Question #4589c

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Question #4589c

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Answer 1 · 2015-03-18T09:41:25

The solution will be acidic.

You're dealing with dimethylammonium chloride, which will dissociate in aqueous solution into ${(C H_{3})}_{2} N H_{2}^{+}$ $(CH_3)_2NH_2^(+)$ and $C l^{-}$ $Cl^(-)$ .

${(C H_{3})}_{2} N H_{2} C l (a q) \to {(C H_{3})}_{2} N H_{2}^{+} (a q) + C l_{(a q)}^{-}$ $(CH_3)_2NH_2Cl(aq) -> (CH_3)_2NH_2^(+)(aq) + Cl_((aq))^(-)$

Notice that the cation is the conjugate acid of a weak base, dimethylamine, ${(C H_{3})}_{2} N H$ $(CH_3)_2NH$ , and the anion is the conjugate base of a strong acid, $H C l$ $HCl$ .

This means that the reaction of interest, after dimethylammonium chloride dissociates, will be

${(C H_{3})}_{2} N H_{2}^{+} (a q) + H_{2} O_{(l)} ⇌ {(C H_{3})}_{2} N H (a q) + H_{3} O_{(a q)}^{+}$ $(CH_3)_2NH_2^(+)(aq) + H_2O_((l)) rightleftharpoons (CH_3)_2NH(aq) + H_3O_((aq))^(+)$

The reaction increases the concetration of hydronium ions, which in turn will make the solution acidic.

As a conclusion, look at the cations and anions that form your salt. In this case, you were dealing with an acid salt. Here's a link detailing the acid/base properties of salts

http://www2.onu.edu/~s-bates/chem172/ABSalts12.pdf

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Question #4589c

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