steps? Calculate the [OHin an aqueous solution that is 0.125 M NH3 and 0.300 M NH4Cl....
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 [OH]- for a solution that is 0.0900 M NH3 and 0.190 M NH4Cl? The Kb of ammonia is 1.8*10^-5
Kb for NH3 is 1.8x10^-5. What is the pH of a 0.35-M aqueous solution of NH4Cl at 25°C?
Calculate the pH of a solution formed by mixing 250.0 mL of 0.900 M NH4Cl with 250.0 mL of 1.60 M NH3. The Kb for NH3 is 1.8 × 10-5. 8.25 9.18 10.83 9.50
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
What is the pH of a 0.720 M aqueous solution of NH4NO3? The Kb for NH3 is 1.8 x 10-5.
A solution is 0.010 M in HCl and 0.010 M in NH4Cl. What is the molar concentration of NH3 at equilibrium? Kb(NH3) = 1.8 x 10-5 (Please explain the process in depth if possible)
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)
What is the pH of 6.0 M aqueous solution of NH3 (ammonia). It's Kb = 1.8 x 10-5.