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.
Advertisements
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
Assuming complete dissociation, calculate the pH of the following solution:
0.002 M HBr
Calculate the pH of the following solutions:
0.3 g of Ca(OH)2 dissolved in water to give 500 mL of solution.
Which of the following solution will have a pH value equal to 1.0?
Define pH.
Derive the equation pH + pOH = 14.
When CuSO4 solution in water is treated with concentrated HCl it turns _______.
Select the INCORRECT relation.
Which of the following when dissolved in water results in neutral solution?
The pH of 0.001 M HCl solution is ______.
The Ka value for HCN is 10−9. What is the pH of 0.4 M HCN solution?
Derive the relationship between pH and pOH.
Define pOH.
Define pOH.
Derive relationship between pH and pOH.
Define pOH.
Define pOH.
Define pOH.
Define the following term:
pOH
Which from the following compound in aqueous medium having minimum pH?
