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Lab Final Review

This guide covers lab questions, terms, calculations, safety rules, and scientific report writing. Learn about measurements, compounds, formulas, reactions, spectroscopy, and redox reactions.

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Lab Final Review

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  1. Lab Final Review Spring 2012 Chem 1111

  2. Format • Definitions, calculations, short answer, True/false • Questions from all labs • Know terms and calculations associated with each experiment; Safety precautions • Know glassware and equipment used throughout semester. • Parts of a Scientific Report: Writing Lab Reports and Scientific Papers - Know what goes into each part

  3. Safety Rules • MSDS What is it and what info is in it • Techniques and procedures • Plotting Data and the meaning of a graph

  4. Exp 1C –Some Measurements of Mass and Volume • Know how to correctly measure volume, mass • Uncertain digits!!! • Calculate density • Use correct sigfigs • How to use standard deviation on a set of data

  5. Math for Chemistry: Dimensional Analysis • Know how to perform all calculations • Density, mols, molecular weight, concentration, % water, % yield, hydrates, titrations

  6. Exp 1A – Identification of An Unknown Compound • Physical vs. chemical properties • How density and boiling point are useful in identifying unknown liquids • How to use critical thinking and the process of elimination to identify unknowns from sets of reactions

  7. Exp 3A – The Empirical Formula of an Oxide • Know the difference between mixtures, elements, pure substances. • Heating, Combustion/ignition techniques • Know the sequence of calculations: • Stoichiometry • Mass and %

  8. Exp 3B – Hydrates and their Thermal Decompositions • Calculate % water • Calculate formula of hydrate

  9. Exp 4A – Conductivity of Aqueous Solutions • Indications of a reaction • Types of reactions observed • Balance chemical equations • Write Ionic Equations • Know the effects of adding two solutions of ionic compounds, additivity principle, solutions of an acid and a base

  10. Exp 4B – Ionic Reactions in Aqueous Solutions • Write and Balance Ionic Equations, net ionic equations • Use solubility tables to predict formation of precipitates • Compare results to identify an unknown

  11. Exp 4C – How Much Acetic Acid is in Vinegar? • Know what a titration is and why we do them. • Macid Vacid = Mbase Vbase for a mole ratio of 1:1 • Macid Vacid x b moles = Mbase Vbase for a mole ratio other than 1:1 • Difference between endpoint and equivalence point • Role of indicator and pH in titration • Calculations for % acid • Study the links on titration technique

  12. Exp.9 – Analysis of KClO3 – KCl mixture • Molar ratio concept • Calculate moles of product from moles of reactant and balanced equation.

  13. Exp 7 – The Absorption Spectrum of CoCl2 • Beer’s Law – in words and as an equation • The meaning of a standard curve • How to use linear regression • How to find standard deviation and use it in reporting experimental values • How a spectrophotometer works

  14. Exp 9A – The Identity of an Insoluble Precipitate • Know how to use stoichiometry to calculate limiting reagents • Use ratios to identify the product • Draw Lewis structures of related ions

  15. Exp 6 – Thermochemistry and Hess’s Law • Exothermic vs. endothermic • Basis for calorimetry • Free energy, entropy, enthalpy (temp change) • Draw a cooling/heating curve and extrapolate values

  16. Exp 19A – Oxidation – Reduction Reactions • Identify: • Substance oxidized, reduced • Reducing agent, oxidizing agent • Make inferences from observed changes

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