What is the hydronium ion concentration of a 0.150 mol L^-1 hypochlorous acid solution with $K _ { \mathrm { a } } = 3.5 \times 10 - 8 ?$ The equation for the dissociation of hypochlorous acid is below: $$\mathrm { HOCl } ( a q ) + \mathrm { H } _ { 2 } \mathrm { O } ( l ) \rightleftharpoons \mathrm { H } _ { 3 } \mathrm { O }^ + ( a q ) + \mathrm { OCl } ^ { - } ( a q )$$ A)1.9 × 10^-4mol L^-1 B)7.2 × 10^-4mol L^-1 C)2.8 × 10^-5mol L^-1 D)7.2 × 10^-5mol L^-1

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The Answer of What is the hydronium ion concentration of a 0.150 mol L^-1 hypochlorous acid solution with $K _ { \mathrm { a } } = 3.5 \times 10 - 8 ?$ The equation for the dissociation of hypochlorous acid is below: $$\mathrm { HOCl } ( a q ) + \mathrm { H } _ { 2 } \mathrm { O } ( l ) \rightleftharpoons \mathrm { H } _ { 3 } \mathrm { O }^ + ( a q ) + \mathrm { OCl } ^ { - } ( a q )$$ A)1.9 × 10^-4mol L^-1 B)7.2 × 10^-4mol L^-1 C)2.8 × 10^-5mol L^-1 D)7.2 × 10^-5mol L^-1

What Is the Hydronium Ion Concentration of a 0 Ka=3.5×10−8?K _ { \mathrm { a } } = 3.5 \times 10 - 8 ?Ka​=3.5×10−8?

What Is the Hydronium Ion Concentration of a 0 $K _ { \mathrm { a } } = 3.5 \times 10 - 8 ?$