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bixtya [17]
3 years ago
5

A chemist prepares a solution of calcium bromide CaBr2 by measuring out 4.81μmol of calcium bromide into a 50.mL volumetric flas

k and filling the flask to the mark with water. Calculate the concentration in /μmolL of the chemist's calcium bromide solution. Round your answer to 2 significant digits.
Chemistry
1 answer:
Mariana [72]3 years ago
4 0

Answer:

The concentration of the CaBr2 solution is 96 µmol/L

Explanation:

<u>Step 1:</u> Data given

Moles of Calciumbromide (CaBr2) = 4.81 µmol

Volume of the flask = 50.0 mL = 0.05 L

<u>Step 2:</u> Calculate the concentration of Calciumbromide

Concentration CaBr2 = moles CaBr2 / volume

Concentration CaBr2 = 4.81 µmol / 0.05 L

Concentration CaBr2 = 96.2 µmol /L = 96.2 µM

The concentration of the CaBr2 solution is 96 µmol/L

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What happened to the mixture as it is poured into the strainer with cloth?​
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Answer:

The solid particles will be trapped behind on the strainer while the liquid molecules will pass or filter through.

Explanation:

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3 0
2 years ago
What is the ph of a buffer prepared by adding 0.809 mol of the weak acid ha to 0.608 mol of naa in 2.00 l of solution? The disso
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The pH of the buffer is 6.1236.

Explanation:

The strength of any acid solution can be obtained by determining their pH. Even the buffer solution strength of the weak acid can be determined using pH. As the dissociation constant is given, we can determine the pKa value as the negative log of dissociation constant value.

pKa=-log[H] = - log [ 5.66 * 10^{-7}]\\ \\pka = 7 - log (5.66)=7-0.753=6.247\\\\pka = 6.247

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pH = 6.247 + log [ 0.304/0.404]

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So, the pH of the buffer is 6.1236.

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3 years ago
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