Determine the pH of a solution by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The value of $K_b$ for $C_6H_5NH_2$ is $4.3 \times 10^{-10}$. Complete Parts 1-4 before submitting your answer.
0.040 mol of solid NaOH is added to a 200.0 mL buffer containing 0.100 mol $C_6H_5NH_3Cl$ and 0.500 M $C_6H_5NH_2$. Fill in the table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of water in the reaction.
$C_6H_5NH_3^+(aq) \quad + \quad OH^-(aq) \quad \rightarrow \quad H_2O(l) \quad + \quad C_6H_5NH_2(aq)$
Before (mol)
0.100
0.040
$-$
0
Change (mol)
-0.040
-0.040
$-$
0.040
After (mol)
0.060
0
$-$
0.040
Incorrect, 2 attempts remaining
