What is the solubility of aluminum hydroxide in water at 25 degrees Celsius if the Ksp is 3 x 10^-34? What is the concentration of Hydroxide at equilibrium?

What is the concentration of a sulfide ion in a 1L solution of cuprous sulfide to which .03mol of cuprous nitrate has been added? The Ksp of cuprous sulfide is 8 x 10^-37

Please post all steps. Thanks!

Solution Preview

The solution is attached.

Thanks for the good questions.

First you need to write and balance the precipitate dissociation reaction.

Aluminum Hydroxide - my first question is, what is the compound formula?
If I do not know there are a number of routes to the answer. One is an internet search and the formula is Al(OH)3

So we have Al(OH)3-----------> Al(III) + 3OH(-)

Ksp = [Al(III)][OH]^3 where the brackets signify concentration

Now the Ksp on order of 10^(-34) means this barely dissociates in water at 25C.

If we start with 1 mole of aluminum hydroxide in 1 Liter water or 1M, we see ...

Solution Summary

This solution is provided in 480 words in an attached .doc file. It uses the balancing of the precipitate dissociation reaction as a step to solving the problem.

Hi:
We are given the following:
zinc sulfate (solubility given as 96.5 g/100 ml's)
zinc hydroxide ---- given Ksp = 2.1 x 10^-16
zinc sulfide ---- given Ksp = 1.1 x 10^-21
We are asked to calculate the Ksp for zinc sulfate and then asked to convert the Ksp's for zinc hydroxide and zinc sulfide into grams/100 ml uni

Please help with the following problems. Provide step by step calculations for each.
5.[a] The molar solubility of barium fluoride, BaF2, is 7.5 x 10-3 M. Calculate the solubility product
constant
[b]Calculate the molar solubility of lead fluoride, PbF2 in water, Ksp = 2.7 x 10-8
6.Calculate the molar solubility of bism

A saturated solution of silver chloride, AgCl contains 1.92 mg of AgCl per liter of solution. What is the value of the solubility product constant Ksp for silver chloride?
I know that soluability for AgCl at 25 degrees celcius ksp = 1.8 x 10 -10, however I am not sure if I would even need to incorporate this into the equatio

The Solubility Product Constant. PbBr2 is a slightly soluble salt. Write A) the chemical equilibrium equation that describes the salt partially dissolving in water and B) the solubility product expression. C) Calculate the Ksp value for lead(II) bromide if the molar solubility in pure water is 1.3 x 10-2 M.

Hi, I need some assistance with the following questions:
1. Calculate the molar solubility of AgCl in a 1.00L solution containing 10.0g of dissolved CaCl2.
2. Compare the molar solubility of Mg(OH)2 in water and in a solution buffered at a pH of 9.0.

The solubility product of silver chromate, Ag2CrO4, at 25 degrees Celsius is 4.05 x 10^-12 mol^3/L^3. Calculate the solubility of silver chromate in:
a) pure water
b) 0.0500 M silver nitrate solution
c) 0.0500 M potassium chromate solution

Please help with the following problem. Provide a step by step solution.
Solubility and the Common-Ion Effect. In problem 1 it was stated that the molar solubility of PbBr2 in pure water is 1.3 x 10-2 M. Calculate the molar solubility of PbBr2 in A) 0.20 M KBr and in B) 0.20 M Pb(NO3)2
Problem 1 in reference is: The Sol

Here is the question:
Calculate the solubility of Ni(OH)2 in a) distilled water and b) at pH of 4.0. Justify your answer.
I know I need to use a mass balance ans the reaction for disolution is
Ni(OH)2 <------> Ni2+ + 2OH-
The ksp for Ni(OH)2 is 6 x 10^-16

Q#1 (Common ion problem)
What is the solubility,in mg/mL of BaF2 in
a)Pure Water
b)in a solution containing 5.0mg/mL of KF
Ksp of BaF2=1.0*10^-6
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a)Calculate the solubility of a saturated solution og Mg(OH)2 on pure water.(My answer is 1.65096*10^-4M
b)Calculate the solubility of the sa