Acids, Bases, Salts, pH, Buffers, Indicators, Titration, Antacids

 Acids          Acids are substances which ionize in water solutions to produce hydrogen ion (H⁺ or free p+). Some ionize more than others. Acids taste sour and turn litmus red.

Bases          Bases are substances which ionize to produce hydroxide ions in water solutions. They taste bitter, feel slippery to the touch, and turn litmus blue.

Salts             Salts are crystalline compounds composed of the negative ions of an acid and the positive ions of a base.

Hydronium ion        H+ combines with a water molecule to form H₃0+     any solution containing hydronium ions is acidic and the strength of an acid is based on the number of hydronium ions in solution.

 Ionization          Ionization is the formation of ions in solution.

 Dissociation      Dissociation is the separation of ions in solution.

 Neutralization       Neutralization is the reaction of an acid and a base to form a salt plus water.

 Hydrolysis      Hydrolysis is a reaction of a salt with water to form a weak acid or base.

 Titration     Titration is a technique for measuring the relative strength of a solution.

 Endpoint      Endpoint is the point in a titration where equal amounts of reactants are present.

 Buffer      A buffer is a solution which can receive moderate amounts of of either acid or base without significant changes in pH.

 Indicator      An indicator is used to indicate the pH of a solution.

pH or pOH      pH is the negative log of the hydrogen ion concentration.          In-depth look at math behind pH

 pOH is the negative log of the hydroxide ion concentration.

 A weak acid/base ionizes only slightly in solution whereas a strong acid/base completely ionizes (dissociates) into positive and negative ions in solution.

 

Demonstration Procedure:

 I. heat 75 mL of 0.1 M HCI on hot plate

II. crush antacid tablet and add this to acid

III. add solution to graduated cylinder with enough water to have 100 mL

IV. place 25 mL of solution in Erlenmeyer flask

V. add phenolphthalein as indicator

VI. titrate with 0.1 M NaOH to endpoint

VII. test solution with calibrated pH meter (using buffer solutions)