1. A substance that gives up or donates hydrogen ions during a chemical reaction. a. Bronsted-Lowry acid c. Conjugate acid b. Bronsted-Lowry base d. Conjugate base 2. A substance that accepts hydrogen ions during a chemical reaction. a. Bronsted-Lowry acid c. Conjugate acid b. Bronsted-Lowry base d. Conjugate base 3. A way to measure the strengths of acids and bases. a. Bronsted-Lowry acid c. pH scale b. Bronsted-Lowry base d. Ion-concentration constant 4. What is the pH of a solution with a hydrogen-ion concentration of 3.75 x 10-³ M? a. 2.42 c. 9.96 d. 6.99 b. 4.22 5. Calculate the pH of a solution with [OH-] = 1.0 x 10-²M and identify if it's acidic or basic. a. pH = 2.0 acidic c. pH = 2.0 basic b. pH = 12.0 acidic d. pH = 12.0 basic

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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.