Given a solution of nitric acid whose $p H = 4$ $pH=4$ , what are $[H_{3} O^{+}]$ $[H_3O^+]$ , and $[N O_{3}^{-}]$ $[NO_3^(-)]$ ?

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Given a solution of nitric acid whose $p H = 4$ $pH=4$ , what are $[H_{3} O^{+}]$ $[H_3O^+]$ , and $[N O_{3}^{-}]$ $[NO_3^(-)]$ ?

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Answer 1 · 2016-12-30T19:13:24

$[H N O_{3}] = 0.0001 \cdot m o l \cdot L^{- 1}$ $[HNO_3]=0.0001*mol*L^-1$

Explanation:

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

We are given that $p H = 4$ $pH=4$

And thus $[H_{3} O^{+}] = 0.0001 \cdot m o l \cdot L^{- 1}$ $[H_3O^+]=0.0001*mol*L^-1$ (since ${log}_{10} 0.0001 = {log}_{10} 10^{- 4} = - (- 4) = 4$ $log_(10)0.0001=log_(10)10^-4=-(-4)=4$ .

In water, nitric acid would undergo complete dissociation, according to the following rxn:

$H N O_{3} (a q) + H_{2} O (l) \to H_{3} O^{+} + N O_{3}^{-}$ $HNO_3(aq) + H_2O(l)rarrH_3O^+ + NO_3^-$

And thus the formal concentration of nitric acid is equivalent to $[H_{3} O^{+}]$ $[H_3O^+]$ and $[N O_{3}^{-}]$ $[NO_3^-]$ .

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Given a solution of nitric acid whose $p H = 4$ $pH=4$ , what are $[H_{3} O^{+}]$ $[H_3O^+]$ , and $[N O_{3}^{-}]$ $[NO_3^(-)]$ ?

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Given a solution of nitric acid whose pH=4pH=4, what are [H3O+][H_3O^+], and [NO−3][NO_3^(-)]?

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Given a solution of nitric acid whose $p H = 4$ $pH=4$ , what are $[H_{3} O^{+}]$ $[H_3O^+]$ , and $[N O_{3}^{-}]$ $[NO_3^(-)]$ ?