Chemistry

Tutorial assignment introduces students to McGraw Hill's Chemistry Virtual Labs. In the tutorial, students will learn how to navigate the simulation, collect data in their lab notebook, and submit their completed experiment.

Students will observe and compare the buffer capacity for acetic acid, aqueous sodium chloride, and an acidic buffer solution using a pH meter. Students will calculate the pH of an acidic buffer solution using the Henderson-Hasselbalch equation.

Students will determine the enthalpy of neutralization for a strong acid–strong base reaction.

Students will determine the heat capacity for a coffee-cup calorimeter using heated water and chilled water.

Students will perform an iodine test on a potato solution and an onion solution.

Students will perform a Benedict's test, a Barfoed's test, and a Seliwanoff's test on three unknown solutions, where each solution contains one carbohydrate.

Students will be introduced to common laboratory safety equipment and learn the reasons behind each precaution and the importance of following the rules set by their lab instructor or supervisor.

Students will determine the freezing point of an aqueous solution at three different concentrations and graphically determine its van't Hoff factor.

Students will determine density of a plastic cube using caliper method, water displacement method, and suspension method.

Students will construct electrochemical cells and compare the reduction potential for metals. Students will construct concentration cells, graphically relate the voltage to the reaction quotient, and determine the concentration of an unknown solution.

Students will observe how changing only the concentration of the enzyme catalase affects the enzyme's total activity. Students will also observe how changing only the reaction's temperature will affect the catalase's activity.

Students will apply the Beer-Lambert law to create a calibration curve and calculate the value of the equilibrium constant for the formation of the iron(III) thiocyanate complex ion.

Students will react magnesium metal with concentrated hydrochloric acid to generate hydrogen gas, which is collected over water in an eudiometer tube. Students will calculate the value for the ideal gas constant.

Students will determine the distance each gas traveled through air and its diffusion rate and use Graham's law to calculate an experimental molar mass for a gas.

Students will calculate the initial rate of reaction at different concentrations and different temperatures to observe the effect of changing the concentration or temperature on reaction rates.

Students will use a top-loading balance to measure out a sample of sodium chloride.

Students measure the temperature using an alcohol thermometer to measure the temperature using both Celsius and Fahrenheit and graphically determine the relationship between the Fahrenheit and Celsius temperature scales.

Students will use rulers with different precisions to measure the diameter of different circles and be introduced to the concept of uncertainty in a measurement.

Students will learn how to identify the meniscus and measure the volume of water in a graduated cylinder.

Students will measure the volume of liquids using a buret and a pipet.

Students will prepare a stock solution by measuring out the required mass of copper(II) sulfate pentahydrate and then make an initial and subsequent dilution.

Students will observe the effects of osmosis and tonicity using synthetic and biological semipermeable membranes.

Students will conduct an experiment to determine the effectiveness of different types of commercially available antacids.

Students will perform a biuret test and a ninhydrin test on gelatin, albumin, and glycine solutions. Using their results, they will classify an unknown solution as an amino acid or a polypeptide.

Students will observe indications of a chemical change after mixing aqueous solutions or adding a metal to an aqueous solution. Students will classify the chemical reaction and identify the net ionic equation.

Students will combine mixtures of aqueous ionic compounds and look for indications of a chemical reaction. Then, they will determine the products for each chemical change and balance its chemical reaction.

Students will use the steps of the scientific method to design a controlled experiment to determine if pill bugs prefer sand or cornstarch, based on some observations that have already been established.

Students will combine six aqueous solutions in pairs and record their observations. Using qualitative analysis, students determine the identity of each solution and the cation in an unknown aqueous solution.

Students will identify the analytical wavelength of a blue, red, or yellow dye. Using several dye solutions, students will generate a calibration curve and use it to calculate the concentration of an unknown dye solution.

Students will react aqueous sodium carbonate with aqueous calcium chloride to produce calcium carbonate. Using vacuum filtration, students will collect the precipitate, dry it to a constant mass, and determine the percent yield.

Students will perform a titration using a standardized solution of sodium hydroxide to calculate the molarity of an acetic acid solution. Phenolphthalein is used as an indicator.

Students will perform a weak acid–strong base titration while monitoring the pH using a pH meter. Students will create a titration curve and use it to identify the unknown weak acid.

Students will perform a titration using potassium hydrogen phthalate (KHP) to standardize a solution of sodium hydroxide. Phenolphthalein is used as an indicator.

Students will use Lewis structures and VSEPR theory to predict shapes of small molecules and polyatomic ions.