What is the pH of a solution containing H^{+} | vedclass

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(A) The $pH$ of a solution is calculated using the formula: $pH = -\log [H^{+}]$.Given $[H^{+}] = 2.5 	imes 10^{-3} \ mol \ dm^{-3}$.Substituting the

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$2.6$

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(A) The $pH$ of a solution is calculated using the formula: $pH = -\log [H^{+}]$.Given $[H^{+}] = 2.5 	imes 10^{-3} \ mol \ dm^{-3}$.Substituting the value: $pH = -\log (2.5 	imes 10^{-3})$.Using the property $\log (a 	imes b) = \log a + \log b$: $pH = -(\log 2.5 + \log 10^{-3})$.$pH = -(\log 2.5 - 3)$.$pH = 3 - \log 2.5$.Given $\log 2.5 = 0.3979$,so $pH = 3 - 0.3979 = 2.6021$.Rounding to one decimal place,the $pH$ is approximately $2.6$.

What is the $pH$ of a solution containing $H^{+}$ ion concentration $2.5 \times 10^{-3} \ mol \ dm^{-3}$? (Given $\log 2.5 = 0.3979$)

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