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The [OH-] of an aqueous solution is #4.62 * 10^-4# M. What is the pH of this solution?
1 Answer
Explanation:
For pure water at #25^@'C'#, the concentration of hydronium ions, #'H'_3'O'^(+)#, is equal to the concentration of hydroxide ions, #'OH'^(-)#.
More specifically, water undergoes a self-ionization reaction that results in the formation of equal concentrations of hydronium and hydroxide anions.
#2'H'_2'O'_text((l]) rightleftharpoons 'H'_3'O'_text((aq])^(+) + 'OH'_text((aq])^(-)#
At room temperature, the self-ionization constant of water is equal to
#K_W = ['H'_3'O'^(+)] * ['OH'^(-)] = 10^(-14)#
This means that neutral water at this temperature will have
#['H'_3'O'^(+)] = ['OH'^(-)] = 10^(-7)'M'#
As you know, pH and pOH are defined as
#'pH' = - log( ['H'_3'O'^(+)])#
Office 365 monthly uk. #'pOH' = - log(['OH'^(-)])#
and have the following relationship
#'pH' + 'pOH' = 14#
In your case, the concentration of hydroxide ions is bigger than #10^(-7)'M'#, which tells you that you're dealing with a basic solution and that you can expect the pH of the water to be higher than #7#.
A pH equal to #7# is characteristic of a neutral aqueous solution at room temperature.
So, you can use the given concentration of hydroxide ions to determine the pOH of the solution first
Another Version 625
#'pOH' = - log( 4.62 * 10^(-4)) = 3.34#
This means that the solution's pH will be
#'pH' = 14 - 'pOH'#
#'pH' + 'pOH' = 14#
In your case, the concentration of hydroxide ions is bigger than #10^(-7)'M'#, which tells you that you're dealing with a basic solution and that you can expect the pH of the water to be higher than #7#.
A pH equal to #7# is characteristic of a neutral aqueous solution at room temperature.
So, you can use the given concentration of hydroxide ions to determine the pOH of the solution first
Another Version 625
#'pOH' = - log( 4.62 * 10^(-4)) = 3.34#
This means that the solution's pH will be
#'pH' = 14 - 'pOH'#
#'pH' = 14 - 3.34 = color(green)(10.66)#
Indeed, the pH is higher than #7#, which confirms that you're dealing with a basic solution.
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