Calculate the concentration of all species in a 0.240 MC6H5NH3Cl solution. Enter your answers numerically separated by commas. Express your answer using two significant figures. [C6H5NH+3], [Cl−], [C6H5NH2],[H3O+], [OH−] =
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.
|
|
[C6H5NH+3], [Cl−], [C6H5NH2],[H3O+], [OH−] =
|
|
|
The concentrations of given species is to be calculated from given salt concentration.
Given:
[C6H5NH3Cl] = 0.240 M
Salts of acid or base are ionic compounds and dissociates completely into their respective ions.
Weak acids dissociates partially in an aqueous solution. The concentration of ions can be determined using dissociation equilibrium constant.
Kb = 1.00 10-14/ Ka
Trending now
This is a popular solution!
Step by step
Solved in 2 steps
