In an experiment similar to this one, the solubility of potassium hydrogen oxala

Question

In an experiment similar to this one, the solubility of potassium hydrogen oxalate (KHC204, molar mass = 128.13 g mol-1) is determined. A 5.0 x 10 2M aqueous solution of KCl is saturated with potassium hydrogen oxalate. The following equilibrium results: Calculate the following: number of moles of NaOH needed, mol Following saturation, the solution is filtered. Portions of the filtered saturated solution are titrated with 0.1172M NaOH solution. The following data are obtained: number of moles of HC204-titrated, mol soi'n [K+]inrtial [K+]I from dissolved KHC2 O4 [K+] sat. soi'n average Ksp solubility of KHC204 in 5.0x10-2MKcl.molL-1 average solubility of KHC204 in 5.0x10-2WKCl, molL-1 solubility of KHC204 in 5.0 x 10"2MKCI. g per 100 mL

Explanation / Answer

no of moles of NaOH = conc. x volume = 0.1172 x 36.88 x 10^-3 = 4.32 x 10^-3

(we multiplied by 10^-3 becaus the volume is in ml and we have to covert it to meter cube)

Related Questions

Navigate

• Browse (All)
• Browse I
• Subjects

---

---

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