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Calculate the [CH3NH3+] of a 7.02×10-3 M solution of the weak base CH3NH2 (make an approximate calculation assuming that initial concentration is equal to the equilibrium concentration). Round your answer to 3 significant digits.

CH3NH2 + H2O = CH3NH3+ + OH-

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    Set up an ICE chart and substitute into the Kb expression.

    Kb = ?? = (CH3NH3^+)(OH^-(/(CH3NH2)
    (CH3NH3^+) = (OH^-) = x
    ((CGH3NH2) = 7.02 x 10^-3

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