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A student placed 15.5 g of glucose (C6H12O6) in a volumetric flask, added enough water to dissolve the glucose by swirling, then carefully added additional water until the 100. mL mark on the neck of the flask was reached. The flask was then shaken until the solution was uniform. A 35.0 mL sample of this glucose solution was diluted to 0.500 L. How many grams of glucose are in 100. mL of the final solution?

1 Answer

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Answer: The mass of glucose in final solution is 1.085 grams

Step-by-step explanation:

To calculate the molarity of solution, we use the equation:


\text{Molarity of the solution}=\frac{\text{Mass of solute}* 1000}{\text{Molar mass of solute}* \text{Volume of solution (in mL)}} ......(1)

Given mass of glucose = 15.5 g

Molar mass of glucose = 180.2 g/mol

Volume of solution = 100 mL

Putting values in equation 1, we get:


\text{Molarity of glucose solution}=(15.5* 1000)/(180.2* 100)\\\\\text{Molarity of glucose solution}=0.860M

To calculate the molarity of the diluted solution, we use the equation:


M_1V_1=M_2V_2

where,


M_1\text{ and }V_1 are the molarity and volume of the concentrated glucose solution


M_2\text{ and }V_2 are the molarity and volume of diluted glucose solution

We are given:


M_1=0.860M\\V_1=35.0mL\\M_2=?M\\V_2=0.500L=500mL

Putting values in above equation, we get:


0.860* 35.0=M_2* 500\\\\M_2=(0.860* 35.0)/(500)=0.0602M

Now, calculating the mass of glucose by using equation 1, we get:

Molarity of glucose solution = 0.0602 M

Molar mass of glucose = 180.2 g/mol

Volume of solution = 100 mL

Putting values in equation 1, we get:


0.0602=\frac{\text{Mass of glucose solution}* 1000}{180.2* 100}\\\\\text{Mass of glucose solution}=(0.0602* 180.2* 100)/(1000)=1.085g

Hence, the mass of glucose in final solution is 1.085 grams

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