Advertisements
Advertisements
Question
The solubility of Sr(OH)2 at 298 K is 19.23 g/L of solution. Calculate the concentrations of strontium and hydroxyl ions and the pH of the solution.
Solution
Solubility of Sr(OH)2 = 19.23 g/L
Then, concentration of Sr(OH)2
`= 19.23/121.63 "M"`
= 0.1581 M
\[\ce{Sr(OH)_{2(aq)} -> Sr^{2+}_{(aq)} + 2(OH^-)_{(aq)}}\]
`therefore ["Sr"^(2+)] = 0.1581 "M"`
`["OH"^(-)] = 2 xx 0.1581 "M"= 0.3126 "M"`
Now
`"K"_"w" = ["OH"^-]["H"^+]`
`10^(-14)/0.3126 = ["H"^+]`
`=> ["H"^+] = 3.2 xx 10^(-14)`
`therefore "pH" = 13.495; 13.50`
APPEARS IN
RELATED QUESTIONS
Calculate the pH of the following solutions:
0.3 g of Ca(OH)2 dissolved in water to give 500 mL of solution.
Calculate the pH of the following solution:
0.3 g of NaOH dissolved in water to give 200 mL of solution.
Answer the following in one sentence:
The pH of a solution is 6.06. Calculate its H⊕ ion concentration.
Answer the following in brief :
The pH of a weak monobasic acid is 3.2 in its 0.02 M solution. Calculate its dissociation constant.
Define pOH.
Which complex among the following gives a white precipitate on treatment with an aqueous solution of barium chloride?
The CORRECT match between transition metal ion and its colour in aqueous solution.
Select the INCORRECT relation.
What is the pH of the resulting solution when equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed?
Calculate the pH of 1.5 × 10−3 M solution of Ba(OH)2.
50 ml of 0.05 M HNO3 is added to 50 ml of 0.025 M KOH. Calculate the pH of the resultant solution.
The pH of a weak monoacidic base is 11.2, and its OH– ion concentration is ______.
The degree of dissociation of 0.1 M monobasic acid is 0.4%. Its dissociation constant 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.
Derive the relationship between pH and pOH.
Define pH.
Define pH.
Define pOH.
