High School

Oxalic acid dihydrate is a solid, diprotic acid that can be used in the laboratory as a primary standard. Its formula is \(\text{H}_2\text{C}_2\text{O}_4 \cdot 2\text{H}_2\text{O}\).

A student dissolves 0.647 grams of \(\text{H}_2\text{C}_2\text{O}_4 \cdot 2\text{H}_2\text{O}\) 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?

Answer :

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.

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