The concentration of an unknown sample of sulfuric acid was determined by the method used in this experiment. In the first titration, the sodium hydroxide was standardized by titrating 0.1852g of oxalic acid dihydrate (molar mass = 126.07g/mol) with 32.30 mL of sodium hydroxide solution. In the second titration, 10.00mL of the unknown sulfuric acid solution was titrated with 12.85mL of the sodium hydroxide solution. What was the concentration of the sulfuric acid? Part C. Determination of UnknownBalanced chemical equation:Hcl+ Na O4-o Narl t HaaUnknown number NATrial 1Trial 2Trial 3Volume of unknown HCltitrated10.00mLNANAInitial burette reading0.90mLFinal burette reading30.90mL_Volume NaOH added20 00MLg0.0OML X.0.144 m=432mmoles NaOH added4.335m(Use average molarity from part 'Band multiply it by the volume you added)moles HCI4.335m0.00435 m=0.4335m10.00MLmolarity of HCl04335 MActual Molarity (from instructor)0.3150Mpercentage error37,6%-O 4335 M - D.3150m0.3150MX100)= 37.G:/.

Given that: mass of oxalic acid = 0.1852 g volume of NaOH = 32.30 mL = 0.03230 L (first titration)…

Answered: The concentration of an unknown sample…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter4: Types Of Chemical Reactions And Solution Stoichiometry

Section: Chapter Questions

Problem 47E

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The concentration of an unknown sample of sulfuric acid was determined by the method used in this experiment. In the first titration, the sodium hydroxide was standardized by titrating 0.1852g of oxalic acid dihydrate (molar mass = 126.07g/mol) with 32.30 mL of sodium hydroxide solution. In the second titration, 10.00mL of the unknown sulfuric acid solution was titrated with 12.85mL of the sodium hydroxide solution. What was the concentration of the sulfuric acid?

Part C. Determination of Unknown
Balanced chemical equation:
Hcl+ Na O4-o Narl t Haa
Unknown number NA
Trial 1
Trial 2
Trial 3
Volume of unknown HCl
titrated
10.00mL
NA
NA
Initial burette reading
0.90mL
Final burette reading
30.90mL_
Volume NaOH added
20 00ML
g0.0OML X.0.144 m=432m
moles NaOH added
4.335m
(Use average molarity from part 'B
and multiply it by the volume you added)
moles HCI
4.335m
0.00435 m
=0.4335m
10.00ML
molarity of HCl
04335 M
Actual Molarity (from instructor)
0.3150M
percentage error
37,6%-
O 4335 M - D.3150m
0.3150M
X100)= 37.G:/.

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