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sashaice [31]
3 years ago
12

Silver sulfate dissolves in water according to the reaction: Ag2SO4(s) ∆ 2 Ag+(aq) + SO42-(aq) Kc = 1.1 * 10-5 at 298 K A 1.5-L

solution contains 6.55 g of dissolved silver sulfate. If addi- tional solid silver sulfate is added to the solution, will it dissolve?
Chemistry
1 answer:
antiseptic1488 [7]3 years ago
6 0

Answer:

additional solute will not dissolve.

Explanation:

First we must obtain the number of moles of Ag+ and SO4^2- ions present.

Number of moles of the compound = mass/ molar mass

Molar mass of compound= (2×108) + 32 + 4(16)= 216 + 32 + 64= 312gmol-1

Number of moles of compound= 6.55g/312gmol-1= 0.021moles

Concentration of Ag+ = (2×0.021)/1.5 =0.028M

Concentration of SO4^2- = 0.021/1.5= 0.014M

Qsp = [Ag+]^2[SO42-]= (0.028)^2 ( 0.014)=1.1 x 10^-5 = Ksp

Since Qsp=Ksp, additional solute will not dissolve.

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Boiling point depends on different intermolecular force such as molecular wight, dipole-dipole attraction force, hydrogen bonding, ionic attraction force.

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