# Problem: A solution containing AgNO3 is mixed with a solution of NaCl to form a solution that is 0.10 M in AgNO3 and 0.075 M in NaCl. What will happen once these solutions are mixed? Ksp (AgCl) = 1.77 × 10 -10. A) Nothing will happen since the molar solubility of AgCl is higher than the solution concentrations. B). Nothing will happen since NaCl and AgNO3 are both soluble compounds. C) Silver chloride will precipitate out of solution, leaving an unsaturated solution of AgCl D) Silver chloride will precipitate out of solution, leaving a saturated AgCl solution. E) There is not enough information to say anything about this solution.

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###### Problem Details

A solution containing AgNO3 is mixed with a solution of NaCl to form a solution that is 0.10 M in AgNO3 and 0.075 M in NaCl. What will happen once these solutions are mixed?

Ksp (AgCl) = 1.77 × 10 -10.

A) Nothing will happen since the molar solubility of AgCl is higher than the solution concentrations.

B). Nothing will happen since NaCl and AgNO3 are both soluble compounds.

C) Silver chloride will precipitate out of solution, leaving an unsaturated solution of AgCl

D) Silver chloride will precipitate out of solution, leaving a saturated AgCl solution.

E) There is not enough information to say anything about this solution.

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Selective Precipitation concept. If you need more Selective Precipitation practice, you can also practice Selective Precipitation practice problems.

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Our tutors rated the difficulty ofA solution containing AgNO3 is mixed with a solution of NaCl...as medium difficulty.

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Based on our data, we think this problem is relevant for Professor Ruggles' class at VERMONT.