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IONIC COMPOUNDS Chapter 5

K + (aq) + MnO 4 - (aq). IONIC COMPOUNDS Chapter 5. Many reactions involve ionic compounds, especially reactions in water — aqueous solutions. KMnO 4 in water. An Ionic Compound, CuCl 2 , in Water. Aqueous Solutions. How do we know ions are present in aqueous solutions?

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IONIC COMPOUNDS Chapter 5

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  1. K+(aq) + MnO4-(aq) IONIC COMPOUNDSChapter 5 Many reactions involve ionic compounds, especially reactions in water — aqueous solutions. KMnO4 in water

  2. An Ionic Compound, CuCl2, in Water

  3. Aqueous Solutions How do we know ions are present in aqueous solutions? The solutions conduct electricity! They are called ELECTROLYTES HCl, MgCl2, and NaCl are strong electrolytes. They dissociate completely (or nearly so) into ions.

  4. Aqueous Solutions HCl, MgCl2, and NaCl are strong electrolytes. They dissociate completely (or nearly so) into ions.

  5. Aqueous Solutions Acetic acid ionizes only to a small extent, so it is a weak electrolyte. CH3CO2H(aq) ---> CH3CO2-(aq) + H+(aq)

  6. Aqueous Solutions Acetic acid ionizes only to a small extent, so it is a weak electrolyte. CH3CO2H(aq) ---> CH3CO2-(aq) + H+(aq)

  7. Aqueous Solutions Some compounds dissolve in water but do not conduct electricity. They are called nonelectrolytes. Examples include: sugar ethanol ethylene glycol

  8. Water Solubility of Ionic Compounds If one ion from the “Soluble Compd.” list is present in a compound, the compound is water soluble. Screen 5.4 & Figure 5.1 Guidelines to predict the solubility of ionic compounds

  9. Iron pyrite, a sulfide Orpiment, arsenic sulfide Azurite, a copper carbonate Water Solubility of Ionic Compounds Common minerals are often formed with anions that lead to insolubility: sulfide fluoride carbonate oxide

  10. HNO3 ACIDS An acid -------> H+ in water Some strongacids are HCl hydrochloric H2SO4 sulfuric HClO4 perchloric HNO3 nitric

  11. ACIDS An acid -------> H+ in water HCl(aq) ---> H+(aq) + Cl-(aq)

  12. HCl - Cl H O + H O 2 3 hydronium ion The Nature of Acids

  13. Acetic acid Weak Acids WEAK ACIDS = weak electrolytes CH3CO2H acetic acid H2CO3 carbonic acid H3PO4 phosphoric acid HF hydrofluoric acid

  14. ACIDS Nonmetal oxides can be acids CO2(aq) + H2O(liq) ---> H2CO3(aq) SO3(aq) + H2O(liq) ---> H2SO4(aq) and can come from burning coal and oil.

  15. BASESsee Screen 5.9 and Table 5.2 Base ---> OH- in water NaOH(aq) ---> Na+(aq) + OH-(aq) NaOH is a strong base

  16. Ammonia, NH3An Important Base

  17. BASES Metal oxides are bases CaO(s) + H2O(liq) --> Ca(OH)2(aq) CaO in water. Indicator shows solution is basic.

  18. Know the strong acids & bases!

  19. Net Ionic Equations Mg(s) + 2 HCl(aq) --> H2(g) + MgCl2(aq) We really should write Mg(s) + 2 H+(aq) + 2 Cl-(aq) ---> H2(g) + Mg2+(aq) + 2 Cl-(aq) The two Cl- ions are SPECTATOR IONS — they do not participate. Could have used NO3-.

  20. Net Ionic Equations Mg(s) + 2 HCl(aq) --> H2(g) + MgCl2(aq) Mg(s) + 2 H+(aq) + 2 Cl-(aq) ---> H2(g) + Mg2+(aq) + 2 Cl-(aq) We leave the spectator ions out — Mg(s) + 2 H+(aq) ---> H2(g) + Mg2+(aq) to give the NET IONIC EQUATION

  21. Chemical Reactions in WaterSections 5.2 & 5.4-5.6—CD-ROM Ch. 5 Pb(NO3) 2(aq) + 2 KI(aq) ----> PbI2(s) + 2 KNO3 (aq) We will look at EXCHANGE REACTIONS The anions exchange places between cations.

  22. Precipitation Reactions The “driving force” is the formation of an insoluble compound — a precipitate. Pb(NO3)2(aq) + 2 KI(aq) -----> 2 KNO3(aq) + PbI2(s) Net ionic equation Pb2+(aq) + 2 I-(aq) ---> PbI2(s)

  23. Acid-Base Reactions • The “driving force” is the formation of water. NaOH(aq) + HCl(aq) ---> NaCl(aq) + H2O(liq) • Net ionic equation OH-(aq) + H+(aq) ---> H2O(liq) • This applies to ALL reactions of STRONG acids and bases.

  24. Acid-Base Reactions CCR, page 162

  25. Acid-Base Reactions • A-B reactions are sometimes called NEUTRALIZATIONSbecause the solution is neither acidic nor basic at the end. • The other product of the A-B reaction is a SALT, MX. HX + MOH ---> MX + H2O Mn+ comes from base &Xn- comes from acid This is one way to make ionic compounds!

  26. Gas-Forming Reactions This is primarily the chemistry of metal carbonates. CO2 and water ---> H2CO3 H2CO3(aq) + Ca2+ ---> 2 H+(aq) + CaCO3(s) (limestone) Adding acid reverses this reaction. MCO3 + acid ---> CO2 + salt

  27. Gas-Forming Reactions CaCO3(s) + H2SO4(aq) ---> 2 CaSO4(s) + H2CO3(aq) Carbonic acid is unstable and forms CO2 & H2O H2CO3(aq) ---> CO2 (g) + water (Antacid tablet has citric acid + NaHCO3)

  28. See also: Gas Forming Reactions in Biological Systems Three of the pioneers in working out the roles of NO forming reactions shared a Nobel Prize in 1988 for their discoveries.

  29. Quantitative Aspects of Reactions in SolutionSections 5.8-5.10

  30. Terminology In solution we need to define the - • SOLVENT the component whose physical state is preserved when solution forms • SOLUTE the other solution component

  31. moles solute ( M ) = Molarity liters of solution Concentration of Solute The amount of solute in a solution is given by its concentration. Concentration (M) = [ …]

  32. 1.0 L of water was used to make 1.0 L of solution. Notice the water left over. CCR, page 177

  33. PROBLEM: Dissolve 5.00 g of NiCl2•6 H2O in enough water to make 250 mL of solution. Calculate molarity. Step 1: Calculate moles of NiCl2•6H2O Step 2: Calculate molarity [NiCl2•6 H2O] = 0.0841 M

  34. The Nature of a CuCl2 SolutionIon Concentrations CuCl2(aq) --> Cu2+(aq) + 2 Cl-(aq) If [CuCl2] = 0.30 M, then [Cu2+] = 0.30 M [Cl-] = 2 x 0.30 M

  35. moles = M•V USING MOLARITY What mass of oxalic acid, H2C2O4, is required to make 250. mL of a 0.0500 M solution? Because Conc (M) = moles/volume = mol/V this means that

  36. USING MOLARITY What mass of oxalic acid, H2C2O4, is required to make 250. mL of a 0.0500 M solution? Step 1: Calculate moles of acid required. (0.0500 mol/L)(0.250 L) = 0.0125 mol Step 2: Calculate mass of acid required. (0.0125 mol )(90.00 g/mol) = 1.13 g moles = M•V

  37. Preparing Solutions • Weigh out a solid solute and dissolve in a given quantity of solvent. • Dilute a concentrated solution to give one that is less concentrated.

  38. PROBLEM: You have 50.0 mL of 3.0 M NaOH and you want 0.50 M NaOH. What do you do? Add water to the 3.0 M solution to lower its concentration to 0.50 M Dilute the solution!

  39. PROBLEM: You have 50.0 mL of 3.0 M NaOH and you want 0.50 M NaOH. What do you do? But how much water do we add?

  40. moles of NaOH in ORIGINAL solution = moles of NaOH in FINAL solution PROBLEM: You have 50.0 mL of 3.0 M NaOH and you want 0.50 M NaOH. What do you do? How much water is added? The important point is that --->

  41. PROBLEM: You have 50.0 mL of 3.0 M NaOH and you want 0.50 M NaOH. What do you do? Amount of NaOH in original solution = M • V = (3.0 mol/L)(0.050 L) = 0.15 mol NaOH Amount of NaOH in final solution must also = 0.15 mol NaOH 0.15/Volume of final solution = 0.5 M/ 1 L Volume of final solution = (0.15 mol NaOH)(1 L/0.50 mol) = 0.30 L or 300 mL

  42. PROBLEM: You have 50.0 mL of 3.0 M NaOH and you want 0.50 M NaOH. What do you do? Conclusion: add 250 mL of water to 50.0 mL of 3.0 M NaOH to make 300 mL of 0.50 M NaOH.

  43. Preparing Solutions by Dilution A shortcut Cinitial • Vinitial = Cfinal • Vfinal

  44. The pH Scale pH = log (1/ [H+]) = - log [H+] Remember : log a = b if 10b=a In a neutral solution, [H+] = [OH-] = 1.00 x 10-7 M at 25 oC pH = - log [H+] = -log (1.00 x 10-7) = - (-7) = 7 See CD Screen 5.17 for a tutorial

  45. pH, a Concentration Scale pH: a way to express acidity -- the concentration of H+ in solution. Low pH: high [H+] High pH: low [H+] Acidic solution pH < 7 Neutral pH = 7 Basic solution pH > 7

  46. [H+] and pH If the [H+] of soda is 1.6 x 10-3 M, the pH is ____? Because pH = - log [H+] then pH= - log (1.6 x 10-3) pH = - (-2.80) pH = 2.80 What’s the origin of the name of the soda 7up ?

  47. Oxalic acid, H2C2O4 ACID-BASE REACTIONSTitrations H2C2O4(aq) + 2 NaOH(aq) ---> acidbase Na2C2O4(aq) + 2 H2O(liq) Carry out this reaction using a TITRATION.

  48. Setup for titrating an acid with a base CCR, page 186

  49. Titration 1. Add solution from the buret. 2. Reagent (base) reacts with compound (acid) in solution in the flask. 3. Indicator shows when exact stoichiometric reaction has occurred. 4. Net ionic equation H+ + OH- --> H2O 5. At equivalence point moles H+ = moles OH-

  50. LAB PROBLEM #1: Standardize a solution of NaOH — i.e., accurately determine its concentration. 1.065 g of H2C2O4 (oxalic acid) requires 35.62 mL of NaOH for titration to an equivalence point. What is the concentration of the NaOH?

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