reactions in aqueous solutions ms. mack chapter 10, section 3 chemistry i- 3/24/09
TRANSCRIPT
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Reactions in Aqueous Solutions
Ms. Mack
Chapter 10, Section 3
Chemistry I- 3/24/09
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Introduction
• Many reactions involve substances dissolved in water.
• When this happens, solutions form– Solutions (homogeneous substances)
• Two parts:– SOLUTES- substances dissolved in water– SOLVENTS- the most plentiful substance in a solution
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Water, the universal solvent (H2O)
• Examples of Solutes:– Molecular compounds that exist as molecules– Molecular compounds that form ions when
they dissolve in water (H+ ions=acids)– Ionic compounds
• When dissolved in water, the ions can separate
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The Products
• When 2 aqueous solutions that contain ions are combined, the ions may react with one another in a DOUBLE-REPLACEMENT reaction producing:A.A. Precipitate (s)Precipitate (s)
B. B. Water (l)Water (l)
C. C. Gas (g)Gas (g)
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A. Precipitate
• Use ionic equations to show the details of reactions that involve ions in aqueous solutions
• Substances are written as ions
• Complete ionic equations- show all particles involved in a chemical reaction
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NaCl (aq) + AgNO3 (aq) NaNO3 (aq) + AgCl (s)AgCl (s)
Complete:
Na+(aq) + Cl- (aq) + Ag+ (aq) + NO3-(aq)
Na+ (aq) + NO3- (aq) + AgCl (s)
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Spectator Ions
• Notice, that there are ions that appear on both sides of the equation
• These ions do not participate in the formation of the solid product
• These ions are called spectator ions. – What were the spectator ions in the previous
slide?
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Net Ionic Equations
• Equations that show only the ions involved- omitting the spectator ions are called complete ionic equations!
From the previous example:
Cl- + Ag+ AgCl (s)
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Practice!
• Write the chemical, balanced, complete ionic and net ionic equation for the following:
Aqueous solutions of potassium iodide and silver nitrate are mixed, forming
the precipitate silver iodide.
See white board for solution!
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B. Water
• Some reactions form water
• No evidence of the chemical reaction can be observed. Why?
• Example:
HCl (aq) + KOH (aq) H2O (l) + KCl (aq)
H+ (aq) + OH- (aq) H2O (l)
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Practice!
Sulfuric acid (H2SO4) and aqueous potassium hydroxide
react to produce water and potassium sulfate.
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C. Gas
• Common gases produced: carbon dioxide, hydrogen cyanide, and hydrogen sulfide
Example:
Na2S (aq) + HCl (aq) NaCl (aq) + HH22S S (g)(g)
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Practice!
Sulfuric acid and aqueous rubidium sulfide with
production of hydrogen sulfide gas