CHAPTER 4. AQUEOUS REACTION CHEMISTRY

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1 CAPTER. AQUEOUS REACTION CEMISTRY solution - homogeneous mixture of or more substances; uniform distribution of particles and same properties throughout. A solution is composed of a solute dissolved in a solvent: solute - substance present in lesser amount solvent - substance present in greatest amount aqueous solution water is solvent; write (aq) after formula PROPERTIES AND CLASSIFICATION OF AQUEOUS SOLUTIONS 1) Strong electrolyte - a solution that is a good conductor of electricity. Substance that totally dissociates or ionizes in water. (Many ions) Soluble ionic compounds, strong acids, strong bases. E.g. NaCl, Cl, NaO ) Nonelectrolyte - solution that does not conduct electricity. Neutral molecules are present in solution. (No ions) Molecular compounds such as O, C 6 1 O 6 (sugar) ) Weak Electrolyte - solution that conducts electricity poorly. Substance that partially ionizes in water. (few ions) Weak acids or weak bases such as C O, N Understand how ionic compounds & molecular compounds dissolve in water ACID, BASE & SALT DEFINITIONS Acid: substance that produces ions in aqueous solutions. Strong acids completely ionize in water: E.g. NO NO - only ions and NO - ions are present in water NOW 7 Strong acids: Cl, Br, I, NO, SO, ClO, ClO All other acids are weak and only partially ionize in water (reversible rxn): E.g. C O C O - All species are present - most of the acid molecules have not ionized Base: substance that accepts ions in aqueous solns.; forms O - ions NaO (aq) Na O - Common Strong bases: Group 1A hydroxides (e.g. LiO, NaO, O) & heavy Group A hydroxides (Ca(O), Ba(O), Sr(O) ) Weak bases: N, several others exist but don t need to recognize yet. NEUTRALIZATION RXN (Type of DR rxn): ACID BASE SALT O Salt - ionic compound formed from base cation & acid anion during acid-base rxn. E.g. Cl NaO NaCl O

2 DOUBLE REPLACEMENT REACTIONS: AX BY AY BX Ions trade partners DR reactions occur when: 1) Insoluble product (solid ppt) forms. Refer to solubility rules - will be provided. ) Weak or nonelectrolyte forms. One of products is a weak acid, weak base or molecular compound. ) Gas forms. Note: DR rxn does not occur if soluble salts form. Precipitation reactions solubility - maximum amount of solid that will dissolve in a given amount of liquid at a given temperature. Solubility is a physical constant (like BP, density) 6.0 g NaCl E.g. NaCl solubility in water at 0 C: 100 g O Solubility Rules table.1, p. 111 now compounds containing 1A or N are always soluble; other ions, refer to table If insoluble in water, symbol is (s); if soluble in water, symbol is (aq) E.g. Na CO (aq) CaCl (aq) NaCl (aq) CaCO (s) NET IONIC REACTIONS Molecular Equation- write full formulas of all substances. See example above. Total Ionic Equation: Split up formulas of soluble salts, strong acids and strong bases into ions. Don't split apart solids, liquids, gases, weak or non-electrolytes. Net Ionic Equation: An ionic equation in which the spectator ions have been removed - net result after canceling common ions in total ionic equation. Spectator ions: Ions present on both sides of the equation. Must include (s), (g) or (l) symbols, but can omit (aq) symbol in writing rxns Total ionic: Na Net ionic: CO Ca CaCO (s) CO Ca Cl - Na Cl - CaCO (s) Exercise. Write molecular, total & net ionic rxns for the following: 1. molecular: Pb(NO ) (aq) Cl (aq) PbCl (s) NO (aq) Total: Pb NO Cl - PbCl (s) NO Net: Pb Cl - PbCl (s)

3 . Molecular: FeBr (aq) Ca(O) (aq) Fe(O) (s) CaBr (aq) Total: Fe 6Br - Ca 6O - Fe(O) (s) Ca 6Br - Net: Fe 6O - Fe(O) (s) Fe O - Fe(O) (s) Acid-base neutralization reaction nonelectrolyte e ( O) is formed Molecular: SO (aq) NaO (aq) O (l) Na SO (aq) Total: Net: SO Na O - O (l) Na SO O - O (l) O - O (l) note that formation of water is net result when strong acid & strong base react Gas formation during acid-base reactions This occurs if (A) a gas such as S forms Na S (aq) NO (aq) NaNO (aq) S (g) Total: Na S - NO Na NO S (g) Net: S - S (g) (B) an unstable product forms & breaks down. E.g. CO (aq) CO (g) O (l) Total: Na Na CO (aq) Cl (aq) NaCl (aq) O (l) CO (g) CO Cl - Na Cl - O (l) CO (g) Net: CO O (l) CO (g) Oxidation numbers- bookkeeping system for keeping track of e- these are values we assign; don t necessarily correspond to true number of e- gained or lost by atom write /- sign before number instead of after Rules 1) Uncombined elements: ox number = 0. E.g. Na or O ) monatomic ion: ox number = charge for ion; S - : ox # = -; Mg : ox # = ) : ox # = 1 (except for M compounds, = -1) ) O: ox # = - (except O, O = -1, 5) F: ox # = -1; other halogens usually 1 except when combined with O 6) polyatomic: sum of ox # s = charge on ion neutral compound: sum of ox # s = 0 E.g. assign ox # s to atoms in the following: 1. SF F: -1; S:. CO O: - C (-) = - C -6 = - C=. ClO O: - Cl (-) = -1 Cl -6 = -1 Cl = 5

4 . NO : 1; O: -; 1 N (-) = 0 N 5 = 0 N = 5 SINGLE REPLACEMENT (OXIDATION-REDUCTION) REACTIONS: A BC B AC oxidation: loss of electrons, substance becomes more (LEO) Mg Mg e - reduction: gain of electrons, substance becomes more - (GER) Ag e - Ag oxidizing agent: causes other substance to be oxidized; ox. agent is reduced reducing agent: causes reduction & becomes oxidized Ca (s) Cl (aq) CaCl (aq) (g) Net: Ca (s) (aq) Ca aq) (g) Which is oxidizing agent? reduced gains e-: Which is reducing agent? oxidized loses e-: Ca Many reactions involve oxidation & reduction not just SR: E.g. For the following reaction PbS O PbO SO 0 a. Identify the species oxidized S - _ b. Identify the species reduced O c. Oxidized element goes from oxidation number _-_ to. d. Reduced element goes from oxidation number 0_ to -. e. Oxidizing agent _O f. Reducing agent PbS Predict products for SR rxns Not all single replacement reactions occur - depends on activity of metal Use activity series to decide if reaction occurs (Table on p. 1) Elements at top are more reactive (more likely to become oxidized and form ions). An element in the series can replace elements below it but cannot replace elements above it. Complete the following reactions. Write NR if reaction does not occur. 1. Zn (s) PO Zn (PO ) (g). Ag (s) Cl (aq) NR. Mg (s) AgNO (aq) Mg(NO ) (aq) Ag (s). Al (s) SO (aq) Al (SO ) (aq) (g) 5. (g) CuBr (aq) Cu (s) Br (aq)

5 SOLUTION CONCENTRATION Because chemical reactions between solids are usually slow, we carry out these reactions by dissolving the solids in water. (Dissolved ions are more mobile & come into contact more frequently) The most common unit for expressing the concentration of the solution is called Molarity. moles solute moles Molarity = M = Units: M = Liter of solution Liter 1) 0.6 g NaO are dissolved in enough water to make 50 ml of solution. Calculate the molarity. NaO 0.6 g NaO = mol NaO; 50 ml = 0.5 L 0.0 g NaO 1000mL mol 0.765mol NaO M = = =. M L 0.5 L ) ow many ml of 0.56 M Cl will contain 10.0 mol of Cl? Cl 10.0 mol Cl 1000 ml 0.56mol Cl = 9100 ml Molarity of ions Soluble ionic compounds completely dissociate in solution E.g. What is the molarity of ions in a 0.0 M CO solution? What is the molar concentration of the carbonate ions? 0.0mol CO mol 0.0 mol = = 0.0 M CO 0.0mol CO CO 0.0mol CO = = 0.0 M CO CO SOLUTION STOICIOMETRY Grams or Grams or L or M of soln moles given moles wanted L or M of soln g To go from g moles use MM = mol mole To go from L (or M) of soln moles use M = L 1. ow many L of 0.00 M CaCl is needed to react with.90 g PO? CaCl (aq) PO (aq) Ca (PO ) (s) 6Cl (aq) g PO mol PO mol CaCl L CaCl mol PO mol CaCl.90 g PO = 0.50 L CaCl 98.0 g PO mol PO 0.00 mol CaCl. ow many grams of S can be produced from 15 ml of 0.55 M Cl solution? Cl (aq) S (aq) S (g) Cl (aq) ml Cl L Cl moles Cl moles S g S

6 0.55mol Cl S. 1g S 15 ml = 1.18 g S 1000 ml mol Cl mol S WORSEET FOR MOLARITY & SOLUTION STOICIOMETRY 1. What is the molarity of Na and PO ions in a 0.5 M solution of Na PO? 0.5mol NaPO mol Na NaPO PO NaPO = 0.75M Na = 0.5 M PO 0.5mol NaPO. Find the mass of NaCl present in 150 ml of 1.50 M NaCl mol 58.5 g NaCl 150 ml 1000 ml NaCl = 1. g NaCl. ow many ml of 0.5 M AgCl solution will contain.5 g of AgCl? AgCl.5 g AgCl AgCl 1000mL 1. g AgCl = 8.90 x10 ml AgCl 0.5mol AgCl. What is the molarity of SO solution if ml of SO is required to neutralize.00 ml of M NaO? SO NaO O Na SO ml NaO L NaO moles NaO moles SO M SO mol NaO SO.00 ml = moles SO 1000 ml mol NaO mole mol M = = SO 1000 ml L = M 50.00mL 5. ow many L of 0.16 M Ca(O) is needed to neutralize 5.00 ml of 0.58 M Cl solution? Ca(O) Cl CaCl O 0.58 moles Cl Ca( O ) 5.00 ml = 0.09 L 1000 ml L mol Cl 0.16mol Ca( O ) Titration- procedure used to determine the concentration of a solution by measuring the volume of one reagent required to react with a known mass or volume of another reagent. Standard solution solution with a known concentration Indicator substance that changes color at end point of titration Equivalence point pt at which the two reagents are present in stochiometrically equivalent amounts

7 DILUTION Dilution - process of adding more solvent to solution to prepare a more dilute solution. concentrated solution - a solution containing a relatively large amount of solute dilute solution - a solution containing a relatively small amount of solute. In dilution problems moles before dilution equal moles after dilution: moles 1 = moles Dilution formula: M 1 x V 1 = M x V 1) a) ow many ml of 16 M NO will you use to prepare 750. ml of 0.69 M NO? b) ow many ml of water were added to make this solution? M 1 = 0.69 M NO ; V 1 = 750 ml; M = 16 M NO ; V =? a) V = M 1V M 1 = ( 0.69 M )( 750 ml ) 16 M b) 750 ml - ml = 78 ml = ml ) What is the molarity of a solution prepared by diluting 15 ml of 0.00 M Cl to 1000 ml of Cl solution? M 1 = 0.00 M Cl; V 1 = 15 ml; M =?; V = 15 ml 875 ml = 1000 ml M = M 1V V 1 = ( 0.00 M )( 15mL ) 1000mL = M DON'T USE DILUTION FORMULA FOR SOLUTION STOICIOMETRY PROBLEMS!!!

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