Reactions in Aqueous Solution
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1 1 Reactions in Aqueous Solution Chapter 4 For test 3: Sections 3.7 and 4.1 to 4.5 Copyright The McGrawHill Companies, Inc. Permission required for reproduction or display. 2 A solution is a homogenous mixture of 2 or more substances The solute is(are) the substance(s) present in the smaller amount(s) The solvent is the substance present in the larger amount Solution Solvent Solute Soft drink(l) Air(g) Soft Solder(s) H 2 O N 2 Pb Sugar, CO 2 O 2, Ar, CH 4 Sn aqueous solutions of KMnO 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. nonelectrolyte weak electrolyte strong electrolyte 3
2 4 Conduct electricity in solution? Cations (+) and Anions () Strong Electrolyte 100% dissociation NaCl(s) H 2 O Na + (aq) + Cl (aq) Weak Electrolyte not completely dissociated CH 3 COOH CH 3 COO (aq) + H + (aq) 4 5 CH 3 COOH Ionization of acetic acid CH 3 COO (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. 5 6 Hydration is the process in which an ion is surrounded by water molecules arranged in a specific manner. d d + H 2 O 6
3 7 Nonelectrolyte does not conduct electricity? No cations (+) and anions () in solution C 6 H 12 O 6 (s) H 2 O C 6 H 12 O 6 (aq) 7 8 A process in which one or more substances is changed into one or more new substances is a chemical reaction A chemical equation uses chemical symbols to show what happens during a chemical reaction reactants products 3 ways of representing the reaction of H 2 with O 2 to form H 2 O From Chapter 3 section How to Read Chemical Equations 2 Mg + O 2 2 MgO 2 atoms Mg + 1 molecule O 2 makes 2 formula units MgO 2 moles Mg + 1 mole O 2 makes 2 moles MgO 48.6 grams Mg grams O 2 makes 80.6 g MgO NOT 2 grams Mg + 1 gram O 2 makes 2 g MgO From Chapter 3 section 3.7 9
4 10 Balancing Chemical Equations 1. Write the correct formula(s) for the reactants on the left side and the correct formula(s) for the product(s) on the right side of the equation. Ethane reacts with oxygen to form carbon dioxide and water C 2 H 6 + O 2 CO 2 + H 2 O 2. Change the numbers in front of the formulas (coefficients) to make the number of atoms of each element the same on both sides of the equation. Do not change the subscripts. 2C 2 H 6 NOT C 4 H 12 From Chapter 3 section Balancing Chemical Equations 3. Start by balancing those elements that appear in only one reactant and one product. C 2 H 6 + O 2 CO 2 + H 2 O start with C or H but not O 2 carbon on left C 2 H 6 + O 2 1 carbon on right 2CO 2 + H 2 O multiply CO 2 by 2 6 hydrogen on left 2 hydrogen on right multiply H 2 O by 3 C 2 H 6 + O 2 2CO 2 + 3H 2 O 11 From Chapter 3 section Balancing Chemical Equations 4. Balance those elements that appear in two or more reactants or products. C 2 H 6 + O 2 2CO 2 + 3H 2 O multiply O 2 by oxygen on left 4 oxygen (2x2) + 3 oxygen (3x1) = 7 oxygen on right C 2 H O 2 2CO 2 + 3H 2 O 2 2C 2 H 6 + 7O 2 4CO 2 + 6H 2 O remove fraction multiply both sides by 2 From Chapter 3 section
5 13 Balancing Chemical Equations 5. Check to make sure that you have the same number of each type of atom on both sides of the equation. 2C 2 H 6 + 7O 2 4CO 2 + 6H 2 O 4 C (2 x 2) 4 C 12 H (2 x 6) 12 H (6 x 2) 14 O (7 x 2) 14 O (4 x 2 + 6) Reactants 4 C 12 H 14 O From Chapter 3 section 3.7 Products 4 C 12 H 14 O Precipitation Reactions Precipitate insoluble solid that separates from solution precipitate Pb(NO 3 ) 2 (aq) + 2NaI(aq) PbI 2 (s) + 2NaNO 3 (aq) molecular equation Pb NO 3 + 2Na + + 2I PbI 2 (s) + 2Na + + 2NO 3 ionic equation PbI 2 Pb I PbI 2 (s) net ionic equation Na + and NO 3 are spectator ions Precipitation of Lead Iodide Pb I PbI 2 (s) PbI 2 15
6 16 Solubility is the maximum amount of solute that will dissolve in a given quantity of solvent at a specific temperature Examples of Insoluble Compounds CdS PbS Ni(OH) 2 Al(OH) Writing Net Ionic Equations 1. Write the balanced molecular equation. 2. Write the ionic equation showing the strong electrolytes completely dissociated into cations and anions. 3. Cancel the spectator ions on both sides of the ionic equation 4. Check that charges and number of atoms are balanced in the net ionic equation Write the net ionic equation for the reaction of silver nitrate with sodium chloride. AgNO 3 (aq) + NaCl(aq) AgCl(s) + NaNO 3 (aq) Ag + + NO 3 + Na + + Cl AgCl(s) + Na + + NO 3 Ag + + Cl AgCl(s) 18
7 19 Properties of Acids Have a sour taste. Vinegar owes its taste to acetic acid. Citrus fruits contain citric acid. Cause color changes in plant dyes. React with certain metals to produce hydrogen gas. 2HCl(aq) + Mg(s) MgCl 2 (aq) + H 2 (g) React with carbonates and bicarbonates to produce carbon dioxide gas 2HCl(aq) + CaCO 3 (s) Aqueous acid solutions conduct electricity. CaCl 2 (aq) + CO 2 (g) + H 2 O(l) 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: Arrhenius acid is a substance that produces H + (H 3 O + ) in water Arrhenius base is a substance that produces OH in water 21
8 22 Hydronium ion, hydrated proton, H 3 O A Brønsted acid is a proton donor A Brønsted base is a proton acceptor base acid acid base A Brønsted acid must contain at least one ionizable proton! Monoprotic acids HCl H + + Cl Strong electrolyte, strong acid HNO 3 H + + NO 3 CH 3 COOH H + + CH 3 COO Strong electrolyte, strong acid Weak electrolyte, weak acid Diprotic acids H 2 SO 4 H + + HSO 4 HSO 4 H + + SO 2 4 Strong electrolyte, strong acid Weak electrolyte, weak acid Triprotic acids H 3 PO 4 H + + H 2 PO 4 Weak electrolyte, weak acid H 2 PO 4 H + + HPO 2 4 HPO 2 4 H + + PO 3 4 Weak electrolyte, weak acid Weak electrolyte, weak acid 24
9 25 Identify each of the following species as a Brønsted acid, base, or both. (a) HI, (b) CH 3 COO, (c) H 2 PO 4 HI (aq) H + (aq) + I (aq) Brønsted acid CH 3 COO (aq) + H + (aq) CH 3 COOH (aq) Brønsted base H 2 PO 4 (aq) H + (aq) + HPO 2 4 (aq) H 2 PO 4 (aq) + H + (aq) H 3 PO 4 (aq) Brønsted acid Brønsted base Neutralization Reaction acid + base salt + water HCl(aq) + NaOH(aq) H + + Cl + Na + + OH H + + OH NaCl(aq) + H 2 O Na + + Cl + H 2 O H 2 O Neutralization Reaction Involving a Weak Electrolyte weak acid + base salt + water HCN(aq) + NaOH(aq) HCN + Na + + OH HCN + OH NaCN(aq) + H 2 O Na + + CN + H 2 O CN + H 2 O 27
10 28 Neutralization Reaction Producing a Gas acid + base salt + water + CO 2 2HCl(aq) + Na 2 CO 3 (aq) 2NaCl(aq) + H 2 O +CO 2 2H + + 2Cl + 2Na + + CO 3 2 2Na + + 2Cl + H 2 O + CO 2 2H + + CO 3 2 H 2 O + CO OxidationReduction Reactions (electron transfer reactions) 2Mg 2Mg e Oxidation halfreaction (lose e ) O 2 + 4e 2O 2 Reduction halfreaction (gain e ) 2Mg + O 2 + 4e 2Mg O 2 + 4e 2Mg + O 2 2MgO
11 31 Zn(s) + CuSO 4 (aq) Zn Zn e Cu e Cu Zn is oxidized Cu 2+ is reduced ZnSO 4 (aq) + Cu(s) Zn is the reducing agent Cu 2+ is the oxidizing agent Copper wire reacts with silver nitrate to form silver metal. What is the oxidizing agent in the reaction? Cu(s) + 2AgNO 3 (aq) Cu Cu e Cu(NO 3 ) 2 (aq) + 2Ag(s) Ag + + 1e Ag Ag + is reduced Ag + is the oxidizing agent Oxidation number The charge the atom would have in a molecule (or an ionic compound) if electrons were completely transferred. 1. Free elements (uncombined state) have an oxidation number of zero. Na, Be, K, Pb, H 2, O 2, P 4 = 0 2. In monatomic ions, the oxidation number is equal to the charge on the ion. Li +, Li = +1; Fe 3+, Fe = +3; O 2, O = 2 3. The oxidation number of oxygen is usually 2. In H 2 O 2 and O 2 2 it is The oxidation number of hydrogen is +1 except when it is bonded to metals in binary compounds. In these cases, its oxidation number is Group IA metals are +1, IIA metals are +2 and fluorine is always 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, O 2, is ½. HCO 3 What are the oxidation numbers of all the elements in HCO 3? O = 2 H = +1 3x( 2) + 1 +? = 1 C = +4 33
12 34 The Oxidation Numbers of Elements in their Compounds What are the oxidation numbers of all the elements in each of these compounds? NaIO 3 IF 7 K 2 Cr 2 O 7 IF 7 F = 1 7x(1) +? = 0 NaIO 3 I = +7 Na = +1 O = 2 3x(2) + 1 +? = 0 I = +5 K 2 Cr 2 O 7 O = 2 K = +1 7x(2) + 2x(+1) + 2x(?) = 0 Cr = Types of OxidationReduction Reactions Combination Reaction A + B C Mg + N 2 MgN 2 Decomposition Reaction C A + B KClO 3 2KCl + 3O 2 36
13 37 Types of OxidationReduction Reactions Combustion Reaction A + O 2 B S + O 2 SO Mg + O 2 2MgO Types of OxidationReduction Reactions Displacement Reaction A + BC Sr + 2H 2 O Sr(OH) 2 + H TiCl 4 + 2Mg Ti + 2MgCl Cl 2 + 2KBr 2KCl + Br 2 AC + B Hydrogen Displacement Metal Displacement Halogen Displacement The Activity Series for Metals Hydrogen Displacement Reaction M + BC MC + B M is metal BC is acid or H 2 O B is H 2 Ca + 2H 2 O Ca(OH) 2 + H 2 Pb + 2H 2 O Pb(OH) 2 + H 2 39
14 40 The Activity Series for Halogens F 2 > Cl 2 > Br 2 > I 2 Halogen Displacement Reaction Cl 2 + 2KBr 2KCl + Br 2 I 2 + 2KBr 2KI + Br Classify each of the following reactions. Ca 2+ + CO 2 3 CaCO 3 NH 3 + H + NH + 4 Zn + 2HCl ZnCl 2 + H 2 Ca + F 2 CaF 2 Precipitation AcidBase Redox (H 2 Displacement) Redox (Combination) Gravimetric Analysis 1. Dissolve unknown substance in water 2. React unknown with known substance to form a precipitate 3. Filter and dry precipitate 4. Weigh precipitate 5. Use chemical formula and mass of precipitate to determine amount of unknown ion 42
15 43 Titrations In 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 complete Indicator substance that changes color at (or near) the equivalence point Slowly add base to unknown acid UNTIL the indicator changes color Titrations can be used in the analysis of Acidbase reactions H 2 SO 4 + 2NaOH 2H 2 O + Na 2 SO 4 Redox reactions 5Fe 2+ + MnO 4 + 8H + Mn Fe H 2 O CH3 (part) and 4 HW Questions and Problems Page & 3.64 Questions and Problems Pages , 4.10, 4.12, 4.14, 4.18, 4.20, 4.22, 4.24, 4.32, 4.34, 4.40, 4.42, 4.44, 4.46, 4.48,
Reactions in Aqueous Solution
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