Match the term to the correct definition.


Screenshot 2024 01 17 173530

Screenshot 2024 01 17 173530

Step 1 of 2

Given is the match the term to the correct definition.

  1. Acid Ionization constant
  2. Lewis Acids
  3. Percent Ionization
  4. Strong Acids/Base
  5. Conjugate Acid-Base Pair
  6. Weak Acid/Base
  7. Base Ionization Constant
  8. pH
  9. Salt Hydrolysis
  10. Lewis Base
  11. Ion-Product Constant

We found out the definition and formula of the given above A to K terms and match with given statements.

Explanation:

Here we use the concept of acids and bases, chemical and ionic equilibrium.

Step 2 of 2

  1. Acid ionization constant is the equilibrium constant for the ionization of acid.

HA(aq)+H2O↽−−⇀H3O(aq)+A−(aq)

Ka = [H3O] [A] / [HA]

  1. Lewis acids are the electron acceptor and has vacant p or d orbital for accepting electrons and their octet is not complete and are electron deficient compounds.
  2. Percentage ionization is defined as ionized acid concentration (A) at equilibrium divided by the initial concentration of acid (HA) times 100%.

% ionization= [A] *100 / [HA]

  1. Strong Acid / Base

Strong acids are those which dissociates completely in solution and has high Ka value and low pKa value and pH<7. Example HClO4.

Strong bases are those which dissociates completely in solution and has high Kb value and low pKb value and pH>7. Example NaOH.

 

  1. Conjugate Acid -Base Pair. Every Bronsted acid has a conjugate base, and every Bronsted base has a conjugate acid.

 

HCl + H2O ⟶ H3O+ + Cl

Acid Base Conjugate Conjugate

acid base

Bronsted acid is a substance capable of donating a proton (H+).

Bronsted base is a substance that can accepts a proton.

Note – weak acid has strong conjugate acid and weak base has strong conjugate base and vice-versa.

 

  1. Weak Acid/Base.

Weak acid are those substance which dissociates very less in solution. Example is CH3COOH.

Weak base are those substance which dissociates very less in solution. Example is NH4OH⋅

  1. Base Ionization Constant (Kb) is the equilibrium constant for the reaction between a base, B, and water forming the conjugate acid, HB+, and OH.

Kb = [HB+] [OH] / [B]

 

pKb=-logKb

  1. pH is the negative logarithm of the hydrogen ion (H+) or hydronium ion (H3O) concentration.

pH = -log [H+]

or pH = -log [H3O+]

  1. Salt hydrolysis is defined as the reaction of the anion or cation of the salt with aqueous solution to produce either acidic or basic solution.

 

  1. Lewis Base are those substance that can donate one or more lone pair of electrons. All anions can acts as Lewis base and they are electron rich molecules. Example F, MgO etc.

 

  1. Ion Product Constant is the product of the molar concentration of H+ and OH ions at a particular temperature .

 

Kw= [H+] [OH]

At 298K Kw=10-14

pKW=-log KW

pKw=14

pKw=pH + pOH

14= pH + pOH

Explanation:

Hence from the given definition we find the term A, H, C, G, and K .

Final solution

Hence the given definitions are of term A, H, C, G and K respectively.

 

 

 

 

 

Leave a Reply

Your email address will not be published. Required fields are marked *

Call Now Button