N Awasthi Physical Chemistry
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)
22
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 ]
22
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]
22
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
22
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 ?
22
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]
22
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 [...]
In the titration of solution of a weak acid HA and NaOH, the pH is 5.0 after 10 mL of NaOH solution has been added and 5.60 after 20 mL NaOH has been added. What is the value of pKa for HA?
22
Nov
In the titration of solution of a weak acid HA and NaOH, the pH is 5.0 after 10 mL of NaOH solution has been added and 5.60 after 20 mL NaOH has been added. What is the value of pKa for HA? In the titration of solution of a weak acid HA and NaOH the [...]
Calculate approximate pH of the resultant solution formed by titration of 25 mL of 0.04 M Na2CO3 with 50 mL of 0.025 M HCl. [Given:pKa1=6.4 and pKa2 = 10.3 for H2CO3]
22
Nov
Calculate approximate pH of the resultant solution formed by titration of 25 mL of 0.04 M Na2CO3 with 50 mL of 0.025 M HCl. [Given:pKa1=6.4 and pKa2 = 10.3 for H2CO3] Calculate approximate pH of the resultant solution formed by titration of 25 mL of 0.04 M Na2CO3 with 50 mL of 0.025 M HCl. [...]
When a 20 mL of 0.08 M weak base BOH is titrated with 0.08 M HCl, the pH of the solution at the end point is 5. What will be the pOH if 10 mL of 0.04 M NaOH is added to the resulting solution? [Given : log2 = 0.30 and log3 = 0.48]
22
Nov
When a 20 mL of 0.08 M weak base BOH is titrated with 0.08 M HCl, the pH of the solution at the end point is 5. What will be the pOH if 10 mL of 0.04 M NaOH is added to the resulting solution? [Given : log2 = 0.30 and log3 = 0.48] the [...]
A solution of weak acid HA was titrated with base NaOH. The equivalent point was reached when 40 mL. Of 0.1 M NaOH has been added. Now 20 mL of 0.1 M HCl were added to titrated solution, the pH was found to be 5.0 What will be the pH of the solution obtained by mixing 20 mL of 0.2 M NaOH and 20 mL of 0.2 M HA?
22
Nov
A solution of weak acid HA was titrated with base NaOH. The equivalent point was reached when 40 mL. Of 0.1 M NaOH has been added. Now 20 mL of 0.1 M HCl were added to titrated solution, the pH was found to be 5.0 What will be the pH of the solution obtained by [...]
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Chapter 6 - Ionic Equilibrium (Level 1 and Level 2)
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Chapter 7 - Equilibrium
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N Awasthi Physical Chemistry
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A solution of weak acid HA was titrated with base NaOH. The equivalent point was reached when 40 mL. Of 0.1 M NaOH has been added. Now 20 mL of 0.1 M HCl were added to titrated solution ,
the pH was found to be 5.0 What will be the pH of the solution obtained by mixing 20 mL of 0.2 M NaOH and 20 mL of 0.2 M HA? ,