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Solution Stoichiometry Problems Questions

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User Generated
Subject
Chemistry
Type
Worksheet
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1). When 30.0 mL of 0.500 M AgNO
3
is added to 25.0 mL of 0.300 M NH
4
Cl, how many
grams of AgCl are formed?
B). When 30.0 mL of 0.500 M AgNO
3
is added to 25.0 mL of 0.300 M NH
4
Cl, What would be
the concentrations of the NH
4
+
, Ag
+
, NO
3
-
, Cl
-
ions in the final solution?
2). If 150. mL of 0.100 M Na
2
SO
4
is added to 200. mL of 0.100 M BaCl
2
, what is the
concentration of Na
+
and SO
4
2-
ions in the final solution? Assume that the volumes are additive.
Key:
1). When 30.0 mL of 0.500 M AgNO
3
is added to 25.0 mL of 0.300 M NH
4
Cl, how many

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grams of AgCl are formed?
A).
Answer: 1.07 g
B). When 30.0 mL of 0.500 M AgNO
3
is added to 25.0 mL of 0.300 M NH
4
Cl, What would be
the concentrations of the NH
4
+
, Ag
+
, NO
3
-
, Cl
-
ions in the final solution?
ME: AgNO
3
(aq) + NH
4
Cl(aq) → AgCl(s) + NH
4
NO
3
(aq)
NIE: (tells us the change)
Ag
+
(aq) + Cl
-
(aq) AgCl(s)
Initial Solution
0.0150 moles Ag
+
0.0300 L x 0.500M AgNO
3
= 0.0150 moles AgNO
3
0.0150 moles NO
3
-
0.00750 moles NH
4
+
0.0250L x 0.300 M NH
4
Cl = 0.00750 moles NH
4
Cl
0.00750 moles Cl
-
Final solution, after the reaction
Ag
+
(aq) + Cl
-
(aq) AgCl(s)
0.0150moles 0.00750moles
Since the reaction is one to one it’s clear that the Cl
-
is limited and will run out.
So we will be left with 0.00 moles of Cl
-
, 0.0150moles 0.0075moles = 0.00750 moles of Ag
+
, 0.00750 moles NH
4
+
(spectator ion) and 0.0150 moles NO
3
-
(spectator ion).
Final Molarity of each ion would be:
0.00 M for Cl
-
, 0.00750moles Ag
+
/ 0.0550L = 0.136 M Ag
+
0.00750moles NH
4
+
/ 0.0550L = 0.136 M NH
4
+
, 0.0150moles NO
3
-
/ 0.0550L = 0.273 M NO
3
-
2). If 100. mL of 0.150 M Na
2
SO
4
is added to 200. mL of 0.100 M BaCl
2
, what is the
concentration of Na
+
and SO
4
2-
ions in the final solution? Assume that the volumes are additive.

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1). When 30.0 mL of 0.500 M AgNO3 is added to 25.0 mL of 0.300 M NH4Cl, how many grams of AgCl are formed? B). When 30.0 mL of 0.500 M AgNO3 is added to 25.0 mL of 0.300 M NH4Cl, What would be the concentrations of the NH4+ , Ag+, NO3-, Cl- ions in the final solution? 2). If 150. mL of 0.100 M Na2SO4 is added to 200. mL of 0.100 M BaCl2 , what is the concentration of Na+ and SO42- ions in the final solution? Assume that the volumes are additive. Key: 1). When 30.0 mL of 0.500 M AgNO3 is added to 25.0 mL of 0.300 M NH4Cl, how many grams of AgCl are formed? A). Answer: 1.07 g B). When 30.0 mL of 0.500 M AgNO3 is added to 25.0 mL of 0.300 M NH4Cl, What would be the concentrations of the NH4+ , Ag+, NO3-, Cl- ions in the final solution? ME: AgNO3(aq) + NH4Cl(aq) → AgCl(s) + NH4NO3(aq) NIE: (tells us the change) Ag+(aq) + Cl- (aq) → AgCl(s) Initial Solution 0.0150 moles Ag+ 0.03 ...
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