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CHAPTER 5

Reactions in Aqueous Solution

Turn in homework for Chapter 4 Turn in homework for Chapter 4

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Road MapRoad MapWhere we wereWhere we were

Chemical equations and chemical Chemical equations and chemical analysis review problemsanalysis review problems

Where we are goingWhere we are goingCritical skills: naming common Critical skills: naming common

ions, writing electrically neutral ions, writing electrically neutral formulas/reactions, stoichiometric formulas/reactions, stoichiometric conversionsconversions

Types of reactionsTypes of reactionsUse: Use: Figure 5.3, page 179 Figure 5.3, page 179 Know: Table 5.2, pg 182Know: Table 5.2, pg 182

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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, undissociatedtotal 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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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 forTotal Net

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Practice Problem 10-2

Write the Total Ionic and Net Ionic equations forCaCl2(aq) + Na2CO3(aq) →

CaCO3(s) + 2 NaCl(aq)

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Practice Problem 10-3

Solutions of iron (III) chloride and Solutions of iron (III) chloride and potassium hydroxide give iron (III) potassium hydroxide give iron (III) hydroxide and potassium chloride hydroxide and potassium chloride when combined.when combined.

Write theWrite theMolecular equationMolecular equation Total ionic equationTotal ionic equation Net ionic equationNet ionic equation

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5.3 – Acids and Bases5.3 – Acids and Bases(know table 5.2)(know table 5.2)

Acid: increases the HAcid: increases the H++ concentration concentrationBase: increases the OHBase: increases the OH--

concentrationconcentrationStrong acid: completely Strong acid: completely

dissociates/ionizesdissociates/ionizesWeak acid: partial ionizationWeak acid: partial ionization

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5.4 - Reactions of Acids and 5.4 - Reactions of Acids and BasesBases

An Acid reacting with a base produce An Acid reacting with a base produce a a

salt and watersalt and water Neutralization reaction: a strong Neutralization reaction: a strong

acid with a strong baseacid with a strong base

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Practice Problem 10 - 4

Calcium chloride and potassium phosphate combine to form calcium phosphate and potassium chloride.

Write the molecular equation3 CaCl2(aq) + 2 K3PO4(aq) →

Ca3PO4(s) + 6 KCl(aq)Write the Total Ionic and Net Ionic

equations

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3 CaCl2(aq) + 2 K3PO4(aq) → Ca3PO4(s) + 6

KCl(aq)Write the Total Ionic and Net Ionic

equationsCombining 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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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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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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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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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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Next LessonNext Lesson

Chapter 5Chapter 5Gas forming reactionsGas forming reactionsClassifying reactionsClassifying reactionsOxidation reactionsOxidation reactionsMeasuring concentrations of compounds Measuring concentrations of compounds

in solutionin solutionpHpH Stoichiometry of reactions in aqueous Stoichiometry of reactions in aqueous

solutionsolution

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Practice Problem 10 - 5

Write the Total Ionic and Net Ionic equations forZn(s) + H2SO4(aq) →

ZnSO4(aq) + H2(g)

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Practice Problem 10-6

Write the Total Ionic and Net Ionic equations forHCl(aq) + NaOH(aq) →

NaCl(aq) + H2O(l)