Solving a polyprotic acid equilibrium composition problem2 -Suppose a 0.23 M aqueous solution of phosphoric acid (H, PO4) is prepared. Calculate the equilibrium molarity of HPO,the properties of phosphoric acid in the ALEKS Data resource.You'll find information onRound your answer to 2 significant digits.ol [-] pK, of weak acids at 25°CNameFormulapKą1pKą2pКазacetic acidCH3CO2H4.756benzoic acidCH5CO2H4.204butanoic acidСзн,со2н4.834-chlorobutanoic acidC3H,CICO,H4.52crotonic acidC3H5CO2H4.69охalic acidH2C2O41.253.81phosphoric acidНзРО42.167.2112.32propionic acidC2H5CO2H4.87sulfuric acidH2SO4strong acid1.99trimethylacetic acidC4H9CO2H5.03

Answered: Image /qna-images/answer/6d6b1d1a-1fdd-4eec-b732-d724c018d7e2.jpg

Answered: Solving a polyprotic acid equilibrium…

General, Organic, and Biological Chemistry

7th Edition

ISBN:9781285853918

Author:H. Stephen Stoker

Publisher:H. Stephen Stoker

Chapter10: Acids, Bases, And Salts

Section: Chapter Questions

Problem 10.45EP

See similar textbooks

Similar questions

The odor of vinegar is due to the presence of acetic acid, CH3CO2H, a weak acid. List, in order of descending concentration, all of the ionic and molecular species present in a 1-M aqueous solution of this acid.
Consider a 0.33 M solution of the diprotic acid H2X. H2X H+(aq)+ HX(aq)Ka1=3.3 10 4 HX H+(aq)+ X2(aq)Ka2=9.7 10 8 Calculate the pH of the solution and estimate [HX-] and [X2-].
Calculate [OH-] and pH in a solution in which the hydrogen sulfite ion, HSO3-, is 0.429 M and the sulfite ion is (a) 0.0249 M (b) 0.247 M (c) 0.504 M (d) 0.811 M (e) 1.223 M
. The concepts of acid-base equilibria were developed in this chapter for aqueous solutions (in aqueous solutions, water is the solvent and is intimately involved in the equilibria). However, the Brønsted-Lowry acid-base theory can be extended easily to other solvents. One such solvent that has been investigated in depth is liquid ammonia. NH3. a. Write a chemical equation indicating how HCl behaves as an acid in liquid ammonia. b. Write a chemical equation indicating how OH- behaves as a base in liquid ammonia.
Which of the following substances are acids in terms of the Arrhenius concept? Which are bases? Show the acid or base character by using chemical equations. a P4O10 b Na2O c N2H4 d H2Te
A certain sodium compound is dissolved in water to liberate Na+ ions and a certain negative ion. What evidence would you look for to determine whether the anion is behaving as an acid or a base? How could you tell whether the anion is a strong base? Explain how the anion could behave simultaneously as an acid and a base
What is the concentration of the hydroxide ion, OH-, in solution at equilibrium if the pH of the solution is 7.65? Nitrogen and oxygen react at high temperatures according to the following equation: N2(g) +O2(g) ⇄ 2NO(g) where ∆H=181kJ At equilibrium what will happen to the concentrations of N2, O2, and NO at equilibrium if N2 is removed? Calculate the pH of the following weak base: 0.5M NH3 with Kb =1.8x10−5
On a shelf in the lab storeroom marked “Solutions of Acids”, a bottle has a torn label. All that can be seen on the label is the concentration: 643 x 10-3 M, not the name of the acid. In trying to find the identity of the acid, you measure the pH of this solution and find it to be 3.382. Of the acids listed on the chart of Acid Dissociation Constants (attached), WHICH ACID could this be? There is only one correct answer. Hint: Use the given information to find Ka. Use all sig figs in the pH.
In the following equation HNO2 (aq) + H2O (l) ↔ H3O+ (aq) + NO2-(aq), 0.37 M of nitrous acid was found in the resulting aqueous solution. Ka for HNO2 is 4.5 x10 -4. What will be the percent ionization of the weak acid?
A soft drink has a pH of 5; find the following: pOH [H3 O+ ] [OH- ] *Provide computations
For the following A and B reactions between recatant I and II, decide which reactant is the Lewis base and acid (LB/LA), and if they are also Bronsted acids/bases (BA/BB)
Sulfurous acid, H2SO3, is a diprotic acid Ka1 = 1.3 × 10-2 and Ka2 = 6.3 × 10-8. The acid forms when sulfur dioxide (a gas with a suffocating odor) dissolves in water. What is the pH of a 0.25 M solution of sulfurous acid? What is the concentration of sulfite ion, SO32-, in the solution? Note that Ka1 is relatively latge.

SEE MORE QUESTIONS

Recommended textbooks for you

General, Organic, and Biological Chemistry

Chemistry

ISBN:

9781285853918

Author:

H. Stephen Stoker

Publisher:

Cengage Learning

Introductory Chemistry For Today

Chemistry

ISBN:

9781285644561

Author:

Seager

Publisher:

Cengage

Introductory Chemistry: A Foundation

Chemistry

ISBN:

9781337399425

Author:

Steven S. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

General, Organic, and Biological Chemistry

Chemistry

ISBN:

9781285853918

Author:

H. Stephen Stoker

Publisher:

Cengage Learning

Introductory Chemistry For Today

Chemistry

ISBN:

9781285644561

Author:

Seager

Publisher:

Cengage

Introductory Chemistry: A Foundation

Chemistry

ISBN:

9781337399425

Author:

Steven S. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

Chemistry by OpenStax (2015-05-04)

Chemistry

ISBN:

9781938168390

Author:

Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:

OpenStax

SEE MORE TEXTBOOKS