What is the ion-product constant, #K_w#?

Answer 1

For water, this is the measure of the #"autoprotolysis reaction"#....

#2H_2O(l) rightleftharpoonsH_3O^+ + HO^-#
And #K_w=[HO^-][H_3O^+]=10^-14# at #298*K#.
And when we take #-log_10# of both sides we get the useful expression...........
#pH+pOH=14#, where #pH=-log_10[H_3O^+]# etc.
How do you think #K_w# would develop if non-standard conditions pertained; e.g. if temperature was say #373*K#. Would #K_w# remain constant, decrease, increase? Remember that the autoprotolysis reaction as shown is a #"bond-breaking reaction"#.
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Answer 2

The ion-product constant, Kw, is the equilibrium constant for the autoionization of water. It represents the product of the concentrations of hydronium ions (H3O+) and hydroxide ions (OH-) in water at a given temperature. At 25°C, Kw is equal to 1.0 x 10^-14.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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