Answer
$0.0100M$ $NH_4Cl$ is stronger.
Work Step by Step
1. Identify the conjugate pair of each ion:
First solution:
$ N{H_4}^+: NH_3$
$Cl^- : HCl$
Second solution:
$CH_3N{H_3}^+: CH_3NH_2$
$Br^-: HBr$
2. Now, determine which solution is more acidic.
- They both have strong acids, $HCl$ and $HBr$, so, the difference is the bases.
- The solution with the weaker base will be less basic, therefore, more acidic.
$K_b(NH_3) < K_b(CH_3NH_2)$
Therefore, the more acidic solution will be the $NH_4Cl$ one.
