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ad-work [718]
3 years ago
13

What is the total volume of solution that was dispensed from this burette? before after

Chemistry
2 answers:
Lemur [1.5K]3 years ago
8 0

Answer : The correct option is, (C) 0.6 ml

Explanation : Given,

Initial volume of solution in the burette = 32.3 ml

Final volume of solution in the burette = 32.9 ml

As the liquid is colorless. So, we are taking the lower meniscus for the correct reading of the solution.

Now we have to calculate the total volume of solution that was dispensed from this burette.

\text{Total volume of solution dispensed}=\text{Final volume of solution in the burette}-\text{Initial volume of solution in the burette}

Now put all the values in this formula, we get the total volume of solution that was dispensed from this burette.

\text{Total volume of solution dispensed}=32.9ml-32.3ml=0.6ml

Therefore, the the total volume of solution that dispensed from this burette was, 0.6 ml

monitta3 years ago
6 0
Yeah answer should be .6 ml
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Answer:

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b)  Percentage by mass of chlorine: 80.37%

c) Molecular formula: C_{2} H Cl_{3}

Explanation:

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Assuming that we have 100g of the compound, it is possible to determine the number of moles of each element in the compound:

18.3g C*\frac{1mol C}{12g C} = 1.52mol C

0.77g H*\frac{1mol H}{1g H} = 0.77mol H

80.37gCl*\frac{1molCl}{35.45g Cl} = 2.27mol Cl

Dividing each of the quantities above by the smallest (0.77mol), the  subscripts in a tentative formula would be

C=\frac{1.52}{0.77} = 1.97 ≈ 2

H = \frac{0.77}{0.77} = 1

Cl =\frac{2.27}{0.77}=2.94≈3

The empirical formula for the compound is:

C_{2} H Cl_{3}

The mass of this empirical formula is:

mass of C + mass of H + mass of Cl= 24g +1+ 106.35 =131.35g

This mass matches with the molar mass, which means that the supscript in the molecular formula are the same of the empirical one.

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