Calculate the pH when 20.0 mL of 0.200M ethylamine (C2H5NH2) are titrated with 10.0 mL of 0.300M nitric acid. Kb for ethylamine is 1.1Ã10-6.
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Part A Aspirin (acetylsalicylic acid, C9H8O4) is a weak monoprotic acid. To determine its acid-dissociation constant, a student dissolved 2.00 g of aspirin in 0.600 L of water and measured the pH. What was the Ka value calculated by the student if the pH of the solution was 2.60? Express your answer numerically using two significant figures. Hints Ka = SubmitMy AnswersGive Up Part B A 0.100 M solution of ethylamine (C2H5NH2) has a pH of 11.87. Calculate the Kb for ethylamine. Express your answer numerically using two significant figures. Hints Kb = SubmitMy AnswersGive Up
The pH of an aqueous solution of 0.538 M ethylamine (a weak base with the formula C2H5NH2) is __________.
The hydroxide ion concentration, [OH-], of an aqueous solution of 0.538 M ammonia, Kb = 1.8Ã10-5 is:
[OH-] = _____ M.
A 25.0-mL sample of 0.10 M C2H3NH2 (ethylamine) is titrated with 0.15 M HCl. What is the pH of the solution after 9.00 mL of acid have been added to the amine? Kb = 6.5 Ã 10-4
The correct answer is 10.88 but I am unsure about how to get there.