CHEM 101 1nd Edition Lecture 13Outline of Last Lecture I. Precipitation ReactionsII. Acids and BasesIII. Why do acids and bases burn?IV. Acids and BasesV. Acid-Base ReactionsOutline of Current Lecture I. Acid-Base ReactionsII. Oxides of NonmetalsIII. Gas Forming ReactionsIV. Oxidation and ReductionCurrent LectureI. Acid-Base Reactionsa. Neutralization Reactionsi. Write the balanced net equation for the reaction of ammonia (NH3) and perchloric acid (HClO4)1. Formula Unit Equationa. NH3 (aq) + HClO4 (aq) --> NH4ClO4 (aq)2. Equation is Balanced3. Identifya. NH3 is weak baseb. HClO4 is strong acidc. NH4ClO4 is a soluble salt4. Total Ionic Equationa. NH3 (aq) + H+ (aq) + ClO4- (aq) --> NH4+ (aq) + ClO4- (aq)i. orb. NH3 (aq) + H3O+ (aq) + ClO4- (aq) --> NH4+ (aq) + ClO4- (aq) + H2O (l)5. Net Ionic Equationa. NH3 (aq) + H+ (aq) --> NH4+ (aq) b. NH3 (aq) + H3O+ (aq) --> NH4+ (aq) + H2O (l)i. More CorrectThese 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. Write the balanced net equation for the reaction of phosphoric acid (H3PO4) and sodium hydroxide (NaOH)1. Formula Unit Equationa. H3PO4 (aq) + NaOH (aq) --> Na3PO4 (aq) + H2O2. Balance Equationa. H3PO4 (aq) + 3 NaOH (aq) --> Na3PO4 (aq) + 3 H2O3. Identifya. H3PO4 is a weak acidb. NaOH is a strong basec. Pa3PO4 is a soluble salt4. Total Ionic Equationa. H3PO4 (aq) + 3 Na+ (aq) + 3 OH- (aq) --> 3 Na+ (aq) + PO43- (aq) + 3 H2O (l)5. Net Ionic Equationa. H3PO4 (aq) + 3 OH- (aq) --> PO4 3- (aq) + 3 H2O (l)II. Oxides of Nonmetalsa. Oxides of non metals (CO2, SO2, SO3, NO2) have no hydrogen atoms but react withwater to product H3O+i. 2 SO2 (g) + O2 (g) --> 2 SO3 (g)ii. SO3 (g) + H2O(l) --> H2SO4 (aq)b. Scientists discovered, and have confirmed, that sulfur dioxide and nitrogen oxides are the primary cause of acid rain. In the US about ⅔ of SO2 and ¼ of all nitrogen oxides comes from electrical power generation that relies on burning fossil fuels like coal.III. Gas Forming Reactiona. Several Different chemical reactions lead to gas formationsb. Most common are those leading to CO2 formationi. NOTE1. Overall reaction below could be simplified to net ionic reaction (Cl-is spectator)ii. CaCO3 (s) + 2 HCl (aq) --> CaCl2 (aq) + H2CO3 (aq)iii. H2CO3 (aq) --> H2O (l) + CO2 (g)iv. Overall Reaction1. CaCO3 (s) + 2 HCl (aq) --> CaCl2 (aq) + H2O (l) + CO2 (aq)'c. For these reactions refer to table 3.3 in book.IV. Oxidation and Reductiona. Many reaction (called redox) involve the transfer of electrons from one species toanotheri. Acid-base and precipitation reaction do not involve redoxb. In order to keep track of the number f electrons oat or gained during a redox reaction, the concept of oxidation state is usedi. Do oxidation state reflect the actual electric charge on an atoms in a molecule or ion?1. In most cases no.2. Ex:a. In what the H atoms have a +1 oxidation state and the O has a -2 oxidation statec. Why use oxidation numbers?i. Provides a way to divide up the electrons among the atoms ii. be used to decide if a redox reaction has occurred iii. Distinguish oxidizing and reducing agentsd. An atom is oxidized when it loses electrons (LEO). An atom is reduced when it gains electrons (GER)i. Another acronym is OILRIGii. Oxidation Is Loss Reduction Is Gaine. Assigning Oxidation Statesi. Elements in their elemental form have an oxidation number of 0ii. The oxidation number of a monatomic ion is the same as its chargeiii. When combined with other elements, fluorine always has an oxidation number of -1iv. The oxidation state of oxygen in -2 in most compounds1. Except when oxygen is combined with fluorine, it takes on a positive oxidationv. Cl, Br, and I have an oxidation number -11. Except when combined with O and Fvi. The oxidation state of H is +1 in most compounds1. Except when bound to a metal, then it has a -1