8:04 PM Fri Nov 27ll7 43%AAA sjc.cengagenow.com+Latest LineF5 Dynamic...Group Resea...10-16 Acid-..Mastery 10-16X OWLV2 | Onli...G green and w...C dept. CSIERRASIERRASIERRAModule 10-12[Review Topics][References]1. Buffer Solu...Use the References to access important values if needed for this question.A buffer solution is made that is 0.376 M inHCN and 0.376 M in2. Buffer S...2reqQuestionNaCN.QuestionIfQuestionKa forHCN is3. Buffer Solu...M)-104.00 x 10-, what is the pH of the buffer solution?pH :Write the net ionic equation for the reaction that occurs when 0.089 mol HCl is added to 1.00 L of the buffersolution.the lowest poscoefficients. Omit states of matter. Use H3 0t instead of Ht)++Submit AnswerRetry Entire Group8 more group attempts remainingProgress:2/3 groupsDue Nov 28 at11:55 PMPreviousNextFinish AssignmentSave and Exit

Hello. Since the question contains multiple parts, the first part is solved. In case the solution for other part is required, then repost the entire question and specify the part that has to be solved.Given, Concentration of HCN = 0.376 M. Concentration of NaCN = 0.376 M. If Ka of HCN = 4.00 × 10-10 HCN is a weak acid and NaCN is salt. pH = pKa + log [salt][acid]pH =-log (4×10-10)+log0.3760.376pH = -log (4×10-10)+0pH= 9.398

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A buffer solution is made that is 0.376 M in HCN and 0.376 M in NACN. If Ka for HCN is 4.00 x 10-10, what is the pH of the buffer solution? pH

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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