Question 24 1 pts Calculate the pH of a 0.236 M solution of Sr(OH)2 Remember that...

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Answer 1

Answer #1

Dear Student, solved the first question, Question 24 as per HOMEWORKLIB RULES, post multiple question to get the remaining answers

Question 24:

Sr(OH)2 is a strong base, hence it will dissociate fully to form Sr(2+) and 2OH- ions

Molarity of OH- = 2 * 0.236 = 0.472 [because one mole of Sr(OH)2 will give 2 moles of OH- ions]

pOH = -log[OH-] = -log(0.472) = 0.326

pH = 14 - pOH = 14 - 0.326 = 13.674

Note - Post any doubts/queries in comments section.

Answer 2

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