What is the pH of a .500 M solution of $H N O_{3}$ $HNO_3$ ?

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What is the pH of a .500 M solution of $H N O_{3}$ $HNO_3$ ?

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Answer 1 · 2016-06-20T20:59:18

$p H = 0.30$ $pH=0.30$

Explanation:

$H N O_{3} (a q) + H_{2} O (l) ⇌ H_{3} O^{+} + N O_{3}^{-}$ $HNO_3(aq) + H_2O(l) rightleftharpoonsH_3O^+ + NO_3^-$

$p H = - {log}_{10} [H_{3} O^{+}]$ $pH=-log_10[H_3O^+]$ . Since the equilibrium lies almost entirely to the right, we take $[H_{3} O^{+}] = 0.500 \cdot m o l \cdot L^{- 1}$ $[H_3O^+]=0.500*mol*L^-1$ .

${log}_{10} (0.500)$ $log_10(0.500)$ $=$ $=$ $- 0.301$ $-0.301$ , and $p H = ? ?$ $pH=??$

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What is the pH of a .500 M solution of $H N O_{3}$ $HNO_3$ ?

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