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ahrayia [7]
3 years ago
14

What is the concentration of OH − and pOH in a 0.00066 M solution of Ba ( OH ) 2 at 25 ∘ C? Assume complete dissociation.

Chemistry
1 answer:
Allushta [10]3 years ago
3 0

<u>Answer:</u> The hydroxide ion concentration and pOH of the solution is 1.32\times 10^{-3}M  and 2.88 respectively

<u>Explanation:</u>

We are given:

Concentration of barium hydroxide = 0.00066 M

The chemical equation for the dissociation of barium hydroxide follows:

Ba(OH)_2\rightarrow Ba^{2+}+2OH^-

1 mole of barium hydroxide produces 1 mole of barium ions and 2 moles of hydroxide ions

pOH is defined as the negative logarithm of hydroxide ion concentration present in the solution

To calculate pOH of the solution, we use the equation:

pOH=-\log[OH^-]

We are given:

[OH^-]=(2\times 0.00066)=1.32\times 10^{-3}M

Putting values in above equation, we get:

pOH=-\log(1.32\times 10^{-3})\\\\pOH=2.88

Hence, the hydroxide ion concentration and pOH of the solution is 1.32\times 10^{-3}M  and 2.88 respectively

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1374.75 is the concentration in milligrams per ml of a solution containing 23.5 meq sodium chloride per milliliter.

Concentration in chemistry is calculated by dividing a constituent's abundance by the mixture's total volume.

It is calculated in mg/ml.

The unit of measurement frequently used for electrolytes is the milliequivalent (mEq). This value compares an element's chemical activity, or combining power, to that of 1 mg of hydrogen.

Formula for calculating concentration in mg/ml is

Conc. (mg/ml) = M(eq) /ml ×  Molecular weight / Valency

Given

M(eq) NaCl/ ml = 23.5

Molecular weight pf NaCl = 58.5 g/mol

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Putting the values into the formula

Conc. (mg/ml) = 23.5 ×58.5/1

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Hence, 1374.75 is the concentration in milligrams per ml of a solution containing 23.5 meq sodium chloride per milliliter.

Learn more about Concentration here brainly.com/question/14500335

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