CHEM 1A03 Study Guide - Final Guide: Dynamic Equilibrium, Exothermic Process, Nitric Acid

• School: McMaster University
• Department: Chemistry
• Course: CHEM 1A03
• Professor: David J.H.Emslie

Document Summary

Solids dissolve to some degree when placed in water. If we put lead iodide in water, some ions would go into solution. The equation and ksp for dissolution of lead iodide is shown: Already have lead dissolved, so not as much lead iodide needs to be dissolve to reach equilibrium, and solubility of lead iodide decreases also referred to common ion effect. Common ion effect where an ion which is part of the equilibrium is already present in the solution, and this impacts the equilibrium, in this case suppressing the dissolution of lead iodide. When a reaction is exothermic, it can be thought of as having heat as a product. Endothermic, heat can be thought as a reactant. Ha(cid:271)er bos(cid:272)h pro(cid:272)ess takes advantage of le chatelier"s principle. Le chatelier"s prin(cid:272)iple - states that when a system is in dynamic equilibrium, it will respond to an external stress by relieving the stress to re-establish an equilibrium state.