A solution of the weak acid HCN was prepared at 0.145 M. At equilibrium, the resulting pH was 3.59. a) Calculate concentration at equilibrium for each reagent. Report your answer to 4 significant figures. [HCN] = M [H30¹] = [CN] = b) What is Ka of the acid? O 0.00026 Σ Σ M 02.15-106 09.77-10-9 646 O2.05-10-8 04.66.10 7 A solution of the weak acid HCN was prepared at 0.145 M. At equilibrium, the resulting pH was 3.59.a) Calculate concentration at equilibrium for each reagent. Report your answer to 4 significant figures.[HCN] =M[H₂0'1=[(CN 1-Mb) What is K, of the acid?0.00026M02.15-1009.77-10902.05-1004.06-10

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Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A solution of the weak acid HCN was prepared at 0.145 M. At equilibrium, the resulting pH was 3.59. a) Calculate concentration at equilibrium for each reagent. Report your answer to 4 significant figures. [HCN] = M [H30¹] = [CN] = b) What is Ka of the acid? O 0.00026 Σ Σ M 02.15-106 09.77-10-9 646 O2.05-10-8 04.66.10 7

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