Advertisements
Advertisements
Question
pH of a saturated solution of Ca(OH)2 is 9. The Solubility product (Ksp) of Ca(OH)2
Options
0.5 × 10−15
0.25 × 10−10
0.125 × 10−15
0.5 × 10−10
Advertisements
Solution
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
RELATED QUESTIONS
Assuming complete dissociation, calculate the pH of the following solution:
0.003 M HCl
Answer the following in one sentence:
The pH of a solution is 6.06. Calculate its H+ ion concentration.
Which of the following is CORRECT for an aqueous solution of NH4CN?
[Ka of HCN = 4.0 × 10−10, Kb for NH4OH = 1.8 × 10−5]
The least basic hydroxide from the following is:
Following solutions were prepared by mixing different volumes of NaOH of HCl different concentrations.
i. 60 mL `"M"/10` HCl + 40 mL `"M"/10` NaOH
ii. 55 mL `"M"/10` HCl + 45 mL `"M"/10` NaOH
iii. 75 mL `"M"/5` HCl + 25 mL `"M"/5` NaOH
iv. 100 mL `"M"/10` HCl + 100 mL `"M"/10` NaOH
pH of which one of them will be equal to 1?
The aqueous solutions of sodium formate, anilinium chloride and potassium cyanide are respectively.
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?
If pKb for CN− at 25°C is 4.7, the pH of 0.5 M aqueous NaCN solution is ______.
Define pOH.
Define pH.
