ΔS is -ve

dispersion medium-gas
dispersed phase-liquid

x ml of 0.1 M NaOH + x mL of 0.01 M HCI
No. of moles of NaOH = 0.1 x X x 10^-3
= 0.1 X x 10^-3
No. of moles of HCI = 0.01 x X x 10^-3
= 0.01 X x 10^-3
No. of moles of NaOH after mixing
= 0.1 X x 10^-3 - 0.01 X x 10^-3
= 0.09 X x 10^-3
Concentration of NaOH\(= (\frac{0.09x \times 10^{-3}}{2x \times 10^{-3}}) = 0 .045\)
[OH^-] = 0.045
pOH =-log (4.5 x 10^-2)
= 2 -log 4.5
= 2 - 0.65 = 1.35
pH = 14 - 1.35 = 12.65

for n ≠ 1 t_1/2 = \(\frac{2^{n-1} -1}{(n- 1) k[A_{0}]^{-1}}\)
for n = 0; t_1/2 = \(\frac{1}{2 k[A_{0}]^{-1}}\)
t_1/2 = \(\frac{[A_{0}]}{2 k}\)
t_1/2 α [A₀] ...(1)
Given [A₀] = 0.002 M; t_1/2 = 10 min
[A₀] = 0.04M; t_1/2 = ?
Substitute in (1)
10 min α 0.02 M...(2)
t_1/2 α 0.04M ....(3)
(3)(2)
⇒ t_1/2 / 10 min
= 0.04 M/0.02 M
t_1/2 = 2 x 10 min = 20 min

If number of close packed atoms = N, then
The number of Tetrahedral holes formed = 2N
The number of Octahedral holes formed = N
Therefore, N:2N = 1:2

a) Zn²⁺ (d¹⁰ ⇒  diamagnetic)
b) Co³⁺ (d⁶ Low spain ⇒  t_2g⁶ e⁰_g ; diamagnetic)
c) Ni²⁺  (d⁸ Low spain ⇒  t_2g⁶ e²_g ; paramagnetic)
d) [Ni(CN)₄]²⁺ (dsp² ; square planar, diamagnetic)

In the complex [M(en)₂(Ox)]Cl For the central metal ion M3+
The primary valence is = +3
The secondary valence = 6
sum of primary valence and secondary valence = 3 + 6 = 9

Homogenous catalysis	Heterogeneous catalysis
1. In a catalysed reaction, the reactants, products and catalyst are present in the same phase. Ex: \( 2\mathrm{SO}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})}+[\mathrm{NO}]_{(\mathrm{g})} \rightarrow 2 \mathrm{SO}_{3(\mathrm{~g})}+[\mathrm{NO}]_{(\mathrm{g})} \) [NO] - catalyst; gaseous state SO2, O2 & SO3 are gases.	1. In a catalysed reaction, the catalyst is present in a different phase (ie) it is not present in the same phase as that of the reactants or products. Ex: \(\mathrm{N}_{2(\mathrm{~g})}+3 \mathrm{H}_{2(\mathrm{~g})} \stackrel{\mathrm{Fe}_{(\mathrm{s})}}{\longrightarrow} 2 \mathrm{NH}_{3(\mathrm{~g})}\) Fe - catalyst; solid N2, H2 & NH3 are gases.
2. It is not a contact catalysis.	2. It is a contact catalysis and the mental catalyst will be in finely divided metal or as gauze.
3. It is explained by intermediate compound formation theory.	3. It is explained by adsorption theory.

(i) Zeolites are microporous, crystalline, hydrated, alumino silicates, made of silicon and aluminium tetrahedra.
(ii) There are about 50 natural zeolites and 150 synthetic zeolites.
(iii) As silicon is tetravalent and aluminium is trivalent, the zeolite matrix carries extra negative charge.
(iv) To balance the negative charge, there are extra framework cations for example H⁺or Na⁺ons. Zeolites carrying protons are used as solid acids, catalysis and they are extensively used in the petrochemical industry for cracking heavy hydrocarbon fractions into gasoline, diesel, etc.,
(v) Zeolites carrying Na⁺ ions are used as basic catalysis.
(vi) One of the most important applications of zeolites is their shape selectivity.
(vii) In zeolites, the active sites namely protons are lying inside their pores. So, reactions occur only inside the pores of zeolites.
Reactant selectivity:
When bulkier molecules in a reactant mixture are prevented from reaching the active sites within the zeolite crystal, this selectivity is called reactant shape selectivity.
Transition state selectivity:
If the transition state of a reaction is large compared to the pore size of the zeolite, then no product will be formed.
Product selectivity:
It is encountered when certain product molecules one too big to diffuse out of the zeolite pores.

In an Octahedral complex, the d-orbitals of the central metal ion, divide (1) into two sets of different energies. The separation in energy is the crystal field splitting energy.
The d-orbitals lying along the axes dx², dy² and dz² orbitals will experience strong repulsion and raise in energy to a greater extent than the orbitals with lobes directed between the axes (d_xy, d_yz, and d_zx)Thus the degenerate d-orbitals now split into two sets and the process is called crystal field splitting.

S. No	Double salts	Co-ordination compound
1.	They usually contain two simple salt in equimolar proportions	The simple salts from which they are formed may or may not be in equimolar proportion.
2.	They exists only in the solid state. In aqueous solution they dissociate completely into ions.	They exist in the solid state as well as in aqueous solution. This is because even in solution, the complex ion does not dissociate into ions.
3.	They are ionic compounds and do not contain any co-ordinate bond.	They may or may not be ion but the complex part always contain coordinate bonds
4.	The properties of the double salts are same as those of its constituent compounds.	The properties of the coordination compounds are different for its constituent bonds.
5.	In a double salt, the metal ion show their normal valency.	In a coordinate compound the metal ion satisfies its two types of valence called primary & secondary valenices.
6.	A double salt loses its identity and dissociates into its constitute simple ions in solution.	The complex ion does not lose its identity and never dissociate to give simple ions.
	Example: FeSO4 (NH4)2 SO4.6H2O	Example: K4[Fe(CN)6), K3[Fe(SCN)6)

(i) Ellingham diagram is constructed based only on thermodynamic considerations. It gives information about the thermodynamic feasibility of a reaction. It does not tell anything about the rate of the reaction. More over, it does not give any idea about the possibility of other reactions that might be taking place.
(ii) The interpretation of \(\triangle\)G is based on the assumption that the reactants are in equilibrium with the product which is not always true.

(a) If we apply DC current through the conductivity cell, it will lead to the electrolysis of the solution taken in the cell.
(b) So, AC current is used for this measurement to prevent electrolysis.

First law:
The mass of the substance (m) liberated at an electrode during electrolysis is directly proportional to the quantity of charge (Q) passed through the cell.
m α Q \(\left[\because \mathrm{I}=\frac{\mathrm{Q}}{\mathrm{t}} \Rightarrow \mathrm{Q}=\mathrm{It}\right]\)
m α It
m = ZIt
Where Z = electro chemical equivalent of the substance
I = current
t = time of passage of current
Second law:
When the same quantity of charge is passed through the solutions of different electrolytes, the amount of substances liberated at the respective electrodes are directly proportional to their electrochemical equivalents.
m α Z
\(\frac{m_{1}}{Z_{1}}=\frac{m_{2}}{Z_{2}}\)
m = mass of the metal deposited
Z = electro chemical equivalent

	hcp structure	ccp structure
1.	This is 'aba' pattern of arrangement.	This is 'abc' pattern of arrangement.
2.	The spheres can be arranged so as to fit into the depression in such a way that the third layer is directly over a first layer.	The third layer may be placed over the second layer in such a way that all the spheres of the third layer fit in octahedral voids.
3.	The tetrahedral voids of the second layer are covered by the spheres of the third layer.	This arrangement of the third layer is different from other two layers and the stacking of layers continued.
4.	6 spheres are present	4 spheres are present

(i) Helium is used to provide inert atmosphere in electric-arc welding of metals.
(ii) Helium has lowest boiling point hence used in cryogenics.
(iii) It is much less denser than air and hence used for filling air balloons.

(i) Borax is used for the identification of coloured metal ions.
(ii) In the manufacture optical and borosilicate glass, enamels and glazes for pottery.
(iii) It is also used as a flux in metallurgy.
(iv) It acts as a good preservative.

Cathodic protection:
In this technique, unlike galvanising the entire surface of the metal to be protected need not be covered with a protecting metal. Instead, metals such as Mg or zinc which is corroded more easily than iron can be used as a sacrificial anode and the iron material acts as a cathode. So iron is protected, but Mg or Zn is corroded. This known as sacrificial protection. (or) Cathodic protection.

(i) p^H = -log₁₀ [H₃O⁺]
(ii) The pH of a solution is defined as the negative logarithm of base 10 of the molar concentration of the hydronium ions present in the solution.

The solubility product of a compound is defined as the product of the molar concentration of the constituent ions, each raised to the power of its stoichiometric co - efficient in a balanced equilibrium equation.
X_mY_n (s) \(\rightleftharpoons\) mXⁿ⁺ _(aq) + nY^m-_(aq)
K_sp=[Xⁿ⁺]^m[Y^m-]ⁿ

\({ }_{22} \mathrm{Ti}-{ }_{18}[\mathrm{Ar}] 4 \mathrm{s}^{2} 3 \mathrm{d}^{2} / {}_{21}\mathrm{Sc}-{ }_{18}[\mathrm{Ar}] 4 \mathrm{~s}^{2} 3 \mathrm{~d} \)
\({ }_{22} \mathrm{Ti}^{3+}-{ }_{18}[\mathrm{Ar}] 3 \mathrm{~d}^{1} /{ }_{18} \mathrm{Sc}^{3+}{ }_{18}[\mathrm{Ar}] 3 \mathrm{~d}^{0}\)
(i) In this complex the central metal ion is Ti³⁺, which has d¹ configuration. This single electron occupies one of the t_2g orbitals in the octahedral aqua ligand field. When white light falls on this complex the electron absorbs light and promotes itself to e_g level. The spectral data show the absorption maximum is at 20000 cm^-1 corresponding to the crystal field splitting energy \(\left(\Delta_{o}\right)\) 239.7 kJmol^-1. The transmitted colour associated with this absorption is purple and hence the complex appears purple in colour.
(ii) Thus in \(\left[\mathrm{Ti}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+} \mathrm{d}-\mathrm{d}\) transition takes place.
(iii) But in \(\left[\mathrm{Sc}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+} \mathrm{Sc}^{3+}\) has the outer electronic configuration of 3d⁰ where d-d transition is not possible and it is colourless.

\((i) \quad 4 \mathrm{NaCl}+\mathrm{MnO}_{2}+4 \mathrm{H}_{2} \mathrm{SO}_{4} \rightarrow \mathrm{Cl}_{2}+\mathrm{MnCl}_{2}+4 \mathrm{NaHSO}_{4}+2 \mathrm{H}_{2} \mathrm{O} \)
\((ii) \quad \mathrm{NaNO}_{2}+\mathrm{HCl} \rightarrow \mathrm{NaCl}+\mathrm{HNO}_{2} \)
\((iii) \quad \mathrm{P}_{4}+3 \mathrm{NaOH}+3 \mathrm{H}_{2} \mathrm{O} \rightarrow 3 \mathrm{NaH}_{2} \mathrm{PO}_{2}+\mathrm{PH}_{3} \uparrow \)
\((iv) \quad 3 \mathrm{AgNO}_{3}+\mathrm{PH}_{3} \rightarrow \mathrm{Ag}_{3} \mathrm{P}+3 \mathrm{HNO}_{3} \)
\((v) \quad 4 \mathrm{Mg}+10 \mathrm{HNO}_{3} \rightarrow 4 \mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}+\mathrm{N}_{2} \mathrm{O}+6 \mathrm{H}_{2} \mathrm{O} \)
\((vi) \quad 2 \mathrm{KClO}_{3} \stackrel{\Delta}{\longrightarrow} 2 \mathrm{KCl}+3 \mathrm{O}_{2} \uparrow \)
\((vii) \quad \mathrm{Cu}+Con. Hot \mathrm{H}_{2} \mathrm{SO}_{4} \rightarrow \mathrm{CuSO}_{4}+2 \mathrm{H}_{2} \mathrm{O}+\mathrm{SO}_{2} \uparrow \)
\((viii) \quad 2 \mathrm{Sb}+3 \mathrm{Cl}_{2} \rightarrow 2 \mathrm{SbCl}_{3} \)
\((ix) \quad 2 \mathrm{HBr}+\mathrm{H}_{2} \mathrm{SO}_{4} \rightarrow 2 \mathrm{SO}_{2}+2 \mathrm{H}_{2} \mathrm{O}+\mathrm{Br}_{2} \)
\((x) \quad \mathrm{XeF}_{6}+3 \mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{XeO}_{3}+6 \mathrm{HF} \)
\((xi) \quad 5 \mathrm{XeO}_{6}^{4-}+2 \mathrm{Mn}^{2+}+14 \mathrm{H}^{+} \rightarrow 2 \mathrm{MnO}_{4}^{-}+5 \mathrm{XeO}_{5}+7 \mathrm{H}_{2} \mathrm{O} \)
\((xii) \quad 2 \mathrm{XeOF}_{4}+\mathrm{SiO}_{2} \rightarrow 2 \mathrm{XeO}_{2} \mathrm{~F}_{2}+\mathrm{SiF}_{4} \)
\((xiii) \quad Xe+{ 3F }_{ 2 }\overset { Ni/200atm }{ \underset { 400^{ 0 }C }{ \longrightarrow } }XeF_6\)

Argon prevents the oxidation of hot filament and prolongs the life in filament bulbs.