Copyright © Houghton Mifflin Company. All rights reserved.4 | 1 Parts of Solutions Solution-...

Copyright © Houghton Mifflin Company. All rights reserved. 4 | 1

Parts of Solutions

• Solution- homogeneous mixture.• Solute- what gets dissolved.• Solvent- what does the dissolving.• Soluble- Can be dissolved.• Miscible- liquids dissolve in each other.


Figure 4.1 The Water Molecule


Hydration

• The process of breaking the ions of salts apart.

• Ions have charges and are attracted to the opposite charges on the water molecules.


Figure 4.2 Polar Water Molecules Interact with the Positive and Negative Ions of a Salt

Assisting in the Dissolving Process


How Ionic solids dissolve

O H

H HO

HHO

HH

O

HH

O

H HOH

H O

HH

O

Click here for Animation


Solubility

• How much of a substance will dissolve in a given amount of water.

• Usually g/100 mL• Varies greatly, but if they do dissolve the

ions are separated,• and they can move around.• Water can also dissolve non-ionic

compounds if they have polar bonds.


Figure 4.3a The Ethanol Molecule Contains a Polar O-H Bond Similar to Those in the

Water Molecule


Figure 4.3b The Polar Water Molecule Interacts Strongly with the Polar-O-H bond in

Ethanol


Electrolytes

• Electricity is moving charges.• The ions that are dissolved can move.• Solutions of ionic compounds can conduct

electricity.• Solutions are classified three ways.


Types of solutions

Strong electrolytes- completely dissociate (fall apart into ions).

a) Many ions- Conduct well.

Weak electrolytes- Partially fall apart into ions.

a) Few ions -Conduct electricity slightly.

Non-electrolytes- Don’t fall apart.a) No ions- Don’t conduct.


Figure 4.4a-c Electrical Conductivity of Aqueous Solutions


Figure 4.5 NaCl Dissolves


Figure 4.6 HCL is Completely Ionized


Figure 4.7 An Aqueous Solution of Sodium Hydroxide


Figure 4.8 Acetic Acid (HC2H3O2)


Figure 4.9 The Reaction of NH3 in Water


Measuring Solutions

• Concentration- how much is dissolved.• Molarity = Moles of solute

Liters of solution• abbreviated M• 1 M = 1 mol solute / 1 liter solution• Calculate the molarity of a solution with

34.6 g of NaCl dissolved in 125 mL of solution.


Figure 4.10a-c Steps Involved in the Preparation of a Standard Aqueous Solution


Figure 4.11a-b Measuring Pipets and Volumetric Pipets Measure Liquid Volume


Figure 4.12a-c A Measuring Pipet is Used to Add Acetic Solution to a Volumetric Flask


Figure 4.14 a&b Reactant Solutions


Figure 4.15 a&b The Reaction of K2CrO4 and Ba(NO3)2


Figure 4.17 Molecular-Level Representations Illustrating the Reaction of KCl (aq) with AgNO3 (aq) to Form AgCl (s)


Writing Net Ionic Equations

• Strong acids are all written in net ionic form-Binary acids – are all strong (except for HF(aq) ) -Oxyacids-If the number of oxygens exceeds the number of hydrogens by 2 or more they are considered strong.-Polyprotic acids ionize one (1) hydrogen at a time. All subsequent ionizations of acidic hydrogens are considered weak.(except for HSO4(aq) 1- )

H2SO4(aq) → H(aq) 1+ + HSO4(aq) 1-

• Strong bases are all written in ionic form.-Group IA and IIA metal hydroxides are strong bases.

• All weak acids and bases (those not mentioned above) are always written in molecular form.

• Ionic Salts-If soluble-written in ionic form -if insoluble written in molecular/undissociated form.


Writing Net Ionic Equations

• Oxides are always written in molecular/undissociated form.

• Gases are always written in molecular form.

• Molecular compounds are always written in molecular form.


Determining the Mass of Product Formed


Determining the Mass of Product Formed


Performing Calculations for Acid-Base Reactions


Neutralization Reactions I







Neutralization Reactions II


Neutralization Titration


Figure 4.19 The Reaction of Solid Sodium and Gaseous Chlorine to Form Solid Sodium

Chloride


Figure 4.20 A Summary of Oxidation-Reduction Process


The Half-Reaction Method (Acidic Solution)


The Half-Reaction Method (Basic Solution)


Figure 4.4a-c Electrical Conductivity of Aqueous Solutions


An Aqueous Solution of Co(NO3)2.


Figure 4.10 Steps Involved in the Preparation of a Standard Aqueous Solution


Figure 4.13 Yellow Aqueous Potassium


Figure 4.14a-b Reactant Solutions


Figure 4.15c Solution Post-Reaction


Figure 4.16 Addition of Silver Nitrate to Aqueous Solution of Potassium Chloride


Figure 4.17 Reaction of KCI(aq) with AgNO3(aq) to form AgCI(s).


Lead Sulfate


KOH and Fe(NO3)3 Mix to Create Solid Fe(OH)3.


Figure 4.18a-c The Titration of an Acid with a Base


Figure 4.19 The Reaction of Solid Sodium and Gaseous Chlorine to Form Solid Sodium

Chloride


Oxidation of Copper Metal by Nitric Acid


Magnetite


Aluminum and Iodine Mix to Form Aluminum Iodide


Chocolate


When Potassium Dichromate Reacts with Ethanol, the Solution Contains Cr3+.


Table 4.1 Simple Rules for the Solubility of Salts in Water


Table 4.2 Rules for Assigning Oxidation States

Date post:	12-Jan-2016
Category:	Documents
Upload:	millicent-wade
View:	214 times
Download:	0 times

Copyright © Houghton Mifflin Company. All rights reserved.4 | 1 Parts of Solutions Solution-...

Documents