Free NEET Chemistry multiple-choice questions on Solubility Product. Attempt each question and reveal the answer with a full explanation.
The solubility of AgI in 0.1 M KI solution is much lower than in pure water. This phenomenon is known as: Common ion effect Odd ion effect Solubility product effect Complex formation At 298 K , the solubility of a sparingly soluble salt M 2X 3 is S mol L -1 . The solubility product K sp is: 108 S 5 6 S 5 108 S 4 36 S 5 The solubility product ( K sp ) of a sparingly soluble salt A 2B 3 is related to its molar solubility S by the expression: K sp = 108 S 5 K sp = 69 S 5 K sp = 108 S 4 K sp = 36 S 5 The solubility of Ca 3(PO 4) 2 in water is S mol/L . Its solubility product K sp is: 108 S 5 108 S 4 27 S 4 16 S 3 Identify the correct order of solubility in aqueous medium CuS > ZnS > Na2S ZnS > Na2S > CuS Na2S > CuS > ZnS Na2S > ZnS > CuS If the solubility product of Ag 2CrO 4 is 1.1 10 -12 at 298 K , what is the solubility of Ag 2CrO 4 in mol L -1 ? 6.5 10 -5 1.1 10 -12 1.5 10 -4 1.5 10 -5 The solubility of BaSO 4 in water is 2.42 10 -3 g L -1 at 298 K . The value of its solubility product ( K sp ) will be (Molar mass of BaSO 4 = 233 g mol -1 ): 1.08 10 -10 mol 2 L -2 1.08 10 -12 mol 2 L -2 1.08 10 -14 mol 2 L -2 1.08 10 -8 mol 2 L -2 The solubility of AgCl(s) with solubility product 1.6 10 -10 in 0.1 M NaCl solution would be: 1.6 10 -9 M 1.6 10 -5 M 1.26 10 -5 M 1.6 10 -11 M In a saturated solution of the sparingly soluble strong electrolyte AgIO 3 (molecular mass = 283 ), the equilibrium which sets in is AgIO 3(s) Ag +(aq) + IO 3 -(aq) . If the solubility product constant K sp of AgIO 3 at a given temperature is 1.0 10 -8 , what is the mass of AgIO 3 contained in 100 mL of its saturated solution? 2.83 10 -3 g 2.83 10 -2 g 1.0 10 -7 g 1.0 10 -4 g The K sp of Mg(OH) 2 is 1 10 -12 . At what pH will Mg 2+ ions start precipitating from a solution containing 0.01 M Mg 2+ ions? 9 5 8 11 What is the relation between the solubility ( S ) and solubility product ( K sp ) for Al 2(SO 4) 3 ? K sp = 108 S 5 K sp = 27 S 4 K sp = 69 S 5 K sp = 108 S 4 What is the relation between the solubility S of PbI 2 in water and its K sp ? K sp = 4S 3 K sp = S 2 K sp = 27S 4 K sp = 108S 5 The solubility of BaSO 4 in 0.1 M BaCl 2 solution is 1.1 10 -9 M . What is the K sp of BaSO 4 ? 1.1 10 -10 1.1 10 -9 1.21 10 -18 1.1 10 -8 The solubility of Ag 2CO 3 ( K sp = 8 10 -12 ) in water is: 1.26 10 -4 M 2.82 10 -6 M 2 10 -4 M 1.41 10 -6 M The K sp of AgCl is 1.8 10 -10 . If [Ag +] = 10 -5 M and [Cl -] = 10 -4 M in a solution, then: AgCl will precipitate Solution is unsaturated Solution is at equilibrium Solubility increases The solubility of AgCl(s) in 0.1 M AgNO 3 solution is (Given K sp of AgCl = 1.6 10 -10 ): 1.6 10 -9 M 1.26 10 -5 M 1.6 10 -11 M 4.0 10 -5 M The K sp of CaF 2 is 5.3 10 -11 . Its solubility in 0.1 M NaF solution is: 5.3 10 -9 M 5.3 10 -10 M 5.3 10 -11 M 2.3 10 -4 M The solubility of Zr 3(PO 4) 4 is denoted by S . The solubility product K sp is given by: 6912 S 7 108 S 5 144 S 7 6912 S 5 The solubility of PbCl 2 ( K sp = 1.6 10 -5 ) in a 0.2 M NaCl solution is: 4.0 10 -4 M 1.6 10 -5 M 2.0 10 -2 M 4.0 10 -5 M The molar solubility of Ni(OH) 2 in 0.1 M NaOH is (Given: ionic product of Ni(OH) 2 is 2 10 -15 ): 2 10 -13 M 2 10 -15 M 1 10 -13 M 1 10 8 M The solubility of AgCl will be minimum in: 0.1 M AgNO 3 0.1 M NaCl Pure water 0.1 M NH 3 The solubility product of Ag 2CrO 4 is 3.2 10 -11 . What is the molar solubility? 2 10 -4 M 3.2 10 -4 M 1.8 10 -4 M 4 10 -4 M The solubility product of a sparingly soluble salt A 2X 3 is K sp . Its solubility S in mol L -1 is: (K sp /108) 1/5 (K sp /72) 1/5 (K sp /108) 1/2 (K sp /54) 1/5 The solubility of BaSO 4 in 0.01 M H 2SO 4 solution is ( K sp of BaSO 4 = 1.1 10 -10 ): 1.1 10 -8 M 1.1 10 -10 M 1.05 10 -5 M 1.1 10 -12 M Which of the following will decrease the degree of dissociation of NH 4OH in water? Addition of NH 4Cl Addition of HCl Addition of water Increasing temperature The solubility of AgCl in a 0.01 M CaCl 2 solution is (Given K sp of AgCl = 1.6 10 -10 ): 8.0 10 -9 M 1.6 10 -8 M 4.0 10 -9 M 1.26 10 -5 M If the solubility product of M 3X 2 is K sp , its solubility S is given by: S = (K sp / 108) 1/5 S = (K sp / 72) 1/5 S = (K sp / 108) 1/2 S = (K sp ) 1/5 The solubility of CaF 2 ( K sp = 4 10 -11 ) in 0.1 M NaF solution is: 4 10 -9 M 2 10 -5 M 4 10 -10 M 1 10 -7 M MY and NY3 , two nearly insoluble salts, have the same K sp values of 6.2 10 -13 at room temperature. Which statement would be true in regard to MY and NY3 ? The molar solubilities of MY and NY3 in water are identical. The molar solubility of MY in water is less than that of NY3 The salts MY and NY3 are more soluble in 0.5 M KY than in pure water. The addition of the salt of KY to solution of MY and NY3 will have no effect on their solubilities. The solubility of BaSO4 in water is 2.42 10 -3 gL -1 at 298 K. The value of its solubility product ( K sp ) will be (Given molar mass of BaSO4 = 233 g mol -1 ) 1.08 10 -14 mol 2 L -2 1.08 10 -12 mol 2 L -2 1.08 10 -10 mol 2 L -2 1.08 10 -8 mol 2 L -2 pH of a saturated solution of Ca(OH)2 is 9. The solubility product ( K sp ) of Ca(OH)2 is: 0.5 10 -10 0.5 10 -15 0.25 10 -10 0.125 10 -15 Find out the solubility of Ni(OH)2 in 0.1 M NaOH. Given that the ionic product of Ni(OH)2 is 2 10 -15 2 10 -8 M 1 10 -13 M 1 10 8 M 2 10 -13 M In a qualitative analysis, Bi 3+ is detected by appearance of precipitate of BiO(OH)(s) . Calculate pH when the following equilibrium exists at 298 K. BiO(OH)(s) <=> BiO+(aq) + OH-(aq) , K = 4 10 -10 (Given : 2 = 0.3010 ) 4.699 5.286 8.714 9.301 The solubility of a sparingly soluble salt AB 2 in water is 1.0 10 -5 mol L -1 . Its solubility product K sp is: 4.0 10 -15 1.0 10 -15 1.0 10 -10 4.0 10 -10 The pH of a saturated solution of Ca(OH) 2 is 9. The solubility product ( K sp ) of Ca(OH) 2 is: 0.5 10 -15 0.25 10 -10 0.125 10 -15 0.5 10 -10 The solubility product of PbCl 2 is 1.6 10 -5 . What is the molar solubility of PbCl 2 in water? 1.59 10 -2 M 2.52 10 -2 M 4.0 10 -3 M 1.6 10 -5 M If the concentration of OH - ions in the reaction Fe(OH) 3(s) Fe 3+ (aq) + 3OH -(aq) is decreased by 1 4 times, then equilibrium concentration of Fe 3+ will increase by: 64 times 16 times 4 times 8 times The molar solubility of PbI 2 in 0.1 M KI solution is (given K sp of PbI 2 = 7.1 10 -9 ): 7.1 10 -7 M 7.1 10 -8 M 1.3 10 -3 M 8.4 10 -5 M The solubility product of CuS , Ag 2S , and HgS are 10 -31 , 10 -44 , and 10 -54 respectively. The correct order of their solubility in water is: Ag 2S > CuS > HgS HgS > CuS > Ag 2S CuS > Ag 2S > HgS Ag 2S > HgS > CuS Calculate the degree of hydrolysis of 0.1 M sodium acetate solution ( K a of acetic acid = 1.8 10 -5 ). 7.45 10 -5 1.8 10 -5 1.0 10 -7 2.3 10 -3 The solubility product of Ag 2C 2O 4 at 25 C is 1.29 10 -11 . A solution is saturated with Ag 2C 2O 4 . The concentration of Ag + ions in this solution is: 2.95 10 -4 M 1.52 10 -4 M 5.34 10 -4 M 1.29 10 -4 M Calculate the degree of hydrolysis ( h ) of 0.1 M KCN solution. Given K a (HCN) = 5 10 -10 and K w = 1 10 -14 . 1.41 10 -2 2 10 -5 4.5 10 -3 1.41 10 -4 The solubility product of Fe(OH) 3 is 1.0 10 -38 . The pH at which Fe 3+ ions start precipitating from a 0.1 M FeCl 3 solution is: 1.67 3.0 5.5 12.33 If the solubility of Mg(OH) 2 in water is 1.0 10 -4 mol/L , what is its solubility in a solution with pH = 12 ? 4.0 10 -8 mol/L 1.0 10 -10 mol/L 4.0 10 -12 mol/L 1.0 10 -4 mol/L The solubility product ( K sp ) of a sparingly soluble salt A 3 B 2 in terms of its molar solubility S is given by: 108S 5 36S 5 72S 5 108S 4 Which species is the strongest Lewis acid among the boron trihalides? BI 3 BBr 3 BCl 3 BF 3 The correct order of solubility of the given salts in water at 298 K is Hg2Cl2 > Zn(OH)2 > AgBr AgBr > Zn(OH)2 > Hg2Cl2 Hg2Cl2 > AgBr > Zn(OH)2 Zn(OH)2 > AgBr > Hg2Cl2 The solubility product of Silver oxalate ( Ag 2 C 2 O 4 ) is expressed in terms of its molar solubility S as: 4S 3 S 2 27S 4 108S 5 If the solubility of AgCl in water is S , its solubility in a 0.1 M NaCl solution will be (assuming S' is very small): K sp / 0.1 K sp S 0.1 / K sp The solubility of MgF 2 is S mol/L . Its solubility product K sp is: 4S 3 S 2 4S 2 108S 5 If the concentration of OH - ions in a saturated solution of Mg(OH) 2 is 2 10 -4 mol L -1 , the solubility product K sp of Mg(OH) 2 is: 4 10 -12 8 10 -12 2 10 -12 1 10 -11