What is the pH of H3PO4 solution with a molarity of 1-5-10-4- Assume 100

The correct option is B 3.35 nbsp;The dissociation of H_3PO_4 is given by H_3PO_4⇌ 3H^+ + PO_4^ (Assuming 100 ...

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Standard XII

Chemistry

pH the Power of H

What is the p...

Question

What is the pH of $H_{3} P O_{4}$ solution with a molarity of $1.5 \times 10^{- 4} ?$
( Assume 100% complete dissociation)

3.82

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3.35

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4.3

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None of the above

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Solution

The correct option is B 3.35
The dissociation of $H_{3} P O_{4}$ is given by $H_{3} P O_{4} ⇌ 3 H^{+} + P O_{4}^{-}$ (Assuming 100% complete dissociation)
Total concentration of $H^{+} = 3 \times 1.5 \times 10^{- 4}$
we know that pH value is given by
$\begin{matrix} p H & = - l o g [H^{+}] p H & = - l o g [3 \times 1.5 \times 10^{- 4}] p H & = 3.35 \end{matrix}$

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pH the Power of H

Standard XII Chemistry

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What is the pH of H3PO4 solution with a molarity of 1.5×10−4? ( Assume 100% complete dissociation)

The correct option is B 3.35 The dissociation of H3PO4 is given by H3PO4⇌3H++PO−4 (Assuming 100% complete dissociation) Total concentration of H+=3×1.5×10−4 we know that pH value is given by pH=−log[H+]pH=−log[3×1.5×10−4]pH=3.35

What is the pH of $H_{3} P O_{4}$ solution with a molarity of $1.5 \times 10^{- 4} ?$
( Assume 100% complete dissociation)