Chem7

Question 1

Acids and bases

Answer 1

Acids ar, stingy, and colourless in phenolphthalein. Bases are, slippery, and pink in phenolphthalein. Both acids and bases are aqueous, electrically conductive and they both change the pH of a solution. Acids release hydrogen when reacted with active metals and CO2 when reacted with carbonate. Binary acids are hydrogen with a nonmetal. The arrhenious theory says that acids ionized a hydrogen proton in water and Bases released a hydroxide in water. But that definition of a base was limited to ionic hydroxides and couldn’t explain oxides of metals or compounds with a hydroxide like ammonia. The definition of acid was limited to compounds containing hydrogen and couldn’t explain acidic compounds like nonmetal oxides. The bronsted lowry theory said that acids donated a proton and bases accepted a proton.
Hydroxides of all the group 1 and 2 metals exempt for barium are strong bases and disassociate completely in water. Ammonia and its derivatives are weak bases and do not disassociate completely in water. The strong bases are How Could Santa Have Big Houses In The North Pole. Water and some other things are Amphoterics. When acids react they form conjugate bases and when bases react they form conjugate acids.

Question 2

neutralization reactions

Answer 2

There are two others: Acid plus carbonate into carbon dioxide and salt and water, base plus ammonium into ammonia and salt and water. A titration uses one to finds an unknown concentration. For those you ignore any volumes that aren’t the right colour, or with 0.2 of each other. The volume of titrant that causes the solution to change colour is the endpoint. Ideally its as close as possible to the equivalency point, which is the volume where the moles of acid and base are equal. Take the average volume to turn it into a stoichiometric.

Question 3

How do acids taste

Answer 3

Sour