Problem: When solutions of silver nitrate and magnesium chloride are mixed, silver chloride precipitates out of solution according to the equation.     2AgNO3(aq)+MgCl2(aq) → 2AgCl(s) + Mg(NO3)2(aq)a) What mass of silver chloride can be produced from 1.49L of a 0.254M solution of silver nitrate?b) The reaction described in Part A required 4.00L of magnesium chloride. What is the concentration of this magnesium chloride solution?

FREE Expert Solution
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FREE Expert Solution

For Part a) We’re being asked to calculate the mass of silver chloride (AgCl) that can be produced from 1.49L of a 0.254M solution of silver nitrate.


Recall that molarity is the ratio of the moles of solute and the volume of solution (in liters)

In other words:

Molarity (M)=moles of soluteLiters of solution


We need to perform a mole-to-mole comparison between each reactant and BaSO4

81% (193 ratings)
Problem Details

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

2AgNO3(aq)+MgCl2(aq) → 2AgCl(s) + Mg(NO3)2(aq)

a) What mass of silver chloride can be produced from 1.49L of a 0.254M solution of silver nitrate?

b) The reaction described in Part A required 4.00L of magnesium chloride. What is the concentration of this magnesium chloride solution?

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Based on our data, we think this problem is relevant for Professor Eroy-Reveles' class at UCSC.