Ka=-log(Ka)=-log(5.6*10^-10)=9.25 According to Henderson Hasselbalch Equation pH = pka + log[salt]/[acid] pH = 9.25 log[Nh3]/[Nh4+] = 9.25+log(0.2/0.6) pH=8.77 (2) NH3 + HCl =======> NH4Cl I 0.2 0.10 0.6 C 0.2-0.1 -0.1 +0.1 E 0.1 0 0.7 pH = pka + log[salt]/[acid] pH = 9.25 log[Nh3]/[Nh4+] = 9.25+log(0.1/0.7) pH=8.40 (3) NH4Cl + NaOH =============> NH3 + NaCl + H2O I 0.6 0.20 0.2 C -0.20 -0.20 +0.20 E 0.4 0 0.4 pH = pka + log[salt]/[acid] pH = 9.25 log[Nh3]/[Nh4+] = 9.25+log(0.4/0.4) = 9.25 Solution Ka=-log(Ka)=-log(5.6*10^-10)=9.25 According to Henderson Hasselbalch Equation pH = pka + log[salt]/[acid] pH = 9.25 log[Nh3]/[Nh4+] = 9.25+log(0.2/0.6) pH=8.77 (2) NH3 + HCl =======> NH4Cl I 0.2 0.10 0.6 C 0.2-0.1 -0.1 +0.1 E 0.1 0 0.7 pH = pka + log[salt]/[acid] pH = 9.25 log[Nh3]/[Nh4+] = 9.25+log(0.1/0.7) pH=8.40 (3) NH4Cl + NaOH =============> NH3 + NaCl + H2O I 0.6 0.20 0.2 C -0.20 -0.20 +0.20 E 0.4 0 0.4 pH = pka + log[salt]/[acid] pH = 9.25 log[Nh3]/[Nh4+] = 9.25+log(0.4/0.4) = 9.25.