N Awasthi Physical Chemistry
Statement 1 : In an acid-basic titration involving a strong base and a weak acid, methyl orange can be used as an indicator. Statement 2 : Methyl red changes its colour in the pH range 4.2 to 6.3.
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Nov
Statement 1 : In an acid-basic titration involving a strong base and a weak acid, methyl orange can be used as an indicator. Statement 2 : Methyl red changes its colour in the pH range 4.2 to 6.3. methyl orange can be used as an indicator. Statement 2 : Methyl red changes its colour in [...]
Statement 1 : When 0.1 m weak diprotic acid h2a dissociates with its dissociated constant ka1 = 10^3, then Ka2 = 10^8, then A^2- is almost equal to 10^3 M. Statement 2 : Since Ka2
18
Nov
Statement 1 : When 0.1 m weak diprotic acid h2a dissociates with its dissociated constant ka1 = 10^3, then Ka2 = 10^8, then A^2- is almost equal to 10^3 M. Statement 2 : Since Ka2 Statement 1 : When 0.1 m weak diprotic acid h2a dissociates with its dissociated constant ka1 = 10^3 then A^2- [...]
Assertion : In a titration of weak acid with strong base, the pH at the half equivalence point is pKa Reason : At half equivalence point, it will form acidic buffer at it’s maximum capacity where [acid] = [salt]
18
Nov
Assertion : In a titration of weak acid with strong base, the pH at the half equivalence point is pKa Reason : At half equivalence point, it will form acidic buffer at it’s maximum capacity where [acid] = [salt] Assertion : In a titration of weak acid with strong base it will form acidic buffer [...]
Statement-1: pH value of acidic buffer solution changes , If buffer solution is diluted up to very large extent. Statement-2: [H+] decreases due to change in concentration as well as α increases and decreases in concentration is more as compared to increases in α .
18
Nov
Statement-1: pH value of acidic buffer solution changes , If buffer solution is diluted up to very large extent. Statement-2: [H+] decreases due to change in concentration as well as α increases and decreases in concentration is more as compared to increases in α . Statement-1: pH value of acidic buffer solution changes To what [...]
What is the concentration of CH3COOH(aq.) in a solution prepared by dissolving 0.01 mole of NH+4CH3COO− in 1 L H2O? [Ka(CH3COOH)=1.8×10^−5),Kb(NH4OH)=1.8×10^−5]
18
Nov
What is the concentration of CH3COOH(aq.) in a solution prepared by dissolving 0.01 mole of NH+4CH3COO− in 1 L H2O? [Ka(CH3COOH)=1.8×10^−5),Kb(NH4OH)=1.8×10^−5] Kb(NH4OH)=1.8×10^−5] What is the concentration of CH3COOH(aq.) in a solution prepared by dissolving 0.01 mole of NH+4CH3COO− in 1 L H2O? [Ka(CH3COOH)=1.8×10^−5) November 18, 2020 Category: Chapter 6 - Ionic Equilibrium (Level 1 and [...]
Calcium lactate is a salt of weal organic acid and strong base represented as Ca(LaC)2. A saturated solution of Ca(LaC)2 contains 0.6 mole in 2 litre solution. pOH of solution is 5.60. If 90% dissociation of the salt takes place then what is pKa of lactic acid?
18
Nov
Calcium lactate is a salt of weal organic acid and strong base represented as Ca(LaC)2. A saturated solution of Ca(LaC)2 contains 0.6 mole in 2 litre solution. pOH of solution is 5.60. If 90% dissociation of the salt takes place then what is pKa of lactic acid? To what volume of 10 litre of 0.5 [...]
H3A is a weak triprotic acid (Ka1=10^−5, Ka2 = 10^−9, Ka3 = 10^−13 What is the value of pX of 0.1 M H3A (aq.) solution ? Where pX=-log X and X=[A^3−]/[HA^2−]
18
Nov
H3A is a weak triprotic acid (Ka1=10^−5, Ka2 = 10^−9, Ka3 = 10^−13 What is the value of pX of 0.1 M H3A (aq.) solution ? Where pX=-log X and X=[A^3−]/[HA^2−] H3A is a weak triprotic acid (Ka1=10^−5 Ka2 = 10^−9 Ka3 = 10^−13 What is the value of pX of 0.1 M H3A (aq.) [...]
If first dissociation of X(OH)3 is 100% whereas second dissociation is 50% and third dissociation is negligible then the pH of 4×10^−3 M X(OH)3 is :
18
Nov
If first dissociation of X(OH)3 is 100% whereas second dissociation is 50% and third dissociation is negligible then the pH of 4×10^−3 M X(OH)3 is : If first dissociation of X(OH)3 is 100% whereas second dissociation is 50% and third dissociation is negligible then the pH of 4×10^−3 M X(OH)3 is : November [...]
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 ?
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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 [...]