1 / 24

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

melva
Télécharger la présentation

SOLUTIONS

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  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

More Related