Ionic Equilibrium PYQs Set 6 (PDF)

Set 6 of 8 · Questions 151-180 of 233

In the print window choose “Save as PDF”. The file prints without a web address or date line.

Mere Teacher · Previous Year Questions NEET Chemistry · Ionic Equilibrium · Set 6 (Q151-180)
Scan or visit mereteacher.com for free PYQ practice, timed CBT tests, step-by-step solutions and BroBot AI. Answers and solutions are free with a sign-up.
151. $For ammonia formation from constituent elements, the expression for K_{C} is$ (1) $K_{C} = \frac{( NH _{3} ) ^{3}}{( N _{2} ) ^{3} ( H _{2} ) ^{3}}$ (2) $K_{C} = \frac{( NH _{3} ) ^{2}}{( N _{2} ) ( H _{2} ) ^{3}}$ (3) $K_{C} = \frac{( NH _{3} )}{( N _{2} ) ( H _{2} )}$ (4) $K_{C} = (NH_{3})^{2}$ 152. $If K_{1} and K_{2} are the respective equilibrium constants for the two reactions, X e F_{6 (g)} + H_{2} O_{(g)} \to X e O F_{4 (g)} + 2 H F_{(g)} X e O_{4 (g)} + X e F_{6 (g)} \to X e O F_{4 (g)} + X e O_{3} F_{2 (g)}, the equilibrium constant of the reaction, X e O_{4 (g)} + 2 H F_{(g)} \to X e O_{3} F_{2 (g)} + H_{2} O_{(g)}, will be$ (1) $K_{1} / K_{2}$ (2) $K_{1} \cdot K_{2}$ (3) $K_{1} / (K_{2})^{2}$ (4) $K_{2} / K_{1}$ 153. $40 mL of a mixture of CH_{3} COOH and HCl (aqueous solution) is titrated against 0.1 M NaOH solution conductometrically. Which of the following statement is correct?$ (1) $The concentration of CH_{3} COOH in the original mixture is 0.005 M$ (2) $The concentration of HCl in the original mixture is 0.005 M$ (3) $CH_{3} COOH is neutralised first followed by neutralisation of HCl$ (4) $Point 'C' indicates the complete neutralization of HCl$ 154. $Calculate the pO H of asolution at 2 5^{0} C that contains 1 \times 1 0^{- 10} M ofhydronium ions, i.e. H_{3} O^{+}$ (1) $4.000$ (2) $9.000$ (3) $1.000$ (4) $7.000$ 155. $One mole of PCl_{5} (g) was heated in a 1 L closed flask at 500 K . At equilibrium, 0.1 mole of Cl_{2} (g) was formed. What is its K_{p} (in atm)? (Given R = 0.082 L atm mol^{- 1} K^{- 1})$ (1) $2.7 \times 10^{- 4}$ (2) $0.455$ (3) $0.0111$ (4) $90.0$ 156. $The ionization constant of ammonium hydroxide is 1.77 \times 1 0^{- 5} at 298 K. Hydrolysis constant of ammonium chloride is$ (1) $6.50 \times 1 0^{- 12}$ (2) $5. 65 \times 1 0^{- 13}$ (3) $5. 65 \times 1 0^{- 12}$ (4) $5. 65 \times 1 0^{- 10}$ 157. $The solubility o f A g C 1_{(s)} with solubility product 1.6 \times 1 0^{- 10} in 0.1 MNaCl solution would be$ (1) $1. 26 \times 1 0^{- 5} M$ (2) $1. 6 \times 1 0^{- 9} M$ (3) $1. 6 \times 1 0^{- 11} M$ (4) $zero.$ 158. $20 mL of 0.1 M N H_{4} OH is mixed with 40 mL of 0.05 M HC1. The pH of the mixture is nearest to: (Given: K_{b} (N H_{4} OH) = 1 x 1 0^{- 5}, log 2 = 0.30, log 3 = 0.48, log 5 = 0.69, log 7 = 0.84, log 11 =1.04)$ (1) $3.2$ (2) $4.2$ (3) $5.2$ (4) $6.2$ 159. $A 20litre container at 400 K contains C O_{2 (g)} at pressure 0.4 atm and an excess of S r O (neglect the volume of solid S r O). The volume of the container is now decreased by moving the movable piston fitted in the container. The maximum volume of the container, when pressure of C O_{2} attains its maximum value, will be (Given that: K_{p} = 1.6 a t m)$ (1) $10litre$ (2) $4litre$ (3) $2litre$ (4) $5litre$ 160. $Which of the following molecules acts as a Lewis acid?$ (1) $(C H_{3})_{2} O$ (2) $(C H_{3})_{3} P$ (3) $(C H_{3})_{3} N$ (4) $(C H_{3})_{3} B$ 161. $In which of the following equilibrium K_{c} and K_{p} are not equal?$ (1) $2N O_{(g)} ⇌ N_{2 (g)} + O_{2 (g)}$ (2) $S O_{2 (g)} + N O_{2 (g)} ⇌ S O_{3 (g)} + N O_{(g)}$ (3) $H_{2 (g)} + I_{2 (g)} ⇌ 2H I_{(g)}$ (4) $2 C_{(s)} + O_{2 (g)} ⇌ 2C O_{2 (g)}$ 162. $0.1 mole of C H_{3} N H_{2} (K_{b} = 5 \times 1 0^{-4}) is mixed with 0.08 mole of HCl and diluted to one litre. What will be the H^{+} concentration in the solution ?$ (1) $8 \times 1 0^{-2} M$ (2) $8 \times 1 0^{-11} M$ (3) $1.6 \times 1 0^{-11} M$ (4) $8 \times 1 0^{-5} M$ 163. $K M n O_{4} can be prepared from K_{2} M n O_{4} as per the reaction, + 4 O H^{-} The reaction can go to completion by removing O H^{-} ions by adding$ (1) $C O_{2}$ (2) $S O_{2}$ (3) $HCl$ (4) $KOH$ 164. $Conjugate base for Bronsted acids H_{2} O and HF are:$ (1) $O H^{-} and H_{2} F^{+}, respectively$ (2) $H_{3} O^{+} and F^{-}, respectively$ (3) $O H^{-} and F^{-}, respectively$ (4) $H_{3} O^{+} and H_{2} F^{+},respectively$ 165. $For any reversible reaction, if we increase concentration of the reactants, then effect on equilibrium constant$ (1) $depends on amount of concentration$ (2) $unchange$ (3) $decrease$ (4) $increase.$ 166. $Following solutions were prepared by mixing different volumes of NaOH and H C l of different concentrations: A. 60 m L \frac{M}{10} H C l + 40 m L \frac{M}{10} NaOH B. 55 m L \frac{M}{10} H C l + 45 m L \frac{M}{10} NaOH C. 75 m L \frac{M}{5} H C l + 25 m L \frac{M}{5} NaOH D. 100 m L \frac{M}{10} H C l + 100 m L \frac{M}{10} NaOH p H of which one of them will be equal to 1?$ (1) $B$ (2) $A$ (3) $D$ (4) $C$ 167. $Solution of 0.1 N NHOH and 0.1 N N H_{4} C I has p H 9.25 . Then find out p K_{b} of NHOH.$ (1) $9.25$ (2) $4.75$ (3) $3.75$ (4) $8.25$ 168. $Which one of the following conditions will favour maximum formation of the product in the reaction? ∆_{r} H = - X k J ?$ (1) $Low temperature and high pressure$ (2) $Low temperature and low pressure$ (3) $High temperature and high pressure$ (4) $High temperature and low pressure$ 169. $For a given exothermic reaction, K_{p} and K_{p}^{^{'}} are the equilibrium constants at temperatures T_{1} and T_{2}, respectively. Assuming that heat of reaction is constant in temperature range between T_{1} and T_{2}, it is readily observed that$ (1) $K_{p} > K_{p}^{^{'}}$ (2) $K_{p} < K_{p}^{^{'}}$ (3) $K_{p} = K_{p}^{^{'}}$ (4) $K_{p} = \frac{1}{K _{p}^{^{'}}}$ 170. $Given below are two statements. Statement I: In the titration between strong acid and weak base methyl orange is suitable as an indicator. Statement II: For titration of acetic acid with NaOH phenolphthalein is not a suitable indicator. In the lightof the above statements, choose the most appropriate answer from the options given below:$ (1) $Statement I is false but Statement II is true$ (2) $Statement I is true but Statement II is false$ (3) $Both Statement I and Statement II are true$ (4) $Both Statement I and Statement II are false$ 171. $The correct order of p K_{a} values for the following compounds is:$ (1) $c>a>d>b$ (2) $b>d>a>c$ (3) $b>a>d>c$ (4) $a>b>c>d$ 172. $50 mL of 0.2 M ammonia solution is treated with 25 mL of 0.2 M HCl . If p K_{b} of ammonia solution is 4.75, the pH of the mixture will be :$ (1) $4.75$ (2) $3.75$ (3) $9.25$ (4) $8.25$ 173. $200 mL of 0.01 M HC1 is mixed with 400 mL of 0.01M H_{2} S O_{4} . The pH of the mixture is____.$ (1) $1.14$ (2) $1.78$ (3) $2.34$ (4) $3.02$ 174. $Solubility of M_{2} S salt is 3. 5 \times 1 0^{- 6} then find out solubility product.$ (1) $1.7 \times 1 0^{- 6}$ (2) $1.7 \times 1 0^{- 16}$ (3) $1. 7 \times 1 0^{- 18}$ (4) $1.7 \times 1 0^{- 12}$ 175. $What is the [O H^{-}] in the final solution prepared by mixing 20.0 mL of 0.050 M HCl with 30.0 mL of 0.10 M Ba (OH)_{2} ?$ (1) $0.40 M$ (2) $0.0050 M$ (3) $0.12 M$ (4) $0.10 M$ 176. $The rapid change ofpH near the stoichiometric point of an acid‐base titration is the basis of indicator detection. p H of the solution is related to ratio of the concentrations of the conjugate acid (HIn) and base (In) forms of the indicator by the expression$ (1) $lo g \frac{[ I n ^{-} ]}{[ H I n ]} = p K_{I n} - p H$ (2) $lo g \frac{[ H I n ]}{[ I n ^{-} ]} = p K_{I n} - p H$ (3) $lo g \frac{[ H I n ]}{[ I n ^{-} ]} = p H - p K_{I n}$ (4) $lo g \frac{[ I n ^{-} ]}{[ H I n ]} = p H - p K_{I n}$ 177. $The value of ∆ H for the reaction is less than zero. Formation of X Y_{4 (g)} will be favoured at$ (1) $high temperature and high pressure$ (2) $low pressure and low temperature$ (3) $high temperature and low pressure$ (4) $high pressure and low temperature$ 178. $Accumulation of lactic acid (H C_{3} H_{5} O_{3}), a monobasic acid in tissues leads to pain and a feeling of fatigue. In a 0.10 M aqueous solution, lactic acid is 3.7% dissociates. The value of dissociation constant, K_{a}, for this acid will be$ (1) $1.4 \times 1 0^{- 5}$ (2) $1.4 \times 1 0^{- 4}$ (3) $3.7 \times 1 0^{- 4}$ (4) $2. 8 \times 1 0^{- 4}$ 179. $An aqueous solution contains an unknown concentration of B a^{2 +} . When 50 mL of a 1M solution of N a_{2} S O_{4} is added, B a S O_{4} just begins to precipitate. The final volume is 500 mL. The solubility product of B a S O_{4} is 1 \times 1 0^{-10} . What is the original concentration of B a^{2 +} .$ (1) $1.1 \times 1 0^{-9} M$ (2) $1.0 \times 1 0^{-10} M$ (3) $5 \times 1 0^{-9} M$ (4) $2 \times 1 0^{-9} M$ 180. $0.1 M solution of which one of these substances will act basic?$ (1) $Sodium borate$ (2) $Ammonium chloride$ (3) $Calcium nitrate$ (4) $Sodium sulphate$