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guajiro [1.7K]
3 years ago
9

If the [H+] in a solution is 1 × 10–1 mol/L, what is the [OH–]? Show your work.

Chemistry
1 answer:
AVprozaik [17]3 years ago
3 0
Hello!

The basic equations to solve this is
pH = -log[H+]
pOH = -log[OH-]
pH + pOH = 14
------------------------------------------------------------------------------------------------------
Find pH

pH = -log(1 * 10^-1)
pH = 1
------------------------------------------------------------------------------------------------------
Find pOH
1 + pOH = 14

pOH = 13
------------------------------------------------------------------------------------------------------
Find OH-
[OH-] = 10^(-pOH)
[OH-] = 1 * 10^-13mo/L

The answer is [OH-] = 1 * 10^{-13} mol/L

Hope this helps!
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Answer:

True

Explanation:

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Assuming that there is some residual liquid left after equilibrium is reached, no matter how much liquid is present, at any given temperature, the vapor pressure will be the same because it is an intensive property.

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In the laboratory a student combines 47.8 mL of a 0.321 M aluminum nitrate solution with 21.8 mL of a 0.366 M aluminum iodide so
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Substitute the values into above formula as follows.

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