What is the pH of a 6.2 x 10-2 mol/L solution of nitric acid?

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What is the pH of a 6.2 x 10-2 mol/L solution of nitric acid?

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Answer 1 · 2017-06-05T03:40:46

$p H = - {log}_{10} [H_{3} O^{+}] = 1.21$ $pH=-log_10[H_3O^+]=1.21$

Explanation:

$p H = - {log}_{10} [H_{3} O^{+}]$ $pH=-log_10[H_3O^+]$

We know that nitric acid is a moderately strong acid for which protonolysis of the water solvent is relatively complete, i.e. the given equilibrium lies to the right...........

$H N O_{3} (a q) + H_{2} O (l) \to H_{3} O^{+} + N O_{3}^{-}$ $HNO_3(aq) + H_2O(l) rarr H_3O^+ + NO_3^-$

That is the solution is stoichiometric in $H_{3} O^{+}$ $H_3O^+$ .

And we simply take ${log}_{10}$ $log_10$ ............

$- {log}_{10} (6.2 \times 10^{- 2}) = - (- 1.207) = 1.21$ $-log_10(6.2xx10^-2)=-(-1.207)=1.21$ .

For more details, see this [old answer.](https://socratic.org/questions/ph-value-definition)

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What is the pH of a 6.2 x 10-2 mol/L solution of nitric acid?

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