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Consider a 1 liter solution in which silver (Ag+) has a concentration of 10^-2.94 moles/L. Then...

Consider a 1 liter solution in which silver (Ag+) has a concentration of 10^-2.94 moles/L. Then if 0.53g of NaCl is added to the solution and it comes to equillibrium, show that AgCl will precipitate. Determine the weight in grams of AgCl that will precipitate from the 1L solution. The solution is ideal. The Ksp of AgCl is 10^-9.75. Assume the NaCl completely dissolves.

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Answer #1

The molar mass of NaCl is 58.4 g/mol.

The Ksp of AgCl is

Hence, precipitation of AgCl will occur.

After precipitation,

Before precipitation

During precipitation, the change in

Since total volume is 1 L, the molar concentration is equal to the number of moles.

Change in number of moles of silver ions during precipitation is 0.001148 moles. It is equal to the number of moles of AgCl formed. The molar mass of AgCl 143.3 g/mol. The mass of AgCl precipitated

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