Calculate how much NaOH solution you will need to reach the equivalence point wh

Question

Calculate how much NaOH solution you will need to reach the equivalence point when standardizing the NaOH with KHP. Assuming that you've made exactly a 0.25 M NaOH solution and you were able to measure out exactly 0.5 g of KHP. Write this value in the "Notes" section under "Titrating with the KHP standard," show your work. Calculate the volume you will need of concentrated HCI to make 100 mL of 1.16 M HCI. Repeat your calculations to determine the volumes of dilute HCI you will need in the other serial dilutions. Write these values in the "Notes" section under "Serial Dilution of HCI," show your work.

Explanation / Answer

Q7

volume of NaOh solution required for equivalence point:

NaOH = 0.25 M

m = 0.5 g of KHP

MW of KHP = 204.22

mol = 0.5/204.22 = 0.002448 mol of KHP

now..

KHP + NaOH = KNaP + H2O

ratio is 1:1

so

0.002448 mol of base is require

for volume:

M = mol/V

V = mol/M

V= 0.002448/0.25

V = 0.009792 L required of base

Q8

Calculate

V = 100 mL = 0.1 L

M = 1.16 M

mol = MV = 0.1*1.16 = 0.116 mol

mass = mol*MW = 0.116*36.5 = 4.234 g of HCl requried

Related Questions

Navigate

• Browse (All)
• Browse C
• Subjects

---

---

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