The value of `K_(w)`, at the physiological temperature `37^(@)C` is `2.56 xx 10^(-14)`. What is the `pH` at the neutral point of water at this temperature where there are equal numbers of `H^(o+)` and `overset(Θ)OH` ions?

Explanation

To find the pH at the neutral point of water at 37°C, given that the value of \( K_w \) is \( 2.56 \times 10^{-14} \), we can follow these steps:

### Step 1: Calculate \( pK_w \)
The relationship between \( K_w \) and \( pK_w \) is given by the formula:
\[ pK_w = -\log(K_w) \]
Substituting the given value of \( K_w \):
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