Solved papers for NEET Chemistry Equilibrium / साम्यावस्था NEET PYQ-Ionic Equilibrium

done NEET PYQ-Ionic Equilibrium Total Questions - 44

• question_answer1) 

  The concentration of \[[{{H}^{+}}]\] and concentration of \[[O{{H}^{-}}]\] of a 0.1 M aqueous solution of 2% ionised weak monobasic acid is:

  [ionic product of water\[=1\times {{10}^{-14}}\]]                                                [AIPMT 1999]

  A)
         \[0.02\times {{10}^{-3}}\,M\] and \[5\times {{10}^{-11}}\,M\]
  done clear
  B)
        \[1\times {{10}^{-3}}\,M\] and \[3\times {{10}^{-11}}\,M\]
  done clear
  C)
   \[2\times {{10}^{-3}}\,M\] and \[5\times {{10}^{-12}}\,M\]                  
  done clear
  D)
   \[3\times {{10}^{-2}}\,M\] and \[4\times {{10}^{-13}}\,M\]
  done clear
  View Answer play_arrow

• question_answer2) The solubility of a saturated solution of calcium fluoride is \[2\times {{10}^{-4}}\,mol/L\]. Its solubility product is:                                                                                                                                                      [AIPMT 1999]
  A)
   \[12\times {{10}^{-2}}\]                     
  done clear
  B)
   \[14\times {{10}^{-4}}\]
  done clear
  C)
   \[22\times {{10}^{-11}}\]
  done clear
  D)
                    \[32\times {{10}^{-12}}\]
  done clear
  View Answer play_arrow

• question_answer3)  Which of the following statements about pH and \[{{H}^{+}}\] ion concentration is incorrect?           [AIPMT 2000]
  A)
   Addition of one drop of concentrated HCl in \[N{{H}_{4}}OH\] solution decreases pH of the solution
  done clear
  B)
        A solution of the mixture of one equivalent of each of \[C{{H}_{3}}COOH\] and NaOH has a pH of 7
  done clear
  C)
        pH of pure neutral water is not zero
  done clear
  D)
   A cold and cone. \[{{H}_{2}}S{{O}_{4}}\] has lower \[{{H}^{+}}\] ion concentration than a dilute solution of \[{{H}_{2}}S{{O}_{4}}\]
  done clear
  View Answer play_arrow

• question_answer4) Which one of the following is true for any diprotic acid, \[{{H}_{2}}X\]?                             [AIPMT 2000]
  A)
   \[{{K}_{{{a}_{2}}}}={{K}_{{{a}_{1}}}}\]   
  done clear
  B)
        \[{{K}_{{{a}_{2}}}}>{{K}_{{{a}_{1}}}}\]
  done clear
  C)
   \[{{K}_{{{a}_{2}}}}<{{K}_{{{a}_{1}}}}\]
  done clear
  D)
        \[{{K}_{{{a}_{2}}}}=\frac{1}{K{{a}_{1}}}\]
  done clear
  View Answer play_arrow

• 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]
  A)
   \[3.4\times {{10}^{-4}}\]
  done clear
  B)
                    \[3.4\times {{10}^{3}}\]
  done clear
  C)
   \[6.8\times {{10}^{-4}}\]
  done clear
  D)
                    \[6.8\times {{10}^{-3}}\]        
  done clear
  View Answer play_arrow

• question_answer6) Solubility of a \[{{M}_{2}}S\] salt is \[3.5\times {{10}^{-6}},\] then find out solubility product:          [AIPMT 2001]
  A)
  \[1.7\times {{10}^{-6}}\]                     
  done clear
  B)
   \[1.7\times {{10}^{-16}}\]
  done clear
  C)
   \[1.7\times {{10}^{-18}}\]       
  done clear
  D)
        \[1.7\times {{10}^{-12}}\]
  done clear
  View Answer play_arrow

• 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]
  A)
   \[5\times {{10}^{-12}}\]         
  done clear
  B)
        \[25\times {{10}^{-10}}\]        
  done clear
  C)
  \[1\times {{10}^{-13}}\]          
  done clear
  D)
        \[5\times {{10}^{-13}}\]
  done clear
  View Answer play_arrow

• question_answer8)  Which has highest pH?                                                                                                    [AIPMT 2002]
  A)
   \[C{{H}_{3}}COOK\]              
  done clear
  B)
   \[N{{a}_{2}}C{{O}_{3~~}}\]
  done clear
  C)
  \[N{{H}_{4}}Cl\]  
  done clear
  D)
     \[NaN{{O}_{3}}\]
  done clear
  View Answer play_arrow

• 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]
  A)
         9.25                
  done clear
  B)
        4.75                
  done clear
  C)
   3.75      
  done clear
  D)
    8.25
  done clear
  View Answer play_arrow

• 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]
  A)
   \[1.0\times {{10}^{-10}}\]
  done clear
  B)
                    \[1.0\times {{10}^{-8}}\]        
  done clear
  C)
   \[1.0\times {{10}^{-16}}\]
  done clear
  D)
                    \[1.0\times {{10}^{-12}}\]
  done clear
  View Answer play_arrow

• 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]
  A)
   \[\text{5}.\text{6}\times {{10}^{-\text{6}}}\]               
  done clear
  B)
  \[\text{3}.\text{1}\times {{10}^{-\text{4}}}\]
  done clear
  C)
   \[\text{2}\times {{10}^{-\text{4}}}\]    
  done clear
  D)
        \[\text{4}\times {{10}^{-\text{4}}}\]
  done clear
  View Answer play_arrow

• 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]
  A)
   \[2.0\times {{10}^{-6}}\,mol\,{{L}^{-1}}\]     
  done clear
  B)
   \[1.0\times {{10}^{-5}}\,mol\,{{L}^{-1}}\]
  done clear
  C)
   \[1.0\times {{10}^{-6}}\,mol\,{{L}^{-1}}\]
  done clear
  D)
        \[1.0\times {{10}^{-7}}\,mol\,{{L}^{-1}}\]
  done clear
  View Answer play_arrow

• 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]
  A)
   \[p{{H}_{1}}>p{{H}_{2}}>~p{{H}_{3}}>p{{H}_{4}}\]
  done clear
  B)
   \[p{{H}_{1}}<p{{H}_{2}}<p{{H}_{3}}<p{{H}_{4}}\]
  done clear
  C)
   \[p{{H}_{1}}<p{{H}_{2}}<p{{H}_{3}}<~p{{H}_{4}}\]
  done clear
  D)
   \[p{{H}_{1}}>p{{H}_{2}}>p{{H}_{3}}>p{{H}_{4}}\]
  done clear
  View Answer play_arrow

• 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
  done clear
  B)
        presence of HCl increases the sulphide ion concentration
  done clear
  C)
        solubility product of group II sulphides is more than that of group IV sulphides
  done clear
  D)
        sulphides of group IV cations are unstable in HCl
  done clear
  View Answer play_arrow

• question_answer15) Which of the following pairs constitutes a buffer?                                                                 [AIPMT (S) 2006]
  A)
         \[HN{{O}_{2}}\] and \[NaN{{O}_{2}}\]
  done clear
  B)
        \[NaOH\] and \[NaCl\]
  done clear
  C)
   \[HN{{O}_{3}}\] and \[N{{H}_{4}}N{{O}_{3}}\]        
  done clear
  D)
   \[HCl\] and \[KCl\]
  done clear
  View Answer play_arrow

• 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]
  A)
   \[1.0\times {{10}^{-6}}M\]
  done clear
  B)
                    \[1.0525\times {{10}^{-7}}M\]
  done clear
  C)
   \[9.525\times {{10}^{-8}}M\]
  done clear
  D)
        \[1.0\times {{10}^{-8}}M\]
  done clear
  View Answer play_arrow

• 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]
  A)
   7.00
  done clear
  B)
                    4.00    
  done clear
  C)
   9.00                
  done clear
  D)
        1.00
  done clear
  View Answer play_arrow

• 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]
  A)
   99.0%   
  done clear
  B)
                    1.00%
  done clear
  C)
   99.9%   
  done clear
  D)
                    0.100%
  done clear
  View Answer play_arrow

• 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]
  A)
   \[1.11\times {{10}^{-4}}M\]    
  done clear
  B)
   \[3.7\times {{10}^{-4}}M\]
  done clear
  C)
   \[3.7\times {{10}^{-3}}M\]      
  done clear
  D)
        \[1.11\times {{10}^{-3}}M\]
  done clear
  View Answer play_arrow

• 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]
  A)
   8 times         
  done clear
  B)
        16 times          
  done clear
  C)
   64 times             
  done clear
  D)
   4 times
  done clear
  View Answer play_arrow

• 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]
  A)
   \[SrC{{l}_{2}}\]          
  done clear
  B)
        \[BaC{{l}_{2}}\]
  done clear
  C)
   \[MgC{{l}_{2}}\]         
  done clear
  D)
        \[CaC{{l}_{2}}\]
  done clear
  View Answer play_arrow

• 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]
  A)
   \[5.65\times {{10}^{-10}}\]     
  done clear
  B)
        \[6.50\times {{10}^{-12}}\]
  done clear
  C)
   \[5.65\times {{10}^{-13}}\]     
  done clear
  D)
        \[5.65\times {{10}^{-12}}\]
  done clear
  View Answer play_arrow

• 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]
  A)
   0.10 M            
  done clear
  B)
        0.40 M
  done clear
  C)
   0.0050 M         
  done clear
  D)
        0.12 M
  done clear
  View Answer play_arrow

• 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]
  A)
   \[3.0\times {{10}^{5}}\]         
  done clear
  B)
        \[3.0\times {{10}^{-5}}\]
  done clear
  C)
   \[3.0\times {{10}^{-4}}\]        
  done clear
  D)
        \[3.0\times {{10}^{4}}\]
  done clear
  View Answer play_arrow

• question_answer25) If pH of a saturated solution of \[Ba{{(OH)}_{2}}\] is 12, the value of its \[{{K}_{sp}}\]is               [AIPMT (S) 2010]
  A)
   \[4.00\times {{10}^{-6}}{{M}^{3}}\]
  done clear
  B)
        \[4.00\times {{10}^{-7}}{{M}^{3}}\]
  done clear
  C)
   \[5.00\times {{10}^{-6}}{{M}^{3}}\]
  done clear
  D)
        \[5.00\times {{10}^{-7}}{{M}^{3}}\]
  done clear
  View Answer play_arrow

• 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]
  A)
   \[3.5\times {{10}^{-4}}\]        
  done clear
  B)
        \[1.1\times {{10}^{-5}}\]
  done clear
  C)
   \[1.8\times {{10}^{-5}}\]        
  done clear
  D)
        \[9.2\times {{10}^{-6}}\]
  done clear
  View Answer play_arrow

• 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]
  A)
   0.955 M and 1.910 M
  done clear
  B)
   1.910 M and 0.955 M
  done clear
  C)
   1.90 M and 1.910 M
  done clear
  D)
   0.477 M and 0.477 M
  done clear
  View Answer play_arrow

• 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]   
  A)
   10                   
  done clear
  B)
        7                  
  done clear
  C)
   6                    
  done clear
  D)
        4
  done clear
  View Answer play_arrow

• 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]
  A)
   9.43     
  done clear
  B)
        11.72  
  done clear
  C)
   8.73                
  done clear
  D)
        9.08
  done clear
  View Answer play_arrow

• 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]
  A)
   \[[A{{g}^{+}}]=1.8\times {{10}^{-7}}M;[P{{b}^{2+}}]=1.7\times {{10}^{-6}}M\]
  done clear
  B)
   \[[A{{g}^{+}}]=1.8\times {{10}^{-11}}M;[P{{b}^{2+}}]=8.5\times {{10}^{-5}}M\]
  done clear
  C)
   \[[A{{g}^{+}}]=1.8\times {{10}^{-9}}M;[P{{b}^{2+}}]=1.7\times {{10}^{-3}}M\]
  done clear
  D)
   \[[A{{g}^{+}}]=1.8\times {{10}^{-11}}M;[P{{b}^{2+}}]=8.5\times {{10}^{-4}}M\]
  done clear
  View Answer play_arrow

• question_answer31) pH of a saturated solution of \[Ba{{(OH)}_{2}}\] is 12. The value of solubility product K of \[Ba{{(OH)}_{2}}\] is                                                                                                                                     [AIPMT (S) 2012]
  A)
   \[3.3\times {{10}^{-7}}\]        
  done clear
  B)
        \[5.0\times {{10}^{-7}}\]
  done clear
  C)
   \[4.0\times {{10}^{-6}}\]        
  done clear
  D)
        \[5.0\times {{10}^{-6}}\]
  done clear
  View Answer play_arrow

• question_answer32) Equimolar solutions of the following substances were prepared separately. Which one of these will record the highest pH value?                                                                                                                            [AIPMT (S) 2012]
  A)
   \[BaC{{l}_{2}}\]         
  done clear
  B)
        \[AlC{{l}_{3}}\]
  done clear
  C)
   \[LiCl\]
  done clear
  D)
        \[BeC{{l}_{2}}\]
  done clear
  View Answer play_arrow

• question_answer33) Buffer solutions have constant acidity and alkalinity because                                                [AIPMT (S) 2012]
  A)
   these give unionised acid or base on reaction with added acid or alkali
  done clear
  B)
   acids and alkalies in these solutions are shielded from attack by other ions
  done clear
  C)
   they have large excess of \[{{H}^{+}}\] or \[O{{H}^{-}}\] ions
  done clear
  D)
   they have fixed value of pH
  done clear
  View Answer play_arrow

• 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]
  A)
   0.001             
  done clear
  B)
        0.002
  done clear
  C)
   0.003            
  done clear
  D)
        0.01
  done clear
  View Answer play_arrow

• question_answer35) Which of the following salts will give highest pH in water?                                                    [AIPMT 2014]
  A)
   \[KCl\]            
  done clear
  B)
                    \[NaCl\]           
  done clear
  C)
   \[N{{a}_{2}}C{{O}_{3}}\]
  done clear
  D)
        \[CuS{{O}_{4}}\]
  done clear
  View Answer play_arrow

• 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 ]
  A)
   \[Agl\]             
  done clear
  B)
                    \[AgCl\]
  done clear
  C)
   \[AgBr\]       
  done clear
  D)
   \[A{{g}_{2}}Cr{{O}_{4}}\]
  done clear
  View Answer play_arrow

• question_answer37) What is the pH of the resulting solution when equal volumes of 0.1 M \[NaOH\] and M HCl are mixed?                                                                                                                                                    [NEET 2015 (Re)]
  A)
   12.65            
  done clear
  B)
        2.0                  
  done clear
  C)
   7.0            
  done clear
  D)
   1.04
  done clear
  View Answer play_arrow

• question_answer38) Which one of the following pairs of solution is not an acidic buffer?                      [NEET 2015 (Re)]
  A)
    \[HCl{{O}_{4}}\] and \[NaCl{{O}_{4}}\]
  done clear
  B)
   \[C{{H}_{3}}COOH\] and \[C{{H}_{3}}COONa\]
  done clear
  C)
   \[{{H}_{2}}C{{O}_{3}}\] and \[N{{a}_{2}}C{{O}_{3}}\]
  done clear
  D)
   \[{{H}_{3}}P{{O}_{4}}\] and \[N{{a}_{2}}P{{O}_{4}}\]
  done clear
  View Answer play_arrow

• 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.
  done clear
  B)
   The molar solubility of MY in water is less than that of \[N{{Y}_{3}}\]
  done clear
  C)
   The salts MY and \[N{{Y}_{3}}\] are more soluble in 0.5 M KY than in pure water.
  done clear
  D)
   The addition of the salt of KY to solution of MY and \[N{{Y}_{3}}\] will have no effect on their solubilities.
  done clear
  View Answer play_arrow

• 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]
  A)
   \[5.3\times {{10}^{12}}\]        
  done clear
  B)
        \[~2.42\times {{10}^{8}}\]
  done clear
  C)
   \[2.66\times {{10}^{12}}\]      
  done clear
  D)
        \[~4.5\times {{10}^{11}}\]
  done clear
  View Answer play_arrow

• question_answer41) 

  Following solutions were prepared by mixing different volumes of NaOH and HCl of different concentrations :                                                                                                                                                                                                            [NEET - 2018]

  [a] \[\text{60mL}\frac{\text{M}}{\text{10}}\text{HCl+40mL}\frac{\text{M}}{\text{10}}\text{NaOH}\]

  [b] \[\text{55mL}\frac{\text{M}}{\text{10}}\text{HCl+45mL}\frac{\text{M}}{\text{10}}\text{NaOH}\]

  [c] \[\text{75mL}\frac{\text{M}}{\text{5}}\text{HCl+25mL}\frac{\text{M}}{\text{5}}\text{NaOH}\]

  [d] \[\text{100mL}\frac{\text{M}}{\text{10}}\text{HCl+100mL}\frac{\text{M}}{\text{10}}\text{NaOH}\]

  pH of which one of them will be equal to 1?

  A)
   d                    
  done clear
  B)
        a
  done clear
  C)
   b                    
  done clear
  D)
        c
  done clear
  View Answer play_arrow

• question_answer42) 

  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\[\text{BaS}{{\text{O}}_{\text{4}}}\text{=233 g mo}{{\text{l}}^{\text{--1}}}\])

  A)
   \[\text{1}\text{.08 }\!\!\times\!\!\text{ 1}{{\text{0}}^{\text{--14}}}\text{ mol 2}{{\text{L}}^{\text{--2}}}\]
  done clear
  B)
   \[\text{1}\text{.08 }\!\!\times\!\!\text{ 1}{{\text{0}}^{\text{--12}}}\text{mo}{{\text{l}}^{\text{2}}}{{\text{L}}^{\text{--2}}}\]
  done clear
  C)
   \[\text{1}\text{.08 }\!\!\times\!\!\text{ 1}{{\text{0}}^{\text{--10}}}\text{mo}{{\text{l}}^{\text{2}}}{{\text{L}}^{\text{--2}}}\]
  done clear
  D)
   \[\text{1}\text{.08 }\!\!\times\!\!\text{ 1}{{\text{0}}^{\text{--8}}}\text{mo}{{\text{l}}^{\text{2}}}{{\text{L}}^{\text{--2}}}\]
  done clear
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• question_answer43) pH of a saturated solution of \[Ca{{(OH)}_{2}}\]is 9. The solubility product \[({{K}_{sp}})\] of \[Ca{{(OH)}_{2}}\] is- [NEET 2019]
  A)
   \[0.125\times {{10}^{15}}\]    
  done clear
  B)
   \[0.5\times {{10}^{10}}\]
  done clear
  C)
   \[0.5\times {{10}^{15}}\]        
  done clear
  D)
        \[0.25\times {{10}^{10}}\]
  done clear
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• 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]
  A)
   \[2\times {{10}^{8}}M\]         
  done clear
  B)
        \[1\times {{10}^{13}}M\]
  done clear
  C)
   \[1\times {{10}^{8}}M\]         
  done clear
  D)
        \[2\times {{10}^{13}}M\]
  done clear
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