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Question
Answer the following in one sentence :
Classify the following buffers into different types :
NH4OH + NH4Cl
Options
Acidic buffer
Basic buffer
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Solution
NH4OH + NH4Cl - Basic buffer
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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 the formula to calculate pH of buffer solution.
Define buffer solution.
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 ____________.
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.
Write any four applications of buffer solution.
What are buffer solutions?
Calculate pKa of HF if Ka= 7.2 x 10-4.
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)
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].
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?
