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महाराष्ट्र राज्य शिक्षण मंडळएचएससी विज्ञान (सामान्य) इयत्ता १२ वी

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

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प्रश्न

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

पर्याय

  • -5

  • 5

  • 1

  • 10-5

MCQ
रिकाम्या जागा भरा
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उत्तर

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

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पाठ 3: Ionic Equilibria - Multiple choice questions

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?


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.


Choose the most correct answer:

Which of the Na following is a buffer solution?


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 :

Sodium benzoate + benzoic acid


Answer the following in one sentence :

Classify the following buffers into different types :

Cu(OH)2 + CuCl2


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.


Define buffer solution.


Write one application of the following buffer:

Citrate buffer


Write one application of the following buffer:

`"HCO"_3^-  + "H"_2"CO"_3`


Write one application of the following buffer:

NH4OH + NH4Cl


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?


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 ____________.


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.


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]


Explain the types of buffers with example.


What is the pH of buffer solution formed by mixing 0.01 M acetic acid and 0.05 M sodium acetate? (pKa = 4.7447)


What is the pH of buffer solution prepared by mixing \[\text{0.2MNH4OHand0.4MNH4Cl}\] solution. \[(\mathrm{pK_{b}~of~NH_{4}OH=4.620})\]


A buffer solution is prepared by mixing 0.1 M ammonia solution and 0.25 M solution of NH4CI. What is the value of pKb to maintain its pOH at 6?


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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