Question

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?

Answer #1

Q1.

calculate mol of Silver nitrate, AgNO3

mol = MV = 1.97*0.285 = 0.56145 mol of AgNO3

then..

ratio is 2:2 or 1:1 with reswpect to AgNO3 and AgCl

so

mol of AgCl = 0.56145mol

MW of AgCl = 143.32 g/mol

mass = mol*MW = 0.56145*143.32 = 80.467014 g

Q2.

V = 3.62 L of CaCl2 solution...

relate to mol of CaCl2

2:1 ratio of AgNO3:CaCl2

so

0.56145 mol of AgNO3 --> 1/2*0.56145 = 0.280725 mol of CaCl2

then

molarity was:

M = mol/V = **0.280725** /(3.62) = 0.0775483 M of
CaCl2

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 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 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).
What mass of silver chloride can be produced from 1.96 L of a
0.233 Msolution 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.

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 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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