A sample contains an unknown amount of tartaric acid, H2C4H4O6. If 0.3888 g of the sample
requires 37.74 mL of 0.1000 M NaOH to neutralize the H2C4H4O6 completely, what is the percentage of
H2C4H4O6 in the sample? The molar mass of H2C4H4O6 is 150.09 g/mol. The balanced equation for the
reaction is:
H2C4H4O6 + 2 NaOH → 2 H2O + Na2C4H4O6
So i got 72.84
You have 0.6559 g of an unknown monoprotic acid, HA, which reacts with NaOH according to the
balanced equation
HA + NaOH → NaA + H2O
If 36.67 mL of 0.0934 M NaOH is required to titrate the acid to the equivalence point, what is the molar
mass of the acid?
I got 190.5
Am I right? Appreciate any help

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  1. 72.84 yes
    190.5 no but close.

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    2. 👎
  2. 191.5?

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    2. 👎
  3. yes

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