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natulia [17]
3 years ago
12

Calculate the percentage of CL in AL(CLO3)3​

Chemistry
1 answer:
Anna35 [415]3 years ago
5 0

Answer:

38.4%

Explanation:

We'll begin by calculating the molar mass of Al(ClO₃)₃. This can be obtained as follow:

Molar mass of Al(ClO₃)₃

= 27 + 3[35.5 + (16×3)]

= 27 + 3[35.5 + 48]

= 27 + 3[83.5]

= 27 + 250.5

= 277.5 g/mol

Next, we shall determine the mass of Cl in Al(ClO₃)₃. This can be obtained as follow:

Mass of Cl in Al(ClO₃)₃ = 3 × Cl

= 3 × 35.5

= 106.5 g

Finally, we shall determine the percentage of Cl in Al(ClO₃)₃. This can be obtained as follow:

Mass of Cl in Al(ClO₃)₃ = 106.5 g

Mass of Al(ClO₃)₃ = 277.5 g

Percentage of Cl =?

Percentage of Cl = mass of Cl / mass of Al(ClO₃)₃ × 100

Percentage of Cl = 106.5 / 277.5 × 100

Percentage of Cl = 38.4%

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The freezing point of a solution containing 5. 0 grams of KCl and 550.0 grams of water is  - 0.45°C

Using the equation,

ΔT_{f} = iK_{f}m

where:

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i = Van't Hoff factor

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Molality is expressed as the number of moles of the solute per kilogram of the solvent.

Molal concentration is as follows;

MM KCl = 74.55 g/mol

molal concentration = \frac{5.0g*\frac{1mol}{74.55g} }{550.0g*\frac{1kg}{1000g} }

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Now, putting in the values to the equtaion ΔT_{f} = iK_{f}m we get,

ΔT_{f} = 2 × 1.86 × 0.1219

ΔT_{f} = 0.4536°C

So, ΔT_{f} of solution is,

ΔT_{f_{solution} } = 0.00°C - 0.45°C

ΔT_{f_{solution} } =  - 0.45°C

Therefore,freezing point of a solution containing 5. 0 grams of KCl and 550.0 grams of water is  - 0.45°C

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