How do we solve this with dimensional analysis?

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How do we solve this with dimensional analysis? 

13. 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) → NazA(aq) + 3H2O(1)
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)
%3D
Moles of H3A = 0.004976 moles
Molar mass H3A = 0.956 g /0.004976 moles = 192.1 g/mole
%3D
Transcribed Image Text:13. 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) → NazA(aq) + 3H2O(1) 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) %3D Moles of H3A = 0.004976 moles Molar mass H3A = 0.956 g /0.004976 moles = 192.1 g/mole %3D
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