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I have a silly doubt

In acids and bases

As you guys know

The concentration of H+ ions

For a weak acid

Which does not undergo

Complete dissociation

Is given by mod H+=square root of Ka times C

Where C is the initial concentration

Of the acid

And k is the ionization constant

In the same manner

For a weak base

The concentration of OH- ions

Is given in a similar manner

And ka is replaced by kb (assuming C remains constant for both of them)

Now assume that the acid and the base both are at 25 degrees centigrade

Thus kw=10^-14

Now multiplying mod H+

And OH-

We get 10^-14=10^-7 (square root of kw) times C

And thus C comes out to be 10^-7

Here is where the contradiction arises

If the concentration of the acid is less than 10^-7

And same for the base

Dissociation does occur

And their respective ph

Can be found

So why does C appear to be only 10^-7

Why a constant

Because concentration varies as per our will

We can add more solute in a solution or decrease the amount

If we want to!!

Help is much appreciated

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# Acid base confusion

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