0.436 g of an unknown diprotic acid is dissolved in about 60 mL of water in a beaker. The solution is transferred to a 100.00 mL beaker. 25.00 mL of this solution is then transferred to an Erlenmeyer flask for the titration. What mass of the diprotic acid is in the 25.00 mL that is transferred?

Question

Chemistry

Stephen Decker

31 December, 08:03

0.436 g of an unknown diprotic acid is dissolved in about 60 mL of water in a beaker. The solution is transferred to a 100.00 mL beaker. 25.00 mL of this solution is then transferred to an Erlenmeyer flask for the titration. What mass of the diprotic acid is in the 25.00 mL that is transferred?

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Answers (2)

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Kareem Molina · Answer 1

0.182 g

Explanation:

0.436 g of the acid was dissolved in 60 mL of water and then transferred into a 100.00 mL beaker. The volume still remains 60 mL.

25 mL was then transferred to Erlenmeyer flask for titration.

If 60 mL of the solution contains 0.436 g of the unknown diprotic acid, then 25 mL of the same solution would contain:

0.436 x 25/60 = 0.182 g

Hence, the mass of the diprotic acid in the 25.00 mL of the solution is 0.182 g.