a Why is [H3O] = [OH-] + 1.0 X 10-2 M not feasible in water? What would happen if we tried to make such a solution by mixing 1.0 X 10-2 mol/L of KOH with HCl? b. Calculate the pH of a buffer that is 0.020 M in NH3 and 0.030 M in NH4Cl. What is the pH after adding 1.00 mL of 0.01 M NaOH to 0.10 L of this buffer? [Ka for NH4+ if 5.70 x 10-10]

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Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter17: Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria

Section17.2: Controlling Ph: Buffer Solutions

Problem 17.5CYU: Calculate the pH of 0.500 L of a buffer solution composed of 0.50 M formic acid (HCO2H) and 0.70 M...

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a Why is [H_3O] = [OH^-] + 1.0 X 10^-2M not feasible in water? What would happen if we tried to make such a solution by mixing 1.0 X 10^-2 mol/L of KOH with HCl?

b. Calculate the pH of a buffer that is 0.020 M in NH₃ and 0.030 M in NH₄Cl. What is the pH after adding 1.00 mL of 0.01 M NaOH to 0.10 L of this buffer?

[K_a for NH₄⁺ if 5.70 x 10^-10]

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