**Solution Buffering Instruction**A one-liter aqueous solution contains 0.29 M ammonia.To convert this solution into a buffer, you may add one of the following substances. Ensure that the solution's volume remains constant as each substance is added:- 0.15 mol Ba(OH)$_2$- 0.30 mol NH$_4$Br- 0.30 mol HNO$_3$- 0.29 mol BaBr$_2$- 0.15 mol HNO$_3$**Note:** It is important to understand how each addition impacts the solution's buffering capacity and its chemical equilibrium. **Buffer Solution Formation with Hypochlorous Acid**An aqueous solution contains **0.33 M hypochlorous acid**.One liter of this solution could be converted into a buffer by the addition of:(Assume that the volume remains constant as each substance is added.)- 0.34 mol KClO- 0.16 mol HCl- 0.082 mol Ba(OH)₂- 0.34 mol HCl- 0.33 mol KCl**Explanation:**To form a buffer solution, we need to add a substance that will create a conjugate base or acid pair with hypochlorous acid. This allows the solution to resist changes in pH when strong acids or bases are added.

1). We are given the solution of 0.29 M solution of NH3. It is a weak base, therefore to to make a…

An aqueous solution contains 0.29 M ammonia. One liter of this solution could be converted into a buffer by the addition of: (Assume that the volume remains constant as each substance is added.) O 0.15 mol Ba(OH)2 O 0.30 mol NH¿Br O 0.30 mol HNO3 O 0.29 mol BaBr2 O 0.15 mol HNO3

An aqueous solution contains 0.29 M ammonia. One liter of this solution could be converted into a buffer by the addition of: (Assume that the volume remains constant as each substance is added.) O 0.15 mol Ba(OH)2 O 0.30 mol NH¿Br O 0.30 mol HNO3 O 0.29 mol BaBr2 O 0.15 mol HNO3

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.

Question

**Solution Buffering Instruction**

A one-liter aqueous solution contains 0.29 M ammonia.

To convert this solution into a buffer, you may add one of the following substances. Ensure that the solution's volume remains constant as each substance is added:

- 0.15 mol Ba(OH)$_2$
- 0.30 mol NH$_4$Br
- 0.30 mol HNO$_3$
- 0.29 mol BaBr$_2$
- 0.15 mol HNO$_3$

**Note:** It is important to understand how each addition impacts the solution's buffering capacity and its chemical equilibrium.

**Buffer Solution Formation with Hypochlorous Acid**

An aqueous solution contains **0.33 M hypochlorous acid**.

One liter of this solution could be converted into a buffer by the addition of:

(Assume that the volume remains constant as each substance is added.)

- 0.34 mol KClO
- 0.16 mol HCl
- 0.082 mol Ba(OH)₂
- 0.34 mol HCl
- 0.33 mol KCl

**Explanation:**
To form a buffer solution, we need to add a substance that will create a conjugate base or acid pair with hypochlorous acid. This allows the solution to resist changes in pH when strong acids or bases are added.

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