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Question 8Consider a sample of pure liquid water. Since the dissociation of water is[ Select ], as we increase the temperature theequilibrium constant will[ Select ]. Thus, at highertemperature the concentrations of both the hydronium ion and hydroxide ionwill increase. They will no longer be 1x10M; they will be slightly larger.However, the solution will still be neutral . This is because [H O ] is equal toAnswer 1:Answer 2:Answer 3:Answer 4:
3+equal toYes. The concentrations of [H O ] and [OH ] are the same in theproblem.3+
9/30/2018LE12 - Introduction to Acids and Bases: Fa18 - McCord CH302 (50015)10/110.5 / 0.5 ptsQuestion 9Use the following information to answer the remaining questions in thelearning exercise:A solution is neutral when __________.Neutral, Acidic, and BasicSolutions can be classified in comparison to pure water in terms of theconcentrations of HOand OH .In pure water:[H3O+] = [OH]NeutralWhen these concentrations are equal, the solution is neutral. Note, at roomtemperature this would be when [HO] = [OH ] = 1x10M.At other temperatures in a neutral solution, the concentrations of hydroxide andhydronium are still equal, but they will have a different numerical value.If the concentration of [HO] > [OH ], the solution is acidic.[H3O+] > [OH]AcidicIf the concentration of [HO] < [OH ], the solution is basic (or alkaline).[H3O+] < [OH]Basic3+-3+--73+-3+-[H O ] > [OH ]3+pH = 7[H O ] < [OH ]3+when only water molecules are in solution[H O ] = [OH ].3+Yes. The definition of neutrality in a solution is when the concentration ofthe hydronium ion is equal to that of the hydroxide ion.
9/30/2018LE12 - Introduction to Acids and Bases: Fa18 - McCord CH302 (50015)11/110.5 / 0.5 ptsQuestion 10At 25°C, you find that a solution has a hydronium ion concentration of 1.2 x10M. This solution would be considered:
Quiz Score:10out of 10
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