Chemistry Titration Quiz

General Chemistry Lab: Introduction

• The lab covers topics like course syllabus, safety rules, glassware, and lab techniques.

Course Syllabus

• General Chemistry Lab 1 is a one-credit hour course offered in the first semester of 2024-2025.
• Prerequisites are General Chemistry.
• The textbook is a General Chemistry Lab Manual.
• Additional materials needed include a Moodle course, a scientific calculator, goggles, a lab coat, and gloves.

Course Aims and Description

• The lab is a practical freshman chemistry course teaching basic instrumental techniques (weighing, pipetting, titration, and glassware use).
• Students learn safety rules and lab calculations related to experiments.
• The lab introduces students to the basics of chemistry lab reactions and how to use lab tools and instruments.
• Students learn to use different laboratory glassware, basic instrumental techniques (weighing, pipetting, titration), safety rules and lab calculations.

Course Policies

• Class attendance is required.
• Three absences may result in failure.
• Quizzes may be given without prior notice.
• Missing coursework, tests, and exams will result in a loss of marks.
• Make-up exams are not offered.
• Copy-pasted reports will result in a loss of marks.

Course Outline and Calendar

• The course is divided into different weeks, each covering specific topics and experiments.
• Specific topics covered include introduction to chemical laboratory, preparation of solutions, standardization of sodium hydroxide and other solutions, volumetric analysis of vinegar, and more.
• Each week is matched with an experiment number.

Teaching Methods

• The course uses lab experiments, lab reports, independent work, and group work.

Assessment Measures

• Evaluation includes quizzes, homework, reports, and written exams.
• All reports are due one week after the experiment.

Grading System

• Reports account for 40% of the grade.
• Midterm exam accounts for 20%.
• Final exam comprises 30%.
• Evaluation and quizzes are 10% of the grade.

Lab Safety Rules

• Dress appropriately, tie back hair, and wear personal protective equipment (PPE) like gloves, goggles. Don't touch your eyes, nose, or mouth.
• Proper supervision is mandatory; do not perform experiments without instructor approval.
• Designate work areas
• Know your surroundings well (safety equipment, emergency numbers, etc)
• Food and drinks are not allowed in lab.
• Identify and handle hazardous materials safely.
• Handle hot glassware carefully.
• Clean up spills and broken glassware immediately.
• Wash your hands using soap and warm water after the lab.
• Maintain social distancing.

Glassware and Equipment

• Beaker: For carrying chemical reactions.
• Flask: For carrying chemical reactions.
• Test Tube: For carrying chemical reactions.
• Test Tube Rack: To hold test tubes.
• Graduated Cylinder: To measure volumes of liquids.
• Volumetric Flask: To prepare solutions with precise volumes.
• Burette: For measuring volumes (especially for titrations).
• Pipette: For accurate volume transfer.
• Pipette Fillers: To aid in filling pipettes.
• Crucible: For high-temperature reactions.
• Tongs: For handling hot glassware.
• Funnel: For transferring substances.
• Droppers: For precise liquid addition, drop-by-drop.
• Watch Glass: For weighing solids.
• Spatula: For transferring solids.
• Brush: For cleaning glassware.
• Glass Rod: For stirring solutions.
• Thermometer: For measuring temperatures.
• Clamp: For holding glassware.
• Ring Stand: To hold clamps, rings, and burettes.
• Wash Bottle: To carry solvents, must be labeled.
• Hotplate: For heating.
• Oven: For heating.
• Electronic (Analytical Balance): To measure mass and other quantities

Chemistry Lab Techniques

• Measure Mass: Use a balance, set it to zero, add the substance, and record the mass.
• Measure Volume: Use tools like burettes, pipettes, graduated cylinders, and volumetric flasks. Read the liquid meniscus at eye level.
• Measure Temperature: Immerse a thermometer in the liquid, wait until the level is stable and read the temperature from the scale.
• Filtration: A technique for separating solids from liquids using filter paper and funnels.

Experiment 4: Preparation of Solutions

• Objective: To prepare solutions using mass percent and molarity expressions.
• Concepts: Solutions, solute, solvent, mass percent, molarity, weight percent, volume percent, parts per million, normality, parts per billion.
• Procedure: Calculating and weighing the correct amount of solute and solvent, mixing until completely dissolved, and calculating the actual mass percent (m/m%) or molarity.

Experiment 7: Standardization of Sodium Thiosulfate Solution

• Objective: To recognize oxidation-reduction titration and to prepare and standardize a thiosulfate solution.
• Introduction: Titration is used for determining the concentration of an unknown solution through the slow addition of a known solution of the other reactant.
• Types of solutions:
  • Primary standard solutions maintain an accurate concentration. Ex: KIO₃, Na₂CO₃, KHP
  • Secondary standard solutions do not necessarily have accurate initial concentrations. Ex: NaOH
• Titration requirements:
  • Stoichiometric reaction is crucial to accurately measure unknown solutions.
  • Fast reaction with a clear endpoint to accurately find the unknown concentration.
  • No side reactions complicate the quantification of the titrant.
• Oxidation-reduction reactions: Oxidation/Reduction reactions are the type of reaction used in this redox titration. (OIL RIG)

Experiment 11: Standardization of Sodium Hydroxide Solution

• Objective: To standardize a sodium hydroxide (NaOH) solution.
• Introduction: Standard solutions have accurately known concentrations, used to determine the concentration of other solutions. This uses titration, a process where a known volume of one reagent is added to another until the reaction is complete.
• Properties of appropriate standards:
  • High Purity
  • Stable
  • Not hygroscopic
• Acid-base reactions and indicators: These are significant in finding the end point, a clear indication that the reaction is complete.

Experiment 12: Volumetric Analysis of Vinegar

• Objective: To determine the concentration of acetic acid in vinegar using molarity and mass percent.
• Concepts:
  • Vinegar is a solution containing acetic acid (CH₃COOH) in water
  • Titration is used to find the unknown concentration of acid(CH₃COOH).
  • Using standardized NaOH solution and a precise pH indicator, such as phenolphthalein

Experiment 10: Determining Molecular Mass of Solid from Freezing-point Depression

• Objective: To determine the molecular mass of a solid substance using the freezing-point depression method.
• Concepts: Colligative properties — properties of solutions that depend on the number of solute particles rather than their identity. This method utilizes the lowering of a solvent's freezing point when adding a solute.
• Procedure: The procedure in the video describes a laboratory experiment where the substance being tested is first dissolved in a solvent and then measured. The change in freezing point is measured and used to calculate the molar mass.

Experiment 6: Limiting Reactant

• Objective: To determine the limiting reactant in a precipitation reaction.
• Introduction: Limiting reactant is the reactant that is completely used and determines how much product is formed. Excess reactants are those left over at the end of the reaction.
• Chemical kinetics: The speeds of reactions can heavily influence the accuracy of identifying the limiting reactant, so understanding their kinetics could help determine its exact quantity.
• Precipitation reactions: Reactants that create an insoluble product are carried out to determine the limiting reactant.

Experiment 4: Water of Hydration

• Objective: To determine the moles of water of hydration in a crystalline compound.
• Introduction: Hydrates are substances where water is chemically bound to an ionic compound.

Experiment 4: Determination of CaCO3 in Lime Stones

• Objective: To determine the percentage of CaCO3 in limestone samples.
• Introduction and Concepts: Limestone and dolomite are carbonate minerals; therefore, when looking for CaCO3, we consider the material as entirely CaCO3.
• Back Titration: An indirect titration method involving a known excess of a reagent and its subsequent titration to determine the unknown's quantity. Used here because CaCO3 is a weak base against acid which makes finding the point of reaction very difficult.

Bleach Analysis (Experiment 8)

• Objective: To determine the available chlorine concentration in a bleach solution.
• Introduction and Concepts: Bleach is an oxidizing agent; therefore, the process of whitening or sterilization depends on the oxidation of agents such as NaOCl.
• Iodometry: The process of using a standard solution of Na₂S₂O₃ to determine the amount