What is the solubility of AgBr in g/L in 0.0010 M AgNO3 solution? The Ksp for AgBr is 7.7 x 10−13. A. 1.5 x 10−7 g/L B. 7.7 x 10−11 g/L C. 3.6 x 10−7 g/L D. 2.2 x 10−5 g/L E. 4.2 x 10−10 g/L

Question

What is the solubility of AgBr in g/L in 0.0010 M AgNO3 solution?   	The Ksp  for AgBr is 7.7 x 10−13.  	A.	1.5 x 10−7    g/L  	B.	7.7 x 10−11   g/L	 	C.	3.6 x 10−7    g/L 	D.	2.2 x 10−5    g/L 	E.	4.2 x 10−10   g/L

jfraser · Answer

KSP lets us find the maximum solubility of a solute in terms of Mol/L, so we can convert from mol/L into g/L by using the molar mass.

Use the KSP equation$$K_{SP} = [Ag{^+}][Br{^-}] = 7.7*10^{-13}$$ to solve for the concentration of Ag+ ions in solution. Since the ratio of ions in AgBr is 1:1, whatever the concentration of silver ions, the bromide will be the same.$$7.7*10^{-13} = [x][x] = x^2$$ That concentration is in mol/L, so use the molar mass of AgBr to turn those moles of AgBr into grams of AgBr.