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What is the pH of a KOH solution that has [H+] = 1.87 × 10–13 M?
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What is the pH of a KOH solution that has [H+] = 1.87 × 10–13 M?

User Baetacos
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2 Answers

3 votes

Answer: 12.7

Explanation: edge 2020

User GoodKode
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4 votes

Answer:

The pH is 12,73.

Step-by-step explanation:

The pH corresponds to a measure that gives us an idea of the acidity or alkalinity of a solution. It is calculated with the following formula:

pH = -log (H +) = - log (1.87 × 10–13 M)= 12, 73

User Arthur Tsidkilov
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