Calculate the pH of a 0.10 M solution of NaOH Express your answer numerically us

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Explanation / Answer

NaOH is known like SODIUM HYDROXIDE, although you refer to its aqueous solutions. NaOH results a VERY STRONG BASE because : -) it takes part to ionic dissociation in aqueous solutions TO GIVE HYDROXYL IONs (e.g. OH-) NaOH(aq) ---> OH-(aq) + Na+(aq) -) former writing RUNS COMPLETELY KEEPING NO ONE UNDISSOCIATED NaOH EQUIVALENTs. Now, you may assume that |NaOH| = |OH-| so you have |OH-| = 0.10 M. On the other hand, you have to know that WATER IS A CHEMICAL WHICH UNDERGO SELF-IONIZATION EQUILIBRIUM 2 H2O(aq) ---> H3O+(aq) + OH-(aq) Kw = 1.0E.14 = |H3O+| * |OH-| |H3O+| = 1.0E-14 / |OH-| = 1.0E-14 / 0.10 = 1.0E-13 M SO BY DEFINITION YOU CALCULATE pH LEVEL pH = - log(|H3O+|) = - log(1.0E-13) = 13.

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