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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• 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?
In bromine water test Procedure: -Add 3 ml of phenol and ethanol in separate test tube-Add 10 ml of water to each test tubes-Transfer to bigger test tubes-For phenol and ethanol, Add bromine water drop by drop until bromine color persists MUST DO: Observe formation of precipitate P.s I provided photos for better visualization of the overall result procedure, I just need a further and detailed answer based on observation. If answered properly I will upvote, I promise tyyy. Please do focus on the formation of precipitate, thank youuu The first photo is the phenol one (colored one) and the second one is the ethanol (clear one)
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5
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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.