Question

In an experiment similar to this one, the solubility of potassium hydrogen oxalate (KHC2O4, molar mass= 128.13 g mol) is determined. A 5.0 10^-2 M aqueous solution of KCI is saturated with potassium hydrogen oxalate. The following equilibrium results: KHC2O4(s)-----K^+ + HC2O4^-

Following saturation, the solution is filtered. Portions of the filtered saturated solution are titrated with 0.1172M NaOH solution.

The following date are obtained:

Volume of saturated KHC2O4 Solution Titrated, mL Determination #1 25.2 Determination #2 29.1

Volume of NaOH solution used, mL ---------------------Determination #1 36.88 Determination #2 41.81

Temperature of saturated solution, C-------------------- Determination #1 20.1 Determination #2 20.1

Calculate the following:

number of moles off NaOH needed, mol _______________________For both determinations

number of moles of HC2O4 ^- titrated, mol______________________For both determinations

[HC2O4^-] sat. sol'n_______________________________________For both determinations

[K^+]initial______________________________________________For both determinations

[K^+]from dissolved KHC2O4________________________________For both determinations

[K^+] sat. sol'n___________________________________________For both determinations

Ksp___________________________________________________For both determinations

average Ksp

solubility of KHC2O3 in 5.0 x 10^-2M KCI, mol L___________________for both determinations

Average solubility of KHC2O4 in 5.0 x 10^-2 KCI, mol L

solubility of KHC2O4 in 5.0 x 10^-2 M KCI, g per 100 mL

Answer 1