Advertisements
Advertisements
प्रश्न
pH of a saturated solution of Ca(OH)2 is 9. The Solubility product (Ksp) of Ca(OH)2
पर्याय
0.5 × 10−15
0.25 × 10−10
0.125 × 10−15
0.5 × 10−10
Advertisements
उत्तर
0.5 × 10−15
Explanation:
\[\ce{Ca(OH)2 ⇌ Ca^{2+} + 2OH^-}\]
Given that pH = 9
pOH = 14 – 9 = 5
[pOH = – log10 [OH–]]
∴ [OH–] = 10–pOH
[OH–] = 10–5 M
Ksp = [Ca2+] [OH–]2
= `10^-5/2 xx (10^-5)^2`
= 0.5 × 10−15
APPEARS IN
संबंधित प्रश्न
Calculate the pH of the following solutions:
0.3 g of Ca(OH)2 dissolved in water to give 500 mL of solution.
The pH of 0.005M codeine (C18H21NO3) solution is 9.95. Calculate its ionization constant and pKb.
Answer the following in one sentence:
The pH of a solution is 6.06. Calculate its H+ ion concentration.
The CORRECT match between transition metal ion and its colour in aqueous solution.
Aqueous solution of ____________ will turn red litmus blue.
The percentage of pyridine (C5H5N) that forms pyridinium ion (C5H5NH) in a 0.10 M aqueous pyridine solution (Kb for C5H5N = 1.7 × 10−9) is ____________.
Equal volumes of three acid solutions of pH 1, 2 and 3 are mixed in a vessel. What will be the H+ ion concentration in the mixture?
The pH of a weak monoacidic base is 11.2, and its OH– ion concentration is ______.
Calculate the pH of the buffer solution containing 0.5 mol NaF and 0.015 mol HF per litre. [pKa = 3.1427].
Define pOH.
