8-39. (a) Write the chemical reactions whose equilibrium constants are K and K for imidazole and imidazole hydrochloride, respectively. (b) Calculate the pH of a solution prepared by mixing 1.00 g of imida- zole with 1.00 g of imidazole hydrochloride and diluting to 100.0 mL. (c) Calculate the pH of the solution if 2.30 mL of 1.07 M HC1O4 are added.

8-39. (a) Write the chemical reactions whose equilibrium constants are K and K for imidazole and imidazole hydrochloride, respectively. (b) Calculate the pH of a solution prepared by mixing 1.00 g of imida- zole with 1.00 g of imidazole hydrochloride and diluting to 100.0 mL. (c) Calculate the pH of the solution if 2.30 mL of 1.07 M HC1O4 are added.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The disinfectant phenol, C₆H₅OH, has a pKₐ of 10.0 in wa-ter, but 14.4 in methanol. (a) Why are the values different? (b) Is methanol is a stronger or weaker base than water? (c) Write the dissociation reaction of phenol in methanol. (d) Write an expres-sion for the autoionization constant of methanol.
COHSOH(ag) + H2On + CeHsO (aq) + H3O*(a9) Ka= 1.12 x 10-10 (a) Phenol is a weak acid that partially dissociates in water according to the equation above. Write the equilibrium-constant expression for the dissociation of the acid in water. (b) What is the pH of a 0.75 M CaHsOH(ag) solution? (C) For a certain reaction involving CaHsOH(ag) to proceed at a significant rate, the phenol must be primarily in its deprotonated form, C3H5O (eg). In order to ensure that the CsHsOH(aq) is deprotonated, the reaction must be conducted in a buffered solution. On the number scale below, circle each pH for which more than 50 percent of the phenol molecules are in the deprotonated form (CoHsO (aq). Justify your answer. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 Justification: (d) CeHsOH(ag) reacts with NaOH(ag). Write a net ionic equation representing this reaction (aka: invasion equation). (e) What is the pH of the resulting solution when 30 mL of 0.40 M CSH5OH(aq) is added to 25 mL of 0.60 M NAOH. Show all work…
A solution of sodium acetate is prepared using 0.56 mol L-1 NaOH as the solvent. The pKapKa of acetic acid is 4.75 . The concentration of sodium acetate after mixing, before any reaction takes place is 0.44 mol L-1 . Calculate the equilibrium concentrations of all acid species: [ CH3COOH ], [ CH3COO- ], the pH and the pOH in the solution. Some assumptions may not work, on the other hand, if you do not make the correct assumptions first, the quadratic formula will give you the wrong answer. [ CH3COOH ] = ___mol L-1 , [ CH3COO- ] = ___mol L-1 , pH = ___ pOH = ____
Calculate the pH for a mixture of one mole of benzoic acid andone mole of sodium benzoate. The pKa of benzoic acid is 4.2.
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Compare the pH of propionic acid and nitric acid when they are dissolved in water at a concentration of 20 mM. This should include writing a balanced equation describing the acid-base reactions involved, calculation of the pKa for both, calculation of pH, and calculation of the percent dissociation of both.
Pyridinium bromide (C5H5NHBr) is a strong electrolyte thatdissociates completely into C5H5NH+ and Br-. An aqueoussolution of pyridinium bromide has a pH of 2.95.(a) Write out the reaction that leads to this acidic pH.(b) Calculate the Ka for pyridiniumbromide.(c) A solution of pyridinium bromide has a pH of 2.95.What is the concentration of the pyridinium cation atequilibrium, in units of molarity?
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