NH3 is a weak base (?b=1.8×10^−5) and so the salt NH4Cl acts as a weak acid. What is the pH of a solution that is 0.056M in NH4Cl at 25 °C?

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A: Acid is a substance which release H+ ions and base is substance which release OH- ions

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A: Given: Concentration of ammonia solution = 0.4 M Kb of ammonia = 1.8×10-5

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A: given, pOH= 10.10

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A: The false statement is     In this reaction H3O+ and OH - are conjugate acid-base pair

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A: pH = -log[H+] Relation between [H+], Ka and C of a weak acid solution: [H+] = (Ka x C)1/2

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Q: If the hydronium ion concentration is 2.5 x 10^-4, what is the pH ? __ Is this am acid or base ?

A: The concentration of hydronium ion (H3O+] = 2.5 × 10-4  pH = ?  This is an acid or base ?

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.