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Explain why a 0.10 HCL solution is assumed to have a pH value 1?
Wiki User
∙ 12y ago
HCl is a strong acid. Therefore, it can be expected to fully dissociate in aqueous solution, yielding one hydrogen ion and one chloride ion per molecule. The concentration of the hydrogen ion should thus be the same as the initial concentration of the HCl. Therefore, a 0.10M HCl solution has an H+ concentration of 0.10M. By the equation pH=-log[H+], the pH of this solution is 1.
Wiki User
∙ 12y ago
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the answer is 2.7x10-2 Start with the reaction (product on top/reactant): Ka=1.0x10-2=[H+][ClO2-] / [HClO2]. We know that we start with 0.100M of HClO2 so we can use that in our equation above. HOWEVER Ka indicates values of a reaction in equilibrium, and the 0.100M is initial value. Construct an ICE table where H+ and ClO2- are both x and the acid value will equal initial minus the change (-x). So what you should have is: 1.0x10-2=x2/0.100-x now solve using quadratic equation. NOTE: in some cases the x could be negligible however it is not negligible in this problem so you must do the quadratic formula to solve for x. X is your concentration of [H+] = 0.0027=2.7x10-2.
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