Chapter 6 – Ionic Equilibrium (Level 1 and Level 2)
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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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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? ,
A buffer solution 0.04 M in Na2HPO4 and 0.02 in Na3PO4 is prepared. The electrolytic oxidation of 1.0 milli-mole of the organic compound RNHOH is carried out in 100 mL of the buffer. The reaction is RNHOH + H2O→RNO2+4H^+ +4e− The approximate pH of solution after the oxidation is complete is : [Given:forH3PO4,pKa1=2.2,pKa2=7.20,pKa3=12]
22
Nov
A buffer solution 0.04 M in Na2HPO4 and 0.02 in Na3PO4 is prepared. The electrolytic oxidation of 1.0 milli-mole of the organic compound RNHOH is carried out in 100 mL of the buffer. The reaction is RNHOH + H2O→RNO2+4H^+ +4e− The approximate pH of solution after the oxidation is complete is : [Given:forH3PO4,pKa1=2.2,pKa2=7.20,pKa3=12] 1.0 L [...]
Which of the following expression for % dissociation of a monoacidic base (BOH) in aqueous solution at appreciable concentration is not correct?
22
Nov
Which of the following expression for % dissociation of a monoacidic base (BOH) in aqueous solution at appreciable concentration is not correct? Which of the following expression for % dissociation of a monoacidic base (BOH) in aqueous solution at appreciable concentration is not correct? November 22, 2020 Category: Chapter 6 - Ionic Equilibrium (Level 1 [...]
A 1.025 g sample containing a weak acid HX (mol. Mass=82) is dissolved in 60 mL. water and titrated with 0.25 M NaOH. When half of the acid was neutralised the pH was found to be 5.0 and at the equivalence point the pH is 9.0. Calculate mass percentage of HX in sample :
22
Nov
A 1.025 g sample containing a weak acid HX (mol. Mass=82) is dissolved in 60 mL. water and titrated with 0.25 M NaOH. When half of the acid was neutralised the pH was found to be 5.0 and at the equivalence point the pH is 9.0. Calculate mass percentage of HX in sample : 1.0 [...]
How many gm of solid KOH must be added to 100 mL of a buffer solution to make the pH of solution 6.0, if it is 0.1 M each w.r.t. acid HA and salt K A. [Given : pKa (HA)=5]
22
Nov
How many gm of solid KOH must be added to 100 mL of a buffer solution to make the pH of solution 6.0, if it is 0.1 M each w.r.t. acid HA and salt K A. [Given : pKa (HA)=5] How many gm of solid KOH must be added to 100 mL of a buffer [...]
How many gm of solid KOH must be added to 100 mL of a buffer solution to make the pH of solution 6.0, if it is 0.1 M each w.r.t. acid HA and salt K A. [Given : pKa (HA)=5]
22
Nov
How many gm of solid KOH must be added to 100 mL of a buffer solution to make the pH of solution 6.0, if it is 0.1 M each w.r.t. acid HA and salt K A. [Given : pKa (HA)=5] How many gm of solid KOH must be added to 100 mL of a buffer [...]
Fe(OH)2 is diacidic base has Kb1=10^−4 and Kb2 = 2.5 × 10^−6 What is the concentration of Fe(OH)2 in 0.1 M Fe(NO3)2 solution?
22
Nov
Fe(OH)2 is diacidic base has Kb1=10^−4 and Kb2 = 2.5 × 10^−6 What is the concentration of Fe(OH)2 in 0.1 M Fe(NO3)2 solution? Fe(OH)2 is diacidic base has Kb1=10^−4 and Kb2 = 2.5 × 10^−6 What is the concentration of Fe(OH)2 in 0.1 M Fe(NO3)2 solution? November 22, 2020 Category: Chapter 6 - Ionic 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 [...]