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10 questions from this quiz
1.00×10−141.00 \times 10^{-14}1.00×10−14 mol² dm⁻⁶
[\ceH+]=[\ceOH−]=1.00×10−7[\ce{H+}]=[\ce{OH-}]=1.00\times10^{-7}[\ceH+]=[\ceOH−]=1.00×10−7
pH+pOH=14\text{pH} + \text{pOH} = 14pH+pOH=14
0.1000.1000.100 mol dm⁻³
The ionic product of water
5.00×10−25.00 \times 10^{-2}5.00×10−2 mol dm⁻³
[\ceH+]<[\ceOH−][\ce{H+}] < [\ce{OH-}][\ceH+]<[\ceOH−]
They completely dissociate in solution
12.70
It is an equilibrium constant
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