Lesson 18 and 19:

In lesson 18, we continued going over acids, bases, and neutrals. Acids are substances that add H+ to solution, bases are substances that add OH- to solution, and neutral substances do not add H+ or OH- to solution. Something important to know is that H+ have just one proton. Also, some important definitions are first Arrhenius Definition of Acids and Bases: An acid is any substance that adds hydrogen ion (H+) to solutions. A base is any substance that adds hydroxide ion (OH- )to solution. The next definition is Bronsted-Lowery Definiton of Acids and Bases: An acid is a proton doner and a bass is a proton acceptor. You should know how to identify Acids, Bases, Conjugate Acids and bases in a chemical equation! Acids and Bases that break a part completely in solutions are called strong acids and bases and acids and bases that do not dissociate completely in solutions are called weak acids and weak bases!

Lesson 19 covered more pH. The pH scale is a logarithmic scale that describes the concentration of H+ ions in a solution. pH is related to (H+) by the formula: pH=-log(H+). Know how to solve equations using this! Next, water dissociates into H+ and OH- ions. (H2O ---> H+ + OH-). pH of water is 7, because in water the H+ concentration is equal to the OH- concentration. Homework below!

Homework:

 

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