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19 solutions and solubility

The document discusses key concepts about solutions including: - The components of a solution are a solvent and one or more solutes. Common solvents include water and gases. - Factors that affect solubility and the rate of dissolving include temperature, agitation, and surface area of the solute. Increasing these factors generally increases solubility. - Solutions can be classified as saturated, unsaturated, or supersaturated depending on the amount of solute dissolved compared to the maximum amount possible at a given temperature. - Solubility is also affected by properties of the solute molecules like polarity, charge, and size - more polar or charged molecules or smaller ions tend to be more soluble. - Solub

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Solutions Solubility& SOLVEN T SOLUTE Solutions Solubility&
Solutions Solubility& SOLUTION A homogenous mixture (looks uniform throughout) SOLVENT In a solution, the solvent is present in the largest amount by volume, mass, or number of moles SOLUTE Other substances present in a solution other than the solvent.
Solutions Solubility& Original state of solute Solvent Example Gas Gas Gas Liquid Gas Solid Hydrogen in palladium Liquid Gas Liquid Liquid Liquid Solid Amalgams (i.e. mercury in silver) Solid Gas Solid Liquid Solid Solid  ACTIVITY 1: Examples of Solutions Observe the samples of solutions and classify each solution under one category: 3 Oxygen in air CO2 in pop Water droplets in air Alcohol in water Dust in the air Sugar in water Copper in bronze
Solutions Solubility&  ACTIVITY 1: Examples of Solutions Hydrogen in palladium: A method for storing hydrogen gas as fuel
Solutions Solubility&  ACTIVITY 1: Examples of Solutions Amalgam: A metal and mercury solution By mass: 43% to 54% mercury, ~20-35% silver, ~10% copper, ~2% zinc, and some tin Remains soft for a short time and then forms a hard and durable compound
Solutions Solubility& Identify the components of these solutions:
Solutions Solubility& Common Types of Solutions: Alloys: Solid solutions of metal Stainless steel: Iron, chromium, nickel, manganese, vanadium
Solutions Solubility& Common Types of Solutions: Alloys: Solid solutions of metal Brass: Copper and zinc
Solutions Solubility& Common Types of Solutions: Liquid solution: A solution with two or more miscible liquids Miscible = Can dissolve in one-another Immiscible = Cannot dissolve in one-another Rubbing alcohol Oil and water
Solutions Solubility& Common Types of Solutions: Gas solution: A solution of two or more gases Air: 78% nitrogen, 21% oxygen, 0.9% argon, 0.03% carbon dioxide
Solutions Solubility& Common Types of Solutions: Aqueous solution: A solution where water is the solvent Tap water
Solutions Solubility& AQUEOUS SOLUTIONS: SOLUBLE VS. INSOLUBLE Not all substances dissolve equally in water. Recall the solubility table (dissolving solids in water): Although substances are classified as either soluble or insoluble in this table, substances are almost never completely insoluble or completely soluble in water. The solubility of a solute is the amount of solute that dissolves in a given quantity of solvent, at a certain temperature. For example, the solubility of sodium chloride in water at 20ºC is 36g per 100mL of water.
Solutions Solubility& AQUEOUS SOLUTIONS: SOLUBLE VS. INSOLUBLE Soluble Partly or slightly soluble Insoluble More than 1g in 100mL OR greater than 0.1mol/L Between 1g and 0.1g in 100mL OR Between 0.1mol/L and 0.01mol/L Less than 0.1g in 100mL OR Less than 0.01mol/L
Solutions Solubility& AQUEOUS SOLUTIONS: SATURATED VS. UNSATURATED One cannot endlessly dissolve salt in water
Solutions Solubility& AQUEOUS SOLUTIONS: SATURATED VS. UNSATURATED Saturated solution: Formed when no more solute will dissolve in a solution, with excess solute present. Unsaturated solution: A solution that is not yet saturated Supersaturated solution: Formed when a solution dissolves more solute than allowed at a specific temperature. No excess solute is present.
Solutions Solubility& AQUEOUS SOLUTIONS: SATURATED VS. UNSATURATED In a saturated solution with excess solute present, the rate of dissolution and precipitation are the same PbSO4(s) Pb2+ (aq) + SO4 2- (aq) precipitate dissolved ions
Solutions Solubility& FACTORS THAT AFFECT THE RATE OF DISSOLVING AND SOLUBILITY ACTIVITY 2: Who Can Dissolve the Most Salt?
Solutions Solubility& FACTORS THAT AFFECT THE RATE OF DISSOLVING AND SOLUBILITY ACTIVITY 2: Who Can Dissolve the Most Salt? (10 min) 6) You must not have precipitate in your solution, and your solution cannot be boiling. 1) Work in groups of 3-4 2) Each group will be given a graduated cylinder of salt and 250mL of water 3) Try to dissolve as much salt as you can 4) Try to alter the physical properties of your solvent and solute to increase the amount of salt that you can dissolve 5) You cannot add water
Solutions Solubility& FACTORS THAT AFFECT THE RATE OF DISSOLVING AND SOLUBILITY ACTIVITY 2: Who Can Dissolve the Most Salt? Factor Affect on rate of dissolving/solubility Temperature Higher temperatures allow more molecules to dissolve Agitation Stirring/agitation allows more molecules to dissolve Surface area Increasing the surface area allows more molecules to dissolve
At higher temperatures, solvent molecules move faster, and collide with undissolved solid molecules more frequently Temperature WARMER COOLER Solutions Solubility&
Agitation brings fresh solvent into contact with undissolved solid Agitation MORE MOLECULES IN CONTACT FEWER MOLECULES IN CONTACT Solutions Solubility&
Surface Area The greater the surface area of the reactant, the greater the molecules are in contact with the solvent LOWER SURFACE AREA HIGHER SURFACE AREA Molecules on the inside are exposed, enabling them to collide with solvent molecules Solutions Solubility&
Factors that affect solubility Solutions Solubility&
Factors that affect solubility Solutions Solubility& 1) Molecule polarity - Compounds dissolve due to the intermolecular forces between solvent and solute molecules Sugar: Forms H-bonds with water O H H OH H O H OH H O H H O H H O H H
Factors that affect solubility Solutions Solubility& 1) Molecule polarity - Compounds dissolve due to the intermolecular forces between solvent and solute molecules Ethanol: Forms H-bonds with water O H H O H H O H H
Factors that affect solubility Solutions Solubility& 1) Molecule polarity - Compounds dissolve due to the intermolecular forces between solvent and solute molecules Methanol: Forms H-bonds with water
Factors that affect solubility Solutions Solubility& 1) Molecule polarity - Compounds dissolve due to the intermolecular forces between solvent and solute molecules Octane: Cannot form H-bonds with water O H H
Factors that affect solubility Solutions Solubility& 1) Molecule polarity CH3OH vs. CH3CH2CH2CH2CH2CH3OH Which has greater solubility in water? CH3OH vs. CH3CH2CH2CH2CH2CH3OH Which has greater solubility in oil? The more attractive intermolecular forces exist between solvent and solute molecules, the greater the solubility
Factors that affect solubility Solutions Solubility& 1) Molecule polarity The addition of solute raises the boiling point of a solvent
Factors that affect solubility Solutions Solubility& 2) Temperature - Greater temperatures result in greater solubility of most solids Instant coffee powder + water at 20°C vs. Instant coffee powder + water at 70°C Which has greater solubility in water?
Factors that affect solubility Solutions Solubility& 2) Temperature - The greater the temperature, the lower the solubility of gases As temperature increases, gas molecules gain kinetic energy and are able to leave a solution. Gases become LESS soluble with increasing temperature.
Factors that affect solubility Solutions Solubility& 3) Molecule charge - Molecules that are charged can form dipole-ion attractions or Van der Waals forces between solute and solvent molecules Cl-Na+ Salt: Ions exert dipole-ion attractive forces with water O HH O H H O HH O HH O HH O HH O HH O H H
Factors that affect ion solubility Solutions Solubility&
Factors that affect ion solubility Solutions Solubility& 1) Ion charge - Ions with small charges tend to be soluble - Increasing the charge increases the force that holds the ions together - (i.e. phosphates, PO4 3+ , tend to be insoluble) 1+ 1- 3+ 3-
Factors that affect ion solubility Solutions Solubility& 2) Ion size - Small ions tend to be less soluble than large ions - Small ions bond more closely together than large ions - Thus the bond between small ions is stronger than the bond between large ions with the same charge 2+ 2-2+ 2-
Net Ionic Equations Solutions Solubility& K2CO3(aq) + CuSO4(aq)  ?K2SO4(aq) + CuCO3(s) Chemical equation: Ionic equation:  Anything that is aqueous must be separated into its component ions 2K+ (aq) + CO3 2- (aq) + Cu2+ (aq) + SO4 2- (aq)  2K+ (aq) + SO4 2- (aq) + CuCO3(s) Net Ionic equation:  Spectator ions* are eliminated Cu2+ (aq) + CO3 2- (aq)  CuCO3(s) *Spectator ions are ions that do not participate in the actual reaction Use the solubility table
Solubility curves Solutions Solubility& A graph that displays the maximum solute that can dissolve in 100g of water at various temperatures. Why does the solubility curve of NH3 have a negative slope? NH3 is a gas. Gases become LESS soluble with increasing temperature.
Solubility curves Solutions Solubility& 1) Is 50g of NH4Cl in 100g of water at 40ºC saturated, unsaturated, or supersaturated? Supersaturated 2) How many grams of KNO3 can dissolve in 50g of water at 70ºC? 65g 3) How much water is required to dissolve 60g of NaNO3 at 50ºC? 115g NaNO3 = 60g NaNO3 100g water x x = 52g water