at a particular temperature, asample of pure water has a Kw of 1.7x10-12. what is the hydroxide concentration of this sample

Hydroxide concentration of the sample is 1.3x10⁻⁶M

Explanation:

The equilibrium constant of water, Kw, is:

H₂O(l) ⇄ H⁺(aq) + OH⁻(aq)

Kw is defined as:

Kw = 1.7x10⁻¹² = [H⁺] [OH⁻]

As the sample is of pure water, both H⁺ and OH⁻ ions have the same concentration because come from the same equilibrium, that is:

[H⁺] = [OH⁻]

We can write the Kw expression:

1.7x10⁻¹² = [OH⁻] [OH⁻]

1.7x10⁻¹² = [OH⁻]²

1.3x10⁻⁶M = [OH⁻]

personal, she chose to do it.

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

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