Please correct answer and don't use hand rating 3) What is the dominant species in a solution of Ni2+ in which the NH3 concentration is 0.0350 M? Use adiagram to explain the answer.

Answered: 3) What is the dominant species in a…

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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Define or illustrate the meaning of the following terms: a. amphoteric b. Kw reaction c. Kw equilibrium constant d. pH e. pOH f. pKw Give the conditions for a neutral aqueous solution at 25C, in terms of [H+], pH, and the relationship between [H+] and [OH]. Do the same for an acidic solution and for a basic solution. As a solution becomes more acidic, what happens to pH, pOH, [H+], and [OH]? As a solution becomes more basic, what happens to pH, pOH, [H+], and [OH]?
For conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)
Using the diagrams shown in Problem 10-37, which of the four acids is the weakest acid?
1. The following equilibrium exists when ammonium is dissolved in water: NH4+ (aq) + H2O (l) « H3O+ (aq) + NH3 (aq) The Ka of NH4 is 5.6 x 10-10. Find the pH of a 3.00 M solution of NH4Cl. (hint: since NH4Cl completely ionizes, the concentration of the ammonium ion is 3.00 M) NH4Cl (s)àNH4+ (aq) + Cl- (aq)
[Review Topics] [References] Use the References to access important values if needed for this question. Consider the following equilibrium between 3-methylbenzoic acid (K,a-5.0x10) and its conjugate base: %3D CH3- CH3- H2O + H30* (1) Will lowering the pH shift the equilibrium to the right or to the left? (2) Calculate the ratio of the concentration of 3-methylbenzoate ion to the concentration of 3-methylbenzoic acid at a pH of 1.59. ratio [conjugate base] / [acid] Submit Answer Retry Entire Group 9 more group attempts remaining
Could a very dilute solution of a strong acid yield a pH above 7?
In which of the following aqueous solutions does the weak acid exhibit the highest percentage ionization? 0.01M HC3H5O2(Ka=1.3x10-5) 0.01M HOCI (Ka= 3.5x10-8) 0.01M H2SO3(Ka= 1.4x10-2) 0.01M HC2H3O2(Ka=1.8x10-5) 0.01M H3BO3(Ka= 5.4x10-10)
the two ammonia species are ammonia (NH3) and the ammonium ion (NH4+. The total ammonia concentration is equal to the sum of both species (NH3+NH4+). Un-ionized NH4+↔NH3+H+ pka=6.34 if the total ammnia species has a concentation of 5M at a pH of 8. what is the concentration of ammonia (NH3)?
A triprotic acid (H3Y) has the following acid ionization constants: Ka1 = 5.3 x 104 Ka2 = 1.7 x 10-8 ; Ka3 = 3.2 × 10-11 If a student wanted to create a buffer solution at a pH of 6.93, which of the following conjugate acid-base pairs should this student choose? HY2- and Y3- H3Y and H2Y1- H2Y1- and Y3- H2Y1- and HY2- H3Y and Y3- H3Y and HY2-
Arrange the following solution from lowest pH to highest pH: 0.75 М CНH,COОН (К, 3 1.8 х 10-5) 0.01 М HNOZ (К, — 4.6 х 10-4) 0.05 М СНООН (К, — 1.8 х 10-4) %3D 0.75 М CH3СООН < 0.01 М HNOZ < 0.0.05 М СНООН b. 0.75 M СH,COОH < 0.05 М СНООН < 0.01 М HNOZ 0.01 М HNO, < 0.05 М СНООН <0.75 М СН,СООН d. 0.05 M СНООН < 0.01 М HNOZ <0.75 М СН,СООН а. С.
A solution contains 0.0000001 (10-7) moles of hydrogen ions [H+] per liter. Which of the following best describes this solution? acidic: H+ acceptor basic: H+ acceptor acidic: H+ donor neutral
(a) Calculate the percent ionization of 0.00800 M butanoic acid (K₂ = 1.5e-05). % ionization = % (b) Calculate the percent ionization of 0.00800 M butanoic acid in a solution containing 0.0610 M sodium butanoate. % ionization = %

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3) What is the dominant species in a solution of Ni2+ in which the NH3 concentration is 0.0350 M? Use a diagram to explain the answer.