C with a [H⁺] = 5.7 × 10⁻⁴ M.

A 345 mL bottle of antacid (Mg(OH)₂) contains 1.45 × 10⁻² moles of hydroxide ions. Determine pH and pOH of the antacid.

Which of the following statement(s) on aqueous solutions is/are correct?

a) aqueous solutions have a pH of 7

b) as concentration of hydronium ion increases, concentration of hydroxide ion decreases

c) solutions of weaker acids generally have a higher pOH then solutions of stronger acids

d) pH of pure water equals to 7 at 35º C.

The pH of an aqueous solution is 4.32. What is the [OH^–]?

What are the concentrations of H₃O⁺ and OH⁻ in tomatoes that have a pH of 4.10?

A solution of ammonia has a pH of 11.8. What is the concentration of OH^– ions in the solution?

What is the ratio of H⁺ ions to OH^– ions at a pH = 7?

The pH of a basic solution is 8.11. what is [H⁺]?

The pH of an acidic solution is 2.11. What is [H⁺]?

If the pH of a solution is 7, what is the molar concentration of H⁺?

The pH of a basic solution is 9.77. What is [OH⁻]?

What is the oh ion concentration of an aqueous solution with a pH of 5?

The OH^- concentration in an aqueous solution at 25 °C is 6.1 × 10^-5. what is [H⁺]?

Bleach has a pH of around 12. What is it considered on the pH scale?

A solution of HCl has = 0.01 M. What is the pH of this solution? use. –2 –1 1 2

Match each H⁺ concentration to its corresponding OH^– concentration in aqueous solution.