Question

0.556 g of a solid white acid are dissolved in water and completely neutralized by the addition of 52.38 mL of 0.396 M NaOH. Calculate the molar mass of the acid, assuming it to be a monoprotic acid

Answer 1

`M_(acid)=26.804g/mol`

Step-by-step explanation:

Hello,

In this case, by knowing that the used NaOH equals in moles the acid (monoprotic) as shown below, during the titration:

`n_(acid)=n_(NaOH)`

By knowing the volume and the concentration of the NaOH, one obtains:

`n_(acid)=0.05238L*0.396(mol)/(L)=0.0207mol`

Thus, the molar mass of the acid is computed based on the previously computed moles and the given mass as follows:

`M_(acid)=(m_(acid))/(n_(acid))=(0.556g)/(0.0207mol)=26.804g/mol`

Best regards.