Select the appropriate species from the drop-down boxes to create a net ionicequation for the following reaction:a) (CH3)2NH + water:CheckCheck4++«(Select the appropriate species from the drop-down boxes to create a net ionicequation for the following reaction:a) HNO₂/LINO2 buffer solution + HClO4:4)(++4)

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Select the appropriate species from the drop-down boxes to create a net ionic equation for the following reaction: a) (CH3)2NH + water: Check 4) + AP ( ( +

Introduction to General, Organic and Biochemistry

11th Edition

ISBN:9781285869759

Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Chapter8: Acids And Bases

Section: Chapter Questions

Problem 8.93P: 8-93 Do a 1.0 M CH3COOH solution and a 1.0 M HCI solution require the same amount of 1.0 M NaOH to...

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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.

Question

Select the appropriate species from the drop-down boxes to create a net ionic
equation for the following reaction:
a) (CH3)2NH + water:
Check
Check
4
+
+
«
(
Select the appropriate species from the drop-down boxes to create a net ionic
equation for the following reaction:
a) HNO₂/LINO2 buffer solution + HClO4:
4)
(
+
+
4)

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8-55 We commonly refer to a buffer as consisting of approximately equal molar amounts of a weak acid and its conjugate base—for example, CH3COOH and CH3COO-. Is it also possible to have a buffer consisting of approximately equal molar amounts of a weak base and its conjugate acid? Explain.
8-60 How is the buffer capacity affected by the ratio of the conjugate base to the conjugate acid?
8-93 Do a 1.0 M CH3COOH solution and a 1.0 M HCI solution require the same amount of 1.0 M NaOH to hit a titration end point? Explain.
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please answer on 1-a,b,c,d. Clear handwriting or type in, thank you! 1. The mixture of anions is an effective blood buffer with the following acid-base equilibrium: HO" (aq) + HPO* (aq) H:POs (aq) + H;O (1) a. For the equilibrium above, what is the effect of decreasing the pH? (give shift) b. As a result of the shift, which ion H:PO, or HPO, would appear to increase? c. For the equilibrium above, what is the effect of increasing the pH? (give shift) d. As a result of the shifl, which ion H:PO, or HPO would appear to increase?
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