What is the pH of a $4 \cdot 10^{- 2}$ $4*10^-2$ $M$ $M$ $H C l$ $HCl$ solution?

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What is the pH of a $4 \cdot 10^{- 2}$ $4*10^-2$ $M$ $M$ $H C l$ $HCl$ solution?

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Answer 1 · 2016-04-27T16:56:02

$p H$ $pH$ $=$ $=$ $- {log}_{10} [H_{3} O^{+}]$ $-log_(10)[H_3O^+]$ $=$ $=$ $- {log}_{10} (4.0 \times 10^{- 2})$ $-log_(10)(4.0xx10^-2)$ $=$ $=$ $1.40$ $1.40$

Explanation:

$p H$ $pH$ $=$ $=$ $- {log}_{10} [H_{3} O^{+}]$ $-log_(10)[H_3O^+]$ $=$ $=$ $- {log}_{10} (4.0 \times 10^{- 2})$ $-log_(10)(4.0xx10^-2)$

We assume (reasonably) that hydrochloric acid will undergo complete dissociation in water to give stoichiometric $H_{3} O^{+}$ $H_3O^+$ ion, according to the given reaction:

$H C l (a q) + H_{2} O (l) \to H_{3} O^{+} + C l^{-}$ $HCl(aq) + H_2O(l) rarr H_3O^(+) + Cl^-$

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What is the pH of a $4 \cdot 10^{- 2}$ $4*10^-2$ $M$ $M$ $H C l$ $HCl$ solution?

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