A chemist adds of a M aluminum sulfate solution to a reaction flask. Calculate the millimoles of aluminum sulfate the chemist has added to the flask. Be sure your answer has the correct number of significant digits.

Answer: The question is incomplete without values, but here is a similar questions that has values; A chemist adds 85.0mL of a 0.125 mol/L aluminum sulfate (Al2 (S04) solution to a reaction flask. Calculate the millimoles of aluminum sulfate the chemist has added to the flask. Be sure your answer has the correct number of significant digits mmol.

Number of moles = 10.625millimoles or 1.06 x 10 millimoles.

Step-by-step explanation:

From number of moles = concentration (mol/L) x volume (L)

Concentration = 0.125mol/L, Volume = 85.0mL (Convert to L) = 85/1000 = 0.085L

Substitute in the equation = 0.125mol/L x 0.085L = 0.010625moles

But 1mole is equivalent to 1000millimoles

convert the 0.010625moles to millimoles = 0.010625moles x 1000millimoles/1mole

Number of moles = 10.625millimoles or 1.06 x 10 millimoles.