Oxalic acid dihydrate is a solid, diprotic acid that can be used in the laboratory as a primary standard. Its formula is H2C2O4•2H2O. A student dissolves 0.647 grams of H2C2O4•2H2O in water and titrates the resulting solution with a solution of barium hydroxide of unknown concentration. If 35.9 mL of the barium hydroxide solution are required to neutralize the acid, what is the molarity of the barium hydroxide solution ?

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sebassandin sebassandin · Answer 1 · 2020-03-23T01:11:10+01:00

Answer:

[tex]M_{base}=0.14M[/tex]

Explanation:

Hello,

In this case, the first step is to compute the oxalic acid dihydrate's moles as shown below, considering its molar mass as 126 g/mol:

[tex]n_{acid}=\frac{0.647g}{126 g/mol} =0.00513mol[/tex]

Now, since the undergoing chemical reaction is:

[tex]Ba(OH)_2+H_2C_2O_4\rightarrow BaC_2O_4+2H_2O[/tex]

Their molar relationship is 1 to 1, therefore:

[tex]n_{acid}=n_{base}[/tex]

Thus, the barium hydroxide's molarity turns out:

[tex]M_{base}=\frac{0.00513mol}{0.0359L}=0.14M[/tex]

Best regards.