**1. A solution of a weak acid was tested with the indicators used in this experiment. The colors observed were as follows:**- Methyl violet: violet- Congo red: violet- Thymol blue: orange- Bromcresol green: yellow- Methyl yellow: red*What is the approximate pH of the solution?* _________________**2. An aqueous solution of NH₃ has a pH of 11.6. The ammonia (NH₃) molecule is the conjugate base of the NH₄⁺ (called “ammonium”) ion. Write the net ionic equation for the reaction that makes an aqueous solution of NH₃ basic. (Eq. 5.)****3. The pH of a 0.10 M HOBr solution is 4.8.**a. *What is [H⁺] in that solution?* _________________Mb. *What is [OBr⁻]? What is [HOBr]? (Where do the H⁺ and OBr⁻ ions come from?)* _________________M; _______________Mc. *What is the value of Kₐ for HOBr? What is the value of pKₐ?* _________________

Since you have asked multiple questions and the first question you posted is incomplete, we will solve the second question for you. If you want any specific question to be solved then please specify the question number or post only that question. A conjugate base is formed when an acid loses its proton. It has one less hydrogen atom and one more negative charge as compared with the acid from which it is formed. A conjugate acid is formed when a base accepts a proton. It has one more hydrogen atom and one more positive charge as compared with the base from which it is formed.Ammonia (NH3) is the conjugate base of ammonium ion (NH4+) and ammonium ion (NH4+) is the conjugate acid of ammonia (NH3). NH3 is a base. So when added to water, NH3 accepts one H+ ion from H2O molecule and forms its conjugate acid NH4+ and hydroxide ion OH-. These OH- ions are responsible for the basic nature of the aqueous solution of ammonia. The net ionic equation can be written as follows: NH3aq+H2Ol↔NH4+aq+OH-aq Hence it may be concluded that aqueous solution of NH3 is basic due to presence of OH- ions.

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2. An aqueous solution of NH, has a pH of 11.6. The ammonia (NH) molecule is the conjugate base of the NH, (called "ammonium") ion. Write the net ionic equation for the reaction that makes an aqueous solution of NH, basic. (Eq. 5.)

2. An aqueous solution of NH, has a pH of 11.6. The ammonia (NH) molecule is the conjugate base of the NH, (called "ammonium") ion. Write the net ionic equation for the reaction that makes an aqueous solution of NH, basic. (Eq. 5.)

Chemistry

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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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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

**1. A solution of a weak acid was tested with the indicators used in this experiment. The colors observed were as follows:**

- Methyl violet: violet
- Congo red: violet
- Thymol blue: orange
- Bromcresol green: yellow
- Methyl yellow: red

*What is the approximate pH of the solution?*
_________________

**2. An aqueous solution of NH₃ has a pH of 11.6. The ammonia (NH₃) molecule is the conjugate base of the NH₄⁺ (called “ammonium”) ion. Write the net ionic equation for the reaction that makes an aqueous solution of NH₃ basic. (Eq. 5.)**

**3. The pH of a 0.10 M HOBr solution is 4.8.**

a. *What is [H⁺] in that solution?*
_________________M

b. *What is [OBr⁻]? What is [HOBr]? (Where do the H⁺ and OBr⁻ ions come from?)*
_________________M; _______________M

c. *What is the value of Kₐ for HOBr? What is the value of pKₐ?*
_________________

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