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3 years ago

What is the ph of a 0.006 m koh solution? 1. 11.78 2. 7.00 3. 2.22 4. 8.88 5. 5.12?

1 answer:

4 0

The concentration of OH⁻ is first converted to pOH bu using followinf formula,

pOH = -log [OH⁻]
Putting value,
pOH = -log (0.006)

pOH = 2.221
As we know,
pH + pOH = 14
Solving for pH,
pH = 14 - pOH
Putting value of pOH,
pH = 14 - 2.221

pH = 11.779
Result:
Option-1 is the correct answer.

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$51.9torr\times 2.20L=n\times 62.364\text{ L. Torr }mol^{-1}K^{-1}\times 292K\\\\n=\frac{51.9\times 2.20}{62.364\times 292}=0.0063mol$

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3 years ago

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