2 aqueous solutions of KMnO4 A solution is a homogenous mixture of 2 or more substancesThe solute is(are) the substance(s) present in the smaller amount(s)The solvent is the substance present in the larger amountaqueous solutions of KMnO4SolutionSolventSoluteSoft drink(l)H2OSugar, CO2Air(g)N2O2, Ar, CH4Soft Solder(s)PbSn
3 An electrolyte is a substance that, when dissolved in water, results in a solution that can conduct electricity.A nonelectrolyte is a substance that, when dissolved, results in a solution that does not conduct electricity.nonelectrolyteweak electrolytestrong electrolyte
4 Conduct electricity in solution? Cations (+) and Anions (-)Strong Electrolyte – 100% dissociationNaCl(s) Na+(aq) + Cl-(aq)H2OWeak Electrolyte – not completely dissociatedCH3COOH CH3COO-(aq) + H+(aq)
5 Ionization of acetic acid CH3COOH CH3COO-(aq) + H+(aq)A reversible reaction. The reaction can occur in both directions.Acetic acid is a weak electrolyte because its ionization in water is incomplete.
6 Hydration is the process in which an ion is surrounded by water molecules arranged in a specific manner.d+d-H2O
7 Nonelectrolyte does not conduct electricity? No cations (+) and anions (-) in solutionC6H12O6(s) C6H12O6(aq)H2O
8 Precipitation Reactions Precipitate – insoluble solid that separates from solutionPbI2precipitatePb(NO3)2(aq) + 2NaI(aq) PbI2(s) + 2NaNO3(aq)molecular equationPb2+ + 2NO3- + 2Na+ + 2I PbI2(s) + 2Na+ + 2NO3-ionic equationPb2+ + 2I PbI2(s)net ionic equationNa+ and NO3- are spectator ions
9 Precipitation of Lead Iodide Pb2+ + 2I PbI2(s)PbI2
10 Solubility is the maximum amount of solute that will dissolve in a given quantity of solvent at a specific temperature.
11 Examples of Insoluble Compounds CdSPbSNi(OH)2Al(OH)3
12 Writing Net Ionic Equations Write the balanced molecular equation.Write the ionic equation showing the strong electrolytes completely dissociated into cations and anions.Cancel the spectator ions on both sides of the ionic equationCheck that charges and number of atoms are balanced in the net ionic equationWrite the net ionic equation for the reaction of silver nitrate with sodium chloride.AgNO3(aq) + NaCl(aq) AgCl(s) + NaNO3(aq)Ag+ + NO3- + Na+ + Cl AgCl(s) + Na+ + NO3-Ag+ + Cl AgCl(s)
13 Properties of AcidsHave a sour taste. Vinegar owes its taste to acetic acid. Citrusfruits contain citric acid.Cause color changes in plant dyes.React with certain metals to produce hydrogen gas.2HCl(aq) + Mg(s) MgCl2(aq) + H2(g)React with carbonates and bicarbonatesto produce carbon dioxide gas2HCl(aq) + CaCO3(s) CaCl2(aq) + CO2(g) + H2O(l)Aqueous acid solutions conduct electricity.
14 Properties of Bases Have a bitter taste. Feel slippery. Many soaps contain bases.Cause color changes in plant dyes.Aqueous base solutions conduct electricity.Examples:
15 Arrhenius acid is a substance that produces H+ (H3O+) in water Arrhenius base is a substance that produces OH- in water
25 Zn(s) + CuSO4(aq) ZnSO4(aq) + Cu(s) Zn Zn2+ + 2e-Zn is oxidizedZn is the reducing agentCu2+ + 2e CuCu2+ is reducedCu2+ is the oxidizing agentCopper wire reacts with silver nitrate to form silver metal.What is the oxidizing agent in the reaction?Cu(s) + 2AgNO3(aq) Cu(NO3)2(aq) + 2Ag(s)Cu Cu2+ + 2e-Ag+ + 1e AgAg+ is reducedAg+ is the oxidizing agent
26 Li+, Li = +1; Fe3+, Fe = +3; O2-, O = -2 Oxidation numberThe charge the atom would have in a molecule (or anionic compound) if electrons were completely transferred.Free elements (uncombined state) have an oxidation number of zero.Na, Be, K, Pb, H2, O2, P4 = 0In monatomic ions, the oxidation number is equal to the charge on the ion.Li+, Li = +1; Fe3+, Fe = +3; O2-, O = -2The oxidation number of oxygen is usually –2. In H2O2 and O22- it is –1.4.4
27 HCO3- O = –2 H = +1 3x(–2) + 1 + ? = –1 C = +4 The oxidation number of hydrogen is +1 except when it is bonded to metals in binary compounds. In these cases, its oxidation number is –1.Group IA metals are +1, IIA metals are +2 and fluorine is always –1.6. The sum of the oxidation numbers of all the atoms in a molecule or ion is equal to the charge on the molecule or ion.7. Oxidation numbers do not have to be integers. Oxidation number of oxygen in the superoxide ion, O2-, is –½.HCO3-O = –2H = +1What are the oxidation numbers of all the elements in HCO3- ?3x(–2) ? = –1C = +4
28 The Oxidation Numbers of Elements in their Compounds
29 IF7 F = -1 7x(-1) + ? = 0 NaIO3 I = +7 Na = +1 O = -2 K2Cr2O7 What are the oxidation numbers of all the elements in each of these compounds?NaIO IF K2Cr2O7F = -17x(-1) + ? = 0NaIO3I = +7Na = +1O = -2K2Cr2O73x(-2) ? = 0O = -2K = +1I = +57x(-2) + 2x(+1) + 2x(?) = 0Cr = +6
30 Types of Oxidation-Reduction Reactions Combination ReactionA + B C+2-33Mg + N MgN2Decomposition ReactionC A + B+1+5-2+1-12KClO KCl + 3O2
31 Types of Oxidation-Reduction Reactions Combustion ReactionA + O B+4-2S + O SO2+2-22Mg + O MgO
32 Types of Oxidation-Reduction Reactions Displacement ReactionA + BC AC + B+1+2Sr + 2H2O Sr(OH)2 + H2Hydrogen Displacement+4+2TiCl4 + 2Mg Ti + 2MgCl2Metal Displacement-1-1Cl2 + 2KBr KCl + Br2Halogen Displacement
33 The Activity Series for Metals Hydrogen Displacement ReactionM + BC MC + BM is metalBC is acid or H2OB is H2Ca + 2H2O Ca(OH)2 + H2Pb + 2H2O Pb(OH)2 + H2
34 The Activity Series for Halogens F2 > Cl2 > Br2 > I2Halogen Displacement Reaction-1-1Cl2 + 2KBr KCl + Br2I2 + 2KBr KI + Br2
35 Classify each of the following reactions. Ca2+ + CO CaCO3PrecipitationNH3 + H NH4+Acid-BaseZn + 2HCl ZnCl2 + H2Redox (H2 Displacement)Ca + F CaF2Redox (Combination)
36 Solution Stoichiometry The concentration of a solution is the amount of solute present in a given quantity of solvent or solution.M = molarity =moles of soluteliters of solutionWhat mass of KI is required to make 500. mL of a 2.80 M KI solution?M KIM KIvolume of KI solutionmoles KIgrams KI1 L1000 mLx2.80 mol KI1 L solnx166 g KI1 mol KIx500. mL= 232 g KI
38 Dilution is the procedure for preparing a less concentrated solution from a more concentrated solution.DilutionAdd SolventMoles of solutebefore dilution (i)after dilution (f)=MiViMfVf=
39 How would you prepare 60. 0 mL of 0 How would you prepare 60.0 mL of M HNO3 from a stock solution of 4.00 M HNO3?MiVi = MfVfMi = 4.00 MMf = MVf = LVi = ? LVi =MfVfMi=0.200 M x L4.00 M= L = 3.00 mLDilute 3.00 mL of acid with water to a total volume of 60.0 mL.
40 Gravimetric Analysis Dissolve unknown substance in water React unknown with known substance to form a precipitateFilter and dry precipitateWeigh precipitateUse chemical formula and mass of precipitate to determine amount of unknown ion
41 Equivalence point – the point at which the reaction is complete TitrationsIn a titration a solution of accurately known concentration is added gradually added to another solution of unknown concentration until the chemical reaction between the two solutions is complete.Equivalence point – the point at which the reaction is completeIndicator – substance that changes color at (or near) theequivalence pointSlowly add baseto unknown acidUNTILthe indicatorchanges color
42 Titrations can be used in the analysis of Acid-base reactions Redox reactionsH2SO4 + 2NaOH H2O + Na2SO45Fe2+ + MnO4- + 8H Mn Fe3+ + 4H2O
43 WRITE THE CHEMICAL EQUATION! What volume of a M NaOH solution is required to titrate mL of a 4.50 M H2SO4 solution?WRITE THE CHEMICAL EQUATION!H2SO4 + 2NaOH H2O + Na2SO4Macidrxncoef.Mbasevolume acidmoles redmoles basevolume base4.50 mol H2SO41000 mL solnx2 mol NaOH1 mol H2SO4x1000 ml soln1.420 mol NaOHx25.00 mL= 158 mL
44 WRITE THE CHEMICAL EQUATION! 16.42 mL of M KMnO4 solution is needed to oxidize mL of an acidic FeSO4 solution. What is the molarity of the iron solution?WRITE THE CHEMICAL EQUATION!5Fe2+ + MnO4- + 8H Mn Fe3+ + 4H2OMredrxncoef.Voxidvolume redmoles redmoles oxidM oxid16.42 mL = L25.00 mL = Lmol KMnO41 Lx5 mol Fe2+1 mol KMnO4x1L Fe2+xL= M