Question

**When solutions of silver nitrate and magnesium chloride
are mixed, silver chloride precipitates out of solution according
to the equation
2AgNO _{3}(aq)+MgCl2(aq)→2AgCl(s)+Mg(NO_{3})_{2}(aq).**

What mass of silver chloride can be produced from 1.96 L of a
0.233 *M*solution of silver nitrate? Express your answer
with the appropriate units. **Mass of AgCl=65.3**

The reaction described in Part A required 3.46 L of magnesium chloride. What is the concentration of this magnesium chloride solution? Express your answer with the appropriate units.

Answer #1

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

no of moles of AgNO3 = Molarity x volume = 0.233 x 1.96 = 0.45668 moles

from the balanced equation it is clear that 2 moles of AgNO3 will give 2 moles of AgCl

so from 0.45668 moles of AgNO3 will produce 0.45668 moles of AgCl

mass of silver chloride = moles x molar mass = 0.45668 x 143.32 = 65.4 grams

Part B

from the balanced equation

2 moles of AgNO3 required one mole of MgCl2

0.45668 moles of AgNO3 required 0.45668/2 moles of MgCl2 = 0.22834 moles of MgCl2

now we have moles and voleme we can find the concentration

Molarity M = 0.22834 / 3.46 = 0.066M

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).
What mass of silver chloride can be produced from 1.96 L of a
0.233 M solution of silver nitrate? Express your answer
with the appropriate units.
The reaction described in Part A required 3.46 L of magnesium
chloride. What is the concentration of this magnesium chloride
solution? Express your answer with the appropriate units.

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)
Part A: What mass of silver chloride can be produced from 1.31 L
of a 0.156 M solution of silver nitrate?
Express your answer with the appropriate units.
Part B:
The reaction described in Part A required 3.43 L of magnesium
chloride. What is the concentration of this magnesium chloride
solution?
Express your answer with the appropriate units.

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)
Part A
What mass of silver chloride can be produced from 1.28 L of a
0.267 M solution of silver nitrate?
Express your answer with the appropriate units.
Part B
The reaction described in Part A required 3.60 L of calcium
chloride. What is the concentration of this calcium chloride
solution?
Express your answer with the appropriate units

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)
Part A
What mass of silver chloride can be produced from 1.09 L of a
0.281 M solution of silver nitrate?
Express your answer with the appropriate units.
Part B
The reaction described in Part A required 3.16 L of calcium
chloride. What is the concentration of this calcium chloride
solution?
Express your answer with the appropriate units.

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 1.97 L of a
0.285 M solution of silver nitrate?
2.The reaction described in Part A required 3.62 L of calcium
chloride. What is the concentration of this calcium chloride
solution?

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) Part A What
mass of silver chloride can be produced from 1.94 L of a 0.126 M
solution of silver nitrate? Part B The reaction described in Part A
required 3.49 L of calcium chloride. What is the concentration of
this calcium chloride solution?

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).
A) What mass of silver chloride can be produced from 1.90 L of a
0.133 M solution of silver nitrate?
B) The reaction described in Part A required 3.67 L of potassium
chloride. What is the concentration of this potassium chloride
solution?
Please help!

Solution Stoichiometry:
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 1.46 L
of a 0.218 M solution of silver nitrate?
Part B. The reaction described in Part A required 3.17 L of
potassium chloride. What is the concentration of this potassium
chloride solution?

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)
Part A
What mass of silver chloride can be produced from 1.55 L of a
0.183 M solution of silver nitrate?
Express your answer with the appropriate units.
Hints
mass of AgCl =
SubmitMy...

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)
Part A
What mass of silver chloride can be produced from 1.64 L of a
0.124 M solution of silver nitrate?
Express your answer with the appropriate units.
mass of AgCl =
g
Part...

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