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In which of the following acid-base titr...

In which of the following acid-base titrations, `pH` is greater than `8` at the equivalent point?

A

Acetic acid versus ammonia.

B

Acetic acid versus sodium hydroxide

C

Hydrochloric acid versus ammonia

D

Hydrochloric acid versus soidum hydroxide.

Text Solution

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The correct Answer is:
B
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Acid-base indicator such as methy 1 orange, phenolphthalein, and bromothymol blue ate substances which change colour accroding to the hydrogen ion concentration of the solution to which they are added. Most indicators are weak acids (or more rarely weak base) in which the undissociated and dissociated forms have different and distinct colours. If methy 1 orange is used as the examples and the un-dissociated forms is written as HMO , then dissociation occurs as shown below: Reaction: {:(HMOhArr,H^(o+)+,MO^(Theta),,),(Red,"Colourless","Yellow",,):} The indicator should have a sharp colour change with the equivalence point of the titration. Usually the colour change of the indicator occurs over a range of about two pH units. It should be noted that the eye cannot detect the exact end point of the tiytration. The pK_(a) of the indicator should be near the pH of the solution at the equivalance point. Which of the following sitution exists at the equivalence point of titration?

In acid-base titration react rapidly to neutralise each other. Equivalence point is a point at which the acid and the base (or oxidising agent and reducing agent) have beem added in equivalent quantities. The end point in the point at which the titration stops. since the purpose of the indicator is to stop the titration close to the point at which the acid and base were added in equivalent quantities, it is important that the equivalent point and the end point be as close as must change colour at a pH close to that of a solution of the salt of the acid base. Singificantly, the pH changes most rapidly near the equivalent point. The exact shape of a titration curve depends on K_(a) and K_(b) of acid and base. The following curve represents titration curve of HCI against KOH . The pH at equivalent point is Examine the titration curve below and answer the question.

An acid-base titration consists of the controlled addition of a dissolved base to a dissolved acid (or the reverse). Acid and base react rapidly to neutralize each other. At the equivalence point, equivalents of reacting substances are equal. The pH during a titration changes every time with a drop of titrant added, but the rate of this change varies enormously. A titration curve, graph of pH as a function of the volume of titrant, displays in detail how the pH changes over the course of an acid base titration. Significantly. the pH changes most rapidly near the equivalence point. The exact shape of a titration curve depends on the K_(a) and K_(b) of acid and base The suitable indicator for this titration will be:

During the titration of a weak diprotic acid (H_(2)A) against a strong base (NaOH) , the pH of the solution half-way to the first equivalent point and that at the first equivalent point are given respectively by:

In acid-base titration react rapidly to neutralise each other. Equivalence point is a point at which the acid and the base (or oxidising agent and reducing agent) have beem added in equivalent quantities. The end point in the point at which the titration stops. since the purpose of the indicator is to stop the titration close to the point at which the acid and base were added in equivalent quantities, it is important that the equivalent point and the end point be as close as must change colour at a pH close to that of a solution of the salt of the acid base. Singificantly, the pH changes most rapidly near the equivalent point. The exact shape of a titration curve depends on K_(a) and K_(b) of acid and base. The curve represents the titration of

VMC MODULES ENGLISH-ICONIC EQUILIBRIUM-EFFICIENT
  1. The ionisation constant of ammonium hydroxide is 1.77xx10^(-5) at 298 ...

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  2. Which one of the following is not a buffer solution ?

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  3. In which of the following acid-base titrations, pH is greater than 8 a...

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  4. In a basic buffer, 0.0025 mole of 'NH4 Cl' and 0.15 mole of NH4OH are...

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  5. A certain buffer solution contains equal concentartion of X^(Theta) an...

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  6. The pK(b) of CN^(Theta) is 4.7. The pH is solution prepared by mixing ...

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  7. When 10 ml of 0.1 M acetic acid (pk(a)=5.0) is titrated against 10 ml ...

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  8. How much of the following are strong electrolytes? a. NH(3) b. NH(4)...

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  9. The pK(a) value of NH(3) is 5. Calculate the pH of the buffer solution...

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  10. Calculate the pH at the equivalence point during the titration of 0.1M...

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  11. The rapid change of pH near the stoichiometric point of an acid base t...

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  12. Solution of 0.1 N NH(4)OH and 0.1 N NH(4)Cl has pH 9.25, then find out...

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  13. When 0.1 mole of an acid is added to 2 L of a buffer solution, the P...

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  14. pH of a buffer solution decreases by 0.02 units when 0.12 g of acetic ...

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  15. The dissociation constants for acetic acid and HCN at 25^@C are 1.5xx...

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  16. A buffer solution contains 0.1 mole of sodium acetate dissolved in 100...

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  17. 100 mL of HCI + 35 mL of NaOH, colour of methyl orange in the solution...

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  18. What is [H^(+)] in mol/L of a solution that is 0.20 M in CH(3)COONa an...

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  19. In a buffer solution containing equal contration of B^(-) and H B, th...

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  20. A buffer solution contains 0.1 mole of sodium acetate dissolved in 100...

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