Rate of reaction lab. Iodine clock reaction. Lab will demonstrate how the chemical reaction will occur based on the time for a specific iodine-starch reaction to occur and show a positive reaction for iodine.

Define rate in terms of concentration and time. Determine that both are measurable. Use an example of the decomposition of a specific compound to outline how to determine the rate of the reaction. Show that the rate is a negative number due to decomposition. Note that the rate is always expressed as positive, even when decomposition. Discuss that the rate of reaction decreases during the course of a reaction.
Review and analyze homework questions and answers.

Prepare a free entry problem to be solved in class. From the formula to determine free energy, and some given numbers, have Joshua derive the entropy an enthalpy needed to solve th fee energy equation. Once each unknown is solved, substitute into the equation and solve for the free energy.Analyze the results and determine if the reaction will proceed spontaneously. View and discuss a AP video which involves Gibbs free enenergy.

Derive a single thermodynamic function which would allow the determination of a spontaneous reaction. Discuss why and how every substance possess free energy, but it is the changes in free energy, delta G, that are measured in chemical and physical reactions. The Gibbs fee energy formula is presented, viewed on a graph, and determined how each result on the graph determines whether the reaction will occur spontaneously or not. Spontaneous reactions are determined by whether G is less than zero, equal to zero, or greater than zero

Describe how buffers will adjust pH of a solution very slightly. Discuss why a buffered solution is resistant to change in the pH when an acid or base is added. Define a buffer in terms of added acid and conjugate base formation. Introduce a buffer problem: What is the pH of a solution that contains a given molarity of acetic acid and a given molarity of sodium acetate. Work through the problem completely, include the formation of an ICE table and derivation of the pH based on the new pH of the solution

Compare changes in blood pH and water pH when a small amount of acid is added to both. Define why a buffer solution works. List the requirements for a buffer solution. Discuss the acid and conjugate base of the acid. Use acetic acid as an example. Discuss the adjustment of the pH of acetic acid when acetate ion is added to the solution. Explain using common ion effect and LeChatekiers principle

Determine how to calculate an alternate method to determine if a formed salt will dissolve. Involves the determination of Q, the reaction quotient by analysis of the ions formed by by solubility the salt. The results will be compared to the solubility constant and then compared to one of the 3 concussions which can be determined. A sample problem will be solved.

Describe an define a metal ore. Determine that in order to utilize the metal from the ore, a series of chemical steps must be followed. Examples are used to best determine how to extract the metal by precipitin. The Reaction Quotient was presented and compared to the solubility constant of the solid in solution. An example description was started and comparisons made between Ksp and Q.

Use an example of a precipitate formation of silver acetate to describe and discuss the results of adding a common ion to the equilibrium solution of silver acetate. Introduce LeChatelier's principle. Define the principle in words and note that the equilibrium is shifted to the left when more product is added at equilibrium

introduce a solubility constant problem to be solved. Discuss and analyze all steps needed to properly solve for the Ksp. Introduce halide acids, and questions why the acid which should be the strongest is the weakest Bronsted acid. Determine the energy questions needed to be answered to best solve the problem. Discuss the bond dissociation energy and the electron attachment energy which would determine the acid strength. Set up a table and determine why and how the acids would be classified as weak or strong