To solve stoichiometry problems, you must always calculate numbers of moles. Rec

Question

To solve stoichiometry problems, you must always calculate numbers of moles. Recall that molarity, M, is equal to the concentration in moles per liter:M=mol/L.

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

2AgNO3(aq)+CaCl2(aq)?2AgCl(s)+Ca(NO3)2(aq

1, What mass of silver chloride can be produced from 1.74L of a 0.262M solution of silver nitrate?

2.The reaction described in Part A required 3.02L of calcium chloride. What is the concentration of this calcium chloride solution?

Explanation / Answer

Part A:
1.74 L X 0.262 mol/L = 0.45588 moles AgNO3
0.45588 moles AgNO3 X (2 mol AgCl / 2 mol AgNO3) = 0.45588 mol AgCl
The molar mass of AgCl is 143.3 g/mol. So
0.45588 mol AgCl X 143.3 g / 1 mol = 65.327 grams AgCl

Part B
Since you began with 0.45588 moles of AgNO3, we'll start with that:
0.45588 mol AgNO3 X (1 mol CaCl2 / 2 mol AgNO3) = 0.227 mol CaCl2

Molarity of CaCl2 solution = 0.227 mol / 3.02 L = 0.0751 M CaCl2

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