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C. Some Properties of Buffers Buffer system selected. NH4-NH3 HB is 1. pH of buffer 2. pH of diluted buffer 156 9.54 9.48 [H*]. [H*] NH4Cl CO.10 M) ? M pK, (by Eq. 4b) pK₁ 3. pH of buffer in which [HB]/[B] = 0.10 pH after addition of excess NaOH M Experiment 19 pH Measurements-Buffers and Their Properties (name the acid) 9.50. 10.54 11.83 pK₁

C. Some Properties of Buffers Buffer system selected. NH4-NH3 HB is 1. pH of buffer 2. pH of diluted buffer 156 9.54 9.48 [H*]. [H*] NH4Cl CO.10 M) ? M pK, (by Eq. 4b) pK₁ 3. pH of buffer in which [HB]/[B] = 0.10 pH after addition of excess NaOH M Experiment 19 pH Measurements-Buffers and Their Properties (name the acid) 9.50. 10.54 11.83 pK₁

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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Calculate H+ and pKa (given is pH) refer to the picture below. ANSWER ALL THE PART THAT HAS QUESTION MARK. PLEASE Please include your solution. PLEASE ANSWER QUESTIONS 1-3 and use the 2nd picture for the formula that must be used
ammonium ion - ammonia C. Some Properties of Buffers Buffer system selected. NH4-NH3 HB is 1. pH of buffer 2. pH of diluted buffer 156 9.54 9.48 [H*]. [H*] NH4Cl CO.10 M) M pK, (by Eq. 4b) M pk, ? Experiment 19 pH Measurements-Buffers and Their Properties 3. pH of buffer in which [HB]/[B] = 0.10 pH after addition of excess NaOH (name the acid) ? ? 9.50. 10.54 11.83 pK₁
Transcribed Image Text:ammonium ion - ammonia C. Some Properties of Buffers Buffer system selected. NH4-NH3 HB is 1. pH of buffer 2. pH of diluted buffer 156 9.54 9.48 [H*]. [H*] NH4Cl CO.10 M) M pK, (by Eq. 4b) M pk, ? Experiment 19 pH Measurements-Buffers and Their Properties 3. pH of buffer in which [HB]/[B] = 0.10 pH after addition of excess NaOH (name the acid) ? ? 9.50. 10.54 11.83 pK₁
a strong The pH of such a buffer is established by the relative concentrations of HB and B in the solution. If we manipulate Equation 4, we can solve for the concentration of H+ ion: [H] = K₂ X [HB]/[B] (4a) This equation is often further modified when working with buffers, by taking the negative logarithm to base 10 of both sides: pH pK,+ log [B]/[HB] (4b)
Transcribed Image Text:a strong The pH of such a buffer is established by the relative concentrations of HB and B in the solution. If we manipulate Equation 4, we can solve for the concentration of H+ ion: [H] = K₂ X [HB]/[B] (4a) This equation is often further modified when working with buffers, by taking the negative logarithm to base 10 of both sides: pH pK,+ log [B]/[HB] (4b)
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