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A solution containing 0.2 mole of dichol...

A solution containing `0.2` mole of dicholoracetice acid `(K_(a)=5xx10^(-2))` and0.1 mole sodium dicholoroacetate in one litre solution has `[H^(+)]` :

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The correct Answer is:
`0.05`;
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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. A solution containing 0.2 mole of dichloroacetic acid (K_(a)=5xx10^(-2)) and 0.1 mole sodium dichloroacetate in one litre solution has [H^(+)] :

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^(+)] :

A one litre solution contains 0.08 mole of acetic acid (K_(a)=1.75xx10^(-5)) . To the solution, 0.02 mole of NaOH is added. Then the P^(H) of resulting solution is [log 1.75=0.273]

A one litre contains 0.08 moleof acetic acid (K_(a) = 1.75 xx 10^(-5)) . To this solution of resulting solution is [log 1.75 = 0.243]

4g of NaOH was dissolved in one litre of a solution containing one mole of acetic acid and one mole of sodium acetete. Find the pH of the resulting solution ( K_(a) of acetic acid is 1.8xx10^(-3) )

What amount of solution propanoate should be added to one litre of an aqueous solution containing 0.02 mole of propanoic acid ( K_(a)=1.0xx10^(-5) at 25^(@)C ) to obtain a buffer solution of pH 6

Calculate the hydrogen ion concentration ( "in mol"//dm^3 ) in a solution containing 0.04 mole of acetic acid and 0.05 mole of sodium acetate in 500 mL of solution.Dissociation constant for acetic acid is 1.75xx10^(-6) Report your answer after multiplying by 2xx10^(6)

The pH of buffer solution containing 4 xx 10^(-3) and 0.4 mole of acetic acid (pK_(a) = 4.76) and sodium acetate respectively will be

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  9. Calculate the pH of the following mixtures given (pK(a) = pK(b) = 4.74...

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  10. A solution containing 0.2 mole of dicholoracetice acid (K(a)=5xx10^(-2...

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  11. 10g of NH(4)CI (mol.wt. 53.5) when dissolved in 1000g water lowered th...

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  12. At 18^(@)C aniline and acetic acid have dissociation constants 5xx10^(...

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  13. Calculate the extent of hydrolysis of 0.005M K(2)CrO(4) K(2)=3.1xx10^(...

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  14. A solution was made up by 0.01M Co(NO(3))(2) and .02 M N(2)H(4) and wa...

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  15. The vapour pressur of 0.01molal solution of weak base BOH in water at ...

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  16. A 0.01M aqueous solution of weak acid HA has an osotic pressure 0.293a...

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  17. The freezing point of 3.75xx10^(-2)M aqueous solution of weak acid HA ...

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  18. Calculate the pH at which an acid indicator with K(a)=1xx10^(-5) chang...

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  19. A solution of HCI has pH = 5. If 1mL of it is diluted to 1L what will ...

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  20. Calculate the pH of 0.010M NaHCO(3) solution. K(1)=4.5xx10^(-7) , K(...

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