When solutions of silver nitrate and potassium chloride are mixed, silver chlori

Question

When solutions of silver nitrate and potassium chloride are mixed, silver chloride precipitates out of a solution according to the equation AgNo3(aq)+KCl(aq)-->AgCl(s)+KNO3(aq).

Part A: What mass of silver chloride can be produced from 1.83 L of a 0.213 M solution of silver nitrate? Express your answer with the appropriate units.

The reaction described in Part A required 3.55 L of potassium chloride. What is the concentration of this potassium chloride solution?

Express your answer with the appropriate units.

Explanation / Answer

The balanced chemical reaction is

AgNo3(aq)+KCl(aq) -------> AgCl(s)+KNO3(aq)

1 mol, --------1 mol, ----------- 1 mol, --- 1 mol

From the above balanced reaction it is clear that equal moles of both the reactants react each other to produce equal moles of each product.

Part-A:

moles of silver nitrate(AgNO3) taken = MxV = 0.213 mol/L x 1.83 L = 0.390 mol

Hence moles of silver chloride(AgCl) produced = moles of AgNO3 taken = 0.390 mol

=> mass of AgCl produced = mol x molar mass of AgCl = 0.390 mol x 143.32 g/mol = 55.9 g (answer)

Let the concentration of KCl be 'M' mol/L

Hence moles of KCl required = MxV = M mol/L x 3.55 L = 3.55M mol

Also moles of KCl taken = moles of AgNO3 taken

=> 3.55M mol = 0.390 mol

=> M = 0.390 / 3.55 = 0.110 mol/L or 0.110 M (answer)

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