The top documents tagged [ice chart]

Applications of Aqueous Equilibria Common Ions When we dissolve acetic acid in water, the following equilibrium is established: –CH 3 COOH CH 3 COO -

ACID/BASE SOLUTIONS. What is an acid? Bronsted-Lowry definition: An acid is a proton donor. So, what’s a base? Bronsted-Lowry definition: A base is a.

Aqueous Equilibria Chapter 15 Applications of Aqueous Equilibria.

The End of Equilibrium! (well, for us!) 1. K sp What is the solubility of FeCO 3 ? Solubility = MAXIMUM amount of a compound that can dissolve in water.

Basic concepts: Acid-Base chemistry & pH 1.Recognizing acid/base and conjugate base/acid 2.Calculation of pH, pOH, [H 3 O + ], [OH - ] 3.Calculating pH.

Buffers AP Chemistry. Common Ion Effect Adding a common ion to an equilibrium system will shift the equilibrium forward or reverse. For a weak acid equilibrium.

Titration Curves What’s in the beaker. Always ask… What’s in the beaker? When I start the titration, there is only water and whatever it is I’m titrating.

Titration Example Problem Suppose that 10.0g of an unknown monoprotic weak acid, HA, is dissolved in 100 mL of water. To reach the equivalence point, 100.0mL.

IICWG-8, 22-26 Oct. 2007

Goes with chapter 19: Silberberg’s Principles of General Chemistry AP Chemistry Mrs. Laura Peck, 2013 1.

Indicators. Acid Base indicators Acid-base indicators can mark the end point of a titration by changing color. The equivalence point is defined.

Buffers