Distinguishing Acids and Bases donates H+ donates OH- accepts H+ Jennifer Simmons

Properties of Acids and Bases pH less than 7 corrosive, can feel irritating taste sour usually have H+ in formula react with metals neutralize bases pH higher than 7 feel slippery taste bitter often have OH- in formula dissolve oils and fats neutralize acids

Acids Donate Protons HNO3  H+ + NO3- H+ is donated by nitric acid, HNO3 H+ = proton The concentration of H+ determines pH Lower pH = higher concentrations of H+

Bases Accept Protons Na2CO3 + H+  HCO3- + 2 Na+ H+ is accepted by Na2CO3, a base The concentration of H+ determines pH Bases remove H+ from the solution, which raises the pH.

Formulas of Acids Since acids are H+ donors, their formulas can often be recognized by a leading H: HNO3 nitric acid H2CO3 carbonic acid HCl hydrochloric acid H2SO4 sulfuric acid HClO3 chloric acid

Formulas of Bases Bases that contain OH- can be recognized by their formula: NaOH sodium hydroxide KOH potassium hydroxide Mg(OH)2 magnesium hydroxide Ca(OH)2 calcium hydroxide Ba(OH)2 barium hydroxide

Reactions with Indicators Acids and bases react differently with chemicals known as indicators. We can use indicators to identify whether a substance is an acid or a base. There are 2 common indicators: Litmus Phenolphthalein

Litmus Indicator Litmus can be used to identify acids and bases: Blue litmus paper turns red in acids (stays blue in bases) Red litmus paper turns blue in bases (stays red in acids)

Phenolphthalein Indicator Phenolphthalein in a neutral solution is pale pink. Phenolphthalein turns colorless in an acid. Phenolphthalein turns dark pink in a base.