The values of Ka for hydrozoic acid (HN3) and hypobromous acid (HBrO) are given below. HN3 Ka = 1.9 × 10-5 HBrO Ka = 2.0 × 10-9 If we mix 0.50 mol HN3 and 0.50 mol NaBrO into a 1-L aqueous solution, which of the following statements is correct concerning the final solution at equilibrium after mixing? Choose one option only.   Options: a. The pH of the final solution is less than 7 because Ka (HN3) < Kb( BrO- ). b. The pH of the final solution is greater than 7 because Ka (HN3) > Kb(BrO-). c. The pH of the final solution is equal to 7 because the neutralization reaction between HN3 and NaBrO. d. The pH of the final solution is less than 7 because Ka (HN3) > Kb( BrO- ). e. The pH of the final solution is greater than 7 because Ka (HN3) < Kb( BrO- ).

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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.