Transcript Ch5lsn11Chem105

CHAPTER 5
Reactions in Aqueous
Solution
Turn in homework for Chapter 4
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Chem 105 Chpt 4 Lsn 11
 Where
Road Map
we were
 Chemical
equations and chemical
analysis review problems
 Where
we are going
 Critical
skills: naming common ions,
writing electrically neutral
formulas/reactions, stoichiometric
conversions
 Types of reactions
 Use: Figure 5.3, page 179
 Know:
Table 5.2, pg 182
Chem 105 Chpt 4 Lsn 11
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5.2 Precipitation reactions
Writing Equations for Aqueous Ionic
Reactions

Three types of equations are used to represent
aqueous ionic reactions: molecular, total ionic, and
net ionic equations.
 molecular equation: shows all reactants and
products as if they were intact, undissociated
 total ionic equation: shows all the soluble ionic
substances dissociated into ions. Charges must
balance
 Spectator ions not involved in chemical change.
 net ionic equation: it eliminates the spectator
ions and shows the actual chemical change taking
place.
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Chem 105 Chpt 4 Lsn 11
Practice Problem 10-1
 molecular
equation
Pb(NO3)2(aq) + K2CrO4(aq) →
PbCrO4(s) + 2 KNO3(aq)
 Write the Total Ionic and Net Ionic
equations for
 Total

 Net
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Chem 105 Chpt 4 Lsn 11
Practice Problem 10-2
 Write
the Total Ionic and Net Ionic
equations for
CaCl2(aq) + Na2CO3(aq) →
CaCO3(s) + 2 NaCl(aq)
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Chem 105 Chpt 4 Lsn 11
Practice Problem 10-3
Solutions of iron (III) chloride and
potassium hydroxide give iron (III)
hydroxide and potassium chloride when
combined.
 Write the

 Molecular
equation
 Total ionic equation
 Net ionic equation
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Chem 105 Chpt 4 Lsn 11
5.3 – Acids and Bases
(know table 5.2)
Acid: increases the H+ concentration
 Base: increases the OH- concentration

 Strong
acid: completely dissociates/ionizes
 Weak acid: partial ionization
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Chem 105 Chpt 4 Lsn 11
5.4 - Reactions of Acids and Bases
An Acid reacting with a base produce a
salt and water
 Neutralization reaction: a strong acid with
a strong base

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Chem 105 Chpt 4 Lsn 11
Practice Problem 10 - 4
 Calcium
chloride and potassium
phosphate combine to form calcium
phosphate and potassium chloride.
 Write the molecular equation
3 CaCl2(aq) + 2 K3PO4(aq) →
Ca3PO4(s) + 6 KCl(aq)
 Write the Total Ionic and Net Ionic
equations
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Chem 105 Chpt 4 Lsn 11
3 CaCl2(aq) + 2 K3PO4(aq) →
Ca3PO4(s) + 6 KCl(aq)
 Write
the Total Ionic and Net Ionic
equations
 Combining 5 grams CaCl2 with 3.5
grams of K3PO4 produced only a 67%
yield of KCl.
 What is the limiting reactant?
 What mass of product did you make?
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Chem 105 Chpt 4 Lsn 11
5.8 Measuring Concentrations

How many moles of each ion are in each
solution?
(a) 2 mol of potassium perchlorate
dissolved in water
(b) 354 g of magnesium acetate dissolved
in water
(c) 1.88 x 1024 formula units of ammonium
chromate dissolved in water
(d) 1.32 L of 0.55 M sodium bisulfate
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Chem 105 Chpt 4 Lsn 11
5.8 Measuring Concentrations
 How
many moles of H+(aq) are present
in 451 mL of 3.20 M hydrobromic acid?
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Chem 105 Chpt 4 Lsn 11
5.4 Acid-Base Reactions:
Acid-Base Titrations

What volume of 0.1292 M Ba(OH)2 would
neutralize 50.00 mL of the HCl solution
standardized in the preceding sample
problem (4.5) ?
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Chem 105 Chpt 4 Lsn 11
Precipitation Reactions: Predicting Whether a
Precipitate Will Form

Predict whether a reaction occurs, and write
balanced total and net ionic equations.
(a) iron(III) chloride(aq) + cesium
phosphate(aq) →
(b) sodium hydroxide(aq) + cadmium
nitrate(aq) →
(c) magnesium bromide(aq) + potassium
acetate(aq) →
(d) silver sulfate(aq) + barium chloride(aq) →
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Chem 105 Chpt 4 Lsn 11
Next Lesson

Chapter 5
 Gas
forming reactions
 Classifying reactions
 Oxidation reactions
 Measuring concentrations of compounds in
solution
 pH
 Stoichiometry of reactions in aqueous
solution
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Chem 105 Chpt 4 Lsn 11
Practice Problem 10 - 5
 Write
the Total Ionic and Net Ionic
equations for
Zn(s) + H2SO4(aq) →
ZnSO4(aq) + H2(g)
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Chem 105 Chpt 4 Lsn 11
Practice Problem 10-6
 Write
the Total Ionic and Net Ionic
equations for
HCl(aq) + NaOH(aq) →
NaCl(aq) + H2O(l)
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Chem 105 Chpt 4 Lsn 11