Problem: When solutions of silver nitrate and potassium chloride are mixed, silver chloride precipitates out of solution according to the equationAgNO3(aq) + KCl(aq) → AgCl(s) + KNO3(aq)Part A: What mass of silver chloride can be produced from 1.97 L of a 0.232 M solution of silver nitrate? Express your answer with the appropriate units.Part B: The reaction described in Part A required 3.65 L of potassium chloride. What is the concentration of this potassium chloride solution? Express your answer with the appropriate units.

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When solutions of silver nitrate and potassium chloride are mixed, silver chloride precipitates out of solution according to the equation

AgNO3(aq) + KCl(aq) → AgCl(s) + KNO3(aq)

Part A: What mass of silver chloride can be produced from 1.97 L of a 0.232 M solution of silver nitrate? Express your answer with the appropriate units.






Part B: The reaction described in Part A required 3.65 L of potassium chloride. What is the concentration of this potassium chloride solution? Express your answer with the appropriate units.

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