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 ____________.
पर्याय
4 : 3
3 : 4
10 : 1
1 : 10
Advertisements
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?
Answer the following in one sentence :
Write one property of a buffer solution.
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
Write the formula to calculate pH of buffer solution.
Explain the types of buffer solutions.
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.
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?
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 buffer action of sodium acetate-acetic acid buffer.
