Silver Iodide Calcium Chromate Barium Hydroxide Sodium Chlorate - - PDF document

Reactions in aqueous solutions.notebook 1 December 14, 2010

Oct 18­2:28 PM

Using Table F determine if the following substances are soluble or insoluble. Silver Iodide Calcium Chromate Barium Hydroxide Sodium Chlorate Strontium Sulfate Lithium Carbonate Bell Task 11/15

Oct 18­2:11 PM

Chapter 4 Reactions in Aqueous solutions Alot of chemistry takes place in water or in aqueous solutions. It is imperative to study these types of reactions.

Reactions in aqueous solutions.notebook 2 December 14, 2010

Oct 18­2:30 PM

4.1 Some ways that chemical reactions occurs There are 3 chemical reactions that take place in aqueous solution:

• 1. Precipitation-insoluble solid formed-Table F
• 2. Acid Base Neutralization
• 3. REDOX-reduction/oxidation

Precipitation Reaction- Table F - Regents Reference Table

• ccurs between 2 aqueous solutions that form an

insoluble product indicated for a solid product formed. Cations and anions exchange partners Example: KI(aq) + Pb(NO3)2 KNO3(aq) + PbI2(s) Soluble or Insoluble: _______________1. Calcium Sulfate _______________2. Silver Iodide _______________3. Ammonium Hydroxide _______________4. Barium Chromate _______________5. Aluminum Sulfide

Memorize Page 112 for Solubility Guidelines Quiz on Wednesday!

Oct 18­2:37 PM

Acid Base Neutralization are reactions between acids and bases that produce salt and water NaOH (aq) + HCl(aq) NaCl(aq) + H2O(l) Remember, definition of Acids in Chapter 2-they produce H+ ions in solution and Bases produce OH- ions in solution. You should be able to predict products of these reactions!

Reactions in aqueous solutions.notebook 3 December 14, 2010

Nov 14­7:44 PM

Problem 4.1 a­c Try these

Nov 16­9:51 AM

Bell Task 11/16

4.32

Problem

Reactions in aqueous solutions.notebook 4 December 14, 2010

Oct 19­10:15 AM Oct 19­9:58 PM

Bell Task Think backwards on this problem. How might you use a precipitation reaction to prepare a sample of PbI2?

Reactions in aqueous solutions.notebook 5 December 14, 2010

Oct 19­9:29 PM

Electrolytes are substances that dissolve in water to produce conducting solution of ions. CH3OH Methanol is an alcohol group that does not conduct current because of the hydroxyl group attached- Any alcohol does not conduct current

• can be weak electrolytes or strong electrolytes
• All ionic bonded substances ARE STRONG

ELECTROLYTES AND will produce MANY ions in solution and dissociate to almost completely.

• All acids and bases will produce ions in solution-SOME

ACIDS AND BASES ARE WEAK AND STRONG remember

• NonPolar covalent bonded substances WILL NOT

CONDUCT CURRENT BECAUSE OF NO DIPOLES PRESENT-no partial charges present.

Oct 19­9:42 PM Difference in Strength of Electrolytes Glucose NaCl

Strong electrolyte is a compound that dissociates almost completely Weak electrolyte is a compound that dissociates to small extent and produces just a few ions in solution

Reactions in aqueous solutions.notebook 6 December 14, 2010

Nov 16­7:09 PM

Practice problems

11/17

Nov 16­7:30 PM

Dissociation of NaCl Video

Dissociation of KMnO4 Video

electrolyte vs. nonelectrolyte video

Strong vs. Weak Electrolyte video

Reactions in aqueous solutions.notebook 7 December 14, 2010

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Reactions in aqueous solutions.notebook 8 December 14, 2010

Nov 16­7:19 PM

Notice the moles of each ion produced! We can use aqueous solution stoichiometry to figure out the molar concentration of ions produced.

Oct 19­9:37 PM

K2SO4(s) 2K+ (aq) + SO4

­2 (aq)

H2O

Sample Problem: What is the total molar concentration of ions in a 0.575 M solution of strong electrolyte Potassium Sulfate, assuming complete dissociation?

Dissociation is a process where a compound splits apart when dissolved in water-See below example!

How many total moles of ions were produced?

Reactions in aqueous solutions.notebook 9 December 14, 2010

Nov 17­10:48 AM

Which one is the strongest electrolyte and weakest electrolyte from the illustration below.

Bell Task 11/18

Below are three different substances.

Nov 17­10:50 AM

Solubility Guidelines from Brown and LeMay Text

Reactions in aqueous solutions.notebook 10 December 14, 2010

Nov 16­7:26 PM

Sample Problem 4.2 What is the molar concentration of Br­ ions in a 0.225 M aqueous solution of FeBr3, assuming complete dissocation.

Nov 16­7:19 PM

Reactions in aqueous solutions.notebook 11 December 14, 2010

Nov 16­7:20 PM Nov 16­7:20 PM

Reactions in aqueous solutions.notebook 12 December 14, 2010

Nov 16­7:20 PM Oct 19­9:46 PM

Memorize table 4.1

NH3

Reactions in aqueous solutions.notebook 13 December 14, 2010

Oct 19­9:48 PM Nov 16­7:40 PM

Bell Task Identify the following as soluble or insoluble using solubility guidelines ________1. PbCrO4 ________2. NaOH ________3. AgBr ________4. (NH4)3PO4 ________5. CaCO3 ________6. KCl

Reactions in aqueous solutions.notebook 14 December 14, 2010

Oct 20­9:48 PM

Bell Task Identify the following as soluble or insoluble using solubility guidelines ________1. PbCrO4 ________2. NaOH ________3. AgBr ________4. (NH4)3PO4 ________5. CaCO3 ________6. KCl

Oct 20­9:23 PM

Solubility Guidelines Soluble Compounds Compounds containing alkali metal ions and Ammonium ion form soluble compounds Nitrates, bicarbonates, and chlorates form soluble compounds Halides(Cl, Br, I) form soluble compounds except Ag+, Hg2

+2, Pb+2

Sulfates form soluble compounds except-Ag+,Ca+2, Sr+2, Ba+2, Hg+2, Pb+2 Insoluble compounds Carbonates, Phosphates, Chromates and Sulfides except when combined with alkali metal ions and Ammonium ion Hydroxides except when combined with alkali metals and the Ba+2 ions

Reactions in aqueous solutions.notebook 15 December 14, 2010

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Reactions in aqueous solutions.notebook 16 December 14, 2010

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Reactions in aqueous solutions.notebook 17 December 14, 2010

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Reactions in aqueous solutions.notebook 18 December 14, 2010

Nov 17­1:09 PM Nov 17­1:11 PM

Sample Problem Write out the balanced net ionic equation for aqueous Potassium Chromate reacting with Barium Nitrate.

Reactions in aqueous solutions.notebook 19 December 14, 2010

Oct 20­8:22 PM

Net Ionic Equations

Nov 19­10:28 AM

Reactions in aqueous solutions.notebook 20 December 14, 2010

Nov 19­10:16 AM Oct 19­10:02 PM

11/22/10 start

Reactions in aqueous solutions.notebook 21 December 14, 2010

Oct 20­8:22 PM Oct 20­8:22 PM

Reactions in aqueous solutions.notebook 22 December 14, 2010

Oct 22­10:22 AM

A chemical reaction occurs between aqueous Chromium III Sulfate and aqueous Ammonium Carbonate. Write the net ionic equation for this reaction.

Sample Problem

Nov 22­10:16 AM

Reactions in aqueous solutions.notebook 23 December 14, 2010

Nov 22­10:19 AM Nov 28­7:20 PM

Bell Task 11/29 3 multiple choice questions

• 1. Which of the following is an electrolyte?
• A. Carbon Dioxide gas
• B. Sulfur Trichloride
• C. Nitrogen Monoxide
• D. Iron III Sulfate
• 2. Which of the following is a redox reaction?
• A. Ba(OH)2 (aq) + HNO3(aq) Ba(NO3)2(aq) + H2O(l)
• B. Na(s) + CoCl2(aq) NaCl(aq) + Co(s)
• C. AgNO3(aq) + KCl(aq) KNO3(aq) + AgCl(s)
• 3. Which of the following is insoluble?
• A. Calcium Hydroxide
• B. Magnesium Chromate
• C. Calcium Sulfate

Reactions in aqueous solutions.notebook 24 December 14, 2010

Nov 28­7:37 PM

Agenda Bell task and review Review Limiting Reactant Lab with Beakers ­final conclusions Review Chapter 3 test Acids and Bases and neutralization reactions

Oct 25­8:41 PM

Section 4.5 Acids, Bases and Neutralization Reactions Neutralization reactions occur in aqueous solution They produce _________ and ___________ Acids have different strength (strong electrolyte vs. weak electrolyte)

• produce H+ ions in solution
• Table 4.2 MAKE SURE YOU KNOW A WEAK ACID/BASE

FROM A STRONG ACID/BASE (page 115)

• Monoprotic Acids produce 1 mole of H+ ions and

dissociate only once HCl (aq) H30+(aq) + Cl-(aq)

• Diprotic Acids produce 2 moles of H+ ions and dissociate

twice H2SO4(aq) H30+ + HSO4

• 2

HSO4

• 2 (aq) H30+ + SO4
• 2
• triprotic acids produce 3 moles of H+ ions and dissociate

three times

H3PO4(aq) H2PO4

­3 + H3O+

Bases

• produce OH- ion in solution
• have different strength (strong vs. weak electrolyte)
• Ammonia weak base dissociates slightly
• NaOH strong base dissociates almost completely

Net ionic equation for neutralization reactions

• What do you think is left in a net ionic equation??

Example: Lithium Hydroxide reacts with Carbonic Acid to produce????

1st dissociation

Reactions in aqueous solutions.notebook 25 December 14, 2010

Oct 25­8:41 PM

Section 4.5 Acids, Bases and Neutralization Reactions Neutralization reactions occur in aqueous solution They produce _________ and ___________ Acids have different strength (strong electrolyte vs. weak electrolyte)

• produce H+ ions in solution
• Table 4.2 MAKE SURE YOU KNOW A WEAK ACID/BASE

FROM A STRONG ACID/BASE (page 115)

• Monoprotic Acids produce 1 mole of H+ ions and

dissociate only once HCl (aq) H30+(aq) + Cl-(aq)

• Diprotic Acids produce 2 moles of H+ ions and dissociate

twice H2SO4(aq) H30+ + HSO4

• 2

HSO4

• 2 (aq) H30+ + SO4
• 2
• triprotic acids produce 3 moles of H+ ions and dissociate

three times

H3PO4(aq) H2PO4

­3 + H3O+

Bases

• produce OH- ion in solution
• have different strength (strong vs. weak electrolyte)
• Ammonia weak base dissociates slightly
• NaOH strong base dissociates almost completely

Net ionic equation for neutralization reactions

• What do you think is left in a net ionic equation??

Example: Lithium Hydroxide reacts with Carbonic Acid to produce????

1st dissociation

Nov 30­10:31 AM

Reactions in aqueous solutions.notebook 26 December 14, 2010

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Reactions in aqueous solutions.notebook 27 December 14, 2010

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Reactions in aqueous solutions.notebook 33 December 14, 2010

Oct 25­8:36 PM

Bell Task

Determine the products and balance using lowest whole number coefficients for the following Barium Hydroxide reacts with sulfuric acid to produce ???

Oct 25­8:54 PM

Oxidation and Reduction (REDOX) How do you know that a redox rx has occurred in aqueous solution? Is the following a redox rx? Mg(s) + HCl(aq) MgCl2 + H2(g) Key terms in redox rx:

• substance oxidized
• substance reduced
• oxidizing agent
• reducing agent
• half reaction for oxidation
• half reaction for reduction

Reactions in aqueous solutions.notebook 34 December 14, 2010

Oct 26­7:56 PM

Bell Task 12/3 Assign the oxidation numbers to each atom in the following substances:

• 1. PO4
• 3 2. KAl(SO4)2 3. Na2Cr2O7

(Potassium Aluminum Sulfate)

• 4. H2S 5. V2O3
• 6. OH-

Dec 3­10:06 AM

Continued Practice of Assigning Oxidation Numbers Name each of the following using IUPAC rules! H2SO4(aq) Li2O Rb2S2O3 H2O2 ****

Reactions in aqueous solutions.notebook 35 December 14, 2010

Dec 2­10:28 AM Dec 3­10:14 AM

Reactions in aqueous solutions.notebook 36 December 14, 2010

Dec 3­10:31 AM Oct 25­9:10 PM

Identify the following as either precipitate, acid base or redox rx.

Bell Task 12/6

Reactions in aqueous solutions.notebook 37 December 14, 2010

Dec 6­10:11 AM Dec 5­8:52 PM

Agenda Bell task and review Review Assigning oxidation number rules Page 121 ­ review trending of elements loss/gain of e­ Writing Balanced redox reactions Problem 4.13 Finish

Reactions in aqueous solutions.notebook 38 December 14, 2010

Oct 25­8:57 PM

Assigning Oxidation numbers in a chem rx

• 1. an atom in its elements state has an ox # of 0.
• 2. an ion has an ox # equal to its charge
• 3. Polyatomic ions are equal to ionic charge-Don't

forget to assign ox # to every part of the ion

• 4. Hydrogen ions can be +1 or -1-depends on what

they are bonded with

• 5. oxygen usually have an ox # of -2.
• 6. Halogens usually have an ox # of -1.
• 7. The sum of ox # in a compound are equal to

ZERO. Don't forget your Periodic Table trends for the

• x #'s.

Oct 26­8:00 PM

Determine if the following reaction is redox? If it is determine the substance oxidized, substance reduced,

• xidizing agent, reducing agent. Write the half reaction for
• xidation and reduction and balance if necessary.

Cu(s) + 2AgNO3(aq) Cu(NO3)2 (aq) + 2Ag(s) substance Oxidized: substance Reduced: Oxidizing agent: Reducing agent: 1/2 reaction for oxidation: 1/2 reaction for reduction

Balanced half reaction

Reactions in aqueous solutions.notebook 39 December 14, 2010

Dec 6­7:50 PM

Bell Task 12/7 5 multiple choice questions

Dec 6­8:05 PM

Agenda Bell task and review Gravimetric Analysis Lab Requirements Activity Series Guided Question: Do all single replacement reactions? How do you predict if a redox reaction will occur then?

Reactions in aqueous solutions.notebook 40 December 14, 2010

Dec 6­8:29 PM

Describe in your own terms the Activity Series Chart (Table J). What is it's purpose? How is it setup? What does it really mean?

Dec 6­8:15 PM

Reactions in aqueous solutions.notebook 41 December 14, 2010

Dec 6­8:24 PM

The Activity Series ranks elements in order of their REDUCING ABILITY in aqueous solutions Elements at the top are very strong reducing agents Elements at the bottoms are very strong oxidizing agents As a result, any element higher in the activity series will reduce the ion of any element lower in the activity series. This chart helps predicts products of a reaction. Is the reaction spontaneous or not!

Oct 26­8:23 PM

Reactions in aqueous solutions.notebook 42 December 14, 2010

Dec 6­8:05 PM Oct 26­8:11 PM

Bell Task

Reactions in aqueous solutions.notebook 43 December 14, 2010

Oct 26­8:10 PM

Table 4.3 Activity Series of the Elements

An 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 below.

Oct 28­10:01 AM

Reactions in aqueous solutions.notebook 44 December 14, 2010

Oct 28­10:15 AM Oct 25­9:14 PM

Bell Task 12/8

1.

• 2. Which of the following will create a spontaneous

reaction?

• A. Ca(s) + CuCl2(aq)
• B. Ag(s) + CuCl2(aq)
• C. Au(s) + Cucl2(aq)
• D. H2(g) + CrI6(aq)

Reactions in aqueous solutions.notebook 45 December 14, 2010

Dec 7­1:26 PM

Agenda Bell task and review Check HW Balancing by Oxidation Number Method

Dec 7­1:30 PM

Sometimes, redox reactions can be too difficult to balance by inspection or by the method taught in Regents! In a laboratory setting, we often encounter more complex redox reactions involving oxoanions: CrO4

­2, Cr2O7 ­2, MnO4 ­,NO3 ­, SO4 ­2.

So, the oxidation­number method focuses more

• n the chemical changes by analyzing species

which are changing their oxidation numbers. Suppose, we are asked to balance the following equation in an acidic medium: This method gives us insight into electron transfer processes! Cr2O7

­2 + Cl­ Cr+3 + Cl2

Reactions in aqueous solutions.notebook 46 December 14, 2010

Oct 29­10:11 AM

net ionic equation where the spectator ions are removed!

Oct 29­10:11 AM

Reactions in aqueous solutions.notebook 47 December 14, 2010

Oct 30­10:21 AM Dec 7­1:42 PM

Reactions in aqueous solutions.notebook 48 December 14, 2010

Oct 30­11:29 AM Dec 13­10:15 AM

Problem #8 from Packet

Reactions in aqueous solutions.notebook 49 December 14, 2010

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Reactions in aqueous solutions.notebook 50 December 14, 2010

Dec 13­10:14 AM Dec 13­10:14 AM

Reactions in aqueous solutions.notebook 51 December 14, 2010

Dec 13­10:29 AM Dec 13­11:52 AM

Bell Task 12/14 Read each statement and determine if it is True or False­write the word.

________________1. Reducing species are located to the right of the stairstep line on the Periodic Table. ________________2. Oxidizing species can be determined by an increase ox number. ________________3. In using the Activity series, the elements positioned at the bottom are strong reducing agents ________________4. The following 2 aqueous solutions will produce a precipitate: AgClO4(aq) + CaBr2(aq) ________________5. CH3COOH (aq) is a strong electrolyte.

Reactions in aqueous solutions.notebook 52 December 14, 2010

Dec 13­8:50 PM

Agenda Bell task and review Practice Redox Titration calculations4.84 Practice balancing equations in basic medium 4.92A and 4.92B

Dec 14­10:31 AM

92B

Attachments Writing Ionic Equations.doc aabthaa0.mov