Equilibrium

Question 1

Henry’s law

Answer 1

Mass of a gas dissolved in a given mass of solvent at any temp is prop to pressure of gas above solvent

Question 2

Character of equilibrium

Answer 2

1. Possible on in closed system
2. Both the opposing processes occur at same rate
3. All measurable qualities remain const

Question 3

Eq. mixture

Answer 3

Mixture of reactants & products in eq state

Question 4

Eq equation also known as

Answer 4

Law of mass action

Question 5

Law of chemical eq

Answer 5

At a temp, product of conc of products raised to their stoichio coeff divided by product of conc of reactants raise to their stoichio coeff is a const

Question 6

Homogeneous system

Answer 6

Reactants & products are in same phase

Question 7

Delta n =

Answer 7

No of moles of (products -reactants)

Question 8

Features of eq const

Answer 8

1. Applicable only when conc of reactants & products have constant value at eq
2. Independent of initial conc
3. Temp dependant
4. Eq const for Reverse reaction = eq const for forward reaction

Question 9

Applications of eq const

Answer 9

1. Predict extrnt of reaction based on its magnitude
2. Predict direction of reaction
3. Calc eq conc

Question 10

If K(c) > 10³

Answer 10

P > R

Question 11

If K(c) < 10^-3

Answer 11

R > P

Question 12

If Q(c) > K(c)

Answer 12

Dir of R

Question 13

If Q(c) < K(c)

Answer 13

Dir of P

Question 14

If delta G is -ve

Answer 14

Fd dir

Question 15

Le chatelier’s principle

Answer 15

Change in any factor that determine eq of a system will cause the system to change to reduce & counteract the change

Question 16

Effect of pressure change on eq

Answer 16

A pressure change obtained by changing volume can affect yield of products where total no of moles of reactants & products are diff

Question 17

If volume is halved, partial pressure & conc

Answer 17

Doubles

Question 18

Effect of inert gas

Answer 18

Addition of it at const volume doesn’t change Laotian pressure or conc

Question 19

Eq const for exothermic when temp increases

Answer 19

Decreases(-ve delta H)

Question 20

Effect if catalyst

Answer 20

No effect

Question 21

Ionic eq

Answer 21

Eq btw ions & unionized molecules

Question 22

Dissociation

Answer 22

Separation of ions in water already existing in solid state of solute

Question 23

Arrhenius concept of acids & bases

Answer 23

Acids dissociate in water to give H+ & bases OH‐

Question 24

Conjugate acid-base pair

Answer 24

Acid-base pair that differs only by 1 proton

Question 25

Bronsted Lowry theory

Answer 25

Acids are capable of donating H+ & bases accepting H+

Question 26

Bronsted acid is strong when

Answer 26

It's conjugate base is weak

Question 27

Lewis acids & bases

Answer 27

Acids accepts e' pair & bases donates e' pair

Question 28

Stronger acid ___ to stronger base

Answer 28

Donates a proton

Question 29

K(w)

Answer 29

Ionic product of water K(w) = [H+][OH-] = 10^-14M²

Question 30

K(w) is ___ dependant

Answer 30

Temp

Question 31

pH of a solution

Answer 31

-log[H+]

Question 32

Dissociation/ionization const

Answer 32

K(a)

Question 33

__ the value of K(a) stronger the acid

Answer 33

Larger

Question 34

Base ionization const

Answer 34

Eq const for base ionization

Question 35

K(b) =

Answer 35

c@²/(1-@)

Question 36

K(net) =

Answer 36

K1 × K2 ×...

Question 37

__ × __ = K(w)

Answer 37

K(a) × K(b)

Question 38

Polyprotic acids

Answer 38

Acids that have > 1 ionizable proton per molecule

Question 39

Extent of dissociation of acid depends on

Answer 39

Strenth & polarity of H-A bond

Question 40

When strength of H-A bond ___, energy to break it ___ so HA becomes stronger acid

Answer 40

Decreases; decreases

Question 41

Acid strength in increasing order

Answer 41

HF<

Question 42

E' -vity of A in increasing order

Answer 42

CH4

Question 43

Common ion effect

Answer 43

Shift in eq on adding a sub that provides more of an ionic species already present in dissociation eq

Question 44

Buffer solution

Answer 44

Solutions which resist change in pH on addition of small amounts

Question 45

Henderson-Hasselbalch equation for acid

Answer 45

pH = pKa + log[Conj base,A-]/[Acid,HA]

Question 46

Henderson-Hasselbalch equation for base

Answer 46

pOH = pKb + log[Conj acid,BH+]/[base,B]

Question 47

pH = pKa +

Answer 47

log[Salt]/[Acid]

Question 48

Henderson equation for acid & base together

Answer 48

pH = pKa + log[Conj acid, BH+]/[Base,B]

Question 49

Solvation enthalpy is always

Answer 49

-ve