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The Ph of basic buffer mixtures is given...

The Ph of basic buffer mixtures is given by : `Ph=Pk_(a)+`log `(["Base"])/(["Salt"])` whereas Ph of acidic buffer mixtures is given by : Ph =`pK_(a)+"log"(["Salt"])/(["Acid"])`. Addition of little acid or base although shows no appreciable change in Ph for all practical purposes, but sicne the ratio `(["Base"])/(["Salt"])` or `(["Salt"])/(["Acid"])` changes, a slight decrease or increase in pH results.
The volume of 0.2 m NaOH needed to prepare a buffer of pH 4.74 with 50 mL of 0.2 m acetic acid `pH_(b)` of `CH_(3)COO^(-)=9.26` is :

A

50mL

B

25mL

C

20mL

D

10mL

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The correct Answer is:
b
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The pH of basic buffer mixtures is given by : pH=pK_(a)+log((["Base"])/(["Salt"])) , whereas pH of acidic buffer mixtures is given by: pH= pK_(a)+log((["Salt"])/(["Acid"])) . Addition of little acid or base although shows no appreciable change for all practical purpose, but since the ratio (["Base"])/(["Salt"]) or (["Salt"])/(["Acid"]) change, a slight decrease or increase in pH results in. The volume of 0.2M NaOH needed to prepare a buffer of pH 4.74 with 50 mL of 0.2M acetic acid is: (pK_(a) of CH_(3)COO^(-)= 9.26)

The pH of basic buffer mixtures is given by : pH=pK_(a)+log((["Base"])/(["Salt"])) , whereas pH of acidic buffer mixtures is given by: pH= pK_(a)+log((["Salt"])/(["Acid"])) . Addition of little acid or base although shows no appreciable change for all practical purpose, but since the ratio (["Base"])/(["Salt"]) or (["Salt"])/(["Acid"]) change, a slight decrease or increase in pH results in. Mole of HCI required to prepare a buffer solution of pH=8.5 with 0.1 mole of NaCN in one litre solution is: (pK_(a) for CN^(-)=4.61)

The Ph of basic buffer mixtures is given by : Ph=Pk_(a)+ log (["Base"])/(["Salt"]) whereas Ph of acidic buffer mixtures is given by : Ph = pK_(a)+"log"(["Salt"])/(["Acid"]) . Addition of little acid or base although shows no appreciable change in Ph for all practical purposes, but sicne the ratio (["Base"])/(["Salt"]) or (["Salt"])/(["Acid"]) changes, a slight decrease or increase in pH results. The amount of (NH_(4))_(2)SO_(4) to be added to 500mL of 0.01 M NH_(4)OH solution (pH_(a)NH_(4)^(+) is 9.26) to prepare a buffer of pH 8.26 is :

The Ph of basic buffer mixtures is given by : Ph=Pk_(a)+ log (["Base"])/(["Salt"]) whereas Ph of acidic buffer mixtures is given by : Ph = pK_(a)+"log"(["Salt"])/(["Acid"]) . Addition of little acid or base although shows no appreciable change in Ph for all practical purposes, but sicne the ratio (["Base"])/(["Salt"]) or (["Salt"])/(["Acid"]) changes, a slight decrease or increase in pH results. The ratio of pH of solution (I) containing 1 mole to pH of solution (II) containing 1 mole of CH_(3)COONa and 1 mole of acetic in one litre is :

The Ph of basic buffer mixtures is given by : Ph=Pk_(a)+ log (["Base"])/(["Salt"]) whereas Ph of acidic buffer mixtures is given by : Ph = pK_(a)+"log"(["Salt"])/(["Acid"]) . Addition of little acid or base although shows no appreciable change in Ph for all practical purposes, but sicne the ratio (["Base"])/(["Salt"]) or (["Salt"])/(["Acid"]) changes, a slight decrease or increase in pH results. A solution containing 0.2 mole of dichloroacetic acid (K_(a)=5xx10^(-2)) and 0.1 mole sodium dichloracetate in one litre solution has [H^(+)] :

The pH of an acidic buffer mixture is:

GRB PUBLICATION-IONIC EQUILIBRIUM-All Questions
  1. The Ph of basic buffer mixtures is given by : Ph=Pk(a)+log (["Base"])...

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  2. The Ph of basic buffer mixtures is given by : Ph=Pk(a)+log (["Base"])...

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  3. The Ph of basic buffer mixtures is given by : Ph=Pk(a)+log (["Base"])...

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  4. The Ph of basic buffer mixtures is given by : Ph=Pk(a)+log (["Base"])...

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  6. The solubility product of a soluble salt A(x)B(y) is given by : K(sp)=...

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  7. The solubility product of a soluble salt A(x)B(y) is given by : K(sp)=...

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  8. The solubility product of a soluble salt A(x)B(y) is given by : K(sp)=...

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  9. The solubility product of a soluble salt A(x)B(y) is given by : K(sp)=...

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  10. For the self-ionisation (protonation) process liquid formic acid at 20...

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  12. For the self-ionisation (protonation) process liquid formic acid at 20...

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  13. Amino acid glycine (NH(2)-CH(2)-COOH) exists as a zwitter ion in aq. S...

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  14. Amino acid glycine (NH(2)-CH(2)-COOH) exists as a zwitter ion in aq. S...

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  15. Following titration method is taken to compute stepwise ionisation con...

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  16. Following titration method is taken to compute stepwise ionisation con...

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  17. Following titration method is taken to compute stepwise ionisation con...

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  18. Acetic acid tends to form dimer due to formation of intermolcular hydr...

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  19. Acetic acid tends to form dimer due to formation of intermolcular hydr...

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  20. Acetic acid tends to form dimer due to formation of intermolcular hydr...

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