### Practice Problems

Convert each hydroxide ion concentration into a pOH. Identify each as an acidic pOH or a basic pOH.

1) 0.0045
pOH = - log 0.0045 = - (- 2.35) = 2.35

This is a basic pOH.

2) 5.0 x 10¯^{10}

pOH = - log 5.0 x 10¯^{10} - (- 9.30) = 9.30

This is an acidic pOH.

3) 1.0

pOH = - log 1.0 = - (-0.00) = 0.00

This is a basic pOH.

4) 3.27 x 10¯^{3}

pOH = - log 3.27 x 10¯^{3} = - (- 2.485) = 2.485

This is a basic pOH.

5) 1.00 x 10¯^{12}

pOH = - log 1.00 x 10¯^{12} = 12.000

This is an acidic pOH.

6) 0.00010

pOH = - log 0.00010 = 4.0

This is a basic pOH.

Keep in mind that the pH + pOH = 14. The ChemTeam also keeps in mind that acidic pH runs up to 7. So, if I have a pOH = 4, I then know that the pH = 10 and that this is a basic solution.

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