What is the pH of a solution that has a hydronium ion concentration of $1.00 \cdot 10^{- 10}$ $1.00*10^-10$ M?

Question

7029 views around the world

You can reuse this answer
Creative Commons License

Answer 1 · 2015-11-05T02:12:37

Take the negative log of your $H_{3} O^{+}$ $H_3O^+$ molarity.

The pH of an aqueous solution can be found simply by taking the negative logarithm of your hydronium ion concentration, or stated mathematically,

pH = $- log [H_{3} O^{+}]$ $-log[H_3O^+]$

So, if we plug in your numbers we'll get:

pH = $- log [1.00 \cdot 10^{- 10}]$ $-log[1.00*10^-10]$

Throw that bad boy in your calculator and you'll find your pH. Or I can just tell you. (It's 10.)

What is the pH of a solution that has a hydronium ion concentration of 1.00*10^-101.00⋅10−101.00*10^-10 M?