Solutions and pH Chapter 2.

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Presentation transcript:

Solutions and pH Chapter 2

Definitions: 1. Solution = a mixture in which one or more substances is distributed in another. 2. Solute = the substance dissolved in the solution 3. Solvent = substance in which the solute is dissolved

**Acids and bases are created due to dissociation. **DISSOCIATION = Breaking apart of water molecules H2O = H+ and OH- Hydrogen Ion Hydroxide Ion

If the number of HYDROGEN IONS is greater than the number of hydroxide ions, the solution is an . . . Acid Ion = an atom or molecule with a net electric charge due to the loss or gain of one or more electrons. H+ > OH-

If the number of HYDROXIDE IONS is greater than hydrogen ions, the solution is a . . . Base OH- > H+

Scientist have developed a Scale to compare the concentration of H+ ions to OH- Ions in Solution called the pH SCALE.

pH Scale Scale ranges from 0 to 14 0=more acidic 7=neutral 14= more basic

---------------------------------------------------------------- The strength of an acid or base is measured on the pH scale. The term “pH” is short for “potential of hydrogen.” It is a measure of how many excess H+ ions there are in a solution. The pH scale runs from 0 to 14, with 0 representing the highest concentration of hydrogen ions. Acidic substances have a pH below 7, while alkaline substances (bases) have a pH above 7. Pure water has a pH of 7 and is considered neutral. ---------------------------------------------------------------- Find the pH of several different substances at the lab tables.

=Chemical substances that Buffers =Chemical substances that neutralize small amounts of either an acid or a base EX: human blood contains a buffer called carbonic acid (H2CO3) and bicarbonate anion (HCO3-). These buffers help to maintain blood pH levels so that they stay between 7.35 and 7.45.

Buffers

Buffers (first 2 mins)