We can observe the common-ion effect in action by comparing how much a pure sample of acid dissociates to how much a sample of an acid dissociates when its conjugate base is in solution. Let's consider the oxoacid HIO, which has a Ka of 2.3×10-11. part 1: Calculate the pH of an aqueous solution of 0.100 M HIO. (Due to the low Ka value, you may apply the 5% approximation to avoid the quadratic equation if you wish.) part 2: Complete the RICE table for the dissociation of 0.100 M HIO in a solution with 0.0150 M IO- by selecting the correct answer from any dropdown boxes available. (Remember that the conjugate bases are typically added in as a soluble salt, such as NaIO, but that the salt dissociates completely and the alkali metal cation is a spectator ion.) part 3: Calculate the pH for the solution made from 0.100 M HIO and 0.0150 M IO- . For this case, you can also make the assumption that x will be negligibly small compared to the starting concentrations of the weak acid and conjugate base in order to simplify your calculations.
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.
We can observe the common-ion effect in action by comparing how much a pure sample of acid dissociates to how much a sample of an acid dissociates when its conjugate base is in solution. Let's consider the oxoacid HIO, which has a Ka of 2.3×10-11.
part 1: Calculate the pH of an aqueous solution of 0.100 M HIO. (Due to the low Ka value, you may apply the 5% approximation to avoid the quadratic equation if you wish.)
part 2: Complete the RICE table for the dissociation of 0.100 M HIO in a solution with 0.0150 M IO- by selecting the correct answer from any dropdown boxes available. (Remember that the conjugate bases are typically added in as a soluble salt, such as NaIO, but that the salt dissociates completely and the alkali metal cation is a spectator ion.)
part 3: Calculate the pH for the solution made from 0.100 M HIO and 0.0150 M IO- . For this case, you can also make the assumption that x will be negligibly small compared to the starting concentrations of the weak acid and conjugate base in order to simplify your calculations.
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