What is the pH of a 1.0 x103 M KOH solution?
A. 11
B. 4.0
C. 10
D. 3.0

Option A. 11

Explanation:

We'll begin by calculating the concentration of Hydroxide ion in the solution. This can be obtained as follow:

KOH (aq) —> K⁺(aq) + OH¯(aq)

From the balanced equation above,

1 mole of KOH produced 1 mole of OH¯.

Therefore, 1×10¯³ M KOH will also produce 1×10¯³ M OH¯.

Next, we shall determine the pOH of the solution. This can be obtained as follow:

Concentration of Hydroxide ion [OH¯] = 1×10¯³ M

pOH =?

pOH = –Log [OH¯]

pOH = –Log 1×10¯³

pOH = 3

Finally, we shall determine the pH of the solution. This can be obtained as follow:

pOH = 3

pH =?

pH + pOH = 14

pH + 3 = 14

Collect like terms

pH = 14 – 3

pH = 11

Therefore, the pH of the solution is 11

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