Chapter 4
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Transcript of Chapter 4
Chapter 4
Aqueous Reactions and Solution Stoichiometry
Properties of Aqueous Solutions
• Solutions are homogeneous mixtures of 2 or more substances
Properties of Aqueous Solutions
• Aqueous Solutions are solutions in which water is the dissolving medium
Properties of Aqueous Solutions
• A solvent is the substance that is present in larger quantities.
Properties of Aqueous Solutions
• A solute is the substance being dissolved into the solvent.
Properties of Aqueous Solutions
• Electrolytes conduct electricity.
Properties of Aqueous Solutions
• Aqueous solutions made of ionic compounds are electrolytes due to the presence of ions.
Properties of Aqueous Solutions
An aqueous solution of a molecular compound is called a nonelectrolyte
Properties of Aqueous Solutions
Strong electrolytes exist in solution completely as ions (soluble ionic compounds)
Properties of Aqueous Solutions
Weak electrolytes exist mostly as molecules
Properties of Aqueous Solutions
Nonelectrolytes exist only as molecules
Properties of Aqueous Solutions
Precipitation Reactions
• Precipitation reactions are those that result in the formation of an insoluble product
Precipitation Reactions
Precipitation Reactions
• Precipitation reactions occur when certain pairs of oppositely charged ions attract to each other so strongly that they form an insoluble ionic solid
Precipitation Reactions
• Solubility of a substance is the amount of that substance that can be dissolved in a given quantity of solvent
Precipitation Reactions
• Any substance with a solubility less than 0.01mol/L will be referred to as insoluble
Precipitation Reactions
• The solubility guidelines for common ionic compounds in water is organized by anions
Precipitation Reactions
Practice 4.2 Soluble or Insoluble?
• Sodium carbonate
Lead (II) sulfate
Barium nitrate
Cobalt(II) hydroxide
Ammonium phosphate
Precipitation Reactions
• To predict whether a precipitate will form when we mix aqueous solutions of electrolytes …
Precipitation Reactions
• (1)note the ions present in the reactants
• (2) consider combinations of anions and cations
• (3) use the table to predict if any of the combinations are insoluble
Precipitation Reactions
• Will a precipitate form when Mg(NO3)2 and NaOH are mixed?
Precipitation Reactions
• This is called a double replacement reaction.
• AX + BY AY + BX
Practice 4.3
• (a) Write the balanced rxn and identify the ppt that forms when the following solutions are mixed:
• (a) BaCl2 and K2SO4
• (b) Ba(NO3)2 and KOH
• (c) Fe2(SO4)3 and LiOH
Precipitation Reactions
• A molecular equation shows the complete chemical formulas of the reactants and the products
Precipitation Reactions
• A complete ionic equation shows all strong electrolytes as ions rather than as compounds
Precipitation Reactions
• Spectator ions are ions that appear as identical forms on both sides of the equation; they are present but don’t play a direct role in the reaction
Precipitation Reactions
• Net ionic equations do not show spectator ions
Writing Net Ionic Equations
• Write a balanced mol. E.q
• Rewrite to show ions that form in solution
• Cancel spectator ions
Practice 4.4
• Write the net ionic equation for the following rxns.
(1) aqueous solutions of calcium chloride and sodium carbonate are mixed.
(2) aqueous solutions of silver nitrate and potassium phosphate are mixed.
Acid-Base Reactions
• Acids produce H+ when dissolved in water
• Acids are proton donors
Acid-Base Reactions
• Bases accept H+ions
• Bases produce OH- when
they dissolve in water
Acid-Base Reactions
• Strong acids and bases are strong electrolytes – ionize completely
Acid-Base Reactions
• Weak acids and bases are weak electrolytes – partially ionize ( do not write in ionized form)
Acid-Base Reactions
• List Strong Acids and Bases
Practice Exercise 4.5
The following diagrams represent aqueous solutions of three acids (HX, HY, and HZ) with water molecules omitted for clarity. Rank them from strongest to weakest.
Identifying Strong, Weak, and Non Electrolytes Chart
Strong Weak Non
IonicSoluble N/A Insoluble
Molecular Strong AcidsWeak Acids
Weak Bases (NH3)
All other compounds
Classifying SE, WE, or NE • 1. Is it ionic or molecular? • 2. If ionic – is it soluble? • 3. If molecular – is it an acid?• 4. If an acid – strong or weak?• 5. Is it weak base NH3?• 6. Everything else is a non
electrolyte
Practice 4.6
SE, WE, NE?CaCl2
HNO3
C2H5OH HCOOHKOHNH3
Practice 4.6
Rank the following solutions in order of least to most electrical conductivity.
Ca(NO3)2
C6H12O6 CH3COONa or NaC2H3O2
CH3COOH or HC2H3O2
Acid-Base Reactions
• A neutralization reaction occurs when an acid and base are mixed producing water and salt
• Salt means any ionic compound whose cation comes from the base and anion from the acid
Acid-Base Reactions
• Example:
• Aq. solutions of hydrobromic acid and sodium hydroxide mix
Acid-Base Reactions
Aq. hydrochloric acid reacts with solid magnesium hydroxide.
Acid-Base Reactions
• Reactions with the S2- ion or CO3
2- ion with acids will form gases with low solubility in water
Acid-Base Reactions
Aq. HCl
reacts with
Baking soda
Acid-Base Reactions
Aq. Hydrochloric acid reacts with Aq. sodium sulfide
Practice 4.7
Write a balanced molecular equation and net ionic equation for the following rxns:(a) aqueous solutions of acetic acid and barium hydroxide(b) aq solns of carbonic acid and potassium hydroxide
Oxidation Numbers
Oxidation numbers of an atom in a substance are a hypothetical charge based on a set of rules.
1. For an atom in its elemental form the oxidation number is always zero
2. For any monatomic ion the oxidation number equals the charge on the ion
Oxidation Numbers
• 3. Nonmetals usually have negative oxidation numbers.
a. O is –2 except in peroxides where O22-
giving each O –1.
b. H is +1 with nonmetals and –1 with
metals .
c. F is –1 in all compounds. Other halogens have –1
except when combined with oxygen they have
positive oxidation states.
•
Oxidation Numbers
• 4. The sum of oxidation numbers of all atoms in a neutral compound is 0.
• The sum of oxidation numbers in a polyatomic ion is equal to the charge of the ion.
Practice 4.8
• Deterimine the ox#’s in the following substances • (a) H2S (b) S8
• (c) SCl2 (d) Na2SO3
• (e) SO42– (f) P2O5
• (g) NaH (h) Cr2O72–
• (i) SnBr4 (j) BaO2
Oxidation-Reduction Reactions
• Reactions where electrons are transferred between reactants
Oxidation-Reduction Reactions
• Oxidized – when an atom, ion, or molecule becomes more positively charged (lost e-)
• Reducing Agent = the substance that is oxidized
Oxidation-Reduction Reactions
• Reduced – when an atom, ion, or molecule has become more negative (gain e-)
• Oxidizing agent = the substance that is reduced
What does Leo the Lion say?
Oxidation-Reduction Reactions
• Determine oxidation numbers, then identify the oxidizing agent and reducing agent in the rxn below.
Oxidation-Reduction Reactions
• A single replacement rxn is when an ion in solution is replaced through oxidation of an element
Oxidation-Reduction Reactions
Oxidation-Reduction Reactions
Practice 4.9
• Write the molecular and net eq for the following:
(a)Aluminum and hydrobromic acid(b)Magnesium and cobalt(II)sulfate
Oxidation-Reduction Reactions
• Activity series is a list of metals arranged in order of decreasing ease of oxidation
• Any metal on the list can be oxidized by the ions of elements below it.
Practice 4.10
1. Will an aq. soln of iron(II) chloride oxidize magnesium metal? If so, write the balanced molecular and net ionic equations for the reaction.
2. Which of the following metals will be oxidized by Pb(NO3)2: Zn, Cu, Fe?
Concentration of Solutions
Concentration of Solutions
• Molarity (M)
= moles of solute / L soln
Practice 4.11
• Calculate the molarity of a solution made by dissolving 23.4 g of sodium sulfate (Na2SO4) in enough water to form 125 mL of solution
Making a Solution:How do you make a 250.0mL soln of 0.1M CuSO4?
Concentration of Solutions
• Electrolytes and Concentration: When an ionic compound dissolves, the
relative concentration of ion depends on the chemical formula
Practice 4.12
• What are the molar concentrations of each of the ions present in a 0.025 M aqueous solution of calcium nitrate?
Concentration of Solutions
• A dilution can be made to concentrated stock solutions by adding water to the solutions, and therefore making them less
concentrated.
M1V1 = M2V2
Practice 4.14
How many milliliters of 3.0 M H2SO4 are needed to make 450 mL of 0.10 M H2SO4?
Solution Stoichiometry
• Use mole conversions (molarity, molar mass, etc.) and mole ratios to solve stoichiometry problems through DA
Solution Stoichiometry
Practice 4.15
• How many grams of Ca(OH)2 are needed to neutralize 25.0 mL of 0.100 M HNO3?
Practice 4.16
• 45.7 mL of 0.500M H2SO4 is required to neutralize 20.0mL of NAOH soln. What is the concentration of NaOH?
Practice 4.17
• How many grams of chloride ion are in a sample of water if 20.2mL of 0.100M Ag+
is needed to react with all the chloride in the sample. If the sample has a mass of 10.0g what percentage of chloride does it contain?
Putting it all together
A sample of 70.5 mg of potassium phosphate is added to 15.0 mL of 0.050 M silver nitrate.
(a) Write the molecular equation for the reaction.
(b) What is the limiting reactant in the reaction?
(c) Calculate the theoretical yield, in grams, of the precipitate that forms.
Putting it all together
A solution of 100.0mL of 0.200M KOH is mixed with a solution of 200.0mL of 0.150M NiSO4.
(a) Write the molecular equation for the reaction. (b) What is the limiting reactant in the reaction? (c) Calculate the theoretical yield, in grams, of the
precipitate that forms.(d) What is the molarity of each ion that remains in
the solution.