Question

# A solution of an unknown acid is prepared by dissolving 5.968 g of the solid acid...

A solution of an unknown acid is prepared by dissolving 5.968 g of the solid acid in sufficient DI water to make 350.00 mL of solution. 20.12 mL of a 0.1666 M NaOH solution are required to neutralize 10.00 mL of this acid solution?

Are you sure, that's your question?. Because in order to know if that volume is required to neutralize the solution, I need the molecular weight of the acid, and I need to know if the acid is monoprotic or diprotic.

In this case, I will assume the acid is monoprotic, and that you want to calculate the concentration of the acid along with the molecular weight.

In this case, we use the following equation: MaVa = MbVb and we solve for Ma:
Ma = 0.1666 M * (20.12/10) = 0.3352 M

Now, let's find out how many moles we have in the 350 mL of solution:
moles = 0.3352 * 0.350 = 0.1173 moles

Finally the molecular weight will be:
MW = 5.968 g / 0.1173 moles = 50.87 g/mol

Hope this helps

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