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A buffer solution made from hydrocyanic acid and potassium cyanide was titrated with hydrochloric acid. What is the net ionic equation for the reaction? H3O+ (aq) + HCN(aq) => H₂O(l) + H2CN(aq) H3O+ (aq) + CN¯(aq) => HCN(aq) + H₂O(1) HCl(aq) + OH-(aq) => H₂O(l) + Cl¯(aq) HCl(aq) + CN- (aq) => HCN(aq) + Cl- (aq)

A buffer solution made from hydrocyanic acid and potassium cyanide was titrated with hydrochloric acid. What is the net ionic equation for the reaction? H3O+ (aq) + HCN(aq) => H₂O(l) + H2CN(aq) H3O+ (aq) + CN¯(aq) => HCN(aq) + H₂O(1) HCl(aq) + OH-(aq) => H₂O(l) + Cl¯(aq) HCl(aq) + CN- (aq) => HCN(aq) + Cl- (aq)

Chemistry
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 buffer solution made from hydrocyanic acid and potassium cyanide was titrated with hydrochloric acid. What is the net ionic equation for the reaction? H3O+ (aq) + HCN(aq) => H₂O(1) + H2CN(aq) H3O+ (aq) + CN-(aq) => HCN(aq) + H₂O(1) HCl(aq) + OH(aq) => H₂O(1) + Cl¯(aq) HCl(aq) + CN- (aq) => HCN(aq) + Cl- (aq)
Transcribed Image Text:A buffer solution made from hydrocyanic acid and potassium cyanide was titrated with hydrochloric acid. What is the net ionic equation for the reaction? H3O+ (aq) + HCN(aq) => H₂O(1) + H2CN(aq) H3O+ (aq) + CN-(aq) => HCN(aq) + H₂O(1) HCl(aq) + OH(aq) => H₂O(1) + Cl¯(aq) HCl(aq) + CN- (aq) => HCN(aq) + Cl- (aq)
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