9. To correctly adjust the pH of a solution to be used in an electrophoretic separation procedure, exactly 60.81 mL of 1.209 M NaOH were added to 100.00 mL of 1.418 M lactic acid (HLac). HLac + NaOH →NaLac + H₂O Please answer the following questions. A. B. C. Determine the equilibrium concentration of lactic acid in the buffer solution. Please provider your answer below. 0² 0₂ Determine the equilibrium concentration of NaLac in the buffer solution. Please provider your answer below. 7² 0² $ → → S ■ Given that Ka = 1.403×10-4 for lactic acid, determine the pH of the buffer solution. pH = Please provider your answer below. M A $ □ M

9. To correctly adjust the pH of a solution to be used in an electrophoretic separation procedure, exactly 60.81 mL of 1.209 M NaOH were added to 100.00 mL of 1.418 M lactic acid (HLac). HLac + NaOH →NaLac + H₂O Please answer the following questions. A. B. C. Determine the equilibrium concentration of lactic acid in the buffer solution. Please provider your answer below. 0² 0₂ Determine the equilibrium concentration of NaLac in the buffer solution. Please provider your answer below. 7² 0² $ → → S ■ Given that Ka = 1.403×10-4 for lactic acid, determine the pH of the buffer solution. pH = Please provider your answer below. M A $ □ M

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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AA Learning Learning prod03-cnow-owl.cengagenow.com Login Learning × Online tea... y dr. marlow... Member L... 1req 1req Use the References to access important values if needed for this question. The Solubility Product Constant for silver bromide is 3.3 x 10-13 Solid ammonium bromide is slowly added to 75.0 mL of a 0.0663 M silver acetate solution. The concentration of bromide ion required to just initiate precipitation is M.
• An unknown acid (HA) was titrated with NaOH(aq). • The following titration curve was constructed using the laboratory data. You will use this titration curve to answer the questions related to this problem. • Assume that all laboratory work was completed at 298 K. 14 12 10 6. 4. 2. 4 9. 8. 10 12 14 16 18 20 22 24 26 28 30 Volume of Titrant / mL Which of the following net ionic equations explains the pH of the analyte solution before any titrant is added? A (aq) + H20(1) HA(aq) + OH (aq) A (aq) + H3O*(aq) --> HA(aq) + H20(1) O H*(aq) + OH (aq) H20(1) --> O HA(aq) + OH (aq) --> H2O(aq) + A (aq) HA(aq) + H20() H3O*(aq) + A (aq)
A student performed three KHP titrations in Part 1 in order to standardize their NaOH solution. They reported the following measurements: Mass of KHP + Vial Mass of 'Empty' Vial Final Burette Reading Initial Burette Reading Determination #1 16.7538 g 16.2649 g 21.67 mL 0.40 mL Determination #2 14.1709 g 13.5560 g 26.98 mL 0.31 mL Determination #3 15.6625 g 15.0833 g 26.04 mL 0.93 mL How many moles of KHC8H4O4 did they use in their second titration? Report your answer to the correct number of significant figures and only report the numerical value (no units).
Why is it normal to add a slight excess of silver nitrate solution when precipitating chloride ion?
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Answer all questions completely. SHOW ALL WORK/CALCULATIONS:
Show all pertinent computations A. The solubility of ferric hydroxide is 4.8 x 10° g/100 ml at room temperature. Calculate its solubility product constant.
can you help me calculate the number of moles for the first three substances?
Scientists determine the quantity of atmospheric sulfur dioxide (SO, ), a large contributor to acid rain, by an indirect titration. First, a scientist collects a sample of air and reacts it with hydrogen peroxide (H, 0, ) to form a solution of sulfuric acid ( H, SO, ). Then, the amount of H, SO, produced is determined by titration with a sodium hydroxide solution (NaOH) of known concentration. H,O,(aq) + SO,(g)– H, SO,(aq) H, SO, (aq) + 2 NaOH(aq) 2 H, O(1) + Na, SO4(aq) Suppose Lane collects a 608.0 g sample of air that is known to contain SO, and reacts it with excess H,O, . A volume of 17.8 mL of 0.010 M NaOH is required to neutralize the H, SO, produced. Calculate the mass percent of SO, in the air sample. mass percent: % SO2
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