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Comprehensive Review of Key Chemistry Laboratory Experiments and Concepts

This review covers essential laboratory experiments in AP Chemistry, including reactions between metals and acids, empirical formulas, and hydration states. It explores the activity series, yields, Hess's law, and freezing-point depression, alongside kinetic studies and molecular shapes. The significance of electrolytes, acid-base titrations, and Graham’s Law in understanding solutions and reaction rates is emphasized. Detailed calculations and scientific principles underpin each experiment, providing a holistic overview to reinforce student comprehension in chemistry.

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Comprehensive Review of Key Chemistry Laboratory Experiments and Concepts

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  1. AP CHEMISTRY • LAB REVIEW

  2. Exp 1 • Zn + 2HCl  ZnCl2 + H2 • Cu + HCl  NO Reaction • Activity Series

  3. Exp 3 • Empirical Formula • ____g Cu / 63.5 = mol • ____g I / 126.9 = mol • Then divide by the smaller. • Iodine makes violet vapors

  4. EXP 4a % Composition • 2KClO3(s) 2KCl(s) + 3O2(g) • g of O2 lost x 100 =%O2 • g of KClO3 started

  5. EXP 6a Hydrates • 1.28g CuSO4 /159.6 g/mol = 0.00802 mol • 0.72g H2O / 18.0 g/mol = 0.0400 mol • 0.00802 mol / 0.00802 mol = 1 • 0.0400 mol / 0.00802 mol = 5CuSO4.5H2O • Copper(II) sulfate pentahydrate

  6. hydrated anhydrous

  7. EXP 6 % YIELD • Cu + 4HNO3 Cu(NO3)2+2NO2 +2H2O • Cu + 4H+ + 2NO3-  Cu2+ + 2NO2 + 2H2O p11

  8. Exp 6 • Zn + CuSO4 ZnSO4 + Cu • Blue Clear • %yield =exp/calc x 100

  9. EXP 9 Rates of Evaporations • IONIC • ION-ION • COVALENT • NONPOLAR-LDF • POLAR – DIPOLE-DIPOLE and HYDROGEN BONDING • Evaporation is a cooling process!

  10. EXP 12HESS’S LAW

  11. EXP 14 • ACTIVITY SERIES • USE THE STANDARD REDUCTION POTENTIALS

  12. EXP 15FREEZING-POINT DEPRESSION Temp Time

  13. EXP 15 • ΔT = Kf x m • MW = g1 x 1000g/kg g2 x m g1 = solute g2 = solvent m = molality

  14. EXP 17KINETICS • 0TH order [conc] Time

  15. EXP 17 • 1st order ln [conc] Time

  16. EXP 17 • 2nd order 1/[CONC] Time

  17. Exp 21Conductivity from Chem I

  18. EXP 21 • GOOD electrolytes • Strong acids and bases • Salts dissolved in water (aqueous) • Molten salts • Metals • Ions must be able to flow.

  19. EXP 21 • Poor or Weak electrolytes • Weak acids and bases • Tap water

  20. EXP 21 • NDC • DISTILLED WATER • SUGAR WATER • COVALENT COMPOUNDS • Solid salts

  21. EXP 21Ka of a WEAK ACID • pH = pKa at ½ of the equivalence point pH 7- ml of NaOH added

  22. EXP 22aShapes of Molecules • Know the VSEPR Theory card • Know polarity • Know hybrid orbitals • Bond angles

  23. EXP 23Titration Curves • Strong acid vs strong base pH 7- ml of NaOH added

  24. EXP 23 • STRONG ACID vs WEAK BASE pH 7- ml of NH4OH added

  25. EXP 23 • Weak Acid vs Weak Base pH 7- ml of NH4OH added

  26. EXP 23 • H3PO4 vs NaOH pH 7- ml of NaOH added

  27. EXP 24GRAHAM’S LAW • NH3(g) + HCl(g) NH4Cl(s) HCl NH3

  28. EXP 25 • Heat of Neutralization • q = m Cp ΔT • Then divide by the # of moles of water produced. Measured in kJ/mol

  29. EXP 26KINETICS • [S2O82-] [I-] Rate (M/s) • 0.10M 0.10M 5 • 0.10M 0.20M 10 • 0.20M 0.10M 10 Rate = k[S2O82-]1[I-]1

  30. EXP 29 • P1V1/T1 = P2V2/T2 • Subtract out the vapor pressure (Dalton’s Law) • . . • (collected over water) • 1 mole any gas = 22.4 liter (@ STP) Press inside = press outside only if water levels =.

  31. EXP 30MW of a Vapor • MW = mRT PV

  32. EXP 31 (from Chem I)Solubility of KNO3 • Solute + solvent + heat  solution • Endothermic if increase solubility with increasing temperature. g KNO3/100g of water Temperature oC

  33. EXP 33 Spec 20 • A = abcAbs & conc direct prop. • λ is set for the complimentary color of the solution. • Absorbance = 2 – log(%T) • Solution must have a color.

  34. EXP 37 • ISOMERS

  35. Structural isomers • n-pentane • 2-methyl butane • 2,2- • dimethylpropane

  36. Optical isomers

  37. Geometric isomers (cis-trans)

  38. Functional isomers

  39. EXP 41HYDROLYSIS • Salt + water  acid + base

  40. EXP 42ACID-BASE TITRATION • ACID + BASE  SALT + WATER • (#H)M1V1 = M2V2(#OH) • Indicator is phenolphthalein • KHP is a standard

  41. EXP 43EQUATIONS • SOLUBILITY RULES • YELLOW PPT • PbI2 • PbCrO4

  42. EXP 44RED-OX TITRATION • FeSO4 + KMnO4 + H2SO4 Fe2(SO4)3 + MnSO4 + K2SO4 + H2O

  43. Exp 13Flame Test (from Chem I) • Na yellow • K lavender • Ca & Li & Sr red • Ba & Cu & B green

  44. Na+ K+ Sr2+ Ba2+ Cu2+ Se

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