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tia_tia [17]
3 years ago
8

A chemist mixes 96.2 g of chloroform with 31.2 g of acetone and 98.1 g of acetyl bromide. Calculate the percent by mass of each

component of this solution Be sure each of your answer entries has the correct number of significant digits. acetyl bromide
Chemistry
1 answer:
stiv31 [10]3 years ago
5 0

Answer:

42.6 % CHCl₃, 13.83 % C₃H₆O and 43.5 % CH₃COBr

Explanation:

This is a solution with 3 compounds:

96.2 g of CHCl₃

31.2 g of C₃H₆O

98.1 g of CH₃COBr

Total mass of solution is : 96.2g + 31.2 g + 98.1g = 225.5 g

Percent by mass is, the mass of the compounds in 100 g of solution

Let's prepare the rule of three

225.5 g of solution have ____ 96.2 g ___ 31.2 g _____98.1 g

100 g of solution would have ____

(100 . 96.2) / 225.5 = 42.6

(100 . 31.2) / 225.5 = 13.83

(100 . 98.1) / 225.5 =  43.5

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lubasha [3.4K]

The pH of the solution is 2.54.

Explanation:

pH is the measure of acidity of the solution and Ka is the dissociation constant. Dissociation constant is the measure of concentration of hydrogen ion donated to the solution.

The solution of C₆H₂O₆ will get dissociated as C₆HO₆ and H+ ions. So the molar concentration of 0.1 M is present at the initial stage. Lets consider that the concentration of hydrogen ion released as x and the same amount of the base ion will also be released.

So the dissociation constant Kₐ can be written as the ratio of concentration of products to the concentration of reactants. As the concentration of reactants is given as 0.1 M and the concentration of products is considered as x for both hydrogen and base ion. Then the

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8 * 10^{-5} =\frac{x^{2}  }{0.1}\\\\\\x^{2} = 8 * 10^{-5}*0.1

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So the pH of the solution is 2.54.

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