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13 Dec 2019

Solid Silver chloride has an extremely low solubility in water. Calculate the molar solubility of AgCl in a mixture of AgCl(s) and 0.03 M NaCl(aq). Ksp = 1.8

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Jarrod Robel
Jarrod RobelLv2
17 Dec 2019

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Related questions

calculate the molar solubilities of AgCl, Hg2Cl2, and PbCl2 in pure water. The equilibria are AgCl(s)=Ag(aq) + Cl(aq) Ksp=1.8*10^-10Hg2Cl2=Hg2(aq)+ 2Cl(aq) Ksp=1.2*10^-18PbCl2=Pb(aq) + 2Cl(aq) Ksp=1.7*10^-5

22) Given the following hydroxides and their solubility productconstants, which would be the most soluble in 1.0 L of water?

A) Magnesium hydroxide; Ksp=1.2x10-11

B) Iron(II) hydroxide;Ksp=1.6x10-14

C) Zinc hydroxide;Ksp=1.8x10-14

D) Copper (II) hydroxide; Ksp=2.2x10-20

E) Calcium Hydroxide; Ksp=8.0x10-6


23) Consider the equilibrium of AgCl(s) in water: AgCl(s) ??Ag+Cl- What is the effect of adding 6.5x10-3 M AgNO3?

a) The concentration will AgCl(s) will increase

b) The concentration will AgCl(s) will decrease

c) AgNO3 will precipitate

d) Silver dichloride precipitates

e) The AgNO3 has no effect on the solubility of AgCl


29) The Ksp of Mg(OH)2 is 3.6x10-4. At what pH will 0.2 M Mg+2solution begin to show precipitation? 1.4, 2.8, 10.7, 11.2,12.6


27) The solubility product for calcium phosphate is Ksp=1.36 x10-26. What is the molar solubility of calcium phosphate?1.3X10-26M, 1.5x10-7M, 2.6x10-6M, 4.6x10-6M,6.6x10-6M Show work, explain or no points

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