A saturated solution of sodium bitartrate (NaC4H5O6) is prepared by adding 2 g o

Question

A saturated solution of sodium bitartrate (NaC4H5O6) is prepared by adding 2 g of NaC4H5O6 to 50.00 mL of 0.200 M NaCl solution. A 20.00 mL sample of the saturated NaC4H5O6 solution was diluted with 25 mL of distilled water then titrated to a phenolphthalein end point by the addition of 16.55 mL of 0.0500 M NaOH. Given the titration reaction below, how many moles of C4H5O6- were in the 20.00 mL sample of solution?

C4H5O6-(aq) + OH-(aq) --> H2O(l) + C4H4O62-(aq)

What was the concentration of C4H5O6- in the 20.00 mL sample of the saturated solution?

What was the concentration of sodium ions (Na+) in the saturated solution?

What is the Ksp of sodium bitartrate?

Explanation / Answer

0.01655 L X 0.050 mol/L = 8.28X10-4 mol NaOH used.

In the titration of sodium bitartrate with NaOH, there is a 1:1 ratio between NaOH and the bitartrate. So, the 20 mL sample contained 8.28X10-4 moles of sodium bitartrate.

A) concentration of C4H5O6- in the 20.00 mL sample of the saturated solution is

=   8.28X10-4 (1000/20) = 0.0415 M

B) Just double = 0.0828 M

C) Ksp = [ NA + ][C4H5O6-] = Multiply answers of pat A and part B

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

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