Question

Let us assume that Cr(OH)3(s) is completely insoluble, which signifies that the precipitation reaction with NaOH(aq)...

Let us assume that Cr(OH)3(s) is completely insoluble, which signifies that the precipitation reaction with NaOH(aq) (presented in the transition) would go to completion.

Cr3+(aq)+3NaOH(aq) → Cr(OH)3(s)+3Na+(aq)

If you had a 0.600 L solution containing 0.0130 M of Cr3+(aq), and you wished to add enough 1.26 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.

Express the volume to three significant figures and include the appropriate units.

Homework Answers

Answer #1

The given equation is :-

Cr3+(aq)+3NaOH(aq) → Cr(OH)3(s)+3Na+(aq)

From the reaction we can predict that there will be three mole of hydroxide ion will be required for one mole precipitation of chromium.

Volume of chromium ion = 0.60 L

Molarity of chromium ion = 0.013 M

Moles of chromium ion = 0.0078 mol

So, the number of Sodium hydroxide required will be = 3 x 0.0078 =0.0234 moles

Molarity of sodium hydroxide = 1.26 M

Volume of Sodium hydroxide required will be :- 0.0234/ 1.26 = 0.0186 L = 18.6 ml

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