Question

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 ?

Answer 1

`M_(base)=0.14M`

Step-by-step 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:

`n_(acid)=(0.647g)/(126 g/mol) =0.00513mol`

Now, since the undergoing chemical reaction is:

`Ba(OH)_2+H_2C_2O_4\rightarrow BaC_2O_4+2H_2O`

Their molar relationship is 1 to 1, therefore:

`n_(acid)=n_(base)`

Thus, the barium hydroxide's molarity turns out:

`M_(base)=(0.00513mol)/(0.0359L)=0.14M`

Best regards.