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Nesterboy [21]
3 years ago
14

Calculate the hydronium ion concentration in an aqueous solution with a pH of 11.7 at 25°C.

Chemistry
1 answer:
DENIUS [597]3 years ago
6 0

Answer:

Approximately 2\times 10^{-12}\;\rm mol \cdot L^{-1}.

Explanation:

The hydronium ion concentration \left[\mathrm{H_3O^{+}}\right] of an aqueous solution can be found from its \rm pH with the equation:

\displaystyle \left[\mathrm{H_3O^{+}}\right] = 10^{-\mathrm{pH}}.

For this solution, \rm pH= 11.7. Hence,

\begin{aligned}& \left[\mathrm{H_3O^{+}}\right] \\ &= 10^{-\mathrm{pH}} \\ &= 10^{-11.7} \approx 2 \times 10^{-12}\end{aligned}.

Note that for this equation, the number of significant figures in \left[\mathrm{H_3O^{+}}\right] should be the same as the number of decimal places in \rm pH. For example, the \rm pH of this question comes with only one decimal place. As a result, there would be only one significant figure in the \left[\mathrm{H_3O^{+}}\right] obtained from the equation.

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