Determine the ph of the following base solutions. (assume that all solutions are at 25°c and the ion-product constant of water, kw, is 1.01 ✕ 10−14.) (a) 1.39 ✕ 10−2 m naoh webassign will check your answer for the correct number of significant figures. (b) 0.0051 m al(oh)3 webassign will check your answer for the correct number of significant figures.

a) The pH of the solution is 12.13.

b) The pH of the solution is 12.17.

Explanation:

Ionic product of water =

Taking negative logarithm on both sides:

The pH is the negative logarithm of hydrogen ion concentration in solution.

The pOH is the negative logarithm of hydroxide ion concentration in solution.

a) of NaOH.

Concentration of hydroxide ions:

So,

pH=13.99-1.86=12.13

b) of NaOH.

Concentration of hydroxide ions:

So,

pH=13.99-1.82=12.17