Chapter 7 – Equilibrium
Sahay Sir > Question Answers > JEE Adv and Mains Chemistry 41 Years Solved Video Solutions 1979 - 2019 > Chemistry > Chapter 7 - Equilibrium
AgBr(s)+2S2O2−3(aq)⇔[Ag(S2O3)2]3−(aq)+Br−(aq) [Ksp(AgBr)=5×10^−13, Kf[Ag(S2O3)2]3−=5×10^13] What is the molar solubility of AgBr in 0.1M Na2S2O3?
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Nov
AgBr(s)+2S2O2−3(aq)⇔[Ag(S2O3)2]3−(aq)+Br−(aq) [Ksp(AgBr)=5×10^−13, Kf[Ag(S2O3)2]3−=5×10^13] What is the molar solubility of AgBr in 0.1M Na2S2O3? AgBr(s)+2S2O2−3(aq)⇔[Ag(S2O3)2]3−(aq)+Br−(aq) [Ksp(AgBr)=5×10^−13 Kf[Ag(S2O3)2]3−=5×10^13] What is the molar solubility of AgBr in 0.1M Na2S2O3? November 22, 2020 Category: Chapter 6 - Ionic Equilibrium (Level 1 and Level 2) , Chapter 7 - Equilibrium , N Awasthi Physical Chemistry ,
There exist an equilibrium between solid SrSO 4 and Sr2+ and SO 4 2− ion in aqueous medium. The possible equilibrium states are shown in the figure as thick line. Now of the equilibrium is distributed by addition of (a) Sr(NO3 )2 and (b) K2SO4 and dotted line represent approach of system towards equilibrium. Match the columns given below
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Nov
There exist an equilibrium between solid SrSO 4 and Sr2+ and SO 4 2− ion in aqueous medium. The possible equilibrium states are shown in the figure as thick line. Now of the equilibrium is distributed by addition of (a) Sr(NO3 )2 and (b) K2SO4 and dotted line represent approach of system towards equilibrium. Match [...]
The simultaneous solubility of AgCN (Ksp = 2.5×10^−16) and AgCl(Ksp=1.6×10^−10) in 1.0 M NH3(aq) are respectively (Kf [Ag(NH3)2]+=10^7)
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Nov
The simultaneous solubility of AgCN (Ksp = 2.5×10^−16) and AgCl(Ksp=1.6×10^−10) in 1.0 M NH3(aq) are respectively (Kf [Ag(NH3)2]+=10^7) The simultaneous solubility of AgCN (Ksp = 2.5×10^−16) and AgCl(Ksp=1.6×10^−10) in 1.0 M NH3(aq) are respectively (Kf [Ag(NH3)2]+=10^7) November 22, 2020 Category: Chapter 6 - Ionic Equilibrium (Level 1 and Level 2) , Chapter 7 - Equilibrium [...]
A solution contains 0.1M is Cl− and 10^−4 M CrO2−4. If solid AgNO3 is gradually added to this solution, what will be the concentration of Cl− when Ag2CrO4 begins to precipitate? (Ksp(AgCl)=10^−10M^2, Ksp(Ag2CrO4)=10^−12M^3)
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Nov
A solution contains 0.1M is Cl− and 10^−4 M CrO2−4. If solid AgNO3 is gradually added to this solution, what will be the concentration of Cl− when Ag2CrO4 begins to precipitate? (Ksp(AgCl)=10^−10M^2, Ksp(Ag2CrO4)=10^−12M^3) A solution contains 0.1M is Cl− and 10^−4 M CrO2−4. If solid AgNO3 is gradually added to this solution Ksp(Ag2CrO4)=10^−12M^3) what will [...]
If 500 ml of 0.4 MAgNO3 is mixed with 50 ml of 2MNH3 solution then what is the concentration of [Ag(NH3)]+ in solution (Kt,[AgNH3]^+ = 10^3,Kf2[Ag(NH3)2]^+=10^4)
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Nov
If 500 ml of 0.4 MAgNO3 is mixed with 50 ml of 2MNH3 solution then what is the concentration of [Ag(NH3)]+ in solution (Kt,[AgNH3]^+ = 10^3,Kf2[Ag(NH3)2]^+=10^4) [AgNH3]^+ = 10^3 If 500 ml of 0.4 MAgNO3 is mixed with 50 ml of 2MNH3 solution then what is the concentration of [Ag(NH3)]+ in solution (Kt Kf2[Ag(NH3)2]^+=10^4) November [...]
A solution is a mixture of 0.01 M KI and 0.1 M KCl. If solid AgNO3 is added to the solution, what is the [I^−] when AgCl begins to precipitate? [Ksp (AgI)=1.5×10^−16 ;[Ksp (AgCl)=1.8×10^−10 ]
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Nov
A solution is a mixture of 0.01 M KI and 0.1 M KCl. If solid AgNO3 is added to the solution, what is the [I^−] when AgCl begins to precipitate? [Ksp (AgI)=1.5×10^−16 ;[Ksp (AgCl)=1.8×10^−10 ] A solution is a mixture of 0.01 M KI and 0.1 M KCl. If solid AgNO3 is added to [...]
A solution is 0.10M in Ba(NO3)2 and 0.10M in Sr(NO3)2. If solid Na2CrO4 is added to the solution, what is [Ba2+], when SrCrO4 beings to precipitate? [Ksp(BaCrO4)=1.2×10^−10,Ksp(SrCrO4)=3.5 × 10^−5]
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Nov
A solution is 0.10M in Ba(NO3)2 and 0.10M in Sr(NO3)2. If solid Na2CrO4 is added to the solution, what is [Ba2+], when SrCrO4 beings to precipitate? [Ksp(BaCrO4)=1.2×10^−10,Ksp(SrCrO4)=3.5 × 10^−5] A solution is 0.10M in Ba(NO3)2 and 0.10M in Sr(NO3)2. If solid Na2CrO4 is added to the solution Ksp(SrCrO4)=3.5 × 10^−5] what is [Ba2+] when SrCrO4 [...]
A3B2 is a sparingly soluble salt with molar mass M(gmol−) and solubility x gm litre−1, the ratio of the molar concentration of B3− to the solubility product of the salt is
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Nov
A3B2 is a sparingly soluble salt with molar mass M(gmol−) and solubility x gm litre−1, the ratio of the molar concentration of B3− to the solubility product of the salt is A3B2 is a sparingly soluble salt with molar mass M(gmol−) and solubility x gm litre−1 the ratio of the molar concentration of B3− to [...]
10 mL of 0.1 M tribasic acid H3A is titrated with 0.1 M NaOH solution. What is the ratio of [H3A]/[A^3−] at 2nd equivalence point ?
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Nov
10 mL of 0.1 M tribasic acid H3A is titrated with 0.1 M NaOH solution. What is the ratio of [H3A]/[A^3−] at 2nd equivalence point ? 10 mL of 0.1 M tribasic acid H3A is titrated with 0.1 M NaOH solution. What is the ratio of [H3A]/[A^3−] at 2nd equivalence point ? November 22, 2020 [...]
50 mL of 0.05 M Na2CO3 is titrated against 0.1 M HCl. On adding 40 mL of HCl, pH of the solution will be [Given for H2CO3, pKa1 =6.35; pKa2 = 10.33; log3=0.477, log2=0.30]
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Nov
50 mL of 0.05 M Na2CO3 is titrated against 0.1 M HCl. On adding 40 mL of HCl, pH of the solution will be [Given for H2CO3, pKa1 =6.35; pKa2 = 10.33; log3=0.477, log2=0.30] 50 mL of 0.05 M Na2CO3 is titrated against 0.1 M HCl. On adding 40 mL of HCl log2=0.30] pH of [...]