Carbon Dioxide

The octet rule cannot be satisfied for all compounds.

Dissociation reactions: Ammonia NH4 ? NH3 + H+

vinegar CH3COOH ? CH3COO- + H+

14.2a Many substances flip-flop color in result to the presence of an acid or an alkali: these are cognize as acid-base indications (Dice, 1998). Examples of commonly used indicators are litmus, phenolphthalein, thymol blue, alizarine yellow, and methyl orange. Acid-base indicators are dyes which are themselves weak acids or bases and their conflate acid-base forms have different colors. Most of the dyes have quite multiform chemical structures. The Bronsted-Lowry equation for the reaction with an indicator is:

HIn + H2O ? H3O+ + In-

At low pH, the indicator is almost entirely in the HIn form, and as the pH increases, the intensity of the color of In- increases as the equilibrium shifts to the right. opposite dyes will change color at different pHs, and pH paper commonly contains a mixture of indicator dyes that change color at different pHs.

The equivalence point for an indicator is the point at which the amount of H3O+ and OH- are equal, and it is important to carry an indicator that changes color near the equivalence point. This is the endpoint of a titration.

14.5a A logarithmic scale is used to describe the assimilation of hydrogen i

14.6a The acid in vinegar is acetic acid, CH3COOH: the acid in vitamin C is ascorbic acid, C6H8O7.

14.3b To measure a solution of club soda pop you would use ammonia, because soda contains carbon dioxide (carbonic acid), and is therefore acidic. You would need to titrate it with a base. vinegar is an acid, ammonia is a base.

Dice, D. (1998). Acid-base indicators. Retrieved at:

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