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

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Question:

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

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The question is incomplete, complete question is :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 =[tex]M_1= 400 mM[/tex]Volume of sodium carbonate solution before dilution = [tex]V_1=73.9 mL[/tex]Concentration of sodium carbonate solution after dilution =[tex]M_2= 125 mM[/tex]Volume of sodium carbonate solution after dilution = [tex]V_2=?[/tex]Dilution equation is given by:[tex]M_1V_1=M_2V_2[/tex][tex]V_2=\frac{M_1V_1}{M_2}[/tex][tex]V_2=\frac{400 mM\times 73.9 mL}{125 mM}= 236.48 mL\approx 236 mL[/tex]1 mL = 0.001 L236 mL = 0.236 LThe final volume of the solution will be 0.236 L.

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