Consider the acid-base nature of sodium nitrite, NaNO2, when it is dissolved in water. (1) What are the acid-base properties of the cation? (2) What are the acid-base properties of the anion? (3) Would an aqueous solution of sodium nitrite be acidic, basic or neutral? C C C

Consider the acid-base nature of sodium nitrite, NaNO2, when it is dissolved in water. (1) What are the acid-base properties of the cation? (2) What are the acid-base properties of the anion? (3) Would an aqueous solution of sodium nitrite be acidic, basic or neutral? C C C

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 7P

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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

Consider the acid-base nature of sodium nitrite, NaNO2, when it is dissolved in water.
(1) What are the acid-base properties of the cation?
(2) What are the acid-base properties of the anion?
(3) Would an aqueous solution of sodium nitrite be acidic, basic or neutral?
C
C
C

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The active ingredient of bleach such as Clorox is sodium hypochlorite (NaClO). Its conjugate acid, hypochlorous acid (HClO), has a Ka of 3.0 × 10–8. (a) The undiluted bleach contains roughly 1 M NaClO.Calculate the pH of 1 M NaClO solution. (b) Some applications require extremely diluted bleach solution, such as swimming pools. Suppose the solution in (a) is diluted by 10,000-fold. Calculate the pH of the diluted solution, and demonstrate that you can still neglect the autoionization of water in your calculation. (c) Suppose the solution in (a) is diluted by 1 million-fold, briefly explain how your approach willbe different. Write the equation with [H3O+] as the unknown, but you do not need to solve it.