Calculate the pH of a 0.187 M solution of a base that has a Kb = 5.86x10^-6

Explanation:

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In this case, since the ionization of the described base is:

Thus, the equilibrium expression in terms of the reaction extent is:

Thus, by solving for x we obtain:

So the values of x are:

So the feasible answer is 0.0010 M, thus we compute the pOH:

And therefore the pH:

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it would be b. 6co2 + 6h2o --> c6h12o6 + 6o2

the answer is barium and copper bromide