Question

A sample of lime juice has a hydronium ion concentration of 6.3 × 10−2 M. Calculate its pH.

Answer 1

Answer:

1.2pH as...

Explanation:

pH=

$- log(h + ) \\ = - log(6.3 \times {10}^{ - 2 } ) \\ = 2 - 0.8 \\ = 1.2$

Answer 2

The pH of given lime juice is 1.2.

Explanation:

We know that relation between pH and hydrogen ion concentration is as follows.

          pH = $-log [H^{+}]$

It is given that hydrogen ion concentration is $6.3 \times 10^{-2}$. Hence, putting the given values into the above formula as follows.

         pH = $-log [H^{+}]$

               = $-log [6.3 \times 10^{-2}]$      

               = 1.2

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