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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
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
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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 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
Transcribed Image Text: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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