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ksp question

So basically part 3 I've been stuck on for ages and I don't know where to start etc.

I would very much appreciate some help in this image-707ec5b6-c248-4d4d-935e-bb787e411eb61489710867-compressed.jpg.jpeg
Work out the solubility product in the saturated solution, using the fact that ksp = [Na+][A-]

Use the value of the negative ion 1x10-2 and substitute into the equation above to find the concentration of the sodium ions required to exceed the value of ksp (and cause precipitation).

Then calculate the mass of that number of moles of NaCl

Don't forget that you are using only 500ml so halve that value.
(edited 6 years ago)

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