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anonymous
 5 years ago
Calculate the solubility of silver chloride in 0.17M AgNO3. (Ksp=1.8E10)
anonymous
 5 years ago
Calculate the solubility of silver chloride in 0.17M AgNO3. (Ksp=1.8E10)

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anonymous
 5 years ago
Best ResponseYou've already chosen the best response.0AgNO3 dissociates into Ag+ and NO3, therefore our Ksp will be: Ksp = [Ag+][NO3] because AgNO3 is a solid and solids & liquids are never counted in equilibrium problems because their concentrations are always constant. X moles of the silver chloride will dissociate which means X moles of both Ag+ and NO3 will be in the solution. To do this, I always set up a chart. AgNO3(s) > Ag+ NO3 .17 0 0 Initial concentration x +x +x Change in concentration .17x x x Equilibrium concentration Now let's take the equilibrium values and then plug them into our Ksp. Ksp = 1x108 Ksp = [Ag+][NO3] 1x108 = [Ag+][NO3] *Now recall our equilibrium values. 1x108 = (x)(x) 1x108 =x^2 x = The square root of 1x108 which is 1x104
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