# Chemistry

posted by .

Use the data in this table to calculate the solubility of each sparingly soluble substance in its respective solution.
(a) silver bromide in 0.066 M NaBr(aq)
mol · L-1
I know how to do this one, found it to be 1.167E-11 which is correct.

(b) nickel(II) hydroxide in 0.256 M NiSO4(aq); For the purpose of this calculation, ignore the autoprotolysis of water.
mol · L-1
Ksp for Ni(OH)2 is 6.5E-18

Here's what I started doing:
NiSO4 -->NI^+ + SO4^-
Ksp = [Ni+][SO4-]

Ni(OH)2--> Ni^2+ + 2OH^-
Ksp = [Ni^2+][OH-]^2

so... [OH-]^2 = Ksp of [Ni^2+][OH-}^2 over [Ni+] from the NiSO4

but I'm not sure what to do because the first compound has Ni+ and the second has Ni 2+ ..

• Chemistry -

I think your only problem is that you think Ni in NiSO4 is +1 but you know SO4 is -2; therefore, Ni must be +2 so Ni in Ni(OH)2 and Ni in NiSO4 are the same animal.
(Ni^+2)(OH^-)^2 = Ksp

I also think you can avoid a lot of confusion if you set up a chart; at least until you get the hang of these problems. This is a common ion problem (the Ni^+2 is the common ion) and all of them are done alike.
Ni(OH)2 ==> Ni^+ + 2OH^-

Let solubility of Ni(OH)2 be S and that is what the problem ask for. At equilibrium,
(Ni^+2) = S from Ni(OH)2 and 0.256 M from NiSO4 to make a total of S+0.256.
(OH^-) = 2S

Then we substitute into Ksp expression as follows:
Ksp = (S+0.256)(2S)^2
Solve for S using the quadratic OR make a simplifying assumption that S+0.256 = 0.256 and solve for S. Making the assumption is the easy way, then check the final answer to see if that assumption is valid.

## Similar Questions

1. ### Chemistry

A conductivity cell was calibrated using KCl solution (0.01 mol dm^-3) with a conductivity of 0.141 S m^-1 and the resistance was found to be 520 Ohms. The resistance of a saturated solution of silver chloride was found to be 3.8 x …
2. ### Chemistry

Question: the conversion of one precipitate to another by the addition of a suitable reagent is a process that involves heterogeneous equilibrium system. for example, silver chloride can be coverted to silver bromide by the additino …
3. ### science

Silver bromide a pale yellow precipitate is more soluble than silver iodide. What would happen if NaBr had been added to the solution
4. ### Chemistry

Use the data in this table to calculate the solubility of each sparingly soluble substance in its respective solution. (a) silver bromide in 0.066 M NaBr(aq) mol · L-1 I know how to do this one, found it to be 1.167E-11 which is correct. …
5. ### chemistry

Silver chromate is sparingly soluble in aqueous solutions. The Ksp of Ag2CrO4 is 1.12× 10–12. What is the solubility (in mol/L) of silver chromate in 1.00 M potassium chromate aqueous solution?
6. ### Chemisty

Photographic film contains silver bromide in gelatin. Once exposed, some of the silver bromide decomposes, producing fine grains of silver. The unexposed silver bromide is removed by treating the film with sodium thiosulfate. Soluble …
7. ### chemistry

silver sulphate is a sparingly soluble salt.2.5litres of saturated solution of this salt contains 14.25g. Calculate the molar solubility of silver sulphate
8. ### chemistry

Silver sulphate is a sparingly soluble salt.2.5litres of saturated solution of this salt contains 14.25g. Calculate the molar solubility of silver sulphate.
9. ### Chemistry

Silver chromate is sparingly soluble in aqueous solutions. The Ksp of Ag2CrO4 is 1.12× 10–12. What is the solubility (in mol/L) of silver chromate in 1.4 M potassium chromate aqueous solution?
10. ### chemistry

In quality control of raw materials for pharmaceutical production often used foul reactions to prove that raw materials in salt form containing the appropriate salt. Hydrochloride (eg. Amitriptyline hydrochloride) can be detected for …

More Similar Questions

Post a New Question