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SOLUTIONS

SOLUTIONS. SOLUTION: HOMOGENEOUS MIXTURE OF 2 OR MORE CHEMICAL SUBSTANCES. SOLUBILITY: MAXIMUM AMOUNT OF SOLUTE THAT CAN BE DISSOLVED AT A GIVEN TEMPERATURE. SATURATED VS. NON-SATURATED. CONCENTRATION: THE RELATIVE AMOUNT OF

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SOLUTIONS

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  1. SOLUTIONS

  2. SOLUTION: HOMOGENEOUS MIXTURE OF 2 OR MORE CHEMICAL SUBSTANCES SOLUBILITY: MAXIMUM AMOUNT OF SOLUTETHAT CAN BE DISSOLVED AT A GIVEN TEMPERATURE SATURATED VS. NON-SATURATED CONCENTRATION: THE RELATIVE AMOUNT OF SOLUTE IN THE SOLVENT OR IN THE SOLUTION DILUTE VS CONCENTRATED MISCIBLE VS IMMISCIBLE

  3. GRAMS OF SOLUTE 100 GRAMS SOLUTION x 100 MASS FRACTION = MASS OF SPECIES OF INTEREST TOTAL MASS OF MIXTURE x 100 = MASS % OR % (m/m) x 106 = PPM x 109 = PPB % (V/V) = ML OF SOLUTE 100 ML SOLUTION MOLARITY[M] = MOLES SOLUTE L SOLUTION

  4. Try these: • What is the molarity of a solution prepared by adding 5.0 g of NaCl to 300 mL of water? • How many mL of water are needed to make a 0.5 M solution of KCl?

  5. Lab Activity: Mix it UP!

  6. YOU HAVE 6.00 g NaCl IN 750 mL H2O. WHAT IS M AND MASS PERCENTAGE OF NaCl? 6.00 g NaCl x 1MOLE/58.4 g NaCl = 0.1027 MOL NaCl M = 0.1027 MOL NaCl/0.750 L SOLUTION MASS % NaCl = 6.00/(6.00+750) x 100 = 0.79% TO PREPARE A 5% SALINE SOLUTION, DISSOLVE 5 g NaCl IN 100 mL WATER. TRUE OR FALSE? FALSE! % (m/m) = 5 g NaCl/105 mL x 100 = 4.8% A 5% SOLUTION IS 5 g SOLUTE AND 95 mL WATER

  7. % (v/v) = 100 mL ALCOHOL 700 mL SOLUTION x 100 HOW MANY MOLES OF SALT (NaCl) ARE IN 40 mL OF 0.15 M NaCl SOLUTION? WHAT IS THE %(v/v), %(m/m) AND M WHEN 100 mL CH3OH IS ADDED TO 600 mL OF WATER? DENSITY = 0.79 g/mL 0.006 MOL = 14.2 % %(v/v) MASS CH3OH = 100 mL x 0.79 g/mL = 79.0 g %(m/m) = 79.0 g CH3OH / 679 g SOLUTION x 100 = 11.6 %(m/m) =2.47 MOL MOLES CH3OH = 79 g CH3OH x 1 MOL/32 g M = 2.47 MOL CH3OH/0.700 L WATER = 3.5 M CH3OH

  8. HOW MANY GRAMS OF CaCl2 ARE REQUIRED TO PREPARE 100 mL of 0.125 M SOLUTION? 0.125 M = 1.4 g CaCl2 WHAT IS THE MOLARITY OF THE Ca2+ AND Cl1- IONS IN THE ABOVE SOLUTION? 2 CaCl  Ca2+ + Cl1- 2 2 1 MOL CaCl2 X 2 MOL Cl1- /MOL M Ca2+ = 0.125 M M Cl1- = 0.250 M

  9. A(s) A H20 H20 H20 H20 A A A A A A A A H20 A A H20 H20 A H20 H20 H20 H20 H20 H20 H20 H20 H20 H20 H20 H20 H20 H20 H20 H20 H20 H20 A H20 H20 H20 (solution) (aq) HSOLUTION HSOLUTION = HSOLUTE + HSOLVENT + HMIXING HSOLVATION < 0 > 0 < 0 IF HSOLUTION > 0, THEN GSOLUTION< 0 LIKES DISSOLVE LIKES!!!

  10. ORGANIC COMPOUNDS: BASED ON CARBON HYDROPHOBIC VS HYDROPHILLIC GREASE & DIRT AGITATE AND OBTAIN MICELLES

  11. ELECTROLYTES OR NON-ELECTROLYTES SOLUTES: + H2O Na1+ (aq) + Cl1- (aq) CH3OH (aq) CH3OH + H2O SOLIDS GASES MOLECULAR COMPOUNDS NON-ELECTROLYTES:

  12. STRONG ELECTROLYTES WEAK TOTALLY DISSOCIATE INTO IONS STRONG ACIDS: HCl, HBr, HI, HNO3, H2SO4, HClO4 STRONG BASES: SOLUBLE METAL HYDROXIDES SOLUBLE IONIC COMPOUNDS PARTIALLY DISSOCIATE INTO IONS ALL OTHER ELECTROLYTES!!! RELATES TO ION-ION INTERACTIONS: HIGH CHARGE, LESS SOLUBLE

  13. SOLUBILITY “RULES” 1. GROUP 1A METAL ION AND NH41+ CPDS - ALL SOLUBLE 2. NO31-, ClO41-, ClO31-, AND ACETATE (C2H3021-) CPDS -- ALL SOLUBLE 3. Cl1-, Br1-, AND I1- CPDS -- SOLUBLE EXCEPT FOR Ag1+, Tl1+, Hg22+ AND Pb2+ 4. SO42- CPDS -- SOLUBLE EXCEPT FOR Ca2+, Sr2+, Ag1+, Ba2+ AND Pb2+ 5. MOST OTHER IONIC COMPOUNDS ARE INSOLUBLE

  14. BASED ON THE SOLUBILITY RULES, WHICH OF THE FOLLOWING ARE SOLUBLE: SOLUBLE SOLUBLE SOLUBLE SOLUBLE SOLUBLE Ca(OH)2 FeCl3 AgNO3 Ag2SO4 PbBr2 Pb(ClO4)2 K2SO4 K2S NiS CuSO3

  15. IN A SOLUTION OF EACH OF THE FOLLOWING, WHAT SPECIES ARE PRESENT: ALL IONS, ALL MOLECULES OR A MIXTURE OF IONS AND MOLECULES Cu(NO3)2 H2SO3 C12H22O12 NaOH ZnCl2 CO2 H1+ , HSO31-ANDH2SO3 Cu2+ AND NO31- Na1+ AND OH1- ALL MOLECULES ALL MOLECULES Zn2+ AND Cl1-

  16. CH4 + 2O2 2H2O + CO2 2Ag + S Ag2S Zn (s) + 2HCl (aq) ZnCl2 (aq) + H2 (g)  BaCl2 (aq) + Na2SO4 (aq) BaSO4 (s) + 2NaCl (aq) 2KClO3 2KCl + 3O2 CHEMICAL REACTIONS COMBINATION: SMALL TO LARGE LARGE TO SMALL DECOMPOSITION: COMBUSTION: DISPLACEMENT: SWAPPING CATIONS SINGLE: DOUBLE: NOTE:

  17. BaCl2 (aq) + Na2SO4 (aq) BaSO4 (s) + 2NaCl (aq) 4. SO42- CPDS -- SOLUBLE EXCEPT FOR Ca2+, Sr2+, Ba2+ AND Pb2+ 1. GROUP 1A METAL ION AND NH41+ CPDS - ALL SOLUBLE Ba2+(aq) + Cl1-(aq) + Na1+(aq) + SO42-(aq) BaSO4 (s) + Na1+(aq) + Cl1-(aq) Ba2+ (aq) + SO42- (aq) BaSO4 (s) 2 2 2 2 FOR AN IONIC REACTION TO OCCUR, ION(S)MUST BE REMOVEDFROM SOLUTION WEAK OR NON-ELECTROLYTE GAS SOLID (PRECIPITATE)

  18. Mg (s) + 2HCl (aq) MgCl2 + H2 Mg (s) + 2H1+ (aq) H2 + Mg2+ (aq) Pb(NO3)2 (aq) + (NH4)2CO3 (aq) PbCO3 + 2NH4NO3 Pb2+ (aq) + CO32- (aq) PbCO3 (s) HCl (aq) + KOH (aq) KCl + H2O H1+ (aq) + OH1- (aq) H2O (l) Rb2SO4 (aq) + MgCO3 (aq) Rb2CO3 + MgSO4 NO REACTION! (aq) (g) (s) (aq) (aq) (l) OR (aq) (aq) (aq)

  19. 1 QUALITATIVELY: KSP SOLUBILITY EQUILIBRIA …….. Sn3(PO4)2 (s) ↔ 3Sn2+ (aq) + 2PO43- (aq) [Sn2+]3 [PO43-]2 PRODUCTS REACTANTS K = SP SMALL VALUE, FEWER IONS LESS SOLUBLE SOLUBLE:  0.1 M SOLUTION SLIGHTLY SOLUBLE:  0.1 M  0.01 M SOLUTION INSOLUBLE:  0.01 M SOLUTON

  20. Lab: Soluble or Not?

  21. Net Ionic Equations from Lab

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