parts of solutions
DESCRIPTION
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. - PowerPoint PPT PresentationTRANSCRIPT
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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.
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Figure 4.1 The Water Molecule
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Hydration
• The process of breaking the ions of salts apart.
• Ions have charges and are attracted to the opposite charges on the water molecules.
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Figure 4.2 Polar Water Molecules Interact with the Positive and Negative Ions of a Salt
Assisting in the Dissolving Process
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How Ionic solids dissolve
O H
H HO
HHO
HH
O
HH
O
H HOH
H O
HH
O
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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.
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Figure 4.3a The Ethanol Molecule Contains a Polar O-H Bond Similar to Those in the
Water Molecule
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Figure 4.3b The Polar Water Molecule Interacts Strongly with the Polar-O-H bond in
Ethanol
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Electrolytes
• Electricity is moving charges.• The ions that are dissolved can move.• Solutions of ionic compounds can conduct
electricity.• Solutions are classified three ways.
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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.
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Figure 4.4a-c Electrical Conductivity of Aqueous Solutions
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Figure 4.5 NaCl Dissolves
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Figure 4.6 HCL is Completely Ionized
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Figure 4.7 An Aqueous Solution of Sodium Hydroxide
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Figure 4.8 Acetic Acid (HC2H3O2)
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Figure 4.9 The Reaction of NH3 in Water
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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.
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Figure 4.10a-c Steps Involved in the Preparation of a Standard Aqueous Solution
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Figure 4.11a-b Measuring Pipets and Volumetric Pipets Measure Liquid Volume
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Figure 4.12a-c A Measuring Pipet is Used to Add Acetic Solution to a Volumetric Flask
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Figure 4.14 a&b Reactant Solutions
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Figure 4.15 a&b The Reaction of K2CrO4 and Ba(NO3)2
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Figure 4.17 Molecular-Level Representations Illustrating the Reaction of KCl (aq) with AgNO3 (aq) to Form AgCl (s)
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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.
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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.
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Determining the Mass of Product Formed
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Determining the Mass of Product Formed
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Performing Calculations for Acid-Base Reactions
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Neutralization Reactions I
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Neutralization Reactions II
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Neutralization Titration
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Figure 4.19 The Reaction of Solid Sodium and Gaseous Chlorine to Form Solid Sodium
Chloride
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Figure 4.20 A Summary of Oxidation-Reduction Process
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The Half-Reaction Method (Acidic Solution)
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The Half-Reaction Method (Basic Solution)
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Figure 4.4a-c Electrical Conductivity of Aqueous Solutions
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An Aqueous Solution of Co(NO3)2.
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Figure 4.10 Steps Involved in the Preparation of a Standard Aqueous Solution
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Figure 4.13 Yellow Aqueous Potassium
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Figure 4.14a-b Reactant Solutions
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Figure 4.15c Solution Post-Reaction
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Figure 4.16 Addition of Silver Nitrate to Aqueous Solution of Potassium Chloride
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Figure 4.17 Reaction of KCI(aq) with AgNO3(aq) to form AgCI(s).
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Lead Sulfate
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KOH and Fe(NO3)3 Mix to Create Solid Fe(OH)3.
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Figure 4.18a-c The Titration of an Acid with a Base
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Figure 4.19 The Reaction of Solid Sodium and Gaseous Chlorine to Form Solid Sodium
Chloride
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Oxidation of Copper Metal by Nitric Acid
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Magnetite
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Aluminum and Iodine Mix to Form Aluminum Iodide
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Chocolate
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When Potassium Dichromate Reacts with Ethanol, the Solution Contains Cr3+.
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Table 4.1 Simple Rules for the Solubility of Salts in Water
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Table 4.2 Rules for Assigning Oxidation States