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99% of Mg2+ is precipitated → 1% is left in the solution
[Mg2+] = 99% (0.052 M)
[Mg2+] = 5.2×10‒4 M
when 99% of Mg2+ is precipitated, 5.2×10‒4 M of Mg2+ is left in the solution
Ksp Mg(OH)2 = 8.9×10‒12 M
[OH‒] = 1.3082×10‒4 M
pOH = ‒log [OH‒]
The concentration of Mg2+ in seawater is 0.052 M. At what pH will 99% of the Mg 2+ be precipitated as the hydroxide salt? [Ksp for Mg(OH)2 = 8.9 X 10 -12.]
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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl 2nd Edition practice problems.