Achemist must dilute of aqueous barium chloride 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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Q) A chemist must dilute 17.8 mL of 961. mM aqueous barium chloride BaCl 2 solution until the concentration falls to 267. mM . 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.

V2 = 64.0666 mL

Explanation

Let us first write down the data

The Initial condition of Bacl2 solution is:-

M1 = 961 mM

V1 = 17.8 mL

The chemist wants to dilute the solution to reach the concentration of 267 mM hence the final conditions will be:-

M2 = 267 mM

V2 = ?

here we are going to use the simple formula to calculate V2,

M1 * V1 = M2 * V2

V2 = (M1 * V1) /M2

V2 = (961*17.8)/267

V2 = 64.0666 mL

120,630,890

step-by-step explanation:

110+10=120,620+10=630,880+10=890