18. The chloride in a 0.12-g sample of 95% pure MgCl2 is to be precipitated...
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18. Write the reaction
MgCl2 + AgNO3 = 2AgCl + Mg(NO3)2
MgCl2 = 24 + 71 = 95 (g/mol)
AgNO3 = 108 + 14 + 48 = 170 (g/mol)
Number of mole of MgCl2 = 0.12*0.95/95 = 0.0012 (mol)
So the number of mole of AgNO3 required to react is also 0.0012 mol.
Volume of ...
The solution provides detailed analysis and explanations for the solubility problems.
Ksp and Solubility: Concentrations of Ions in Solution
What are the concentrations of each of the ions in a saturated solution of PbBr2, given the Ksp of PbBr2 is 2.1 x 10^-6?
I get stuck in solving this question when I get to the equation
4(x^3)=2.1 x 10^-6 and I don't know how to get to the answer
x = 8.07 x 10 ^-3 M which is supposedly the concentration of Pb 2+.
Really the problem is arithmetic here because I am required to do this problem by hand and can not use a calculator.View Full Posting Details