An analytical chemist is titrating 163.3 mL of a 0.5200 M solution of piperidine (C;H1,NH) with a 0.1600 M solution of HNO3. The p K, of piperidine is 2.89.Calculate the pH of the base solution after the chemist has added 558.3 mL of the HNO, solution to it.Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added.Round your answer to 2 decimal places.pH =

Given: Volume of piperidine = 163.3 mL Concentration of piperidine = 0.5200 M Volume of HNO3 = 558.3…

Answered: An analytical chemist is titrating…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 55P

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Weak base B has a pKb of 6.78 and weak acid HA has a pKa of 5.12. a Which is the stronger base, B or A? b Which is the stronger acid, HA or BH+? c Consider the following reaction: B(aq)+HA(aq)BH+(aq)+A(aq) Based on the information about the acid/base strengths for the species in this reaction, is this reaction favored to proceed more to the right or more to the left? Why? d An aqueous solution is made in which the concentration of weak base B is one half the concentration of its acidic salt, BHCl, where BH+ is the conjugate weak add of B. Calculate the pH of the solution. e An aqueous solution is made in which the concentration of weak acid HA twice the concentration of the sodium salt of the weak acid, NaA. Calculate the pH of the solution. f Assume the conjugate pairs B/BH+ and HA/A are capable of being used as color-based end point indicators in acidbase titrations, where B is the base form indicator and BH is the acid form indicator, and HA is the acid form indicator and A is the base form indicator. Select the indicator pair that would be best to use in each of the following titrations: (1) Titration of a strong acid with a strong base. (i) B/BH+ (ii) HA/A (2) Titration of a weak base with a strong acid. (i) B/BH+ (ii) HA/A
Write the chemical equation and the expression for the equilibrium constant, and calculate Kb for the reaction of each of the following ions as a base. (a) sulfate ion (b) citrate ion
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1. The ionization constant (Kb) of trimethylamine ((CH)3)3N) is 7.40 x 10–5. If 5.911 grams of trimethylamine is dissolved in 50.0 mL of water, what are the equilibrium concentration of all species present? 2. A buildup of a certain monoprotic acid in the muscle tissues can cause pain during extreme physical activities. A 0.0288 M solution of this acid is found to have a pH of 2.345. Based on the table below, what most likely is the identity of this unknown acid?
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The pH of a 1.00 M NaCH3COO (aq) solution is 9.38. a/ Determine the concentration of [OH-] in the solution. b/ Write the expression for the Kb of NaCH3COO (aq) and calculate its values. c/ Calculate the pKa of CH3COOH. d/ HCl (aq) is added to 1.00 L solution of 1.00 M NaCH3COO (aq). Write the chemical reaction between HCl (aq) and NaCH3COO (aq). e/ How many mol of HCl (aq) is needed to make a buffer solution with pH = 5.00 from 1.00 L of 1.00 M NaCH3COO (aq).

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