The document is a series of slides from a chemistry textbook discussing reactions in aqueous solutions. It introduces the topics of net ionic equations, which show only the particles directly involved in chemical reactions, and predicting the formation of precipitates based on solubility rules. An example reaction is used to demonstrate a net ionic equation. The document provides guidance on identifying spectator ions and writing balanced net ionic equations. It poses sample problems asking students to predict whether precipitates will form from double displacement reactions based on solubility rules.

1. chemistry
Slide
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2. 11.3
Reactions in Aqueous Solution
Structures in limestone caverns
are formed when carbon dioxide
converts calcium hydrogen
carbonate into calcium carbonate.
The calcium carbonate
precipitates and forms dramatic
stalactites and stalagmites. You
will learn to predict the formation
of precipitates and write equations
to describe the reactions that
produce them.
© Copyright Pearson Prentice Hall
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3. 11.3
Reactions in Aqueous
Solution
>
Net Ionic Equations
Net Ionic Equations
What does a net ionic equation show?
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4. 11.3
Reactions in Aqueous
Solution
>
Net Ionic Equations
A complete ionic equation is an equation
that shows dissolved ionic compounds as
dissociated free ions.
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5. 11.3
Reactions in Aqueous
Solution
>
Net Ionic Equations
An ion that appears on both sides of an
equation and is not directly involved in the
reaction is called a spectator ion.
The net ionic equation is an equation for a
reaction in solution that shows only those
particles that are directly involved in the
chemical change.
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6. 11.3
Reactions in Aqueous
Solution
>
Net Ionic Equations
A net ionic equation shows only those
particles involved in the reaction and is
balanced with respect to both mass and
charge.
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7. 11.3
Reactions in Aqueous
Solution
>
Net Ionic Equations
Sodium ions and nitrate ions are not
changed during the chemical reaction of silver
nitrate and sodium chloride so the net ionic
equation is
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8. Slide
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9. Slide
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10. Slide
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11. Practice Problems for Conceptual Problem 11.9
Problem Solving 11.28 Solve
Problem 28 with the help of an
interactive guided tutorial.
Slide
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12. 11.3
Reactions in Aqueous
Solution
>
Predicting the Formation of a
Precipitate
Predicting the Formation of a Precipitate
How can you predict the formation of a
precipitate in a double-replacement
reaction?
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13. 11.3
Reactions in Aqueous
Solution
>
Predicting the Formation of a
Precipitate
You can predict the
formation of a precipitate by
using the general rules for
solubility of ionic
compounds.
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14. 11.3
Reactions in Aqueous
Solution
>
Predicting the Formation of a
Precipitate
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15. 11.3
Reactions in Aqueous
Solution
>
Predicting the Formation of a
Precipitate
Will a precipitate form when a sodium
carbonate solution is mixed with a barium
nitrate solution?
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16. 11.3
Reactions in Aqueous
Solution
>
Predicting the Formation of a
Precipitate
Sodium nitrate is soluble but barium
carbonate is insoluble. The net ionic equation
is
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17. 11.3 Section Quiz.
Assess students’ understanding
of the concepts in Section 11.3.
Continue to:
-or-
Launch:
Section Quiz
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18. 11.3 Section Quiz.
1. Identify the correct net ionic equation for the following
reaction and the spectator ion, if there is one.
FeO(s) + 2HClO4(aq) → H2O(l) + Fe(ClO4)2(aq)
a. FeO(s) + 2H+(aq) + 2ClO4-(aq) → H2O(l) + Fe2+(aq) +
2ClO4-(aq); no spectator ion
b. FeO(s) + 2H+(aq) + 2ClO4-(aq) → H2O(l) + Fe2+(aq) +
2ClO4-(aq); ClO4- is a spectator ion
c. FeO(s) + 2H+(aq) → H2O(l) + Fe2+(aq); ClO4d. FeO(s) + 2HClO4(aq) → H2O(l) + Fe(ClO4)2(aq); no Slide
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spectator ion
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19. 11.3 Section Quiz.
2. Which one of the following products of doublereplacement reactions would NOT form a
precipitate?
a. AgCl
b. PbSO4
c. Mg(OH)2
d. Mo(NO3)2
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20. 11.3 Section Quiz
3. Which reaction will NOT produce a precipitate
from aqueous solution?
a. Hg2(NO3)2 + KCl
b. FeSO4 + Ba(OH)2
c. Pb(NO3)2 + Na2CO3
d. NaBr + Al2(SO4)2
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21. Reactions in Aqueous
Solution
>
Concept Map 11
Concept Map 11 Solve the
Concept Map with the help of an
interactive tutorial.
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22. END OF SHOW