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Buffer capacity of acidic buffer solutio...

Buffer capacity of acidic buffer solution is maximum when
(1) `P^(H)=P^(k)` (2) [salt ]= [acid ] (3) `p^(K)=7` (4) `[H^(+)]=P^(k)`

A

All are correct

B

(2).(3).(4) are correct

C

(1) and (2) are correct

D

(3) and (2) are correct

Text Solution

Verified by Experts

The correct Answer is:
C
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Higher the amount of acid or base used to produce a definite change of pH in a buffer solutions, higher will be its buffer capacity . Buffer capacity of solution is maximum under the following conditions: [Salt ]= [Acid ](in acid buffer ) ,[Salt ] =[Base] (in base buffer) pH of a buffer solution lies in the range given below : pH= pK_a +1 In other words any buffer solutions can be used as buffer up two pH units only. depending upon the value of pK_a or pK_b . A buffer is said to be efficient when pH = pK_a or pOH =pK_b , Buffer capacity is maximum when:

Higher the amount of acid or base used to produce a definite change of pH in a buffer solution,higher will be its buffer capacity. Buffer capacity of solution is maximum under the following conditions: [Salt= [Acid] (in acid buffer), [Salt] = [Base] (in base buffer) pH of a buffer solution lies in the range given below: pH = pk_(a)pm1 , In other words, any buffer solution can be used as buffer up to two pH units only, depending upon the value of pK_(a) , or pK_(b) ,. A buffer is said to be efficient when pH_(a) =pK_(a) , or pOH= pk_(b) Which among the following solution will be the most efficient buffer?

Higher the amount of acid or base used to produce a definite change of pH in a buffer solution,higher will be its buffer capacity. Buffer capacity of solution is maximum under the following conditions: [Salt= [Acid] (in acid buffer), [Salt] = [Base] (in base buffer) pH of a buffer solution lies in the range given below: pH = pk_(a)pm1 , In other words, any buffer solution can be used as buffer up to two pH units only, depending upon the value of pK_(a) , or pK_(b), . A buffer is said to be efficient when pH_(a) =pK_(a) , or pOH= pk_(b) The bulfer capacity is equal to :

When a salt reacts with water to form acidic (or ) basic solution the process is called salt hydrolysis. The P^(H) of salt solution can be calculated using the following relation P^(H) =(1)/(2) [P^(k_w) +P^(Ka) + log C ] for salt of weak acid and strong base. P^(H) =(1)/(2) [P^(K_w) -P^(K_a) -log C ] for salt of weak base and strong acid , P^(H) =(1)/(2) [P^(K_w) +P^(K_a) - P^(K_b) ] For a salt of weak acid and weak base where .c. represents the concentration of salt . When a weak acid (or) a weak base is not completly neatralised by strong base (or ) strong acid respectively, then formation of buffer takes places. The P^(H) of buffer solution can be calculated using the following relation P^(H) =P^(Ka) +log "" ((["salt")])/(["Acid "]) , P^(OH) =P^(Kb) +log ""(["salt"])/(["base"]) Answer the following questions using the following data pK_a (CH_3COOH) =4.7447 , pK_b (NH_4OH) =4.7447 , P^(K_W) =14. One mole CH_3 COOH and one mole CH_3 COONa are dissolved in water one litre aqueous solution The P^(H) of the resulting solution will be

When a salt reacts with water to form acidic (or ) basic solution the process is called salt hydrolysis. The P^(H) of salt solution can be calculated using the following relation P^(H) =(1)/(2) [P^(k_w) +P^(Ka) + log C ] for salt of weak acid and strong base. P^(H) =(1)/(2) [P^(K_w) -P^(K_a) -log C ] for salt of weak base and strong acid , P^(H) =(1)/(2) [P^(K_w) +P^(K_a) - P^(K_b) ] For a salt of weak acid and weak base where .c. represents the concentration of salt . When a weak acid (or) a weak base is not completly neatralised by strong base (or ) strong acid respectively, then formation of buffer takes places. The P^(H) of buffer solution can be calculated using the following relation P^(H) =P^(Ka) +log "" ((["salt")])/(["Acid "]) , P^(OH) =P^(Kb) +log ""(["salt"])/(["base"]) Answer the following questions using the following data pK_a (CH_3COOH) =4.7447 , pK_b (NH_4OH) =4.7447 , P^(K_W) =14. 0.001 M NH_4 Cl aqueous solution has P^(H)

A certain buffer solution contains equal concentration of X^(-) and HX. K_(b) , for X^(-) is 10^(-10) . Find the pH of buffer.

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AAKASH SERIES-IONIC EQUILLIBRIUM-LECTURE SHEET ( EXERCISE-III) ( Straight Objective Type Questions)
  1. Buffer capacity of acidic buffer solution is maximum when (1) P^(H)...

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  2. To a buffer solution of CH(3),COOH and CH(3),COONa, some HCI is added....

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  3. IM NaCl and IM HCI are present in an aqueous solution. The solution is

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  4. Which of the following pair of solutions does not form a buffer soluti...

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  5. Few drops of HCI is addded to acetic acid buffer. The p^(H) is maintai...

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  6. Aqueous solution of KCI is neutral because

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  7. Assertion (A): Aqueous solution of ammonium acetate is neutral Reaso...

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  8. The nature of 0.1 M solution of sodium bisulphate is

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  9. The no.of hydroxyl ions produced by one molecule of Na(2),CO(3) , on h...

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  10. The nature of aqueous solution of CuSO(4), is

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  11. Aqucous solution of which of the following shows lower P^(H) ?

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  12. The pH of an aqueous solution of a salt is 10. The salt

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  13. Aqueous solution of potash alum is acidic due to the hydrolysis of

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  14. Dissociation of CH(3),COOH is supressed by adding

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  15. Which pair will show common ion effect ?

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  16. Equal volumes of the following solutions are mixed. Which form buffer ...

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  17. pH of (HCN + KCN) buffer can be inreased by .

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  18. Which one of the following is/are buffer solution(s)?

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  19. Which of the following do not show change in pH on dilution?

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  20. Which are acidic salts ?

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