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

Scarlet

3 February, 02:29

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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Barton · 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.