MolesKHP: 0.02498 Molarity of KHPSolution: 0.09994 Mass ofNaOH: 2.116 FIND: 1) M

Question

MolesKHP:                                0.02498
Molarity of KHPSolution:            0.09994
Mass ofNaOH:                           2.116

FIND:
1) Moles of KHP in aliquot:
2) Moles of NaOH reacted:
3) Molarity of NaOH:

1) 0.0200L x 0.09994 = 0.0019988
2) =0.0019988 because [KHC8H4O4(aq) + NaOH(aq) --> H2O(l)+ KNaC8H4O4(aq)] is a 1:1 mole ratio. [Is this right??]
3) this is where I'm a bit stuck... I'll provide some infobelow:

Draw up 20.00mL of the Standard KHP solution and drain into 125mLErlenmeyer flasks. Repeat by adding 20.00ml of standard KHP sol'nto two more 125mL flasks. Fill 50mL buret w/the base solution(NaOH) Open tip and let drip into Erlenmyer flask (KHP) untilendpoint is reached:

Data for First Aliquot:
Volume of KHP
20.00mL
Final Buret Reading
37.90 Initial Buret Reading
19.20 Volume of NaOH used
18.70 The other initial/final readings and volumes used for the other twoaliquots are different but wouldn't the molarity of NaOH for eachbe the same bc (from what I have) the moles of KHP & NaOH areall the same (0.0019988)
It also asks me for the average molarity of NaOH for all threealiquots so for some reason I feel like the numbers should vary?maybe not...

Any help would be GREATLY appreciated. Let me know if anything elseis need/required to solve..

-Scotte

Volume of KHP
20.00mL
Final Buret Reading
37.90 Initial Buret Reading
19.20 Volume of NaOH used
18.70

Explanation / Answer

3) Just divide the moles of NaOH you got in 2) by the volume ofNaOH used during the titration (0.01870 L). molarity = moles/volume. Since the volume you used for eachtitration is different, you should obtain 3 different molarities(even if the moles are the same).

Related Questions

Navigate

• Browse (All)
• Browse M
• Subjects

---

---

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