Question 1 :
For the reaction {tex} \mathrm { CO } ( \mathrm { g } ) + ( 1 / 2 ) \mathrm { O } _ { 2 } ( \mathrm { g } ) = \mathrm { CO } _ { 2 } ( \mathrm { g } ) , K _ { p } / K _ { c } {/tex} is

Question 2 :
Hydrogen ion concentration in {tex} \mathrm { mol } / \mathrm { L } {/tex} in a solution of {tex} \mathrm { pH } = 5.4 {/tex} will be :

Question 3 :
Solubility product constants {tex} \left( \mathrm { K } _ { \mathrm { sp } } \right) {/tex} of salts of types {tex} \mathrm { Mx } , \mathrm { Mx } _ { 2 } {/tex} and {tex} \mathrm { M } _ { 3 } \mathrm { X } {/tex} at temperature {tex} \mathrm { T } {/tex} are {tex} 4.0 \times 10 ^ { - 8 } {/tex}, {tex} 3.2 \times 10 ^ { - 14 } \text { and } 2.7 \times 10 ^ { - 15 }{/tex} respectively. Solubilities {tex}\mathrm {(mol dm} ^ { - 3 } ){/tex} of the salts at temperature '{tex} \mathrm { T } {/tex}' are in the order

Question 4 :
At {tex} 25 ^ { \circ } \mathrm { C } , {/tex} the solubility product of {tex} \mathrm { Mg } ( \mathrm { OH } ) _ { 2 } {/tex} is {tex} 1.0 \times 10 ^ { - 11 } {/tex} . At which {tex} \mathrm { pH } , {/tex} will {tex} \mathrm { Mg } ^ { 2 + } {/tex} ions start precipitating in the form of {tex} \mathrm { of } {/tex} {tex} \mathrm { Mg } ( \mathrm { OH } ) _ { 2 } {/tex} from a solution of {tex}0.001\, \mathrm { M \ Mg } ^ { 2 + } {/tex} ions?

Question 5 :
In which of the following reactions, increase in the volume at constant temperature does not affect the number of moles at equilibrium?

Question 7 :
For the reaction<br>{tex} 2 \mathrm { NO } _ { 2 ( \mathrm { g } ) } \rightleftharpoons 2 \mathrm { NO } _ { ( \mathrm { g } ) } + \mathrm { O } _ { 2 ( \mathrm { g } ) } {/tex} {tex} \left( K _ { c } = 1.8 \times 10 ^ { - 6 } \text { at } 184 ^ { \circ } \mathrm { C } \right) {/tex} {tex} ( R = 0.0831 \mathrm { kJ } / ( \mathrm { mol } \mathrm { K } ) ) . {/tex} When {tex} K _ { p } {/tex} and {tex} K _ { c } {/tex} are compared at {tex} 184 ^ { \circ } \mathrm { C } {/tex} it is found that

Question 8 :
For the equilibrium<br>{tex} \mathrm { CO } + \mathrm { H } _ { 2 } \mathrm { O } \rightleftharpoons \mathrm { CO } _ { 2 } + \mathrm { H } _ { 2 } {/tex}<br>The relation between {tex} \mathrm { K } _ { \mathrm { p } } {/tex} and {tex} \mathrm { K } _ { \mathrm { c } } {/tex} at {tex} 25 ^ { \circ } \mathrm { C } {/tex} and at {tex} 100 ^ { \circ } \mathrm { C } {/tex} are

Question 9 :
For the reaction {tex} \mathrm { SO } _ { 2 ( g ) } + \frac { 1 } { 2 } \mathrm { O } _ { 2 ( g ) } \rightleftharpoons \mathrm { SO } _ { 3 ( g ) } , {/tex} if {tex} K _ { P } = K _ { C } ( R T ) ^ { x } {/tex} where the symbols have usual meaning then the value of {tex} x {/tex} is (assuming ideality):

Question 10 :
The molar solubility (in mol {tex} \left. \mathrm { L } ^ { - 1 } \right) {/tex} of a sparingly soluble salt {tex} M \mathrm { X } _ { 4 } {/tex} is {tex} s {/tex}. The corresponding solubility product is {tex} K_{sp} .{/tex} {tex} \mathrm s{/tex} is given in terms of {tex} K {/tex} by the relation

Question 11 :
Which of the following relation holds true for an equilibrium reaction, if its reaction quotient {tex} ( Q ) = 1 ? {/tex}

Question 12 :
Let the solubility of an aqueous solution of {tex} \mathrm { Mg } ( \mathrm { OH } ) _ { 2 } {/tex} be {tex} x {/tex} then its {tex} K _ { s p } {/tex} is

Question 13 :
Pure {tex} \mathrm { NH } _ { 3 } {/tex} is placed in a vessel at a temperature where its dissociation is appreciable. At equilibrium

Question 14 :
For the reaction, {tex} \mathrm { CO } _ { ( \mathrm { g } ) } + \mathrm { Cl } _ { 2 \mathrm { g } } \Rightarrow \mathrm { COCl } _ { 2 \mathrm { g } } , {/tex} the {tex} K _ { p } / K _ { \mathrm { c } } {/tex} is equal to

Question 15 :
The dissociation constant of monobasic acids {tex}\mathrm {A , B} {/tex} and {tex}\mathrm C {/tex} are {tex} 10 ^ { - 4 } , 10 ^ { - 6 } {/tex} and {tex} 10 ^ { - 10 } {/tex} respectively. The concentration of each monobasic acid is {tex}0.1 \mathrm M{/tex}. Which of the following has been arranged in increasing order of {tex}\mathrm{pH}{/tex}?

Question 16 :
The equilibrium constant at {tex}298 \mathrm { K } {/tex} for a reaction {tex} A + B \rightleftharpoons {/tex} {tex} C + D {/tex} is {tex} 100 . {/tex} If the initial concentration of all the four species were {tex} 1\mathrm { M } {/tex} each, then equilibrium concentration of {tex} D ( \text { in mol } {/tex} {tex} \mathrm { L } ^ { - 1 } {/tex} ) will be :

Question 17 :
The {tex} \mathrm { pK } _ { a } {/tex} of a weak acid, {tex} \mathrm { HA } {/tex}, is {tex}4.80{/tex}. The {tex} \mathrm { pK } _ { b } {/tex} of a weak base, {tex} \mathrm { BOH } {/tex} is {tex} 4.78{/tex}. The {tex} \mathrm { pH } {/tex} of an aqueous solution of the corresponding salt, {tex} \mathrm { BA } , {/tex} will be

Question 18 :
The exothermic formation of {tex} \mathrm { CIF } _ { 3 } {/tex} is represented by the equation:<br>{tex} \mathrm { Cl } _ { 2 } ( \mathrm { g } ) + 3 \mathrm { F } _ { 2 } ( \mathrm { g } ) \rightleftharpoons 2 \mathrm { ClF } _ { 3 } ( \mathrm { g } ) ; \Delta \mathrm { H } = - 329 \mathrm { kJ } {/tex} <br>Which of the following will increase the quantity of {tex} \mathrm { CIF } _ { 3 } {/tex} in an equilibrium mixture of {tex} \mathrm { Cl } _ { 2 } , \mathrm { F } _ { 2 } {/tex} and {tex} \mathrm { ClF } _ { 3 } ? \quad [ 2005 \mathrm { I } ] {/tex}<br>

Question 19 :
For the reaction equilibrium {tex} \mathrm { N } _ { 2 } \mathrm { O } _ { 4 } ( \mathrm { g } ) \rightleftharpoons 2 \mathrm { NO } _ { 2 } ( \mathrm { g } ) {/tex}<br>the concentrations of {tex} \mathrm { N } _ { 2 } \mathrm { O } _ { 4 } {/tex} and {tex} \mathrm { NO } _ { 2 } {/tex} at equilibrium are {tex} 4.8 \times 10 ^ { - 2 } {/tex} and {tex} 1.2 \times 10 ^ { - 2 } \mathrm { mol } \mathrm { L } ^ { - 1 } {/tex} respectively. The value of {tex} K _ { \mathrm { c } } {/tex} for the reaction is<br>

Question 20 :
The solubility in water of a sparingly soluble salt {tex} \mathrm { AB } _ { 2 } {/tex} is {tex} 1.0 \times 10 ^ { - 5 } \mathrm { mol } \mathrm { L } ^ { - 1 } {/tex} . Its solubility product number will be

Question 21 :
The solubility product of a salt having general formula {tex} M X _ { 2 } {/tex}, in water is {tex} 4 \times 10 ^ { - 12 } {/tex} The concentration of {tex} M ^ { 2+ } {/tex} ions in the aqueous solution of the salt is

Question 22 :
Solid {tex} \mathrm { Ba } \left( \mathrm { NO } _ { 3 } \right) _ { 2 } {/tex} is gradually dissolved in a {tex} 1.0 \times 10 ^ { - 4 } \mathrm { M } {/tex} {tex} \mathrm { Na } _ { 2 } \mathrm { CO } _ { 3 } {/tex} solution. At what concentration of {tex} \mathrm { Ba } ^ { 2 + } {/tex} will a precipitate begin to form? {tex} \left( \mathrm { K } _ { \mathrm { SP } } \text { for } \mathrm { BaCO } _ { 3 } = 5.1 \times 10 ^ { - 9 } \right) {/tex}

Question 24 :
The conjugate base of {tex} \mathrm { H } _ { 2 } \mathrm { PO } _ { 4 } ^ { - } {/tex} is

Question 25 :
The pH of a saturated aqueous solution of {tex} \mathrm { CO } _ { 2 } {/tex} is {tex} 5 ; {/tex} For {tex} \mathrm { H } _ { 2 } \mathrm { CO } _ { 3 } , \mathrm {K a _ { 1 }} = 10 ^ { - 7 } {/tex} and {tex} \mathrm{K a _ { 2 }} = 10 ^ { - 11 } . {/tex} At the given pressure the solubility of {tex} \mathrm { CO } _ { 2 } {/tex} in water is {tex} 10 ^ { - 2 } ( \mathrm { M } ) . {/tex} What is the value of {tex} - \log \left[ \mathrm { CO } _ { 3 } ^ { 2 - } \right] {/tex} in the nearest posssible integers?

Question 26 :
For the reaction equilibrium, {tex} \mathrm { N } _ { 2 } \mathrm { O } _ { 4 ( \mathrm { g } ) } \rightleftharpoons 2 \mathrm { NO } _ { 2 ( g ) } {/tex} the concentrations of {tex} \mathrm { N } _ { 2 } \mathrm { O } _ { 4 } {/tex} and {tex} \mathrm { NO } _ { 2 } {/tex} at equilibrium {tex} {/tex} are {tex} 4.8 \times 10 ^ { - 2 } {/tex} and {tex} 1.2 \times 10 ^ { - 2 } \mathrm { mol } \mathrm { L } ^ { - 1 } {/tex} respectively. The value of {tex} K _ { c } {/tex} for the reaction is

Question 27 :
Three reactions involving {tex} \mathrm { H } _ { 2 } \mathrm { PO } _ { 4 } ^ { - } {/tex} are given below:<br> (i) {tex} \mathrm { H } _ { 3 } \mathrm { PO } _ { 4 } + \mathrm { H } _ { 2 } \mathrm { O } \rightarrow \mathrm { H } _ { 3 } \mathrm { O } ^ { + } + \mathrm { H } _ { 2 } \mathrm { PO } _ { 4 } ^ { - } {/tex} <br>(ii) {tex} \mathrm { H } _ { 2 } \mathrm { PO } _ { 4 } ^ { - } + \mathrm { H } _ { 2 } \mathrm { O } \rightarrow \mathrm { HPO } _ { 4 } ^ { 2 - } + \mathrm { H } _ { 3 } \mathrm { O } ^ { + } {/tex} <br>(iii) {tex} \mathrm { H } _ { 2 } \mathrm { PO } _ { 4 } ^ { - } + \mathrm { OH } ^ { - } \rightarrow \mathrm { H } _ { 3 } \mathrm { PO } _ { 4 } + \mathrm { O } ^ { 2 - } {/tex}<br>In which of the above does {tex} \mathrm { H } _ { 2 } \mathrm { PO } _ { 4 } ^ { - } {/tex} act an acid? <br>

Question 28 :
An amount of solid {tex} \mathrm { NH } _ { 4 } \mathrm { HS } {/tex} is placed in a flask already containing ammonia gas at a certain temperature and 0.50 atm pressure. Ammonium hydrogen sulphide decomposes to yield {tex} \mathrm { NH } _ { 3 } {/tex} and {tex} \mathrm { H } _ { 2 } \mathrm { S } {/tex} gases in the flask. When the decomposition reaction reaches equilibrium, the total pressure in the flask rises to 0.84 atm? The equilibrium constant for {tex} \mathrm { NH } _ { 4 } \mathrm {HS } {/tex} decomposition at this temperature is<br>

Question 29 :
Find out the value of {tex}\mathrm K _ {\mathrm C } {/tex} for each of the following equilibria from the value of {tex} \mathrm K _ {\mathrm P } {/tex} :<br>(i) {tex} 2 \mathrm { NOCl } ( \mathrm { g } ) \rightleftharpoons 2 \mathrm { NO } ( \mathrm { g } ) + \mathrm { Cl } _ { 2 } ( \mathrm { g } ) ;\mathrm K _ {\mathrm P } = 1.8 \times 10 ^ { - 2 }{/tex} at {tex}500 \mathrm { K } {/tex}<br>(ii) {tex} \mathrm { CaCO } _ { 3 } ( \mathrm { s } ) \rightleftharpoons \mathrm { CaO } ( \mathrm { s } ) + \mathrm { CO } _ { 2 } ( \mathrm { g } );\mathrm K _ {\mathrm p } = 167 {/tex} at {tex}1073 \mathrm { K } {/tex} <br>The value of {tex}\mathrm K _ {\mathrm c } {/tex} are respectively

Question 30 :
The solubility in water of a sparingly soluble salt {tex} A B _ { 2 } {/tex} is {tex} 1.0 \times 10 ^ { - 5 } \mathrm { mol } \mathrm { L } ^ { - 1 } {/tex}. Its solubility product will be

Question 31 :
What is the conjugate base of {tex} \mathrm { OH } ^ { - } ? {/tex}

Question 32 :
Among the following, which causes the greatest change in pH on addition to {tex}\mathrm{50 \ ml}{/tex} of {tex}\mathrm{0.2\ M}{/tex} oxalic acid solution?

Question 34 :
{tex}\mathrm{pH}{/tex} of {tex}\mathrm {Ba(OH)}{/tex} solution is {tex} 12 . {/tex} Its solubility product is

Question 35 :
$\displaystyle { BaCl }_{ 2 }$ dissociates in water to give one $\displaystyle { Ba }^{ 2+ }$ ion and two $\displaystyle { Cl }^{ - }$ ions. If concentrated $\displaystyle HCl$ is added to this solution :

Question 37 :
{tex} \left. \text { The molar solubility (in mol } \mathrm { L } ^ { - 1 } \right) {/tex} of a sparingly soluble salt {tex} \mathrm { MX } _ { 4 } {/tex} is 's' . The corresponding solubility product is {tex} K _ { s p } . \mathrm { 's } ^ { \prime } {/tex} is given in term of {tex} K _ { s p } {/tex} by the relation:

Question 38 :
{tex} \mathrm { C } ( \mathrm { s } ) + \mathrm { H } _ { 2 } \mathrm { O } ( \mathrm { g } ) \rightleftharpoons \mathrm { H } _ { 2 } ( \mathrm { g } ) + \mathrm { CO } ( \mathrm { g } ) {/tex}<br>What will be the effect of pressure on the above equilibrium process?<br>

Question 39 :
To {tex} 250.0 \mathrm { \ ml } {/tex} of {tex} \mathrm { \ M } / 50 \mathrm { H } _ { 2 } \mathrm { SO } _ { 4 } , {/tex} {tex} 4.0 \mathrm { g } {/tex} of solid {tex} \mathrm { NaOH } {/tex} is added and the resulting solution is diluted to {tex} 1.0 \mathrm {\ L } {/tex}. The pH of the resulting solution is

Question 40 :
In a saturated solution of the sparingly soluble strong electrolyte {tex} \left. \mathrm { AgIO } _ { 3 } \text { (molecular mass } = 283 \right) {/tex} the equilibrium which sets in is <br> {tex} \mathrm { AgIO } _ { 3 ( s ) } \rightleftharpoons \mathrm { Ag } ^ { + } ( \mathrm { aq } ) + \mathrm { IO } _ { 3 } ^ { - } ( \mathrm { aq } ) . {/tex} If the solubility product constant {tex} K _ { s p } {/tex} of {tex} A g I O _ { 3 } {/tex} at a given temperature is {tex} 1.0 \times 10 ^ { - 8 } , {/tex} what is the mass of AgIO {tex} _ { 3 } {/tex} contained in {tex}100 \mathrm { ml } {/tex} of its saturated saolution?<br>

Question 41 :
<font> The pH of a solution obtained by mixing 50 ml of 0.4 N HCl and 50 ml of 0.2 N NaOH is :</font></p>

Question 42 :
<font>What is the minimum pH when Fe(OH)3 starts precipitating from a solution containing 0.1M FeCl3? Ksp of Fe(OH)3 = 8 × 10-13 M3</font></p>

Question 44 :
<font> What will be the pOH of 0.5 × 10</font>^{<font>-4</font>}<font> M H</font>_{<font>2</font>}<font>SO</font>_{<font>4</font>}<font> solution -</font></p>

Question 45 :
<font> 10</font>^{<font>-6</font>}<font> M NaOH is diluted by 100 times. The pH of diluted base is -</font></p>

Question 46 :
<font> When 0.1 mole solid NaOH is added in 1lt of 0.1 M NH3(aq) then which statement is wrong? <br/> (Kb = 2 × 10-5, log 2 = 0.3)</font></p>

Question 47 :
<font>Solubility product of silver bromide is 5.0 × 10-13 . This quantity of potassium bromide (molar mass taken as 120 g mol-1) to be added to 1 litre of 0.05 M solution of silver nitrate to start the precipitation of AgBr is :</font></p>

Question 48 :
<font>At 25</font>^{<font>0</font>}<font>C, the solubility product of Mg(OH)2 is 1.0 ´ 10-11. At Which pH, will Mg2+ ions start precipitating in the form of Mg(OH)2 from a solution of 0.001 M Mg2+ ions ?</font></p>

Question 49 :
<font>Identify the amphoteric species from the following :</font></p> <p align="justify"> <font>(I) H2O</font></p> <p align="justify"> <font>(II) NH3</font></p> <p align="justify"> <font>(III) H2PO4- (IV) HCO3-</font></p>

Question 50 :
<font>At 25ºC pH range of phenolphthalein is 8 - 10. At 100ºC pH range of phenolphthalein would be-</font></p>