- 13M. Calculate the H,O' concentration. Be sure your answer has the correct number of+An aqueous solution at 25 °C has a OH concentration of 1. x 10significant digits.) Mx10

Given-> Concentration of OH- =[OH-] = 1 × 10-13 M

Answered: - 13 An aqueous solution at 25 °C has a…

- 13 An aqueous solution at 25 °C has a OH concentration of 1. × 10 "M. Calculate the H,0" concentration. Be sure your answer has the correct number of significant digits. | M

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 112QRT

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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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- 13
M. Calculate the H,O' concentration. Be sure your answer has the correct number of
+
An aqueous solution at 25 °C has a OH concentration of 1. x 10
significant digits.
) M
x10

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. The concepts of acid-base equilibria were developed in this chapter for aqueous solutions (in aqueous solutions, water is the solvent and is intimately involved in the equilibria). However, the Brønsted-Lowry acid-base theory can be extended easily to other solvents. One such solvent that has been investigated in depth is liquid ammonia. NH3. a. Write a chemical equation indicating how HCl behaves as an acid in liquid ammonia. b. Write a chemical equation indicating how OH- behaves as a base in liquid ammonia.
1. What is [H3O+] in a 0.10 M solution of HCN at 25°C? (K, for HCN = 4.0 × 10−10) 1.6 × 10−9 M 6.3 × 10−6 M 2.0 × 10−5 M 4.0 × 10−11 M
Explain why a sample of pure water at 40 C is neutral even though [H3O+]=1.7107M . Kw is 2.91014 at 40 C.
What is the freezing point of 0.92 M aqueous acetic acid? The density of this solution is 1.008 g/cm3.
. How is the strength of an acid related to the fact that a competition for protons exists in aqueous solution between water molecules and the anion of the acid?
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8-112 Consider an initial 0.040 M hypobromous acid (HOBr) solution at a certain temperature. At equilibrium after partial dissociation, its pH is found to be 5.05. What is the acid ionization constant, Ka, for hypobromous acid at this temperature?
Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H) and the amine group (NHR) are protonated. However, as the pH of the solution increases (say, by adding base), the carboxylic acid proton is removed, usually at a pH between 2 and 3. In a middle range of pHs, therefore, the amine group is protonated, but the carboxylic acid group has lost the proton. (This is called a zwitterion.) At more basic pH values, the amine proton is dissociated. What is the pH of a 0.20 M solution of alanine hydrochloride, [NH3CHCH3CO2H]Cl?
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