Question

How many h+ ions are present in 1ml of a solution whose ph is 13

Answer 1

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Answer 2

pH = -log[$H^{+}$]

So,

pH = 13 (Given)

[$H^{+}$] Concentration = $10^{-13}$ mol/litre

Volume = 1 ml = 0.001 L

Avogadro's No. = 6.022 * $10^{23}$

So,

No. of $H^{+}$ ions = Volume * [$H^{+}$] Concentration * Avogadro's No.

= 0.001 * $10^{-13}$ * 6.022 * $10^{23}$

= 6.022 * $10^{7}$