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Alex73 [517]
1 year ago
12

A solution is 0. 0480 m lif. What is the molarity of the solution if the density is 1. 10 g/ml?.

Chemistry
1 answer:
makkiz [27]1 year ago
3 0

Molarity of the solution is 0.0527 M.

<h3>What is Molarity?</h3>

The amount of a substance in a specific volume of solution is known as its molarity (M). The number of moles of a solute per liter of a solution is known as molarity. The molar concentration of a solution is another name for molarity.

<h3>Calculation of Molarity of the solution</h3>

Assume there is 1 kg of solvent present in the beginning.

Thus, the mole of solute is 0.0480 moles of LiF.

Molar mass of LiF = 25.939 grams/mole

0.0480 mol LiF x 25.939 g/1 mol LiF = 1.245 g LiF

Mass of the solution = 1001.245 g

The molarity of the solution can be determined as illustrated using the supplied density and moles of solute.

[LiF] = mol LiF/ volume of solution

[LiF] = 0.0480 mol/1001.245 g x 1ml/1.10g x 1L/1000mL

Hence, the molarity of LiF = 0.0527 M

Learn more about Molarity here:

brainly.com/question/10851381

#SPJ4

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Where

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What quantity of energy, in joules, is required to raise the temperature of 425 g of tin from room temperature, 25.0 °C, to its
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Answer:

Total energy required to raise the temperature of 425 g of tin from 298.15 K to 505.05 K and to melt the tin at 505.05 K is 45.249 kiloJoules.

Explanation:

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Initial temperature of the tin ,T_1= 25.0 °C = 298.15 K

Final temperature of the tin, T_2= 231.9 °C = 505.05 K

Let the heat required to change the temperature of tin from 298.15 K to 505.05 K be Q.

Q=mc\times (T_2-T_1)

=425 g\times 0.227 J/g K\times (505.05K - 298.15 K)=19,960.68 J=19.961 kJ

Heat required to melt tin at 505.05 K be Q'

The heat of fusion of tin metal =\Delta H_{fus}=59.2 J/g

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= Q+Q' =  19.961 kJ + 25.288 kJ = 45.249 kJ

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