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Hippuric acid (HC9H8NO3), found in horse urine, has pKa=3.62. Part A Calculate the pH in 0.120 M hippuric acid. Express your answer using three significant figures. pH = 0.934 SubmitMy AnswersGive Up Incorrect; Try Again; 4 attempts remaining Part B Calculate the concentration of H3O+ in 0.120 M hippuric acid. Express your answer to two significant figures and include the appropriate units. SubmitMy AnswersGive Up Part C Calculate the concentration of C9H8NO−3 in 0.120 M hippuric acid. Express your answer to two significant figures and include the appropriate units. SubmitMy AnswersGive Up Part D Calculate the concentration of HC9H8NO3 in 0.120 M hippuric acid. Express your answer to two significant figures and include the appropriate units. SubmitMy AnswersGive Up Part E Calculate the concentration of OH− in 0.120 M hippuric acid. Express your answer to two significant figures and include the appropriate units. SubmitMy AnswersGive Up Part F Calculate the percent dissociation in 7.50×10−2 M hippuric acid. Express your answer to two significant figures and include the appropriate units.

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13 Dec 2019

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Related questions

To learn how to calculate ion concentrations in an aqueous solution of a strong diprotic acid.

Sulfuric acid, H2SO4, is a strong acid. Its complete dissociation in aqueous solution is represented as

H2SO4→H++HSO4−

A HSO4− anion can dissociate further by

HSO4−⇌H++SO42−

but the extent of dissociation is considerably less than 100%. The equilibrium constant for the second dissociation step is expressed as

Ka2=[H+][SO42−][HSO4−]=0.012

Part A

Calculate the concentration of H+ ions in a 0.010 M aqueous solution of sulfuric acid.

Express your answer to three decimal places and include the appropriate units.

Hints
[H+] =

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Part B

Calculate the concentration of SO42− ions in a 0.010 M aqueous solution of sulfuric acid.

Express your answer to four decimal places and include the appropriate units.

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[SO42−] =

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Part C

Calculate the concentration of HSO4− ions in a 0.010 M aqueous solution of sulfuric acid.

Express your answer to two significant figures and include the appropriate units.

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[HSO4−] =

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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

Potassium hydroxide is used to precipitate each of the cations from their respective solution. Determine the minimum concentration of KOHrequired for precipitation to begin in each case.

Part A

1.1×10−2 M CaCl2

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