Question

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 1.41 L of a 0.104 M solution of silver nitrate?
Part B: The reaction described in Part A required 3.39 L of potassium chloride. What is the concentration of this potassium chloride solution?

Answer 1

The mass of silver chloride can be calculated using the volume and molarity of silver nitrate, while the concentration of potassium chloride can be calculated using the volume and moles of potassium chloride required.

Step-by-step explanation:

In the given reaction, AgNO3 (silver nitrate) reacts with KCl (potassium chloride) to form AgCl (silver chloride) and KNO3 (potassium nitrate).

Part A: To find the mass of silver chloride produced, we need to use the given volume and molarity of silver nitrate. Firstly, we convert the given volume from liters to milliliters (1.41 L = 1410 mL). Then, we can use the volume and molarity of silver nitrate to calculate the number of moles of silver nitrate. Finally, using the stoichiometry of the reaction, we can convert the moles of silver nitrate to moles of silver chloride and then to the mass of silver chloride.

Part B: To find the concentration of the potassium chloride solution, we can use the given volume of potassium chloride and the moles of potassium chloride required in the reaction. Firstly, we convert the given volume from liters to milliliters (3.39 L = 3390 mL). Then, we use the moles of potassium chloride required (which is equal to the moles of silver chloride produced) to calculate the concentration of potassium chloride.