What is the pH of a solution that has a hydronium ion concentration of $1.00 \times 10^{- 4} M$ $1.00 times 10^-4 M$ ?

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Answer 1 · 2017-06-28T15:08:59

pH = 4

To calculate the pH of a solution, use the equation

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

Since we are given the hydronium ion ( $H_{3} O^{+}$ $H_3O^+$ ) concentration of the solution, we can plug this value into the formula.

$p H = - log [1.00 \times 10^{- 4} M]$ $pH = -log[1.00 xx 10^-4 M]$
$p H = 4$ $pH = 4$

The pH of this solution is 4.

Added notes:
$p H = p H_{3} O^{+}$ $pH = pH_3O^+$ because hydrogen ions attach to water molecules for form hydronium ions.

Some other key things to remember for pH calculations include:

pH + pOH = 14

pH = -log[ $H^{+}$ $H^+$ ]
pOH = -log[ $O H^{-}$ $OH^-$ ]

$[H^{+}] = 10^{- p H}$ $[H^+] = 10^(-pH)$
$[O H^{-}] = 10^{- p O H}$ $[OH^-] = 10^(-pOH)$

The video below explains how to use all this information so that you can complete these types of calculations.

Hope this helps!

What is the pH of a solution that has a hydronium ion concentration of 1.00×10−4M1.00 times 10^-4 M?