Calculate the pH of a solution made by mixing 100.0 mL of 0.635 M NH₃ with 100.0 mL of 0.100 M HCl.(K_b for NH₃ = 1.8 $\times$10^-⁵)

Question

Quizplus · Accepted Answer

The correct answer is A because the pH of the solution is 9.98. The reaction between NH3 and HCl is a neutralization reaction, which results in the formation of NH4Cl. The pH of the solution can be calculated using the following equation:pH = -log[H+],where [H+] is the molar concentration of hydrogen ions in the solution. The molar concentration of hydrogen ions can be calculated using the following equation:[H+] = Kw/[OH-],where Kw is the ion product constant for water (1.0 x 10^-14) and [OH-] is the molar concentration of hydroxide ions in the solution. The molar concentration of hydroxide ions can be calculated using the following equation:[OH-] = Kb[NH3]/[NH4+],where Kb is the base dissociation constant for NH3 (1.8 x 10^-5) and [NH3] and [NH4+] are the molar concentrations of NH3 and NH4+, respectively.Substituting the values of Kw, Kb, [NH3], and [NH4+] into the above equations, we get:[H+] = 1.0 x 10^-14/(1.8 x 10^-5 * 0.3175) = 1.71 x 10^-10 MpH = -log(1.71 x 10^-10) = 9.98

Calculate the PH of a Solution Made by Mixing 100 ×\times×

Calculate the PH of a Solution Made by Mixing 100 $\times$