Question

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?

Answer #1

moles of AgNO3 ( Silven nitrate) in 1.46L of 0.218M= 1.46*0.218=0.318 moles ( Molairty= moles/ volume of solution in L and moles = molarity* volume of solution in L)

From the reaction, AgNO3+ KCl---> AgCl+ KNO3

one mole of AgNO3 gives 1 mole of AgCl

0.318 moles of AgNO3 gives 0.318 moles of AgCl

Mass of AgCl= moles* Molecular weight of AgCl =0.318*143= 45.474 gms

B) 1 mole of AgNO3 requires 1 mole of KCl

0.318 moles require 0.318 moles of KCl

but its volume is 3.17L Molarity= moles/Liter of solution = 0.318/31.7 M=0.100M

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!

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 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)
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 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.

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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