question_answer2) The solubility of a saturated solution of calcium fluoride is \[2\times {{10}^{-4}}\,mol/L\]. Its solubility product is: [AIPMT 1999]
question_answer5) Ionisation constant of \[C{{H}_{3}}COOH\] is \[1.7\times {{10}^{-5}}\] and concentration of \[{{H}^{+}}\] ions is \[3.4\times {{10}^{-4}}\]. Then find out initial concentration of \[C{{H}_{3}}COOH\] molecules: [AIPMT 2001]
question_answer7) Solubility of \[M{{X}_{2}}\]-type electrolytes is \[0.5\times {{10}^{-4}}mol/L\]. Then find out if \[{{K}_{sp}}\] of electrolytes: [AIPMT 2002]
question_answer9) Solution of 0.1 N \[N{{H}_{4}}OH\] and 0.1 N \[N{{H}_{4}}Cl\] has pH 9.25, then find out \[p{{K}_{b}}\] of \[N{{H}_{4}}OH\]. [AIPMT 2002]
question_answer10) The solubility product of \[Agl\] at \[25{}^\circ C\] is\[1.0\times {{10}^{-16}}mo{{l}^{2}}{{L}^{-2}}\]. The solubility of \[Agl\] in \[{{10}^{-4}}N\] solution of \[KI\] at \[25{}^\circ C\] is approximately (in \[mol\text{ }{{L}^{-1}}\]): [AIPMT 2003]
question_answer11) The solubility product of a sparingly soluble salt\[A{{X}_{2}}\] is \[3.2\times {{10}^{-11}}\]. Its solubility (in mol/L) is: [AIPMT (S) 2004]
question_answer12) At \[{{25}^{o}}C,\] the dissociation constant of a base, BOH, is \[1.0\times {{10}^{-12}}\]. The concentration of hydroxyl ions in 0.01 M aqueous solution of the base would be: [AIPMT (S) 2005]
question_answer13) What is the correct relationship between the pHs of isomolar solutions of sodium oxide \[(p{{H}_{1}}),\] sodium sulphide \[(p{{H}_{2}})\] sodium selenide \[(p{{H}_{3}})\] and sodium telluride \[(p{{H}_{4}})\]? [AIPMT (S) 2005]
question_answer14) \[{{H}_{2}}S\] gas when passed through a solution of cations containing HCl precipitates the cations of second group of qualitative analysis but not those belonging to the fourth group. It is because: [AIPMT (S) 2005]
A)
presence of HCl decreases the sulphide ion concentration
doneclear
B)
presence of HCl increases the sulphide ion concentration
doneclear
C)
solubility product of group II sulphides is more than that of group IV sulphides
question_answer16) The hydrogen ion concentration of a \[{{10}^{-8}}M\text{ }HCl\] aqueous solution at \[298\text{ }K\text{ (}{{K}_{w}}={{10}^{-14}})\] is: [AIPMT (S) 2006]
question_answer17) Calculate the \[pOH\] of a solution at \[25{}^\circ C\] that contains \[1\times {{10}^{-10}}\,M\] of hydronium ions. [AIPMT (S) 2007]
question_answer18) A weak acid, \[\Delta H,\] has a \[{{K}_{a}}\] of \[1.00\times {{10}^{-5}}\]. If 0.100 mole of this acid is dissolved in one litre of water, the percentage of acid dissociated at equilibrium is closest to: [AIPMT (S) 2007]
question_answer19) Equal volumes of three acid solutions of pH 3, 4 and 5 are mixed in a vessel. What will be the \[{{H}^{+}}\] ion concentration in the mixture? [AIPMT (S) 2008]
question_answer20) If the concentration of \[O{{H}^{-}}\] ions in the reaction \[Fe{{(OH)}_{3}}(s)F{{e}^{3+}}(aq)+3O{{H}^{-}}(aq)\] is decreased by \[\frac{1}{4}\] times, then equilibrium concentration of \[F{{e}^{3+}}\] will increase by [AIPMT (S) 2008]
question_answer21) Equimolar solutions of the following were prepared in water separately. Which one of the solutions will record the highest pH? [AIPMT (S) 2008]
question_answer22) The ionisation constant of ammonium hydroxide is \[1.77\times {{10}^{-5}}\] at 298 K. Hydrolysis constant of ammonium chloride is [AIPMT (S) 2009]
question_answer23) . 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 \[Ba{{(OH)}_{2}}\]? [AIPMT (S) 2009]
question_answer24) The dissociation constants for acetic acid and HCN at \[{{25}^{o}}C\] are \[1.5\times {{10}^{-5}}\] and \[4.5\times {{10}^{-10}},\] respectively. The equilibrium constant for the equilibrium, \[HCN+C{{H}_{3}}CO{{O}^{-}}\] would be [AIPMT (S) 2009]
question_answer26) What is \[[{{H}^{+}}]\] in mol/L of a solution that is 0.20 M in \[C{{H}_{3}}COONa\] and 0.10 M in \[C{{H}_{3}}COOH\]? (\[{{K}_{a}}\]for \[C{{H}_{3}}COOH=1.8\times {{10}^{-5}}\]) [AIPMT (S) 2010]
question_answer27) 25.3 g of sodium carbonate, \[N{{a}_{2}}C{{O}_{3}}\] is dissolved in enough water to make 250 mL of solution. If sodium carbonate dissociates completely, molar concentration of sodium ion, \[N{{a}^{+}}\] and carbonate ion, \[CO_{3}^{2-}\] are respectively (Molar mass of\[N{{a}_{2}}C{{O}_{3}}=106\,g\,\,mo{{l}^{-1}}\]) [AIPMT (S) 2010]
question_answer28) In a buffer solution containing equal concentration of \[{{B}^{+}}\] and HB, the \[{{K}_{b}}\] for \[{{B}^{-}}\] is \[{{10}^{-10}}\]. The pH of buffer solution is [AIPMT (S) 2010]
question_answer29) A buffer solution is prepared in which the concentration of \[N{{H}_{3}}\] is 0.30 M and the concentration of \[NH_{4}^{+}\] is 0.20 M. If the equilibrium constant, \[{{K}_{b}}\] for \[N{{H}_{3}}\] equals \[1.8\times {{10}^{-5}},\] what is the pH of this solution? \[(\log \text{ }2.7\text{ }=0.43)\] [AIPMT (S) 2011]
question_answer30) In qualitative analysis, the metals of group I can be separated from other ions by precipitating them as chloride salts. A solution initially contains \[A{{g}^{+}}\] and \[P{{b}^{2+}}\] at a concentration of 0.10 M. Aqueous HCl is added to this solution until the \[C{{l}^{-}}\] concentration is 0.10 M. What will be the concentration of \[A{{g}^{+}}\] and \[P{{b}^{2+}}\] be at equilibrium? (\[{{K}_{sp}}\] for \[AgCl=1.8\times {{10}^{-10}},\] \[{{K}_{sp}}\] for \[PbC{{l}_{2}}=1.7\times {{10}^{-5}}\]) [AIPMT (M) 2011]
question_answer32) Equimolar solutions of the following substances were prepared separately. Which one of these will record the highest pH value? [AIPMT (S) 2012]
question_answer34) An excess of \[AgN{{O}_{3}}\] is added to 100 mL of a 0.01 M solution of Dichlorotetraaquachromium (III) chloride. The number of moles of \[\text{AgCl}\] precipitate would be [NEET 2013]
question_answer36) The \[{{K}_{sp}}\] of \[A{{g}_{2}}Cr{{O}_{4}},\,AgCl,\,AgBr\] and \[AgI\] are respectively, \[1.1\times {{10}^{-12}},\,\,1.8\times {{10}^{-10}}\]\[5.0\times {{10}^{-13}},\]\[8.3\times {{10}^{-17}}\]. Which one of the following salts will precipitate last if \[AgN{{O}_{3}}\] solution is added to the solution containing equal moles of \[NaCl,NaBr,NaI\] and\[N{{a}_{2}}CrC{{O}_{4}}\]. [NEET 2015 ]
question_answer39) MY and \[N{{Y}_{3}},\] two nearly insoluble salts, have the same \[{{K}_{sp}}\] values of \[6.2\times {{10}^{13}}\] at room temperature. Which statement would be true in regard to MY and \[N{{Y}_{3}}\]? [NEET - 2016]
A)
The molar solubilities of MY and \[N{{Y}_{3}}\] in water are identical.
doneclear
B)
The molar solubility of MY in water is less than that of \[N{{Y}_{3}}\]
doneclear
C)
The salts MY and \[N{{Y}_{3}}\] are more soluble in 0.5 M KY than in pure water.
doneclear
D)
The addition of the salt of KY to solution of MY and \[N{{Y}_{3}}\] will have no effect on their solubilities.
question_answer40) Concentration of the \[A{{g}^{+}}\] ions in a saturated solution of \[A{{g}_{2}}{{C}_{2}}{{O}_{4}}\] is \[2.2\times {{10}^{-4}}\,mol\,{{L}^{-1}}\]. Solubility product of \[A{{g}_{2}}{{C}_{2}}{{O}_{4}}\] is [NEET-2017]
The solubility of \[\text{BaS}{{\text{O}}_{\text{4}}}\] in water is \[\text{2}\text{.42 }\!\!\times\!\!\text{ 1}{{\text{0}}^{\text{--3}}}\text{g}{{\text{L}}^{\text{-1}}}\] at 298 K. The value of its solubility product\[\text{(}{{\text{K}}_{\text{sp}}}\text{)}\] will be [NEET - 2018]
(Given molar mass of\[\text{BaS}{{\text{O}}_{\text{4}}}\text{=233 g mo}{{\text{l}}^{\text{--1}}}\])
question_answer44) Find out the solubility of \[Ni{{(OH)}_{2}}\] in 0.1 M\[NaOH\]. Given that the ionic product of \[Ni{{(OH)}_{2}}\] is \[2\times {{10}^{15}}\] [NEET 2020]