Question

Information given: The following data is recorded, For the following KHP solution, 10.575g of KHP is dissolved water, and diluted to 250.00mL in a volumetric flask; 20.00mL of the KHP solution are added to an Erlenmeyer flask; a buret is filled with NaOH solution of unknown concentration to a starting volume of 0.18mL, and at the end point if the titration the buret reading is 20.83mL.

1.) Calculate the moles of KHP that were put into the 250.00mL volumetric flask.

2.) Calculate the molarity of the KHP solution that was prepared in the 250-mL volumetric flask.

3.) Calculate the number of mmoles of KHP that are in the 20.00mL aliquot.

4.) Write the balanced chemical equation for the reaction of KHP with sodium hydroxide.

5.) Calculate the number of mmoles of NaOH that will be needed to reach the end point when the 20.00mL aliquot is titrated.

6.) Calculate the volume of NaOH used in the titation.

7.) Calculate the molarity of the NaOH solution.

Answer 1

1.) moles of KHPhat were put into the 250.00mL volumetric flask =weight/MW=10.575/204.22=0.05178

2.) molarity of the KHP solution that was prepared in the 250-mL volumetric flask

                                                                      = moles/Vol in Litres=0.05178/0.25= 0.2071 M

3.) number of mmoles of KHP that are in the 20.00mL aliquot= (51.78/250) x 20 = 4.1424

4.) C₈H₅O₄K + NaOH -------> C₈H₄O₄KNa + H₂O