CHEM 101 1nd Edition Lecture 12Outline of Last Lecture I. Aqueous SolutionsII. Solutions: Soluble Ionic CompoundsIII. Solubility and IonizationIV. Precipitation Reaction: Molecular EquationsOutline of Current Lecture I. Precipitation ReactionsII. Acids and BasesIII. Why do acids and bases burn?IV. Acids and BasesV. Acid-Base ReactionsCurrent LectureI. Precipitation Reactionsa. Molecular Equationsi. The ions in the reactant compounds exchange, or transpose, ions.1. AgNO3 (aq) + KCl (aq) --> AgCl (s) + KNO3 (aq)2. The equation written able are molecular (formula unit) equationsii. However the slats are dissolved in the water and cannot be seen unless the water is boiled awayb. Total Ionic Equationi. Ag+ (aq) + NO3- + K+ (aq) + Cl- (aq) --> AgCl (s) + NO3- (aq)+ K+ (aq)1. Spectator Ionsii. Net Ionic equation1. Ag+ (aq) + Cl- (aq) --> AgCl (s)2. It doesn't really matter where the Ag and Cl came from, but they're here and they're reacting3. This is the preferred way of writing reactionsII. Acids and Basesa. Arrhenius Definitionsi. Acid1. An acid is a substance that, when dissolved in water increase the concentration of hydrogen ions, H+, in solutiona. HClThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.ii. Base1. A base is a substance that, when dissolved in water, increase the concentration of hydroxide ion, OH-, in the 2. Solution a. NaOHiii. Salt: 1. A salt that contains a cation other that H+ and an anion other than OH- or O2-a. NaClb. Hydronium Ioni. A proton in water or H+ (aq) is best represented as H3O+ii. Sometimes we will write it as H+ (aq)iii. HCl (aq) is best represented as a solution of H3O+ and Cl-c. Strong Electrolytesi. Strong Acid1. HCl (aq) --> H+ (aq) + Cl- (aq)ii. Strong Base1. NaOH (aq) --> Na+ (aq) + OH- (aq)iii. Soluble Salt1. NaSO4 (aq) --> 2 Na+ (aq) + SO4- (aq)iv. Note the one way arrow means strongd. Weak Electrolytesi. Weak Acid1. CH3CO2H (aq) + H2O (l) <--> CH3CO2- (aq) + H3O+ (aq)ii. Weak Base1. NH3 (aq) + H2O (l) <--> NH4+ (aq) + OH- (aq)iii. Notice the double headed arrow, it means weake. Will need to memorize the 6 strong acids and 4 strong basesi. Acids1. HCla. Hydrocloric Acid2. HBra. Hydrobromic Acid3. HIa. Hydroiodic Acid4. HNO3a. Nitric Acid5. HClO4a. Perchloric Acid6. H2SO4a. Sulfuric Acidii. Bases1. LiOHa. Lithium Hydroxide2. NaOHa. Sodium Hydroxide3. KOHa. Potassium Hydroxide4. Ba(OH)2a. Barium Hydroxide5. Recognize the WEAK basea. NH3i. AmmoniaIII. Why do acids and bases burn?a. Acids and bases chemically react with fat and proteinb. Based on the reactions that acids and bases undergo when mixedIV. Acids and Basesa. Bronsted-Lowry Definitioni. Acid1. An acid is a proton donorii. Base1. A base is a proton acceptorb. Acid-Base reaction involves transfer of proton from the acid to the base to form anew acid and new basei. HCl + H2O --> H3O+ + Cl-1. Acid + Base --> Conjugate Acid + Conjugate Base a. Acid becomes Conjugate Baseb. Base become Conjugate Acidii. H2O + NH3 --> NH4+ + OH-1. Acid + Base <--> Conjugate Acid + Conjugate Baseiii. Will be expected to identify acids, bases, conjugate acids, and conjugate basesV. Acid-Base Reactionsa. Reaction: acid + base --> salt + wateri. Note that some bases, such as NH3, will not form waterb. Examplei. Write the balance net ionic equation for the reaction of hydrochloric acid and barium hydroxide1. Formula Unit Equationa. HCl (aq) + Ba(OH)2 (aq) --> BaCl2 (aq) + H2O (l)2. Balance Equationa. 2 HCl (aq) + Ba(OH)2 (aq) --> BaCl2 (aq) 2 H2Oi. Trial and Error3. Identify Compoundsa. HCl Stong Acidb. Ba(OH)2 Strong Basec. BaCl2 Soluble Salt4. Write as total Ionic Equationa. 2 H+ (aq) + Cl- (aq) + Ba2+ (aq) + 2 OH- (aq) --> Ba2+ (aq) + 2 Cl- (aq) + H2O (l)5. Remove spectator ions and write net ionic equationa. 2 H+ (aq) + 2 OH- (aq) --> H2O (l)c. Examplei. Write the balance net equation for the reaction of ammonia and perchloric acid1. Formula Unit Equationa. NH3 (aq) + HClO4 (aq) --> NH4ClO4 (aq)2. Equation is Balanced3. Identify Compoundsa. NH3 is a weak baseb. HClO4 is a strong acidc. NH4ClO4 is a soluble salt4. Total Ionic Equationa. NH3 (aq) + H+ (aq) + ClO4- (aq) --> NH4+ (aq) + ClO4 (aq) + H2O (l)5. Net Ionic Equationsa. NH3 (aq) + H+ --> NH4+ (aq) + H2O