Question: how would you expect solubility of product of potassium bitartrate to vary between distilled water and a KNO3 solution? Experiment 2: Determination of the solubility of potassium bitartrate in KNO3 solutionWhat is the common ion in this experiment?ор монand a solution with KNO3?How do you expect the solubility product of KHC4H4O6 to vary between the distilled water solutionHow do you expect the solubility of KHC4H4O6 to vary between the solutions with and without KNO3?Complete the following table: NaoH = 0,001 m0.05.M.0.10 M.0.15 M.0.20. M0.30.M.600 M.Average VNaOH (cm³)23.6833| 18.88333 12.7333310.508.5333KHC4H4O6solubility (M)Draw a graph of solubility of potassium bitartrate against potassium nitrate concentrationusing MS Excel and the data provided in the video. Experiment 2Experiment 2: Determination of the solubility of potassium bitartrate in KN03 solutionApparatus and equipmentChemicalsAnalytical balancePotassium bitartrate ( KHC4H406)250 mL beaker (2)Distilled waterFilter paper (dry)Standard solution 2: NaOHaq (0.01 M)FunnelIndicator: phenolphthaleinBurette5 x different KNO3 solutionsPipette(0.05 M, 0.10 M, 0.15 M 0.20 M, 0.30 M)Thermometer (at tutor)Ehrlenmeyer flasks (4)Experimental procedure6. Repeat the above experiment (1 8) replacing the deionized water in the solution by 150 mL of the assigned potassium nitrate (KNO3) solution, using sodiumhydroxide solution (standard 2) for titration.7. Calculate the solubility and solubility product of potassium bitartrate in both water and the potassium nitrate solution. Show all calculations.8. Use the collected results to plot a graph of the solubility of potassium bitartrate against potassium nitrate concentration. Include the solubility of potassium bitartratein pure water (0.0 M potassium nitrate) on the graph.

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how would you expect solubility of product of potassium bitartrate to vary between distilled water and a KNO3 solution?

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter7: Statistical Data Treatment And Evaluation

Section: Chapter Questions

Problem 7.21QAP

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Question

Question: how would you expect solubility of product of potassium bitartrate to vary between distilled water and a KNO3 solution?

Experiment 2: Determination of the solubility of potassium bitartrate in KNO3 solution
What is the common ion in this experiment?
ор мон
and a solution with KNO3?
How do you expect the solubility product of KHC4H4O6 to vary between the distilled water solution
How do you expect the solubility of KHC4H4O6 to vary between the solutions with and without KNO3?
Complete the following table: NaoH = 0,001 m
0.05.M.
0.10 M.
0.15 M.
0.20. M
0.30.M.
600 M.
Average V
NaOH (cm³)
23.6833| 18.88333 12.73333
10.508.5333
KHC4H4O6
solubility (M)
Draw a graph of solubility of potassium bitartrate against potassium nitrate concentration
using MS Excel and the data provided in the video.

Experiment 2
Experiment 2: Determination of the solubility of potassium bitartrate in KN03 solution
Apparatus and equipment
Chemicals
Analytical balance
Potassium bitartrate ( KHC4H406)
250 mL beaker (2)
Distilled water
Filter paper (dry)
Standard solution 2: NaOHaq (0.01 M)
Funnel
Indicator: phenolphthalein
Burette
5 x different KNO3 solutions
Pipette
(0.05 M, 0.10 M, 0.15 M 0.20 M, 0.30 M)
Thermometer (at tutor)
Ehrlenmeyer flasks (4)
Experimental procedure
6. Repeat the above experiment (1 8) replacing the deionized water in the solution by 150 mL of the assigned potassium nitrate (KNO3) solution, using sodium
hydroxide solution (standard 2) for titration.
7. Calculate the solubility and solubility product of potassium bitartrate in both water and the potassium nitrate solution. Show all calculations.
8. Use the collected results to plot a graph of the solubility of potassium bitartrate against potassium nitrate concentration. Include the solubility of potassium bitartrate
in pure water (0.0 M potassium nitrate) on the graph.

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