alphabeta
  • alphabeta
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
  • Stacey Warren - Expert brainly.com
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SOLVED
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schrodinger
  • schrodinger
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Cuanchi
  • Cuanchi
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)
alphabeta
  • alphabeta
Thank you so much, Cuanchi! Now I understand:-)

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