A buffer contains 0.005 mol of lactic acid (pK,= 3.86) and 0.075 mol of sodium lactate per liter. H₂C. OH Lactic acid OH Calculate the pH of the buffer. H₂C. OH Sodium lactate Calculate the change in pH after adding 5.5 ml. of 0.40 M HCl to 1.0 L of the buffer. O Na Calculate the change in pH after adding 5.5 mL of 0.40 M HCI to 1.0 L of pure water. buffer pH: 5.04 buffer pH change: water pH change: 0.16 2.66 Incorrect units units

A buffer contains 0.005 mol of lactic acid (pK,= 3.86) and 0.075 mol of sodium lactate per liter. H₂C. OH Lactic acid OH Calculate the pH of the buffer. H₂C. OH Sodium lactate Calculate the change in pH after adding 5.5 ml. of 0.40 M HCl to 1.0 L of the buffer. O Na Calculate the change in pH after adding 5.5 mL of 0.40 M HCI to 1.0 L of pure water. buffer pH: 5.04 buffer pH change: water pH change: 0.16 2.66 Incorrect units units

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 contains 0.222 M CH3NH3Br and 0.443 M CH3NH2 (methylamine). Determine the pH change when 0.133 mol HI is added to 1.00 L of the buffer. pH after addition pH before addition = pH change Determine the pH change when 0.045 mol HCIO4 is added to 1.00 L of a buffer solution that is 0.471 M in HCIO and 0.201 M in CIO". pH after addition pH before addition = pH change =
Buffer Intensity?
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-4 A chemistry graduate student is given 500. mL of a 1.60M nitrous acid (HNO₂) solution. Nitrous acid is a weak acid with K =4.5 × 10 NaNO₂ should the student dissolve in the HNO₂ solution to turn it into a buffer with pH. = 3.19? What mass of You may assume that the volume of the solution doesn't change when the NaNO₂ is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.
7
A 1.00 liter solution contains 0.23 M acetic acid and 0.30 M potassium acetate. If 0.150 moles of potassium hydroxide are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of potassium hydroxide.) +A. The number of moles of CH3COOH will remain the same. + B. The number of moles of CH3COO" will remain the same. C. The equilibrium concentration of H30* will remain the same. + D. The pH will remain the same. E. The ratio of [CH3COOH]/[CH;COO"] will decrease.
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