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Ainat [17]
3 years ago
6

A chemistry teacher adds 50.0 mL of 1.50 M H2SO4 solution to 200 mL of water. What is the concentration of the final solution? U

se .
Chemistry
2 answers:
umka2103 [35]3 years ago
7 0

Answer:

option A

Explanation:

just took test on e2020

Aleks [24]3 years ago
6 0
Hello!

The concentration of the final solution when a<span> chemistry teacher adds 50.0 mL of 1.50 M H2SO4 solution to 200 mL of water is 0,3 M

To calculate that, you'll need to use the dilution law, where initial and final concentrations are M1 and M2 respectively, and initial and final volumes are V1 and V2, as shown below. Keep in mind that the final volume is the sum of the 200 mL of water and the 50 mL of H</span>₂SO₄ that were added by the teacher. 

M2= \frac{M1*V1}{V2}= \frac{1,50 (mol H_2SO_4/L)*50mL}{(50 mL + 200 mL)}=0,3(mol H_2SO_4/L)

Have a nice day!
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The question is incomplete, here is the complete question:

A solution contains 0.115 mol  H_2O and an unknown number of moles of sodium chloride. The vapor pressure of the solution at  30°C  is 25.7 torr. The vapor pressure of pure water at this temperature is 31.8 torr. Calculate the number of grams of sodium chloride in the solution. (Hint: Remember that sodium chloride is a strong electrolyte.)

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0.0122mol=\frac{\text{Mass of NaCl}}{58.5g/mol}\\\\\text{Mass of NaCl}(0.0122mol\times 58.5g/mol)=0.714g

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