None Calculate the concentration of Y^4- at equilibrium at pH 8.00 and pH 11.00 if the initial concentration of EDTA is .100Malpha4 at pH 8.00 5.39 x10^-3; alpha4 at pH 11 = 0.85=

Answered: Image /qna-images/answer/f43246bd-6ae9-4352-8402-2373d669b197.jpg

Answered: Calculate the concentration of Y^4- at…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter14: Acids And Bases

Section14.9: Lewis Acids And Bases

Problem 14.26E

See similar textbooks

Similar questions

The hydrogen phthalate ion, C8HsO4, is a weak acid with Ka = 3.91 106. C8H5O4(aq)+H2O(l)C8H4O42(aq)+H3O+(aq) What is the pH of a 0.050 M solution of potassium hydrogen phthalate. KC8H5O4? Note: To find the pH for a solution of the anion, we must take into account that the ion is amphiprotic. It can be shown that, for most cases of amphiprotic ions, the H3O+ concentration is [H3O+]=Ka1Ka2 For phthalic acid, C8H6O4 is Ka1 is 1.12 103, and Ka2 is 3.91 106.
Determine the pKa of an acid; a 4e-3M solution of which has a pH of 2.4
Phosphoric acid (H₂PO4), a triprotic acid, has three pKą values: 2.14, 6.86, and 12.4. What molar ratio of HPO to H₂PO in 4 solution would produce a pH of 8.00? molar ratio=
(8) Answer each of the following questions: (a) Ka for HNO2 is 4.6 x 10-4. What is the Kb for its conjugate base ? (b) Calculate the pH of 0.1 M of HNO2 solution using the ka above.
Calculate the pH of a dilute solution that contains a molar ratio of potassium acetate to acetic acid (pKa = 4.76) of (a) 2:1; (b) 1:3; (c) 5:1; (d) 1:1; (e) 1:10
Like any equilibrium constant, Kᵥᵥ changes with tempera-ture. (a) Given that autoionization is endothermic, how does Kᵥᵥ change with rising T? Explain with a reaction that includes heatas reactant or product. (b) In many medical applications, the value of Kᵥᵥ at 37°C (body temperature) may be more appropri-ate than the value at 25°C, 1.0X10⁻¹⁴. The pH of pure water at 37°C is 6.80. Calculate Kᵥᵥ, pOH, and [OH] at this temperature.
Calculate the pH of the solution after the addition of each of the given amounts of 0.0651 M HNO3 to a 50.0 mL solution of 0.0750 M aziridine. The pKa of aziridinium is 8.04. What is pH at equivalence?
What molar ratio of HPO4 to H2PO4 in solution would produce a pH of 7.0? Phosphoric acid (H:PO4), a triprotic acid, has 3 pKa values: 2.14, 6.86, and 12.4. Hint: Only one of the pKa values is relevant here.
Calculate the pH and the equilibrium concentrations of HTEO3 and TeO32- in a 0.2840 M tellurous acid solution, H2TEO3 (aq). For H2TEO3, Ka1 = 5.40x10-7 and Ka2 = 3.70x10-9 pH = [HTEO3"] = M [TeO32-] = M
A weak acid, HA, has a pKa = 6.2. If a solution of NaA(aq) is prepared, what does the pH of the solution need to be adjusted to in order to achieve the following ratios of deprotonated to protonated species? 1) [A-] / [HA] = 0.01 2) [A-] / [HA] = 10 3) [A-] / [HA] = 1 4) [A-] / [HA] = 106 Note: NaA is the sodium salt of , the conjugate base of HA. Assume NaA completely dissociates in water.
Calculate the pH of a 0.20 M HA solution, given the pKa of HA is 2.22.
a) Calculate the pH of an aqueous solution of the salt NaA, which was made to a concentration of 0.080 M NaA. The Ka of the weak acid HA is 2.0 x 10-5. Your pH should go to two places past the decimal point (i.e. 1.35). b) Aniline, C6H5NH2, has a pKb of 9.40. What is the pH of a solution which is 0.12 M in aniline and 0.38 M in anilinium ion, C6H5NH3+? Your answer should be to two places past the decimal.

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781133949640

Author:

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

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

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

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781133949640

Author:

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

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

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

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

Calculate the concentration of Y^4- at equilibrium at pH 8.00 and pH 11.00 if the initial concentration of EDTA is .100M alpha4 at pH 8.00 5.39 x10^-3; alpha4 at pH 11 = 0.85 =