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A.) The pOH of an aqueous solution of 0.367 M hypochlorous acid is B.) The hydroxide...

A.) The pOH of an aqueous solution of 0.367 M hypochlorous acid is

B.)

The hydroxide ion concentration of an aqueous solution of 0.598 M hypochlorous acid is

[OH-] = M.

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Answer #1

A) ICE table constructed is as follows Initial (M) Change (M): Equilibrium (M): 0.367 0.367-x Acidionization constant ofHOCl= 2.9×10 Lo-1,-1 Acidionization constant, K. - HOCI 2.9×10 = 0367-x) x= 1.0×10.4 M From the equilibrium table, H^O* x 1.0x104M pH=-log! H,0+ |=-log( 1.0×10-4)=4.00 pOH 14.00-pH-14.00-4.00 10.00 B) ICE table constructed is as follows Initial (M) Change(M): Equilibrium (M): 0.598 0.598-x Acidionization constant ofHOCl= 2.9×10 OCI H20 HoCl Acidionization constant, K. - 29×10-(0.598-x) x1.3x10-4 M From the equilibrium table, | H,O+-x = 1.3×10-14 H301-1.3x 10-4-7.6x10-11M

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