Question 4 of the "Week 2 Achieve Homework" states:
"If the Kb of a weak base is 5.4 × 10−6, what is the pH of a 0.17 M solution of this base?"
How can we determine whether this weak base is monoprotic or polyprotic? (Some bases produce 2 moles of OH- per 1 mole of base.)
Week 2 Achieve Homework: Question 4
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Week 2 Achieve Homework: Question 4
Last edited by Sasha Gladkikh 2A on Sun Jan 23, 2022 12:14 am, edited 1 time in total.
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Re: Week 2 Achieve Homework: Question 4
I don't think that there is a way to tell whether an acid is monoprotic or polyprotic by just looking at the problem. Usually, they will have you assume that it is monoprotic or they will specify that it is polyprotic in the question.
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Re: Week 2 Achieve Homework: Question 4
When the compound is unspecified, the assumed chemical equation is:
B(aq) + H2O(l) <-> BH+(aq) + OH-(aq)
It is safe to assume that the base is monoprotic unless otherwise specified.
B(aq) + H2O(l) <-> BH+(aq) + OH-(aq)
It is safe to assume that the base is monoprotic unless otherwise specified.
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Re: Week 2 Achieve Homework: Question 4
Unless the problem specifically states that the base is polyprotic, there is no way to determine that without being given the compound, so you can assume it is monoprotic.
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