Chapter 7 – Equilibrium
Sahay Sir > Question Answers > JEE Adv and Mains Chemistry 41 Years Solved Video Solutions 1979 - 2019 > Chemistry > Chapter 7 - Equilibrium
Ka for the reaction; Fe^3 + (aq.)+H2O(l) ⇌ Fe(OH)^2 + (aq.)+H3O^+ (aq.) is 6.5×10^−3 . What is the maximum pH value which could be used do that at least 80% of the total ion (III) in a dilute solution exists as Fe^3+ ?
22
Nov
Ka for the reaction; Fe^3 + (aq.)+H2O(l) ⇌ Fe(OH)^2 + (aq.)+H3O^+ (aq.) is 6.5×10^−3 . What is the maximum pH value which could be used do that at least 80% of the total ion (III) in a dilute solution exists as Fe^3+ ? 1.0 L solution is prepared by mixing 61 g benzoic acid (pKa=4.2) [...]
1.0 L solution is prepared by mixing 61 g benzoic acid (pKa=4.2) with 72 g of sodium benzoate and then 300 mL 1.0 M HBr solution was added. The pH of final solution is :
22
Nov
1.0 L solution is prepared by mixing 61 g benzoic acid (pKa=4.2) with 72 g of sodium benzoate and then 300 mL 1.0 M HBr solution was added. The pH of final solution is : 1.0 L solution is prepared by mixing 61 g benzoic acid (pKa=4.2) with 72 g of sodium benzoate and then [...]
Amongst the following, the total number of compounds whose aqueous solution turns red litmus paper blue is: NaCN KCL CH3CooNH4 NaH2PO4 ZnCL2
18
Nov
Amongst the following, the total number of compounds whose aqueous solution turns red litmus paper blue is: NaCN KCL CH3CooNH4 NaH2PO4 ZnCL2 Amongst the following the total number of compounds whose aqueous solution turns red litmus paper blue is: NaCN KCL CH3CooNH4 NaH2PO4 ZnCL2 November 18, 2020 Category: Chapter 6 - Ionic Equilibrium (Level 1 [...]
10 mL of H2A(weak diprotic acid) solution is titrated against 0.1M NaOH. pH of the solution is plotted against volume of strong base added and following observation is made. If pH of the solution at first equivalence point is pH1 and at second equivalence point is pH2.Calculate the value of (pH_(2)-pH_(1))at25^ degree C Given: for H_(2)A,pK_(a_1)=4.6 and pK_(a_2)` =8, log 25=1.4
18
Nov
10 mL of H2A(weak diprotic acid) solution is titrated against 0.1M NaOH. pH of the solution is plotted against volume of strong base added and following observation is made. If pH of the solution at first equivalence point is pH1 and at second equivalence point is pH2.Calculate the value of (pH_(2)-pH_(1))at25^ degree C Given: for [...]
A solution is saturated in srco3 and srf2. The CO^2-3 was found to be 10^-3 mol/ L. If the concentration of F^- in solution is represented as y x 10^2 M then what is the value of Y ?
18
Nov
A solution is saturated in srco3 and srf2. The CO^2-3 was found to be 10^-3 mol/ L. If the concentration of F^- in solution is represented as y x 10^2 M then what is the value of Y ? A solution is saturated in srco3 and srf2. The CO^2-3 was found to be 10^-3 mol/ [...]
When one litre of a saturated solution of PbCl2 (molecular weight =278 g/mol) is evaporated, the residue is found to weigh 2.78 g. If Ksp of PbCl2 is represented as y×10^−6 , then find the value of y.
18
Nov
When one litre of a saturated solution of PbCl2 (molecular weight =278 g/mol) is evaporated, the residue is found to weigh 2.78 g. If Ksp of PbCl2 is represented as y×10^−6 , then find the value of y. the residue is found to weigh 2.78 g. If Ksp of PbCl2 is represented [...]
If solubility of AgCl is 0. 2 M solution of AgNO3 is represented as Y×10^−10, then find the value of Y . [Given: Ksp(AgCl)=10^−10]
18
Nov
If solubility of AgCl is 0. 2 M solution of AgNO3 is represented as Y×10^−10, then find the value of Y . [Given: Ksp(AgCl)=10^−10] If solubility of AgCl is 0. 2 M solution of AgNO3 is represented as Y×10^−10 then find the value of Y . [Given: Ksp(AgCl)=10^−10] November 18, 2020 Category: Chapter 6 - [...]
A certain weak acid has Ka = 10^−5 . If the equilibrium constant for its reaction with a strong base is represented by 1×10^y, then find the value of y.
18
Nov
A certain weak acid has Ka = 10^−5 . If the equilibrium constant for its reaction with a strong base is represented by 1×10^y, then find the value of y. A certain weak acid has Ka = 10^−5 . If the equilibrium constant for its reaction with a strong base is represented by 1×10^y then [...]
Calculate the ratio of sodium formate and formic acid (Ka = 2 × 10^-4) in a buffer solution of pH = 4.3 .
18
Nov
Calculate the ratio of sodium formate and formic acid (Ka = 2 × 10^-4) in a buffer solution of pH = 4.3 . Calculate the ratio of sodium formate and formic acid (Ka = 2 × 10^-4) in a buffer solution of pH = 4.3 . November 18, 2020 Category: Chapter 6 - Ionic Equilibrium [...]
Calculate pH of a buffer solution that contains 0.1 M NH4OH(Kb = 10^-5) and 0.1 M NH4Cl .
18
Nov
Calculate pH of a buffer solution that contains 0.1 M NH4OH(Kb = 10^-5) and 0.1 M NH4Cl . Calculate pH of a buffer solution that contains 0.1 M NH4OH(Kb = 10^-5) and 0.1 M NH4Cl . November 18, 2020 Category: Chapter 6 - Ionic Equilibrium (Level 1 and Level 2) , Chapter 7 - Equilibrium [...]