Macmillan Learning Question 7 of 20 > Attempt 1 To a 25.00 mL volumetric flask, a lab technician adds a 0.125 g sample of a weak monoprotic acid, HA, and dilutes to the mark with distilled water. The technician then titrates this weak acid solution with 0.0866 M KOH. She reaches the endpoint after adding 47.47 mL of the KOH solution. Determine the number of moles of the weak acid in the solution. moles of weak acid: 0.00369441 Incorrect Answer Determine the molar mass of the weak acid. 33.8359 molar mass= Incorrect Answer mol g/mol After the technician adds 17.39 ml. of the KOH solution, the pH of the mixture is 5.33. Determine the pKa of the weak acid. 4.68858 PK₁ = Incorrect Answer

Macmillan Learning Question 7 of 20 > Attempt 1 To a 25.00 mL volumetric flask, a lab technician adds a 0.125 g sample of a weak monoprotic acid, HA, and dilutes to the mark with distilled water. The technician then titrates this weak acid solution with 0.0866 M KOH. She reaches the endpoint after adding 47.47 mL of the KOH solution. Determine the number of moles of the weak acid in the solution. moles of weak acid: 0.00369441 Incorrect Answer Determine the molar mass of the weak acid. 33.8359 molar mass= Incorrect Answer mol g/mol After the technician adds 17.39 ml. of the KOH solution, the pH of the mixture is 5.33. Determine the pKa of the weak acid. 4.68858 PK₁ = Incorrect Answer

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter31: Introduction To Analytical Separations

Section: Chapter Questions

Problem 31.17QAP

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Similar questions

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A bottle of concentrated hydroiodic acid is 57% HI by weight and has a density of 1.70 g/mL. A solution of this strong and corrosive acid is made by adding exactly 10.0 mL to some water and diluting to 250.0 mL. If the information on the label is correct, what volume of 0.988 M NaOH is needed to neutralize the HI solution? Suggest an indicator for the titration.
8-115 When a solution prepared by dissolving 0.125 g of an unknown diprotic acid in 25.0 mL of water is titrated with 0.200 M NaOH, 30.0 ml, of the NaOH solution is needed to neutralize the acid. Determine the molarity of the acid solution. What is the molar mass of the unknown diprotic acid?
8-47 A sample of 27.0 mL of 0.310 M NaOH is titrated with 0.740 M H2SO4. How many milliliters of the H2SO4 solution are required to reach the end point?
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100 mL of 0.10 M NH3 (Kb = 1.8 x 10-5) are mixed with 100 mL of 0.10 M HCN (Ka = 4.9 × 10-10). Which statement is true? (3) The resulting solution is neutral O (2) The resulting solution is basic O (4) No answer is correct as not enough information is given. O (1) The resulting solution is acidic E D Moving to the next question prevents changes to this answer. 4 R F % S T G 6. & 7 H C 8 00 K M Question 2 of 37
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3: Based on the ice table and Alan expression determine the ph of the solution