Bryce mixed up his samples for determining the solubilities and Ksp values for p

Question

Bryce mixed up his samples for determining the solubilities and Ksp values for potassium acid tartrate (KHtTar). He titrated, using a 50-mL buret, all his samples with a 0.133 M NaOH (uncertainty is 1.16%) solution using a phenolphthalein indicator and collected the following data

KHtar (s) <-------> K+ (aq) + HTar- (aq) The equilibrium studied

HTar- (aq) + NaOH (aq) ------> H2O (l) + Na+ (aq) + Tar2- (aq) Acid-base Titration

Volume of NaOh

Sample A B C

Trial 1 16.6 mL 5.9 mL 13.4 mL

Trial 2 16.6 mL 5.7 mL 13.6 mL

Average 16.6 mL 5.8 mL 13.5 mL

50.0 mL Samples of solutions A, B, and C were titrated. A 100-mL graduated cylinder was used.

Bryce used the following solvents to dissolve the KHtar, an 0.10 M KNO3 (uncertainty is 0.24 %) solution, an 0.10 M NaNO3 (uncertainty is 0.17 %, and pure water. With your knowledge of solubility, equilibirium, and ionic strength, deduce which sample corresponds to which solvent system. Calculate the solubility of KHTar and Ksp for each deduced solvent system. (a) Explain how the common ion effect changes the solubility of KHtar between 0.10 M NaNO3 and 0.10 M KNO3. Should the Ksp be the same for these two solvents? Do the experimental results agree with your answers to the prevous questions? (b) Is KHtar more soluble in water or in 0.10 M NaNO3? Explain in terms of the intermolecular forces experineced by the solute. (c) Explain why KHTar will dissolve readily in KOH solution. (d) Use the experimental results to predict the solubility of KHTar ina solution that is both 0.950 M in NaNO3 and 0.050 M in KCl (e) Calculate the uncertainty for the solubility and Ksp

Explanation / Answer

http://www.foothill.edu/attach/psme/sinha.KspofKHT.pdf

please check the pdf link... i think it will help you..

Related Questions

Navigate

• Browse (All)
• Browse B
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.