O hypobromous acid O hydrogen malonate ion O ammonium ion O propanoic acid O dihydrogen phosphate ion lactic acid O hydrogen phosphite ion O monochloracetic acid O hydrogen sulfate ion Given the following table of K, values, what would be the best conjugate acid to choose to make a buffer that maintains a pH = %3D 5.67? Species Ka hydrogen 1.2 x 10-2 sulfate ion monochloracetic 1.4 x 10-3 acid lactic acid 1.4 x 104 propanoic acid 1.3 x 10:5 hydrogen 2.0 x 106 malonate ion hydrogen 1.7 x 107 phosphite ion dihydrogen 6.3 x 10-8 phosphate ion hypobromous 2.0 x 10-9 acid ammonium ion 5.6 x 10 10

O hypobromous acid O hydrogen malonate ion O ammonium ion O propanoic acid O dihydrogen phosphate ion lactic acid O hydrogen phosphite ion O monochloracetic acid O hydrogen sulfate ion Given the following table of K, values, what would be the best conjugate acid to choose to make a buffer that maintains a pH = %3D 5.67? Species Ka hydrogen 1.2 x 10-2 sulfate ion monochloracetic 1.4 x 10-3 acid lactic acid 1.4 x 104 propanoic acid 1.3 x 10:5 hydrogen 2.0 x 106 malonate ion hydrogen 1.7 x 107 phosphite ion dihydrogen 6.3 x 10-8 phosphate ion hypobromous 2.0 x 10-9 acid ammonium ion 5.6 x 10 10

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter9: Acids, Bases, And Salts

Section: Chapter Questions

Problem 9.117E

See similar textbooks

Similar questions

A buffer is composed of formic acid and its conjugate base, the formate ion. (a) What is the pH of a solution that has a formic acid concentration of 0.050 M and a sodium formate concentration of 0.035 M? (b) What must the ratio of acid to conjugate base be to have a pH value 0.50 units higher than the value calculated in part (a)?
What mass of NH4Cl must be added to 0.750 L of a 0.100-M solution of NH3 to give a buffer solution with a pH of 9.26? (Him: Assume a negligible change in volume as the solid is added.)
A best buffer has about equal quantities of weak acid and conjugate base present as well as having a large concentration of each species present. Explain.
Phenolphthalein is a commonly used indicator that is colorless in the acidic form (pH 8.3) and pink in the base form (pH 10.0). It is a weak acid with a pKa of 8.7. What fraction is in the acid form when the acid color is apparent? What fraction is in the base form when the base color is apparent?
Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH, stoichiometric points occur at pH = 3.9 and 8.8. A 25.00-mL sample of malonic acid of unknown concentration is titrated with 0.0984 M NaOH, requiring 31.50 mL of the NaOH solution to reach the phenolphthalein end point. Calculate the concentration of the initial malonic acid solution. (Sec Exercise 113.)
A diprotic acid, H2B(MM=126g/moL), is determined to be a hydrate, H2B xH2O. A 10.00-g sample of this hydrate is dissolved in enough water to make 150.0 mL of solution. Twenty-five milliliters of this solution requires 48.5 mL of 0.425 M NaOH to reach the equivalence point. What is x?
When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
In an acid-base titration, 21.16 mL of an NaOH solution are needed to neutralize 20.04 mL of a 0.0997 M HCl solution. To find the molarity of the NaOH solution, we can use the following procedure: First note the value of MH in the HCl solution. ____________M Find MOH- in the NaOH solution. Use Eq.3. ____________M Obtain MNaOH from MOH. ____________M
Ammonia gas is bubbled into 275 mL of water to make an aqueous solution of ammonia. To prepare a buffer with a pH of 9.56, 15.0 g of NH4Cl are added. How many liters of NH3; at 25C and 0.981 atm should be used to prepare the buffer? Assume no volume changes and ignore the vapor pressure of water.