Question

Chemistry I Laboratory Manual, 2019 Revision Questions: 1) What mass of KHP would you need in order to use titrate it? would you need in order to use 35.00 mL of 0.500 M NaOH to 2) A student weighs out 1.051 g of impure KHP, dissolves the sample in deionized water and titrates it with 0.1101 M NaOH solution. If the titration requires 26.10 mL of the NaOH solution, and none of the impurities react with NaOH, what is the percent KHP in the sample?

Answer 1

vate . At equivalence point, No of Moles of KHP = No of Moles of Naoh Now, Molarity = No of Moles volume (in L) - No of Moles & Molarity & volume (in L) - & No of moles of KHP = (MXV) Nach or Mass of KHP = Mnach x V Noor Molar Mass of KHP = 0.500 M X 35.00 L 1000 Mass of KHP 204. 22 gl mol * Mass of KHP = 0.0175 mol 204. 22 g/mol * Mass of KHP = 0.0115 mol X 204. 22 g/mol Mass of KHP = 3.5138 g & Mass of KHP required is 3.5138 g.

Date II 23. During tibration, at equivalence point = No of Moles of KHP = No of Moles of Naoh Mass of KHP = CM X V) Noor Molar Mass of KHP = Mass of KHP 204. 22 g/mol 0.1101 X 26.10 L 1000 M = Mass of KHP = 0.5868 g Thus, from the 1.051g of impure KHP, only 0.5868 g of KHP reacts with Naoh. & Percent KHP in the sample :- 0.5868 g x 100 2 1.0519 * 55.83% Thus, the percent XHP in the sample is 55.83%