William L Masterton Cecile N. Hurley Edward J. Neth University of Connecticut Chapter 14 Equilibria in.
William L Masterton Cecile N. Hurley Edward J. Neth University of Connecticut Chapter 16 Precipitation.
Ch. 13 Equilibrium. Chemical Equilibrium Z The state where the concentrations of all reactants and products remain constant with time. Z On the molecular.
Section 15.4 Disturbing a Chemical Equilibrium Le Chateliers Principle Bill Vining SUNY Oneonta.
1 Buffer Capacity in Chemical Equilibrium How long can you hyperventilate before severe alkalosis sets in? Your blood pH is controlled (buffered) within.
We will call μ the Chemical Potential Right now we will think of it as the molar free energy, but we will refine this definition later… Free Energy.
Strong Acids/ Bases Strong Acids more readily release H+ into water, they more fully dissociate –H 2 SO 4 2 H + + SO 4 2- Strong Bases more readily release.
Acids and Bases Acid-Base chemistry –important in our everyday lives acidity of our blood is carefully controlled making sulfuric acid is an important.
17.1 Liquid – vapour equilibrium 17.1.1 Describe the equilibrium established between a liquid and its own vapour and how it is affected by temperature.
Equilibrium Calculations. How can we describe an equilibrium system mathematically? reactants products ⇌ reactants The Keq is the equilibrium constant-
Reaction Quotient-Q- Or Trial K. The Keq is a constant- a number that does not change Increasing the Temperature of an endothermic equilibrium shifts.
Aqueous Solutions and the Concept of pH Chapter 16.