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.

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01-11-2021
Chemistry

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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 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.

Sagot :

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Polyalchemidn Polyalchemidn · Answer 1 · 2021-11-01T14:48:47-04:00

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

Sagot :

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