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Potassium acid phthalate, KHP (KHC_8H_4O_4), is a primarystandard reagent used to determine exactly the concentation of asolution of base, such as NaOH, whose approximate concentration isknown. KHP is a weak acid, and the equation for the neurtalizationof KHP by NaOH is.....

a)C.A. Isernhagen dissolved .48 grams of KHP in 20.0mL of water.She found out that it required 17.0mL of NaOH to reach the endpointof the titration.

b)How many moles of the acid, KHP, were originally presentbefore the addition of the base?

c)How many moles of NaOH were required to neutralize the amountof KHP in Part b.

d)What is the concentration of the NaOH solution?

e) What is the ppH of the solution at the endpoint? (K_a for KHP= 3.89*10^-6)

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Nelly Stracke
Nelly StrackeLv2
28 Sep 2019
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Related questions

 
Calculate the amount of ascorbic acid in the Vitamin C tablet in (mg).  =?

A vitamin C (ascorbic acid) tablet was dissolved in approximately 50 mL of distilled water and titrated with the standardized NaOH solution. From 
the results of this titration, the mg of ascorbic acid in the tablet was calculated.
Molecular formulas:
Potassium hydrogen phthalate: HKC8H4O4
Acetic acid: C2H4O2
Ascorbic acid: C6H8O6
Assume that all 3 acids are monoprotic acids.



Mass of KHP used for standardization (g) 0.5464
Volume of NaOH required to neutralize KHP (mL) 13.31
Volume of vinegar sample titrated (mL) 5.00
Volume of NaOH required to neutralize vinegar in (mL) 8.40
Molecular weight of ascorbic acid (g/mol) 176.1271
Volume of NaOH required to neutralize ascorbic acid in Vitamin C tablet (mL) 13.85

What is the Molecular Weight of KHP (HKC8H4O4) in g/mol? 204.2220 
How many moles of KHP were used in the standardization of the NaOH solution? 0.002595
Calculate the concentration of NaOH solution in (mol/L). 0.188433
Calculate the molarity of the vinegar solution (mol/L). 0.303377

Suppose a standardstrong-base solution was prepared byweighing out 1.934 g of NaOHin 500 mL of water. This solution wastitrated against KHPdissolved in 200 mL of water required 48.23 mLof the basesolution.

1. Howmany moles of NaOH were initiallyweighed out to prepare the“standard base solution?”

2. What is the apparent molarity of the“standard base,” using the massof NaOH weighed out andthe volume of water used?

3. Howmany moles of KHP were weighed out?

4. Howmany moles of NaOH were required toneutralize the KHP that wasweighed out?

5. What is the molarity of the “standardbase”using the informationobtained from KHP titration?

6. Explain the difference in the answers toquestion 2 and question 5.Which is the “correct”value for the concentration of the standardNaOH solution?

A solution ofH2SO4 with unknownconcentration was titratedwith the standard base described above. Avolume of 5.03 mLof the acid solution required 12.07 mL of thestandard base toreach the end point using phenolphthaleinindicator.

7. Howmany moles of standard base wererequired to neutralize theH2SO4 solution?

8. How many molesof H2SO4 werepresent in the sample of acidtotrated?

9. What is themolarity of the acid solution?

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