What is the pH of a buffer solution that is 0.350 M ethylamine and 0.200 M ethylammonium chloride, after the addition of 0.100 M HNO3? The value of Kb for ethylamine is 4.7 x 10-4.
ANSWER QUESTION 4 ONLY
1. Given below is the dissociation of NH3 in water having a Kb value of 1.8 × 10-5. The reaction started with the equilibration of 0.65 M NH3. A common ion that is 0.25 M NH4Cl, was added to the initial solution and waited for some time for the reaction to reach equilibrium once again.
NH3(aq) + H2O(l) ↔ NH4+(aq) + OH-(aq)
Determine the pH of the solution given after the addition of the common ion. The Kw of water is 1.0 × 10-14.
2. Calculate the pH of a base buffer solution composed of 0.20 M NH3 and 0.15 M NH4Cl after the addition of 0.10 M HCl. The Kb of NH3 at 25oC is 1.80 × 10-5.
3. What is the pOH of a buffer solution that is 0.150 M chloroacetic acid and 0.250 M sodium chloroacetate, after the addition of 0.100 M HNO3? The value of Ka for chloroacetic acid is 1.3 x 10-3.
4. What is the pH of a buffer solution that is 0.350 M ethylamine and 0.200 M ethylammonium chloride, after the addition of 0.100 M HNO3? The value of Kb for ethylamine is 4.7 x 10-4.
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