Advertisements
Advertisements
प्रश्न
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 ____________.
विकल्प
4 : 3
3 : 4
10 : 1
1 : 10
उत्तर
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 1 : 10.
Explanation:
Ka = 1 × 10−3
pH = 4
`(["Salt"])/(["Acid"])` = ?
pH = `"pK"_"a" + log (["Salt"])/(["Acid"])`
4 = `-log_10 (1 xx 10^-3) + log (["Salt"])/(["Acid"])`
4 = `3 + log_10 (["Salt"])/(["Acid"])`
1 = `log_10 (["Salt"])/(["Acid"])`
`(["Salt"])/(["Acid"])` = 101
i.e., `(["Acid"])/(["Salt"]) = 1/10` = 1 : 10
APPEARS IN
संबंधित प्रश्न
When NH4 Cl and NH4OH are added to a solution containing both, Fe3+ and Ca2+ ions, which ion is precipitated first and why?
A solution of NH4Cl and NH4OH acts as a buffer.
Answer the following in one sentence :
Classify the following buffers into different types :
CH3COOH + CH3COONa
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 ______.
____________ forms a basic buffer solution.
Which will make basic buffer?
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): 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 pKa of HF if Ka= 7.2 x 10-4.
