Chapter 6 – Ionic Equilibrium (Level 1 and Level 2)
Sahay Sir > Question Answers > N Awasthi Physical Chemistry > Chapter 6 - Ionic Equilibrium (Level 1 and Level 2)
Calculate the ratio of HCOO^− and F^− in a mixture of 0.2 M HCOOH (Ka = 2×10^−4 ) and 0.1 M HF (Ka = 6.6×10^−4 )
18
Nov
Calculate the ratio of HCOO^− and F^− in a mixture of 0.2 M HCOOH (Ka = 2×10^−4 ) and 0.1 M HF (Ka = 6.6×10^−4 ) Calculate the ratio of HCOO^− and F^− in a mixture of 0.2 M HCOOH (Ka = 2×10^−4 ) and 0.1 M HF (Ka = 6.6×10^−4 ) November 18, 2020 [...]
What concentration of FCH2COOH, (Ka = 2.6 × 10^-3) is needed so that [H + ] = 2 × 10^-3 ?
18
Nov
What concentration of FCH2COOH, (Ka = 2.6 × 10^-3) is needed so that [H + ] = 2 × 10^-3 ? (Ka = 2.6 × 10^-3) is needed so that [H + ] = 2 × 10^-3 ? What concentration of FCH2COOH November 18, 2020 Category: Chapter 6 - Ionic Equilibrium (Level 1 and Level [...]
To what volume of 10 litre of 0.5 M CH3COOH (Ka=1.8×10^−5) be diluted in order to double the hydroxide ion concentration :
17
Nov
To what volume of 10 litre of 0.5 M CH3COOH (Ka=1.8×10^−5) be diluted in order to double the hydroxide ion concentration : To what volume of 10 litre of 0.5 M CH3COOH (Ka=1.8×10^−5) be diluted in order to double the hydroxide ion concentration : November 17, 2020 Category: Chapter 6 - Ionic Equilibrium (Level 1 [...]
20 mL of 0.1 M weak acid HA(Ka=10^−5) is mixed with solution of 10 mL of 0.3 M HCl and 10 mL. of 0.1 M NaOH. Find the value of [A−]/([HA]+[A^(-)])` in the resulting solution :
17
Nov
20 mL of 0.1 M weak acid HA(Ka=10^−5) is mixed with solution of 10 mL of 0.3 M HCl and 10 mL. of 0.1 M NaOH. Find the value of [A−]/([HA]+[A^(-)])` in the resulting solution : 20 mL of 0.1 M weak acid HA(Ka=10^−5) is mixed with solution of 10 mL of 0.3 M HCl [...]
Liquid NH3 dissociation to a slight extent, At a certain temp. its self dissociation constant KSDC(NH3)=10^−30. The number of NH+4 ions are present per 100 cm^(3)` of pure liquid are :
17
Nov
Liquid NH3 dissociation to a slight extent, At a certain temp. its self dissociation constant KSDC(NH3)=10^−30. The number of NH+4 ions are present per 100 cm^(3)` of pure liquid are : At a certain temp. its self dissociation constant KSDC(NH3)=10^−30. The number of NH+4 ions are present per 100 cm^(3)` of pure liquid are : [...]
Equilibrium constant of T2O (T or 1H3 is an isotope of 1 H1 ) and H2O are different at 298 K. Let at 298 K pure T2O has pT (like pH) is 7.62. The pT of a solution prepared by adding 10 mL of 0.2 M TCl to 15 mL of 0.25 M NaOT is:
17
Nov
Equilibrium constant of T2O (T or 1H3 is an isotope of 1 H1 ) and H2O are different at 298 K. Let at 298 K pure T2O has pT (like pH) is 7.62. The pT of a solution prepared by adding 10 mL of 0.2 M TCl to 15 mL of 0.25 M NaOT is: [...]
Consider the following statement and select correct option: (I) Ksp of Fe(OH)3 in aqueous solution is 3.8×10^−38 at 298 K. The concentration of Fe+ will increase when [H+] ion concentration decreases. (II) In a mixture of NH4Cl and NH4OH in water, a further amount of NH4Cl is added. The pH of the mixture will decreases. (III) An aqueous solution of each of the following salt (NH4I,HCOOK) will be basic, acidic respectively.
17
Nov
Consider the following statement and select correct option: (I) Ksp of Fe(OH)3 in aqueous solution is 3.8×10^−38 at 298 K. The concentration of Fe+ will increase when [H+] ion concentration decreases. (II) In a mixture of NH4Cl and NH4OH in water, a further amount of NH4Cl is added. The pH of the mixture will decreases. [...]
What mass of Agl will dissolve in 1.0 L of 1.0 M NH3? Neglect change in conc. Of NH3. [Given: Ksp(AgI) = 1.5×10^−16), Kf[Ag(NH3)+2] = 1.6×10^7], (At. Mass Ag=108,1=127)
17
Nov
What mass of Agl will dissolve in 1.0 L of 1.0 M NH3? Neglect change in conc. Of NH3. [Given: Ksp(AgI) = 1.5×10^−16), Kf[Ag(NH3)+2] = 1.6×10^7], (At. Mass Ag=108,1=127) (At. Mass Ag=108 1=127) Kf[Ag(NH3)+2] = 1.6×10^7] What mass of Agl will dissolve in 1.0 L of 1.0 M NH3? Neglect change in conc. Of NH3. [...]
Find moles of NH4Cl required to prevent Mg(OH)2 from precipitating in a litre of solution which contains 0.02 mole NH3 and 0.001 mole Mg2+ ions. Given : Kb(NH3)=10^−5, Ksp[Mg(OH)2] = 10^−11.
17
Nov
Find moles of NH4Cl required to prevent Mg(OH)2 from precipitating in a litre of solution which contains 0.02 mole NH3 and 0.001 mole Mg2+ ions. Given : Kb(NH3)=10^−5, Ksp[Mg(OH)2] = 10^−11. Find moles of NH4Cl required to prevent Mg(OH)2 from precipitating in a litre of solution which contains 0.02 mole NH3 and 0.001 mole Mg2+ [...]
What is the molar solubility of Mn(OH)2(Ksp = 4.5×10^−14) in a buffer solution containing equal amounts of NH+4 and NH3 (Kb=1.8×10^−5)?
17
Nov
What is the molar solubility of Mn(OH)2(Ksp = 4.5×10^−14) in a buffer solution containing equal amounts of NH+4 and NH3 (Kb=1.8×10^−5)? What is the molar solubility of Mn(OH)2(Ksp = 4.5×10^−14) in a buffer solution containing equal amounts of NH+4 and NH3 (Kb=1.8×10^−5)? November 17, 2020 Category: Chapter 6 - Ionic Equilibrium (Level 1 and Level [...]