Ch. 8 Solutions, Acids, & Bases I. How Solutions Form Definitions Types of Solutions Dissolving Rate of Dissolving

A. Definitions Solution – a mixture that has the same composition throughout the mixture; a homogeneous mixture. Solute - substance being dissolved (in lesser quantity) Solvent – what the solute is dissolved in (in greater quantity)

A. Definitions Solute - KMnO4 Solvent - H2O

Solutions Solution – a mixture that has the same composition throughout the mix. Remember the difference between a mixture and a compound. Compounds have a fixed composition throughout. Mixtures can have a variable composition throughout.

A. Definitions Solubility – The maximum amount of solute that can be dissolved in the solvent at a given temperature.

B. Types of Solutions Saturated solutions – maximum amount of solute at a given temperature. Unsaturated solutions – less than the maximum amount of solute at a given temperature.

Supersaturated solutions – more than the maximum amount of solute at a given temperature; unstable.

B. Types of Solutions concentration UNSATURATED SOLUTION more solute dissolves SATURATED SOLUTION no more solute dissolves SUPERSATURATED SOLUTION becomes unstable, crystals form concentration

C. Dissolving Solvation occurs at the surface of the solute solvent particles surround solute particles (+/- attraction) solute particles are pulled into solution

D. Rate of Dissolving Solids dissolve faster... more stirring small particle size (increased surface area) high temperature

Rate of Dissolving Heat it Crush it Stir it To increase rate of dissolving of SOLIDS: Heat it Crush it Stir it

D. Rate of Dissolving Gases dissolve faster... no shaking or stirring high pressure low temperature

To make a gas dissolve more quickly in a liquid: Cool it Increase the pressure of the gas

Ch. 8 Solutions, Acids, & Bases II. Concentration & Solubility

A. Concentration % by Volume usually liquid in liquid Ex: 10% juice = 10mL juice + 90mL water % by Mass usually solid in liquid Ex: 20% NaCl = 20g NaCl + 80g water

A. Concentration Concentrated solution large amount of solute Dilute solution small amount of solute

B. Solubility Solubility maximum grams of solute that will dissolve in 100 g of solvent at a given temperature varies with temperature based on a saturated solution

B. Solubility Solids are more soluble at... high temperatures Gases are more soluble at... low temperatures high pressures (Henry’s Law)

C. Solubility Charts Reading Solubility Charts If the number in the problem is EQUAL to the value on the chart the solution is considered SATURATED If the number in the problem is LESS than the value on the chart the solution is considered UNSATURATED If the number in the problem is MORE than the value on the chart the solution is considered SUPER SATURATED

C. Solubility Charts Solubility of Compounds in g/100g of Water at various Temperatures Compound 0◦ C 20◦ C 60◦ C 100◦ C Ammonium chloride 29.4 37.2 55.3 77.3 Copper(II) sulfate 23.1 32.0 61.8 114 Lead(II)chloride 0.67 1.0 1.94 3.2 Potassium bromide 53.6 65.3 85.5 104 Sodium chlorate 79.6 95.9 137 204

Answer Questions on your paper Chart How would you classify a solution of 65.3g of potassium bromide at 20ºC? _________ How would you classify a solution of 65.3g of potassium bromide at 60ºC? ____________ How would you classify a solution of 65.3g of potassium bromide at 0ºC? ______________ How would you classify a solution of 37g of ammonium chloride at 20ºC? ___________ How would you classify a solution of 2.5 g of lead (II) chloride at 20ºC? ______________ Saturated Unsaturated Supersaturated Unsaturated Supersaturated

D. Solubility Graphs Solubility Curve shows the dependence of solubility on temperature

Graph How would you classify a solution of 80g of HCl at 20ºC? ____________ How would you classify a solution of 30g of KNO3 at 20ºC? __________ How would you classify a solution of 39g of NaCl at 100ºC? ________ How would you classify a solution of 80g of NaNO3 at 30ºC? __________ How would you classify a solution of 40g of KClO3 at 80ºC? __________ Supersaturated Unsaturated Saturated Unsaturated Unsaturated

How many grams of solute would you need to form a saturated solution of NH4Cl at 50ºC? _____ How would you classify a solution of 20g of SO2 at 0ºC? ___________ How much KI would you need to form a saturated solution at 10ºC? _____ Which solid decreases in solubility as the temperature increases? _______ 50 g Unsaturated 135 g Na2SO4

Acid, Bases & Salt Video Pre Test Post Test Post Test True False Neutralization Base Anion Electrolytes False True Post Test bitter, slippery, high pH Acids donate hydrogen, Bases accept Hydrogen An easy way to gauge is something is a strong/weak acid or base

Ch. 8 Solutions, Acids, & Bases III. Particles in Solution “Like Dissolves Like” Electrolytes

A. “Like Dissolves Like” Polar substances will only dissolve in polar liquids Rubbing alcohol and water Nonpolar substances will only dissolve in nonpolar liquids Oil and butter Substances that aren’t the same don’t mix. Oil and water

A. “Like Dissolves Like” NONPOLAR POLAR Detergents polar “head” with long nonpolar “tail” can dissolve both types (polar and nonpolar)

B. Electrolyte An electrolyte is a substance that when dissolved in water form ions Electrolytes get their name from the fact that the conduct electricity in water. Example: salt dissolved in water Many sports drinks contain “electrolytes” which are salts dissolved in water

B. Electrolytes - + - + - + Electrolyte Weak Electrolyte Non- salt - + acetic acid - + sugar Electrolyte Weak Electrolyte Non- Electrolyte solute exists as ions only Easily conducts electricity solute exists as ions and Molecules Slightly conducts electricity solute exists as molecules only Does NOT conduct electricity

B. Electrolytes Dissociation separation of +/- ions when an ionic compound dissolves in water

B. Electrolytes Ionization breaking apart of polar covalent molecules into ions when dissolving in water

Ch. 8 Solutions, Acids, & Bases IV. Intro to Acids & Bases Definitions Properties Uses

HCl + H2O  H3O+ + Cl– A. Acids Acids contain at least one hydrogen atom that can be removed when the acid is dissolved in water. These form hydronium ions, H3O+. Also called a proton donor HCl + H2O  H3O+ + Cl–

A. Bases Bases form hydroxide ions (OH-) in a water solution. a proton acceptor NH3 + H2O  NH4+ + OH-

A. Indicators Indicators are an organic substance that changes color in an acid or base. Examples: litmus - red/blue phenolphthalein - colorless/pink goldenrod - yellow/red red cabbage juice - pink/green

B. Properties ACIDS BASES bitter taste sour taste pH greater than 7 corrosive electrolytes turn litmus blue slippery feel sour taste pH less than 7 corrosive electrolytes turn litmus red react with metals to form H2 gas

C. Uses ACIDS H3PO4 –phosphoric acid - soft drinks, fertilizer, detergents H2SO4 – sulfuric acid - fertilizer, car batteries HCl – hydrochloric acid - gastric juice HC2H3O2 – acetic acid - vinegar

C. Uses BASES NaOH – sodium hydroxide -lye, drain and oven cleaner Mg(OH)2 – magnesium hydroxide - laxative, antacid NH3 –ammonia - cleaners, fertilizer

Ch. 8 Solutions, Acids, & Bases V. Strength of Acids & Bases Strength vs. Concentration Strong vs. Weak pH

A. Strength vs. Concentration Strong and weak – tells how easy the acid or base dissociates in solution. Concentration – The amount of acid or base in a solution. It is possible to have a dilute concentration of a strong acid that would be less harmful than a concentrated weak acid.

A. Strength of Acids & Bases The strength of an acid or base depends on how completely a compound separates into ions when dissolved in water. Ions can carry an electric charge so a strong acid will carry more electricity than weak acid.

B. Strong vs. Weak Strong Acid/Base 100% ions in water strong electrolyte HCl, HNO3, NaOH, LiOH - + Weak Acid/Base few ions in water weak electrolyte HC2H3O2, NH3 - +

B. Strong Acids Acids that ionize almost completely in a solution are strong acids. Ex: HCl, HNO3, and H2SO4 They have a very low pH (0-1).

B. Strong Bases Bases that dissociate completely in a solution are strong bases. Ex: NaOH They have a very high pH (13-14)

C. pH Scale a measure of the concentration of H+ ions in a solution pH (potential of Hydrogen) a measure of the concentration of H+ ions in a solution measured with a pH meter or an indicator with a wide color range (0-14) 7 INCREASING ACIDITY NEUTRAL BASICITY 14

pH of Common Substances C. pH Scale pH of Common Substances

ConcepTest Which of the following "molecular" pictures best represents a concentrated solution of the weak acid HA? A B

ConcepTest Is the following statement TRUE or FALSE? A strong acid has a lower pH than a weak acid. True- But: Strong/weak refers to amount of ionization whereas pH refers to concentration of H+.

Ch. 8 Solutions, Acids, & Bases VI. Neutralization Neutralization Reaction

A. Neutralization Reaction Chemical reaction between an acid and a base. Products are a salt (ionic compound) and water.

A. Neutralization Reaction ACID + BASE  SALT + WATER HCl + NaOH  NaCl + H2O = Neutralization does not always mean pH = 7.

A. Neutralization Reaction KOH + HNO3  H2O + KNO3 Acid Base Salt HNO3 KOH KNO3