A 0.50 gram precipitate of AgCl is washed with 237 mL of 0.10 M HCl. Calculate t

Question

A 0.50 gram precipitate of AgCl is washed with 237 mL of 0.10 M HCl. Calculate the number of grams of AgCl that dissolves. Ksp = 1.8 Times 10^-10 A solution contains 0.050 mol of KI and 0.15 mole KCl per liter. AgNO_3 is gradually added to this solution. Which will precipitated first, AgI and AgCl? A solution of 0.075 M MnBr_2 is saturated with H_2 S what is the minimum pH which MnS (Ksp = 5.1 Times 10^-15) will precipitate? If the molar solubility of LaCl_2 is 0.0120 M, how many grams will dissolve in 1184 mL of water? What mass of AgBr will dissolve in 1.00 Liter of water?

Explanation / Answer

6. Ksp for AgCl = [Ag+][Cl-]

with,

[Cl-] = 0.1 M x 0.237 = 23.7 mmol

[AgCl] = 0.5 g/143.32 g/mol = 3.5 mmol

As HCl added is excess, nearly al of 0.5 g AgCl would dissolve.

7. When AgNO3 is added to a solution of KI and KCl,

Ksp of AgI is lower than Ksp of AgCl. and hence AgI would precipitate out first from solution.

8. Molar solubility of LaCl2 = 0.012 M

Mass of LaCl2 that would dissolve = 0.012 M x 1.184 L x 209.81 g/mol = 2.98 g

9. Ksp of AgBr = 5 x 10^-13

solubility of AgBr in water = x = sq.rt.(5 x 10^-13) = 7.07 x 10^-7 M

mas of AgBr to be dissolved = 7.07 x 10^-7 M x 1 L x 187.77 g/mol = 1.33 x 10^-4 g

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