A 150.0 ml sample of ethylamine has a pH of 11.55. K-4.3x10-5 [H₂p]. (a) What is the concentration of hydroxide ion present in the solution before titration? 2.81x10 = [H₂0] X (b) What is the initial molar concentration of the ethylamine solution? (c) The 150.0 mL sample is titrated with hydrochloric acid. The equivalence point is reached after 37.50 mL of the HCI solution is added. What is the concentration of the HCI solution? E₂H5NH₂ +H₂O →→→ CzHs NH3 + OH

A 150.0 ml sample of ethylamine has a pH of 11.55. K-4.3x10-5 [H₂p]. (a) What is the concentration of hydroxide ion present in the solution before titration? 2.81x10 = [H₂0] X (b) What is the initial molar concentration of the ethylamine solution? (c) The 150.0 mL sample is titrated with hydrochloric acid. The equivalence point is reached after 37.50 mL of the HCI solution is added. What is the concentration of the HCI solution? E₂H5NH₂ +H₂O →→→ CzHs NH3 + OH

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter4: Stoichiometry: Quantitative Information About Chemical Reactions

Section: Chapter Questions

Problem 111GQ: One half liter (500. mL) of 2.50 M HCl is mixed with 250. mL of 3.75 M HCl. Assuming the total...

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One half liter (500. mL) of 2.50 M HCl is mixed with 250. mL of 3.75 M HCl. Assuming the total solution volume after mixing is 750. mL, what is the concentration of hydrochloric acid in the resulting solution? What is its pH?
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In the following acid-base titration experiment NaOH(aq) + HNO3(aq) ———> NaNO3(aq) + H2O(1). What is the molarity of the HNO3 solution if 18.3 mL of 0.115 M NaOH was used to neutralize 25 mL of HNO3? (a) 0.157 M (b) 0.0842 M (c) 3.978 M (d) 0.0157 M
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