Additional Practice Questions
1 answer:
pH of solution = 13.033
<h3>Further explanation</h3>Given
2.31 g Ba(OH)₂
250 ml water
Required
pH of solution
Solution
Barium hydroxide is fully ionized, means that Ba(OH)₂ is a strong base
So we use a strong base formula to find the pH
[OH ⁻] = b. Mb where
b = number of OH⁻ /base valence
Mb = strong base concentration
Molarity of Ba(OH)₂(MW=171.34 g/mol) :
Ba(OH)₂ ⇒ Ba²⁺ + 2OH⁻(b=valence=2)
[OH⁻]= 2 . 0.054
[OH⁻] = 0.108
pOH= - log 0.108
pOH=0.967
pOH+pH=14
pH=14-0.967
pH=13.033
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Answer: 237 ml of stock solution is taken in a 500 ml volumetric flask and diluted with water until the 500 ml mark to obtain 5.5 M diluted solution
Explanation:
Molarity of a solution is defined as the number of moles of solute dissolved per Liter of the solution.
According to the neutralization law,
where,
= molarity of stock
solution = 11.6 M
= volume of stock
solution = ?
= molarity of dilute
solution = 5.5 M
= volume of dilute
solution = 500 ml
Thus 237 ml of stock solution is taken in a 500 ml volumetric flask and diluted with water until the 500 ml mark to obtain 5.5 M diluted solution