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:

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?

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Solution Stoichiometry concept. You can view video lessons to learn Solution Stoichiometry Or if you need more Solution Stoichiometry practice, you can also practice Solution Stoichiometry practice problems .

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Our tutors rated the difficulty of When solutions of silver nitrate and magnesium chloride are ... as medium difficulty.

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