repared by dissolving 0.171 mol of formic acid (HCOOH, K, -1.77x104) and 0.450 mol of hydrocyanic acid (HCN, K₂ 1.80 L. Also, calculate the equilibrium concentrations of HCOOH, HCOO, HCN, and CN. Do not make an concentration is greater than 1000 x K. (Hint: The pH will be determined by the stronger acid of this pair.) pH = [HCOOH) = THCOO]= [HCN] = [CN'] = M M M M

repared by dissolving 0.171 mol of formic acid (HCOOH, K, -1.77x104) and 0.450 mol of hydrocyanic acid (HCN, K₂ 1.80 L. Also, calculate the equilibrium concentrations of HCOOH, HCOO, HCN, and CN. Do not make an concentration is greater than 1000 x K. (Hint: The pH will be determined by the stronger acid of this pair.) pH = [HCOOH) = THCOO]= [HCN] = [CN'] = M M M M

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

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 4CYU: 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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