For the parts circled in orange, my question is since we are trying to find moles of H3A here, are we dividing by 3 because there are 3 H, or are we dividing by 3 because there are 3NaOH? Basically, why are we dividing by 3 Supplemental Problems from Chapter 53. In an experiment, 0.956 grams of an unknown acid, H3A, is titrated with a standardizedNaOH solution. If 29.1 mL of 0.513 M NaOH solution is required to react completely withthe unknown acid, what is the molar mass of the unknown acid? Hint: write the balancedchemical equation.Because we are dealing with a triprotic acid, the mole ratio between the acid and sodiumhydroxide is not 1:1. The balanced chemical equation for this titration becomes:H3A(aq) +3NAOH(aq) →N33A(aq) + 3H2O(I)We know the grams of unknown acid (0.956 g) so now we need moles of acid to obtain molar mass(molar mass = grams of acid / moles of acid)Moles of H3A = 0.004976 molesMolar mass H3A = 0.956 g / 0.004976 moles = 192.1 g/mole%3D0.0291*0,513=3D0.0149molesNaOH3.=0.0050moles71310.956= 193.1g/mole%3D0.005

Answered: Image /qna-images/answer/9f23771d-a6fa-4e93-be80-34a030fa7a59.jpg

For the parts circled in orange, my question is since we are trying to find moles of H3A here, are we dividing by 3 because there are 3 H, or are we dividing by 3 because there are 3NaOH? Basically, why are we dividing by 3

For the parts circled in orange, my question is since we are trying to find moles of H3A here, are we dividing by 3 because there are 3 H, or are we dividing by 3 because there are 3NaOH? Basically, why are we dividing by 3

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter3: Chemical Reactions

Section: Chapter Questions

Problem 153QRT

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Stoichiometry

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Question

Supplemental Problems from Chapter 5
3. In an experiment, 0.956 grams of an unknown acid, H3A, is titrated with a standardized
NaOH solution. If 29.1 mL of 0.513 M NaOH solution is required to react completely with
the unknown acid, what is the molar mass of the unknown acid? Hint: write the balanced
chemical equation.
Because we are dealing with a triprotic acid, the mole ratio between the acid and sodium
hydroxide is not 1:1. The balanced chemical equation for this titration becomes:
H3A(aq) +3NAOH(aq) →
N33A(aq) + 3H2O(I)
We know the grams of unknown acid (0.956 g) so now we need moles of acid to obtain molar mass
(molar mass = grams of acid / moles of acid)
Moles of H3A = 0.004976 moles
Molar mass H3A = 0.956 g / 0.004976 moles = 192.1 g/mole
%3D
0.0291*0,513
=
3D0.0149molesNaOH
3.
=0.0050moles
7
131
0.956
= 193.1g/mole
%3D
0.005

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