A solution of dimethylamine is prepared by dissolving 1.3525 grams of dimethylamine in 25 mL ethanol and then diluting the solution to 100.00 mL with water. Write the weak base equilibrium and the ICE table and calculate the pH of this basic solution. The base-dissociation constant for dimethylamine (CH3NHCH3) is 9.52x10-7. Initial pH of the solution 10.23 Consider the titration of 10.00 mL of dimethylamine solution with 0.150 M HCI. Write the neutralization equation, weak acid equilibrium and the ICE table and calculate the pH of this acidic solution after the addition of 5.00 mL and 19.50 mL of 0.150 M HCI. pH of the solution after addition of 5.00 mL titrant pH of the solution after addition of 19.50 mL

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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.