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Lab Review for Final Exam. Experiment #1: Density Density = Mass/Volume Volume = length x width x height Units = g/mL or g/cc or g/cm 3 Density Column.

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Presentation on theme: "Lab Review for Final Exam. Experiment #1: Density Density = Mass/Volume Volume = length x width x height Units = g/mL or g/cc or g/cm 3 Density Column."— Presentation transcript:

1 Lab Review for Final Exam

2 Experiment #1: Density Density = Mass/Volume Volume = length x width x height Units = g/mL or g/cc or g/cm 3 Density Column

3 525 mL of water at 25 0 C (density = g/mL) is placed in a container. The water is then cooled to form ice at C (density = g/mL). What is the mass and volume of the ice?

4 Mass = 523 grams Volume = 571 mL

5 Experiment #2: Safety, General Equipment & Techniques Safety equipment Safety Techniques Laboratory equipment Glassware Separation Techniques Safety Shower

6 What is a buret used for?

7 For use with acid-base titrations To deliver the solution of known concentration in a titration

8 Experiment #3: Physical Measurements Volume = length x width x height Displacement Method Density = mass/volume Relative Uncertainty Absolute Uncertainty

9 How do you determine relative uncertainty?

10 Relative Uncertainty is the ratio of the absolute uncertainty of a measurement to the best estimate. It expresses the relative size of the uncertainty of a measurement (its precision). For example, The measurement cm

11 Experiment #4: Composition of a Heterogeneous Mixture Filtration Distillation Decanting Chromatography Electrolysis % Composition

12 How can a heterogeneous mixture be separated?

13 Heating Filtration

14 Experiment #5: Isotopes & Atomic Mass Atomic mass unit (amu) Weighted average of atomic mass from % Different molecule possibilities of isotopes

15 Define an atomic mass unit (amu)

16 1/12 the mass of 1 Carbon – 12 atom

17 Experiment #6: Empirical Formula of a Compound Empirical formula Molecular formula Structural formula Why add water after heating magnesium ribbon? Calculate empirical formula from mass Caffeine

18 What is the empirical formula of magnesium oxide?

19 MgO

20 Experiments #7 & #8: Quantitative Analysis of Hydrates Hydrate Calculate unknown value of a hydrate Calculate mass of water produced in a hydrate Calculate number of moles of water in a hydrate Methane hydrate When organic material decomposes it releases methane, also known as swamp gas. Combine water and swamp gas under low temperatures and high pressures and the result can be a frozen lattice-like substance called methane hydrate. This crystalline combination of a natural gas and water looks remarkably like ice but burns if lit with a flame.

21 If 16.4 grams of oxygen gas react with excess hydrogen, what mass of water is produced?

22 Mass = 18.5 grams

23 Experiment #9: Concentration of acetic acid in vinegar Titration definition & formula End point Calculate molarity Calculate concentration of unknown solution

24 If mL of M acetic acid is transferred into a volumetric flask and diluted to 5.00 x 10 2 mL, What is the concentration of the resulting solution?

25 Concentration = 1.00 x M

26 Experiment #10: Material value of a metal Ionic Bond Covalent Bond Metallic Bond Conductivity Electroplating Electrolysis Electronegativity Floating magnet

27 When the pennies were heated in the NaOH solution, a layer of zinc bonded to the copper penny. What type of bond would exist between the atoms of copper and zinc?

28 Metallic

29 Experiment #11: Molecular Geometry Lewis Structures Lone pairs Molecular geometry chart (review) Hybridization

30 How many lone pairs are on a sulfur atom in the sulfite ion, SO3 2- ?

31 1 lone pair

32 Experiments #12 & #13: Thermochemistry & Hess’ Law Thermochemistry Coffee & Milk solution – heat of solution q = mc ΔT Enthalpy Hess’ Law combustion

33 Gold has a specific heat of J/g 0 C. When a 5.00-g piece of gold absorbs 1.33J of heat, what is the change in temperature?

34 Temperature change = C


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