Calculate the pH of 0.25 M NH4CL given kb= 1.76x10^-5 for NH3 (ans. 4.92)
Find the pH of a 0.1 M NH3 solution. (Kb= 1.76x10-5)
Kb for NH3 is 1.8x10^-5. What is the pH of a 0.35-M aqueous solution of NH4Cl at 25°C?
NH3 is a weak base with a Kb value of 1.76x10–5. Suppose 25.0 mL of a0.180 MNH3 is titrate using HCl. The end point is reach after 35.0 mL HCl had been added. Calculate the pH of the resulting solution at the equivalence-point. Here is the titration equation:NH3(aq) + HCl(aq) →NH4Cl(aq)
What is the pH of a 0.10 M NH4Cl solution? (Kb(NH3) = 1.8 x 10-5 A. 7.25 B. 11.3 C. 5.63 D. 3.40 E. 10.6
What is the pH of a 0.01 M NH4Cl solution? (Kb(NH3) = 1.8 x 10-5 A. 7.25 B. 11.3 C. 5.63 D. 3.40 E. 10.6
NH3 is a weak base (Kb = 1.8 × 10–5) and so the salt NH4Cl acts as a weak acid. What is the pH of a solution that is 0.048 M in NH4Cl at 25 °C? pH=_______?
Determine the pH of a 0.188 M NH3 solution at 25°C. The Kb of NH3 is 1.76x10-5.
What is the pH of a solution that is 0.093 M NH3 and 0.64 M NH4Cl? (NH3; Kb = 1.8 × 10-5)
What is the ratio of [NH4Cl]/[NH3] in order to make a NH3/NH4Cl buffer solution with pH=8.70. (Kb for NH3 is 1.8 x 10^–5)