Equilibrium(nb) 2

Question 1

Relationship between equilibrium constant and gibs free energy

Answer 1

The value of K doesn’t depend upon the rate of reaction is directly proportional to the wiring of G.

Question 2

Mathematical expression for thermodynamical view of equilibrium constant.

Answer 2

K= e^dG/RT

Question 3

Optimum Conditions for Haber’s process

Answer 3

• Temperature= 750 K
• Pressure = 200 atm
• Catalyst = Fe
• Promoter = Mo

Question 4

Electrolyte

Answer 4

Substances that contain electricity in their acquisitions and on as electrolytes. Example inorganic acids, bases, salts

Question 5

Non electrolyte.

Answer 5

Substances that do not conduct electricity are known as non-electrolytes.
example glucose.

Question 6

Strong electrolytes

Answer 6

Substances which should associate almost a completely into ions in aqua solutions are called good conductors of electricity.
Eg: - NaOH, HCl

Question 7

Weak Electrolytes

Answer 7

Substances which are dissociated to a small extent in aqueous solution.
Eg: - CH3COOH

Question 8

Dissociation

Answer 8

When an ionic compound is dissolved in water, the ions are already present in the solid compound or separates out.
Eg: - NaCl

Question 9

Ionization

Answer 9

When a neutral molecule which does not contain ions then dissolves in water splits to produce ions in the solution.
Eg: - HCl ( Polar Covalent compound)

Question 10

The extent to which ionization occurs depends on the

Answer 10

1. Strength of the bond.
2. Extent of solution of ions produced.

Question 11

Ionic equilibrium

Answer 11

It is the equilibrium B/w the ions and the undissociated electrolyte.

Question 12

But is an acid and base based on the classical concept?

Answer 12

Acids are substances that turn blue letters to red lightness and releases dihydrogen on reacting with some metal.
Eg: - HCl
Bases are substances that turn red litmus to blue, better taste to soup to touch.
Eg: - NaOH

Question 13

What are acid and bases based on arhenius concept?

Answer 13

Acids are substances that dissociates in water to give hydration ions while bases are substances which dissociate in water to give hydroxide ions.

H plus ions are very reactive and cannot exist freely in acquisitions so it binds to oxygen atom of a solvent molecule to give trigonal hydronium ion.

Question 14

What is an acid or base based on brownstedt lorry concept.

Answer 14

An acid is a substance which donates a hydrogen ion while a base is a substance of which accepts hydrogen ion.

Question 15

Define conjugate acid base pair

Answer 15

The acid base pair that differs only by one proton is called conjugate acid base pair.

Question 16

limitations of Brownstead Lowry’s concept

Answer 16

Substances like BF3 and AlCl3 do not have any hydrogen so it cannot give Proton but still act as acids.

Question 17

What are acid and bases based on Lewis’s concept of acid and bases.

Answer 17

And acid is substantial which accepts a lone pair of electron while a base is a substance which can donate a lone pair of Electron.

Question 18

What is the strong acid

Answer 18

Substances which almost completely dissociates into their constituencies in an aqueous solution.

Question 19

What is a Strong Base?

Answer 19

substances which completely dissociate into ions in an aqueous medium giving hydroxyl ions.

Question 20

pH scale

Answer 20

It is defined as the negative logarithm to the base 10 of the activity of hydrogen ion.
- at 25 degrees the pH of water is 7.

Question 21

Ionization constants of weak acids and bases

Answer 21

Ka/b = C@^2/ 1-@

Question 22

Relation between Ka and Kb

Answer 22

pKa + pKb = pKw

Question 23

define polybasic acids

Answer 23

Assets having more than one ionizable proton per molecule are known as polybasic acids.

Question 24

Why is Ka1>Ka2

Answer 24

It is more difficult to remove a positively charged proton from a negative charged ion due to electrostatic forces. Greater the charge on the negative ion, more difficult to remove the Proton hence it is less acidic.

Question 24

Strength of HA bond

Answer 24

When the strength of HA bond decreases, the energy required to break the bond decreases so ha becomes a strong acid.

Question 25

Polarity of HA bond

Answer 25

Then Ache bond becomes more polar, the ultra negativity difference between H and a atom increases. Bond breaks easily so strength of the acid is stronger.

Question 26

define common ion effect.

Answer 26

If to the solution of weak electrolytes which ionizes to a small extent a strong electrolyte having a common ion is added which ionizes almost completely. The ionization of weak electrolyte is further suppressed this is known as common ion effect.

Question 27

Buffer solutions

Answer 27

The solution which resist change in ph on dilution or with the addition of small amount of acid or alkali are called a buffer solutions.

Question 28

Solubility product constant

Answer 28

Solubility product of an electrolyte at a specific temperature is defined as the product of the molar concentration of its ions in a saturated solution each concentration raised to the power equal to the number of ions produced on dissociation of one molecule of the electrolyte.

Question 29

Application of solubility product

Answer 29

• In the calculation of solubility of aspiringly soluble salt.
• In predicting ionic or precipitation reactions.
• In the precipitation of soluble salt
• in qualitative analysis, the complete scheme of qualitative analysis is based on the concept of solubility product and common ion effect.

Question 30

Difference between ionic product and solubility product

Answer 30

• Ionic product is applicable to all types of solutions May be saturated or unsaturated. Solubility product is applicable only to a saturated solution in which there is equilibrium between the undissolved salt and ions present in the solution.
• Solubility product of a salt at a constant temperature is constant whereas ionic product depends upon the concentration of ions in the solution.