Write the products of the following acid-base reaction. CH3OH NaNH2 ?

Q: Explain the difference between: a strong acid or base and a weak acid or base

A: pH scale helps us in measuring acidity or basicity of a solution. If a solution is neither acidic…

Q: Calculate the pH of an aqueous solution; 0.015 M KOH

A: Given: Concentration of KOH = [OH-] =  0.015 M

Q: Fill in the missing chemical formulae in the tables below. base conjugate acid H,0 Hpo, 2- НРО 4 OH

A:

Q: The pOH of an acidic solution is 12.87. What is [H⁺]?

A: We have to calculate the concentration of hydrogen ion.

Q: Draw the Lewis structure of the hydronium ion. Is it an acid or a base?

A: An acid is H+ is donor . A base , which accept H+  Hydronium ion donate H+

Q: Select the pair of substances in which an acid is listed followed by its conjugate base.

A: According to Bronsted-Lowry acid-base concept, an acid is a species which can donate proton and a…

Q: In HClO2 + H2O —> ClO2- + H3O+ ; who is the conjugate acid and the conjugate base?

A: We are given a reaction in which we have to find which species act as conjugate acid and which one…

Q: 7. What are the conjugate base and conjugate acid for HSO, ? What is the term used to describe…

A: Conjugate acid is formed when we add protons to a base and conjugate base is formed when proton is…

Q: The pH of 0.0720M solution of a weak acid is 2.670. What is the Ka of the acid

A:

Q: Write formulas for the Lewis acid and the Lewis base that react to form H3NAlBr3.

A: According to the Lewis Concept of acid-base:-  Acids are electron acceptor  bases are electron donor

Q: Calculate the pH of an acqueous solution; 0.0025M Hl

A: HI is a strong acid. 0.0025 M HI results in release of 0.0025 M hydrogen ions.

Q: Why is water both an acid and a base according to the bronsted-lowry definition

A: According to Bronsted-lowery concept, species which donates proton act as acid whereas species which…

Q: Rank the acids in order of increasing acid strength: CH3COOH, CH2CICOOH, CHCI,COOH, CCl;COOH,…

A:

Q: Calculate the [H3O+] in an HCl solution with a pH of 2.3.

A: The pH of the solution can be calculated by using the following expression:  To determine the…

Q: What is the [OH -] in a solution with a pH of 8.97?

A: Since pH = -log[H+] = 14 + log [OH -]

Q: A 0.050 M solution of the salt NB has a pH of 9.00. Calculate the pH of a 0.01 M solution of HB.

A: pOH = 14-pH = 14- 9 =5 pOH = -log[OH-]So[OH-] = 10-pOH[OH-] = 10-5 The  Reaction…

Q: From the fact that H2s is a weak acid, would you predict that a solution of Na2S would be acidic,…

A: When the concentration of hydrogen ions is relatively more than the concentration of hydroxide ions,…

Q: Use the equation of the dissociation of the weak acid and a Le Schatelier principle to answer the…

A:

Q: What is the NIE for any neutralization reaction?

A: Neutralization reaction: Acid and base react to form salt and water, this reaction is known as a…

Q: Is NH4ClO basic, acid, or neutral?

A: When a salt of strong base and weak acid is hydrolysed it gives basic solution i e salt is basic in…

Q: Which of the following chemical formulas corresponds to a base? HCl; KOH; H2SO4; HNO3

A: Acids are H+ (proton) donors and bases donate the OH- ions.

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.