Hi! I need some help with this one; "Which values are correct for a 0.010 mol dm− solution of NaOH (aq) at 298 K? (Kw =1.0×10−14 mol2 dm−6 at 298 K) A. [H+] = 1.0*10^-12 mol dm^-3 and pH = 12.00 B. [OH-] = 1.0*10^-12 mol dm^-3 and pH = 12.00 C. [H+] = 1.0*10^-12 mol dm^-3 and pOH = 12.00 D. [OH-] = 1.0*10^-12 mol dm^-3 and pOH = 12.00" The mark scheme says A. Anyone that can explain this for me? Why is it not D?

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Hi! I need some help with this one; "Which values are correct for a 0.010 mol dm− solution of NaOH (aq) at 298 K? (Kw =1.0×10−14 mol2 dm−6 at 298 K) A. [H+] = 1.0*10^-12 mol dm^-3 and pH = 12.00 B. [OH-] = 1.0*10^-12 mol dm^-3 and pH = 12.00 C. [H+] = 1.0*10^-12 mol dm^-3 and pOH = 12.00 D. [OH-] = 1.0*10^-12 mol dm^-3 and pOH = 12.00" The mark scheme says A. Anyone that can explain this for me? Why is it not D?

Chemistry
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At vero eos et accusamus et iusto odio dignissimos ducimus qui blanditiis praesentium voluptatum deleniti atque corrupti quos dolores et quas molestias excepturi sint occaecati cupiditate non provident, similique sunt in culpa qui officia deserunt mollitia animi, id est laborum et dolorum fuga. Et harum quidem rerum facilis est et expedita distinctio. Nam libero tempore, cum soluta nobis est eligendi optio cumque nihil impedit quo minus id quod maxime placeat facere possimus, omnis voluptas assumenda est, omnis dolor repellendus. Itaque earum rerum hic tenetur a sapiente delectus, ut aut reiciendis voluptatibus maiores alias consequatur aut perferendis doloribus asperiores repellat.

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pH = -log [H+] in the strong base the concentration of [OH-] is equal to the concentration of the base. In the problem you are given the concentration of the base. then Kw= [H+][OH-]=1 x10^(-14)
Thank you so much, Cuanchi! Now I understand:-)

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