AlgebraLab

Chemistry: pH - A Logarithm Application #1

By K Dodd

Directions and/or Common Information:

pH = -log [H3O+]

The pH level of a substance is equal to the negative log of the concentration of the hydronium ion, [H3O+].

[H3O+] × [OH-]= 1.0 × 10-14

In any substance, the product of the concentration of the hydronium ion, [H3O+], and the concentration of the hydroxide ion, [OH-], is always equal to 1.0 × 10-14

Given a substance with a hydronium ion concentration of 2.5 x 10-5 (moles/L)

  1. Find the pH of the substance.
  2. Find the concentration (in moles/L) of the hydroxide ion. [OH-]

Given a substance with a hydronium ion concentration, [H3O+], of 1.2 x 10-12 (moles/L)

  1. Find the pH of the substance.
  2. Find the concentration (in moles/L) of the hydroxide ion. [OH-]

Given a substance with a hydronium ion concentration, [H3O+], of 1.0 x 10-7 (moles/L)

  1. Find the pH of the substance.
  2. Find the concentration ( in  moles/L) of the hydroxide ion, [OH-].

Given a substance with [H3O+] = 5.0 x 10-3 (moles/L)

  1. Find the pH of the substance.
  2. Find the concentration (in moles/L) of the hydroxide ion, [OH-]

Given a substance with a pH value of 8.80

  1. Find [H3O+]
  2. Find [OH-]

Given a substance with a pH value of 6.13

  1. Find [H3O+]
  2. Find [OH-]

Given a substance with a pH value of 1.23

  1. Find [H3O+]
  2. Find [OH-]

Given a substance with a hydroxide ion concentration, [OH-], of 5.6 x 10-4 (moles/L)

  1. Find [H3O+]
  2. Find the pH-]

Given a substance with a hydroxide ion concentration, [OH-], of 1.7 x 10-10 (moles/L)

  1. Find [H3O+]
  2. Find the pH.

Given a substance with a hydroxide ion concentration, [OH-], of 5.0 x 10-5 (moles/L)

  1. Find [H3O+].
  2. Find the pH.