# Chapter 14 - Acids and Bases - Questions for Review and Thought - Topical Questions - Page 652c: 45a

$0.10M$ $H_2CO_3$ is more acidic.

#### Work Step by Step

** You can find the $K_a$ values on table: 14.2 (Page 624) Since both solutions have the same concentration, we just have to determine which compound is more acidic: -$H_2CO_3$: $H_2CO_3$ is an acid with $K_a = 4.3 \times 10^{-7}$ - $NH_4Cl$: It is a salt formed by $N{H_4}^+$ and $Cl^-$. $Cl^-$ has negligible basicity, so, we don't need to consider it. $N{H_4}^+$ is an acid with $K_a = 5.6 \times 10^{-10}$ $H_2CO_3$ has a greater $K_a$ value, therefore, it is more acidic. So $0.10M$ $H_2CO_3$ is more acidic.

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