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Chapter 4,Chemical Reactions,Mr. Watson,HST,Mr. Watson,Solubility Rules,1. All nitrates are soluble.2. All compounds of Group IA metals and the ammonium ion, NH4+, are soluble.3. All chlorides are soluble except: AgCl, Hg2Cl2 and PbCl2.4. All sulfates are soluble except: PbSO4, BaSO4, and SrSO4.,Mr. Watson,Solubility Rules,5. All hydroxides and sulfides are insoluble except those of the Group IA metals and the ammonium ion.6. All carbonates and phosphates are insoluble except those of the Group IA metals and the ammonium ion.,Mr. Watson,A solution of Ba(NO3)2 is added to a solution of Na2SO4 to make a precipitate. From a table of solubility rules, the product isbarium sulfate, sodium nitrate,Mr. Watson,Electrolytes,Conduct electricity in solution due to the presence of ionsStrong electrolyte completely ionized in solutionWeak electrolyte partially ionized in solutionNon-electrolyte nonionic solution,Mr. Watson,Water Conductivity,Mr. Watson,Strong Electrolyte,Mr. Watson,Weak Electrolyte,Mr. Watson,Chemical Equations,Molecular EquationAgNO3(aq) + NaCl(aq) AgCl(s) + NaNO3(aq)Complete or Total Ionic EquationAg+(aq) + NO3-(aq) + Na+(aq) + Cl-(aq) AgCl(s) + Na+(aq) + NO3-(aq)Net Ionic EquationAg+(aq) + Cl-(aq) AgCl(s),Mr. Watson,Types of Reactions,synthesis reactions or combination reactionsdecomposition reactionsprecipitation reactionsneutralization reactionsacidbaseoxidation-reduction reaction,Mr. Watson,Precipitation Reactions,The process of separating a substance from a solution as a solid.AgNO3 + NaCl - AgCl + NaNO3 precipitate,Mr. Watson,Neutralization Reactions,acidbasesalt,Household acids and Bases,Mr. Watson,Neutralization Reactions,acidAny of a large class of sour-tasting substances whose aqueous solutions are capable of turning blue litmus indicators red, of reacting with and dissolving certain metals to form salts, and of reacting with bases or alkalis to form salts.Substance that donates H+ ions to solution,Mr. Watson,Neutralization Reactions,baseAny of a large class of compounds, including the hydroxides and oxides of metals, having a bitter taste, a slippery solution, the ability to turn litmus blue, and the ability to react with acids to form salts.Substance that donates a OH-1 ion to solution,Mr. Watson,Neutralization Reactions,saltThe term salt is also applied to substances produced by the reaction of an acid with a base, known as a neutralization reaction.Salts are characterized by ionic bonds, relatively high melting points, electrical conductivity when melted or when in solution, and a crystalline structure when in the solid state.,Mr. Watson,Neutralization Reactions,acid + base - “salt” + water,Mr. Watson,Neutralization Reactions,acid + base - “salt” + waterHCl + NaOH - NaCl + H2O,Mr. Watson,Neutralization Reactions,acid + base - “salt” + waterH2SO4 + 2KOH - K2SO4 + 2H2O,Mr. Watson,Strong vs. Weak Acids and Bases,strong - completely ionizedweak - partially ionized,Mr. Watson,Oxidation-Reduction Reaction,Oxidation - loss of electrons Reduction - gain of electronsRedox reactionoxidizing agent - substance that causes oxidationreducing agent - substance that cause reduction,Mr. Watson,Synthesis or Combination Reactions,Formation of a compound from simpler compounds or elements.,Mr. Watson,Decomposition Reactions,Separation into constituents by chemical reaction.,Mr. Watson,Electrolysis,decomposition caused by an electric current anodeelectrode where oxidation occurscathodeelectrode where reduction occurs,Mr. Watson,Identify the oxidizing agent in the reaction: 2Al(s) + 6 H+ = 2 Al3+(aq) + 3 H2(g) Al, H+, Al3+, H2Identify the oxidizing agent in the reaction:,Mr. Watson,Oxidation States Rules for Assigning Oxidation States,1. zero for uncombined element2. charge on monatomic ion3. F is always -1; other halogens -1 except when combined with more electronegative halogen or oxygen,Mr. Watson,Oxidation States Rules for Assigning Oxidation States,4. H is +1 except in metal hydrides, where H is -15. O is -2 except when combined with F (then +1 or +2) or in peroxides, -1.6. sum of oxidation states equals charge on ion or molecule,Mr. Watson,Oxidation State,What is the oxidation state of S in H2SO4?H = +1O = -2neutral compound, thus sum equals zero4O = 4*-2 = -82H = 2*+1 = +20 = +2 + (x) + (-8)x = +6,Mr. Watson,Oxidation State,What is the oxidation state of Cl in HClO4?H = +1O = -2neutral compound, thus sum equals zero4O = 4*-2 = -8H = 1*+1 = +10 = +1 + (y) + (-8)y = +7,Mr. Watson,Activity Series of Metals,Highest metal in series is the most reactiveA reactive metal will react with ions of less reactive metal to produce ions of reactive metal and atoms of the less reactive metal,Mr. Watson,Metal Reaction with Acid,Mr. Watson,Single Displacement,Mr. Watson,2Cu(s) + O2 (g) - 2CuO(s) The oxidation number of copper in the product isCu(0), Cu(I), Cu(II)In the reaction, copper metal isreduced, oxidized, unchanged in oxidation state,Mr. Watson,Solution,Solutions, in chemistry, homogeneous mixtures of two or more substances.,Mr. Watson,Solute,The substance that is present in smallest quantity is said to be dissolved and is called the solute. The solute can be either a gas, a liquid, or a solid.,Mr. Watson,Solvent,The substance present in largest quantity usually is called the solvent. The solvent can be either a liquid or a solid.,Mr. Watson,Preparation of a Solution,Mr. Watson,Molarity,The number of moles of solute per liter of solution.,molarity = M,moles of soluteM = - liter of solution,units = molar = moles/liter = M,Mr. Watson,EXAMPLE: Lye, which is sodium hydroxide, can be neutralized by sulfuric acid. How many milliliters of 0.200 M H2SO4 are needed to react completely with 25.0 mL of 0.400 M NaOH?,2 NaOH(aq) + H2SO4(aq) - Na2SO4(aq) + 2 H2O,Mr. Watson,EXAMPLE: Lye, which is sodium hydroxide, can be neutralized by sulfuric acid. How many milliliters of 0.200 M H2SO4 are needed to react completely with 25.0 mL of 0.400 M NaOH?,2 NaOH(aq) + H2SO4(aq) - Na2SO4(aq) + 2 H2O(25.0 mL NaOH) #mL H2SO4 = -,Mr. Watson,EXAMPLE: Lye, which is sodium hydroxide, can be neutralized by sulfuric acid. How many milliliters of 0.200 M H2SO4 are needed to react completely with 25.0 mL of 0.400 M NaOH?,2 NaOH(aq) + H2SO4(aq) - Na2SO4(aq) + 2 H2O(25.0 mL NaOH) (0.400 mol NaOH) #mL H2SO4 = - (1 L NaOH),Mr. Watson,EXAMPLE: Lye, which is sodium hydroxide, can be neutralized by sulfuric acid. How many milliliters of 0.200 M H2SO4 are needed to react completely with 25.0 mL of 0.400 M NaOH?,2 NaOH(aq) + H2SO4(aq) - Na2SO4(aq) + 2 H2O(25.0 mL NaOH) (0.400 mol NaOH)(1 L)#mL H2SO4 = - (1 L NaOH) (1000 mL),Mr. Watson,EXAMPLE: Lye, which is sodium hydroxide, can be neutralized by sulfuric acid. How many milliliters of 0.200 M H2SO4 are needed to react completely with 25.0 mL of 0.400 M NaOH?,2 NaOH(aq) + H2SO4(aq) - Na2SO4(aq) + 2 H2O(25.0) (0.400 mol NaOH)(1) (1 mol H2SO4) #mL H2SO4 = - (1) (1000) (2 mol NaOH),Mr. Watson,EXAMPLE: Lye, which is sodium hydroxide, can be neutralized by sulfuric acid. How many milliliters of 0.200 M H2SO4 are needed to react comp