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Modifié par Winy :
4/2/2013 8:17:39 PM
5
Hey, Chemistry people. Help a brother out, will yah? (Answered)
[quote]What is the pH of a 0.0684 M solution of hypochlorous acid (HClO) which has an ionization constant of 3.5E^-8?[/quote]
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1 commentaireHypochlorous acid is a weak acid, as indicated by the extremely small ionization (Ka) value. As such, when the acid is an aqueous environment, the following equilibrium reaction will occur: HClO + H2O <---> H3O+ + ClO- Create an ICE table, which is a useful organization tool in equilibrium chemistry. HClO + H2O <---> H3O+ + ClO- I 0.0684 0 0 C -x +x +x E 0.0684 x x I stands for initial concentrations; C for change; and E for equilibrium concentrations. The reason why E for HClO is the same as I is because the dissociation constant is much smaller than the initial concentration, which means assuming the HClO concentration did not change is acceptable. Ionization constant = [H3O+][ClO-] / [HClO] [H3O+] = sqrt(3.5e-8 x 0.0684) pH = -log[H3O+] = 4.31
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Modifié par Love Sosa : 4/1/2013 12:03:04 AMedit-never mind I forgot this. This was the third hardest chapter. Electrochemistry and cordination blows nuts
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1 commentaireAre you asking for the pKa value?
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*Does AS level Chemistry* "I can help" *See's question* Oh...
