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Write the formula to calculate pH of buffer solution. - Chemistry

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प्रश्न

Write the formula to calculate pH of buffer solution.

एक पंक्ति में उत्तर

उत्तर

The formula to calculate the pH of acidic buffer solution is:

pH = pKa + log10 `(["Salt"])/(["Acid"])`

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अध्याय 3: Ionic Equilibria - Very short answer questions

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एससीईआरटी महाराष्ट्र Chemistry [English] 12 Standard HSC
अध्याय 3 Ionic Equilibria
Very short answer questions | Q 6

संबंधित प्रश्न

A solution of NH4Cl and NH4OH acts as a buffer.


Cu is precipitated as CuS while  Zn is not precipitated when H2S is passed through an acidic solution of Cu(NO3 )2  and Zn(NO3)2 respectively.


Answer the following in one sentence :

Classify the following buffers into different types :

CH3COOH + CH3COONa


Answer the following in one sentence :

Classify the following buffers into different types :

NH4OH + NH4Cl


Answer the following in one sentence :

Classify the following buffers into different types :

Cu(OH)2 + CuCl2


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


Name the buffer which is used to maintained pH of 8 to 10 for precipitation of cations III A group in qualitative analysis.


Define buffer solution.


Explain the types of buffer solutions.


Write one application of the following buffer:

Citrate buffer


Write one application of the following buffer:

`"HCO"_3^-  + "H"_2"CO"_3`


A buffer solution contains 0.3 mol dm–3 NH4OH (Kb = 1.8 × 10–5) and 0.4 mol dm–3 NH4Cl. Calculate pOH of the solution.


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]


____________ forms a basic buffer solution.


Which will make basic buffer?


The dissociation constant of a weak acid is 1 × 10−3. In order to prepare a buffer solution with a pH = 4, the `(["Acid"])/(["Salt"])` ratio should be ____________.


The hydrogen ion concentration of a buffer solution consisting of a weak acid and its salts is given by ____________.


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?


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.


Explain the types of buffers with example.


Explain buffer action of sodium acetate-acetic acid buffer.


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