Calculate the hydrogen-ion concentration [h+] for the aqueous solution in which [oh-] is 1 x 10-2 mol/l. is this solution acididc, basic, or neutral? show your work.

[H⁺] = 1.0 x 10⁻¹² M.

Explanation:

∵ [H⁺][OH⁻] = 10⁻¹⁴.

[OH⁻] = 1 x 10⁻² mol/L.

∴ [H⁺] =  10⁻¹⁴/[OH⁻] = (10⁻¹⁴)/(1 x 10⁻² mol/L) = 1.0 x 10⁻¹² M.

∵ pH = - log[H⁺] = - log(1.0 x 10⁻¹² M) = 12.0.

∴ The solution is basic, since pH id higher than 7 and also the  [OH⁻] > [H⁺].

where's the diagram?

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

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