## Chemistry: The Molecular Science (5th Edition)

Published by Cengage Learning

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

#### Answer

So $0.10M$ $NaHCO_3$ 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: -$NaHCO_3$: It is a salt formed by $Na^+$ and $HC{O_3}^-$. $Na^+$ has negligible acidity, so, we don't need to consider it. $HC{O_3}^-$ is an acid with $K_a = 4.7 \times 10^{-11}$ - $Na_2HPO_4$: It is a salt formed by $2Na^+$ and $HP{O_4}^{2-}$. $Na^+$ has negligible acidity, so, we don't need to consider it. $HP{O_4}^{2-}$ is an acid with $K_a = 4.6 \times 10^{-13}$ $HC{O_3}^-$ has a greater $K_a$ value, therefore, it is more acidic. So, $0.10M$ $NaHCO_3$ is more acidic.

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