Aqueous Solutions and the Concept of pH

_____ is the concentration of a solution and is defined as the number of moles of solute divided by the volume of the solution in L.

• Ionization constant of water

• Molarity

• Self-ionization of water

Distilled water contains

• H2O, H3O+, OH−

• H2O, H3O+

• H2O

The K_w value for water can be affected by

• dissolving a salt in the solution.

• the presence of a strong acid

• changes in temperature.

A solution has a pH of 4.75. What is the hydronium ion concentration? Is the solution acidic or basic?

• [H3O+] = 1.8 × 10⁻⁵ M; acidic

• [H3O+] = 1.8 × 10⁻⁵ M; neutral

• [H3O+] = 1.8 × 10⁻⁵ M; base

What is the pH of a solution if the [H3O+] is 6.7 × 10-4 M?

• pH = 3

• pH = 3.17

• pH = 7.37

The pH of an aqueous solution is 3.67. Determine [H3O+].

• [H3O+] = 2.1 × 10^-4 M

• [OH-] = 7.8 × 10^-11 M

• [H3O+] = 4.1 × 10^-4 M

What is the pH of a 0.0010 M HNO3?

• 1.0

• 3.0

• 5.0

What is the pH of a 0.0010 M HNO3?Which of the following solutions would have a pH value greater than 7?

• [OH−] = 2.4 × 10⁻² M

• [H3O+] = 1.53 × 10⁻² M

• 0.0001 M HCl

The pH of a solution is 6.32. What is the pOH?

• 6.32

• 4.8 × 10⁻⁷

• 7.68

Determine the pH of

1 × 10^-6 M HClO4

• pH = 9.0

• pH = 6.0

• pH = 4.0