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Helga [31]
2 years ago
8

A student wants to make a 5.00%solution of rubidium chloride using 0.377g of the substance. what mass of water will be needed to

make the solution?
Chemistry
1 answer:
Alenkasestr [34]2 years ago
7 0
 The mass of water that will  be needed to make the solution  is calculated as below

%  solution  =  mass of the solute/mass of the solvent(water) x100

%  solution = 5% = 5/100
mass of the solute =0.377 g
mass of the  solvent = ?

let the mass  of the solvent be  represented by Y

= 5/100 =0.377/y

by cross multiplication

5y=  37.7
divide both side by 5

y =7.54  grams
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Answer:

a) Unsaturated

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Explanation:

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An unsaturated solution contains <u>less solute than it  has the capacity to dissolve. </u>

A supersaturated solution, <u>contains more  solute than is present in a saturated solution</u>. Supersaturated solutions are not very  stable. In time, some of the solute will come out of a supersaturated solution as crystals.

According to these definitions and considering that the solubility of KCl in 100 mL of H₂O at <u>20 °C is 34 g</u>, and at <u>50 °C is 43 g</u> we can label the solutions:

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b) 65 g in 100 mL of H₂O at 50 °C  ⇒ supersaturated

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PV=nRT

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Putting values in above equation, we get:

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To calculate the pressure when temperature and volume has changed, we use the equation given by combined gas law.

The equation follows:

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P_2,V_2\text{ and }T_2 are the final pressure, volume and temperature of the gas

We are given:

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Putting values in above equation, we get:

\frac{755mmHg\times 2.55L}{296K}=\frac{P_2\times 4.10L}{291K}\\\\P_2=\frac{755\times 2.55\times 291}{4.10\times 296}=461.6mmHg

Hence, the number of moles of nitrogen gas are 0.1043 moles and the pressure when volume and temperature has changed is 461.6 mmHg

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