Van der waal's equation

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In reality pressure of a gas is lower than what is expected and volume is larger than expected - as ideal gas equation neglected volume of gas molecules and forces between them. Van der waal corrected it but:-

I need to know then why do we add the constant n^2a/V^2 in pressure and subtract nb in volume


Shouldnt we subtract n^2a/V^2 from pressure as it is lower than what was expected

similarly we should add nb in volume as it is more than what was expected

Im a bit confused over van der waal's equation. Cannot understand it
 

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