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[H + ]

[H + ]. [OH - ] = Kw / [H + ]. [OH - ]. [H + ] > [OH - ]. [H + ] < [OH - ]. [H + ] = [OH - ]. Acidic Solution. Basic Solution. Neutral Solution. What are the concentrations of H + and OH - in a 0.0012 M NaOH solution? Answer: NaOH s completely dissociated:

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[H + ]

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  1. [H+] [OH-] = Kw / [H+] [OH-] [H+]>[OH-] [H+]<[OH-] [H+]=[OH-] Acidic Solution Basic Solution Neutral Solution What are the concentrations of H+ and OH- in a 0.0012 M NaOH solution? Answer: NaOH s completely dissociated: 0.0012 M NaOH (ac)  0.0012 M Na+(ac) + Substituting [OH]- in the Kw equation: Kw = 1x10-14 = [H+][OH-] 1x10-14 = [H+](0.0012) [H+] = 1x10-14/0.0012 = 0.0012 M OH- (ac) 8.3x10-12 M

  2. [H+] pH [OH-] pOH 14,00 13,00 12,00 11,00 10,50 10,00 9,00 8,00 7,00 6,00 5,00 4,50 4,00 3,00 2,00 1,00 0,00 0,00 1,00 2,00 3,50 3,00 4,00 5,00 6,00 7,00 8,00 9,00 10,00 10,50 11,00 12,00 13,00 14,00 BASIC More Basic NEUTRAL More Acidic ACIDIC

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