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If I Had 50.00mL of Saturated Silver Sulfate Solution, When Evaporated Leaving 0.25g of Silver Sulfate What Is?

Posted by junkgurl in Junk Silver Coin FAQ, tags: 0.25g, 50.00mL, evaporated, leaving, saturated, silver, solution, sulfate

Question by scienceguy: If I had 50.00mL of saturated silver sulfate solution, when evaporated leaving 0.25g of silver sulfate what is?
If I had 50.00mL of saturated silver sulfate solution, when evaporated leaving 0.25g of silver sulfate what is the

a) Amount of silver sulfate in the 50ml sample: .25g? b) molar solubility of silver sulfate
c)molar concentration of silver ion in saturated solution
d) molar concentration of sulfate ion in saturated solution
e) what is ksp expression of silver sulfate and how do i calculate it

Thanks for all the help guys

Best answer:

Answer by Trevor H
a) correct - 0.25g This does not agree with my solubility table for solubiity of Ag2SO4 My list says a saturated solution will contain 0.6g Ag2SO4 per 50ml saturated solution. I will use your figures.
Molar mass Ag2SO4 =311.799 g/mol
b) You have 0.25g in 50ml. How much in 1000ml? 1000/50*0.25 =5g
This is 5.0/311.799 = 0.0160mol per litre. Which is the molar solubility.
c) Ag2 = 107.87*2 = 215.74.
Molar conc. of Ag ions = 215.74/311.799*0.0160 = 0.011mol/litre
d)Molar conc. of SO4 ions = 92.066/311.799*0.016 = 0.00493 mol/litre
e) Ag2SO4 (s) → 2 Ag+ (aq) + SO4 2¯ (aq)
Ksp = [Ag+]² * [SO4 2¯ ]
Ksp = (0.011)² * (0.00493)
Ksp = 5.965 * 10^-7

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Originally posted 2010-08-30 13:43:14. Republished by Blog Post Promoter

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