A chemist must dilute 73.9 mL of 400 mM aqueous sodium carbonate solution until the concentration falls to 125 mM . He'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in liters. Be sure your answer has the correct number of significant digits.

Answer:

The final volume of the solution will be 0.236 L.

Explanation:

Concentration of sodium carbonate solution before dilution = $M_1= 400 mM$

Volume of sodium carbonate solution before dilution = $V_1=73.9 mL$

Concentration of sodium carbonate solution after dilution = $M_2= 125 mM$

Volume of sodium carbonate solution after dilution = $V_2=?$

Dilution equation is given by:

$M_1V_1=M_2V_2$

$V_2=\frac{M_1V_1}{M_2}$

$V_2=\frac{400 mM\times 73.9 mL}{125 mM}= 236.48 mL\approx 236 mL$

1 mL = 0.001 L

236 mL = 0.236 L

The final volume of the solution will be 0.236 L.

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3 years ago

Gaseous vapor observed when handling dry ice (solid co_2 2 ) physical or chemical

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<span>Dry ice is frozen carbon dioxide. It is easy to assume that the fog surrounds dry ice is carbon dioxide returning to it's gaseous however, you can not see that process. The vapors you see is the water molecules in the air condensing as a result of the cooling or energy removal by the dry ice. When energy is removed from water molecules they become colder and move slower than water in a gaseous. Similar to clouds in the air, the water condenses into a form that you can see.</span>

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3 years ago