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महाराष्ट्र राज्य शिक्षण मंडळएचएससी विज्ञान (सामान्य) इयत्ता १२ वी

Answer the following in one sentence : Classify the following buffers into different types : CH3COOH + CH3COONa - Chemistry

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प्रश्न

Answer the following in one sentence :

Classify the following buffers into different types :

CH3COOH + CH3COONa

पर्याय

  • Acidic buffer

  • Basic buffer

MCQ
एका वाक्यात उत्तर
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उत्तर

CH3COOH + CH3COONa - Acidic buffer

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Buffer Solutions
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पाठ 3: Ionic Equilibria - Exercises [पृष्ठ ६२]

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बालभारती Chemistry [English] Standard 12 Maharashtra State Board
पाठ 3 Ionic Equilibria
Exercises | Q 2. x. a. | पृष्ठ ६२

संबंधित प्रश्‍न

A solution of NH4Cl and NH4OH acts as a buffer.


Choose the most correct answer:

Which of the Na following is a buffer solution?


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


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


Write the formula to calculate pH of buffer solution.


Explain the types of buffer solutions.


Write one application of the following buffer:

`"HCO"_3^-  + "H"_2"CO"_3`


Write one application of the following buffer:

NH4OH + NH4Cl


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?


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.


Calculate the pH of buffer solution composed of 0.01 M weak base BOH and 0.02 M of its salt BA. [Kb = 1.8 × 10–5 for weak base]


Define Acidic buffer solution.


Calculate pKa of HF if Ka= 7.2 x 10-4.


Explain the types of buffers with example.


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