If you had a 0.200 L solution containing 0.0140 M of Fe3+(aq), and you wished to add enough 1.27 M NaOH(aq) to precipitate all o

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If you had a 0.200 L solution containing 0.0140 M of Fe3+(aq), and you wished to add enough 1.27 M NaOH(aq) to precipitate all o

f the metal, what is the minimum amount of the NaOH(aq) solution you would need to add? Assume that the NaOH(aq) solution is the only source of OH−(aq) for the precipitation.

Chemistry

1 answer:

Lelechka [254] · Answer 1 · 2023-01-18T12:34:52+03:00

Answer: 6.6 ml

Explanation:

If you had a 0.200 L solution containing 0.0140 M of Fe3+(aq), and you wished to add enough 1.27 M NaOH(aq) to precipitate all of the metal, what is the minimum amount of the NaOH(aq) solution you would need to add? Assume that the NaOH(aq) solution is the only source of OH−(aq) for the precipitation.

You have 0.014X0,2 = 0,0028 moles of Fe ion.

You need 0,0028 X 3 = 00084 moles of OH

The NaOH is 1.27 moles/liter

0.084/1.27 = 6.6 ml