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ASHA 777 [7]
3 years ago
6

The pH of a solution is 8.83±0.048.83±0.04 . What is the concentration of H+H+ in the solution and its absolute uncertainty?

Chemistry
1 answer:
slava [35]3 years ago
6 0

Answer:

The concentration of H^{+} is 1.48  × 10^{-9} M

The absolute uncertainty of [{H^{+}] is ±0.12 × 10^{-9} M

The concentration of H^{+} is written as 1.48(±0.12) × 10^{-9} M

Explanation:

The pH of a solution is given by the formula below

pH = -log_{10}[{H^{+}]

∴ [H^{+}] = 10^{-pH}

where [{H^{+}] is the H^{+} concentration

From the question,

pH = 8.83±0.04

That is,

pH =8.83 and the uncertainty is ±0.04

First, we will determine [{H^{+}] from

[H^{+}] = 10^{-pH}

[{H^{+}] = 10^{-8.83}

[{H^{+}] = 1.4791 × 10^{-9} M

[{H^{+}] = 1.48 × 10^{-9} M

The concentration of H^{+} is 1.48  × 10^{-9} M

The uncertainty of [{H^{+}]  ( U_{[H^{+}] } ) from the equation [H^{+}] = 10^{-pH} is

U_{[H^{+}] } = 2.303 \\ × {[H^{+}] } × U_{pH }

Where U_{[H^{+}] } is the uncertainty of [{H^{+}]

U_{pH } is the uncertainty of the pH

Hence,

U_{[H^{+}] } = 2.303 × 1.4791 × 10^{-9} × 0.04

U_{[H^{+}] } = 1.36 × 10^{-10} M

U_{[H^{+}] } = 0.12 × 10^{-9} M

Hence, the absolute uncertainty of [{H^{+}] is ±0.12 × 10^{-9} M

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<em></em>

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