2. S O L U T I O N S

3. 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 SOLUTE IN THE SOLVENT OR IN THE SOLUTION DILUTE VS CONCENTRATED MISCIBLE VS IMMISCIBLE

4. x 100 = MASS % OR % (m/m) x 10 6 = PPM x 10 9 = PPB % (V/V) = ML OF SOLUTE 100 ML SOLUTION MOLARITY[M] = MOLES SOLUTE L SOLUTION MASS FRACTION = MASS OF SPECIES OF INTEREST TOTAL MASS OF MIXTURE GRAMS OF SOLUTE 100 GRAMS SOLUTION x 100

7. 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?

8. Lab Activity: Mix it UP! GroupMass (g)Volume(mL)Molarity 1 2 3 4 5 6 7 8 9 10 Totals

10. YOU HAVE 6.00 g NaCl IN 750 mL H 2 O. 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

11. HOW MANY MOLES OF SALT (NaCl) ARE IN 40 mL OF 0.15 M NaCl SOLUTION? 0.006 MOL % (v/v) = 100 mL ALCOHOL 700 mL SOLUTION x 100 = 14.2 % %(v/v) MASS CH 3 OH = 100 mL x 0.79 g/mL = 79.0 g %(m/m) = 79.0 g CH 3 OH / 679 g SOLUTION x 100 = 11.6 %(m/m) MOLES CH 3 OH = 79 g CH 3 OH x 1 MOL/32 g =2.47 MOL M = 2.47 MOL CH 3 OH/0.700 L WATER= 3.5 M CH 3 OH WHAT IS THE %(v/v), %(m/m) AND M WHEN 100 mL CH 3 OH IS ADDED TO 600 mL OF WATER? DENSITY = 0.79 g/mL

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

13. (solution)  H SOLUTION A(s) A(aq)  H SOLUTION =  H SOLUTE +  H SOLVENT +  H MIXING < 0 < 0 > 0 A H 2 0 A A A A H20H20 H20H20 H20H20 H20H20 H20H20 H20H20 H20H20 A H20H20 A H20H20 A H20H20 A IF  H SOLUTION > 0, THEN  G SOLUTION < 0  H SOLVATION LIKES DISSOLVE LIKES!!!

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

15. ELECTROLYTES OR NON-ELECTROLYTES SOLUTES: + H 2 O Na 1+ (aq) + Cl 1- (aq) CH 3 OH + H 2 O CH 3 OH (aq) NON-ELECTROLYTES: SOLIDS GASES MOLECULAR COMPOUNDS

16. STRONG ELECTROLYTES WEAK TOTALLY DISSOCIATE INTO IONS STRONG ACIDS: HCl, HBr, HI, HNO 3, H 2 SO 4, HClO 4 STRONG BASES: SOLUBLE METAL HYDROXIDES SOLUBLE IONIC COMPOUNDS ALL OTHER ELECTROLYTES!!! RELATES TO ION-ION INTERACTIONS: HIGH CHARGE, LESS SOLUBLE PARTIALLY DISSOCIATE INTO IONS

17. SOLUBILITY “RULES” 1. GROUP 1A METAL ION AND NH 4 1+ CPDS - ALL SOLUBLE 2. NO 3 1-, ClO 4 1-, ClO 3 1-, AND ACETATE (C 2 H 3 0 2 1- ) CPDS -- ALL SOLUBLE 3. Cl 1-, Br 1-, AND I 1- CPDS -- SOLUBLE EXCEPT FOR Ag 1+, Tl 1+, Hg 2 2+ AND Pb 2+ 4. SO 4 2- CPDS -- SOLUBLE EXCEPT FOR Ca 2+, Sr 2+, Ag 1+, Ba 2+ AND Pb 2+ 5. MOST OTHER IONIC COMPOUNDS ARE INSOLUBLE

18. BASED ON THE SOLUBILITY RULES, WHICH OF THE FOLLOWING ARE SOLUBLE: Ca(OH) 2 FeCl 3 AgNO 3 Ag 2 SO 4 PbBr 2 Pb(ClO 4 ) 2 K 2 SO 4 K 2 S NiSCuSO 3 SOLUBLE SOLUBLE

19. IN A SOLUTION OF EACH OF THE FOLLOWING, WHAT SPECIES ARE PRESENT: ALL IONS, ALL MOLECULES OR A MIXTURE OF IONS AND MOLECULES Cu(NO 3 ) 2 H 2 SO 3 C 12 H 22 O 12 NaOH ZnCl 2 CO 2 Cu 2+ AND NO 3 1- H 1+, HSO 3 1- AND H 2 SO 3 ALL MOLECULES Na 1+ AND OH 1- Zn 2+ AND Cl 1- ALL MOLECULES

20. CHEMICAL REACTIONS COMBINATION: SMALL TO LARGE CH 4 + 2O 2 2H 2 O + CO 2 2Ag + S Ag 2 S DECOMPOSITION: LARGE TO SMALL 2KClO 3 2KCl + 3O 2  COMBUSTION: DISPLACEMENT: SWAPPING CATIONS SINGLE: Zn (s) + 2HCl (aq) ZnCl 2 (aq) + H 2 (g) DOUBLE:BaCl 2 (aq) + Na 2 SO 4 (aq) BaSO 4 (s) + 2NaCl (aq) NOTE:

21. BaCl 2 (aq) + Na 2 SO 4 (aq) BaSO 4 (s) + 2NaCl (aq) 4. SO 4 2- CPDS -- SOLUBLE EXCEPT FOR Ca 2+, Sr 2+, Ba 2+ AND Pb 2+ 1. GROUP 1A METAL ION AND NH 4 1+ CPDS - ALL SOLUBLE Ba 2+ (aq) + Cl 1- (aq) + Na 1+ (aq) + SO 4 2- (aq) BaSO 4 (s) + Na 1+ (aq) + Cl 1- (aq) 2 2 2 Ba 2+ (aq) + SO 4 2- (aq) BaSO 4 (s) FOR AN IONIC REACTION TO OCCUR, ION(S) MUST BE REMOVED FROM SOLUTION GAS SOLID (PRECIPITATE) WEAK OR NON-ELECTROLYTE

22. Mg (s) + 2HCl (aq) MgCl 2 + H 2 (aq) (g) Mg (s) + 2H 1+ (aq) H 2 + Mg 2+ (aq) Pb(NO 3 ) 2 (aq) + (NH 4 ) 2 CO 3 (aq) PbCO 3 + 2NH 4 NO 3 (s) (aq) Pb 2+ (aq) + CO 3 2- (aq) PbCO 3 (s) HCl (aq) + KOH (aq) KCl + H 2 O(aq) (l) OR (aq) H 1+ (aq) + OH 1- (aq) H 2 O (l) Rb 2 SO 4 (aq) + MgCO 3 (aq) Rb 2 CO 3 + MgSO 4 (aq) NO REACTION!

23. QUALITATIVELY: SOLUBILITY EQUILIBRIA K SP Sn 3 (PO 4 ) 2 (s) ↔ 3Sn 2+ (aq) + 2PO 4 3- (aq) K = PRODUCTS REACTANTS [Sn 2+ ] 3 [PO 4 3- ] 2 1 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 ……..

24. Lab: Soluble or Not?

25. Net Ionic Equations from Lab