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महाराष्ट्र राज्य शिक्षण मंडळएचएससी विज्ञान (सामान्य) इयत्ता १२ वी

Write one application of the following buffer: HCO3- +H2CO3

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प्रश्न

Write one application of the following buffer:

`"HCO"_3^-  + "H"_2"CO"_3`

एका वाक्यात उत्तर
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उत्तर

pH of blood in our body is maintained at 7.36 –7.42 due to `("HCO"_3^-  + "H"_2"CO"_3)` buffer.

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पाठ 3: Ionic Equilibria - Short answer questions (Type- II)

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संबंधित प्रश्‍न

The ionization constant of benzoic acid is 6.46 × 10–5 and Ksp for silver benzoate is 2.5 × 10–13. How many times is silver benzoate more soluble in a buffer of pH 3.19 compared to its solubility in pure water?


When NH4 Cl and NH4OH are added to a solution containing both, Fe3+ and Ca2+ ions, which ion is precipitated first and why?


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Answer the following in one sentence :

How are basic buffer solutions prepared?


Answer the following in one sentence :

Classify the following buffers into different types :

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Answer the following in one sentence :

Classify the following buffers into different types :

Sodium benzoate + benzoic acid


Answer the following in one sentence :

Classify the following buffers into different types :

Cu(OH)2 + CuCl2


In biochemical system, pH of blood in our body is maintained due to the following buffer:


The pKb of weak base BOH [Kb(BOH) = 1 × 10-5] will be ______.


Write one application of the following buffer:

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What is the pH of 0.5 litre buffer solution containing 0.01 mole of CH3COOH and 0.01 mole of CH3COONa?

[pKa of acid = 4.74]


Which will make basic buffer?


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Ksp of Al(OH)3 is 1 × 10−15 M. At what pH does 1.0 × 10−3 M Al3+ precipitate on the addition of buffer of NH4Cl and NH4OH solution?


Which of the following will produce a buffer solution when mixed in equal volumes?


On the basis of the equation \[\ce{pH}\] = – log \[\ce{[H+]}\], the \[\ce{pH}\] of 10–8 mol dm–3 solution of \[\ce{HCl}\] should be 8. However, it is observed to be less than 7.0. Explain the reason.


Assertion (A): A solution containing a mixture of acetic acid and sodium acetate maintains a constant value of \[\ce{pH}\] on addition of small amounts of acid or alkali.

Reason (R): A solution containing a mixture of acetic acid and sodium acetate acts as a buffer solution around \[\ce{pH}\] 4.75.


Assertion (A): An aqueous solution of ammonium acetate can act as a buffer.

Reason (R): Acetic acid is a weak acid and \[\ce{NH4OH}\] is a weak base.


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Calculate the pOH of a buffer solution formed from 0.3 M weak base and 0.45 M of its salt with strong acid [pKb = 4.7447].


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A buffer solution is prepared by mixing 0.01 М HCN and 0.02 M sodium cyanide. If pKa for HCN is 5.20, what is the pH of solution?


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