Solutions for Question 3 please 1. Identify the Lewis acid and the Lewis base in thefollowing reaction: Agt(aq) + 2NH₂ (aq) àAg(NH3)₂ (aq)2. Identify the stronger acid of the following pairs ofacids. Justify your answer from theory.a. HC1O,(aq) vs. HC1O,(aq)b. HClO,(aq) vs. HIO,(aq)3. Identify the stronger Brønsted-Lowry base of thefollowing pairs of bases. Justify your answer fromtheory.a. HS (aq) vs. HO (aq)b. NH₂ vs. F-4. Calculate the pH of a mixture that contains both0.255 mol HC₂H3O₂ and 0.165 mol NaC₂H₂O₂ in1.00 L solution both before and after adding 0.035mol HCl to the mixture (assume no volume changeupon adding these moles of HCl) (Ka (HC₂H₂O₂) =1.8 x 10-5)?5. Circle all of the following solutions that arebuffered solutions. Justify your answer. (Ka(HC₂H3O₂) = 1.8 x 10-5; K₂(NH3) = 1.8 x 10-5)a. 0.333 mol HC₂H₂O₂ and 0.111 mol KC₂H₂O₂in 1.00 L solutionb. 0.175 mol NaOH and 0.250 mol NH₂Cl in1.00 L solutionc. 0.300 mol NaC₂H₂O₂ and 0.225 mol HCl in1.00 L solutiond. 0.200 mol HC₂H₂O2 and 0.200 mol KOH in1.00 L solution6. Calculate the number of moles of NaOH that mustbe added to 1.0 L of 0.50 M HC₂H3O₂ to produce asolution buffered at pH=4.00. Assume no volumechange upon adding the NaOH. (K₂ (HC₂H₂O₂) =1.8 x 10-5)

Answered: Image /qna-images/answer/96759c56-9c02-4c1f-8e3b-97c4641d4bcc.jpg

Answered: 3. Identify the stronger Brønsted-Lowry…

3. Identify the stronger Brønsted-Lowry base of the following pairs of bases. Justify your answer from theory. a. HS (aq) vs. HO (aq) b. NH₂ vs. F-

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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Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

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Solutions for Question 3 please

1. Identify the Lewis acid and the Lewis base in the
following reaction: Agt(aq) + 2NH₂ (aq) à
Ag(NH3)₂ (aq)
2. Identify the stronger acid of the following pairs of
acids. Justify your answer from theory.
a. HC1O,(aq) vs. HC1O,(aq)
b. HClO,(aq) vs. HIO,(aq)
3. Identify the stronger Brønsted-Lowry base of the
following pairs of bases. Justify your answer from
theory.
a. HS (aq) vs. HO (aq)
b. NH₂ vs. F-
4. Calculate the pH of a mixture that contains both
0.255 mol HC₂H3O₂ and 0.165 mol NaC₂H₂O₂ in
1.00 L solution both before and after adding 0.035
mol HCl to the mixture (assume no volume change
upon adding these moles of HCl) (Ka (HC₂H₂O₂) =
1.8 x 10-5)?
5. Circle all of the following solutions that are
buffered solutions. Justify your answer. (Ka
(HC₂H3O₂) = 1.8 x 10-5; K₂(NH3) = 1.8 x 10-5)
a. 0.333 mol HC₂H₂O₂ and 0.111 mol KC₂H₂O₂
in 1.00 L solution
b. 0.175 mol NaOH and 0.250 mol NH₂Cl in
1.00 L solution
c. 0.300 mol NaC₂H₂O₂ and 0.225 mol HCl in
1.00 L solution
d. 0.200 mol HC₂H₂O2 and 0.200 mol KOH in
1.00 L solution
6. Calculate the number of moles of NaOH that must
be added to 1.0 L of 0.50 M HC₂H3O₂ to produce a
solution buffered at pH=4.00. Assume no volume
change upon adding the NaOH. (K₂ (HC₂H₂O₂) =
1.8 x 10-5)

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