A chemist must dilute 58.2 mL of 4.65 M aqueous iron(II) bromide (FeBr₂) solution until the concentration falls to 1.00 M. She'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. OL X

Suppose 0.324 g of copper(II) acetate is dissolved in 100. mL of a 0.20 M aqueous solution of sodium chromate. Calculate the final molarity of copper(II) cation in the solution. You can assume the volume of the solution doesn't change when the copper(II) acetate is dissolved in it. Be sure your answer has the correct number of significant digits. Ом x10 X 3

A solution containing 405.6 mM CaCl₂ is combined with an equal volume of 176.1 mM NaCl. What is the concentration of chloride (CI) ions in the resulting solution? Express your answer using units of millimolar (mM) using at least three significant figures.

A chemist must prepare 800. mL of 69.0 µM aqueous mercury(II) iodide (HgI,) working solution. He'll do this by pouring out some 0.000101 M aqueous mercury(II) iodide stock solution into a graduated cylinder and diluting it with distilled water. Calculate the volume in mL of the mercury(II) iodide stock solution that the chemist should pour out. Round your answer to 3 significant digits.

Calculate the volume in liters of a  ×9.9010−5 M copper(II) fluoride solution that contains  425.μmol  of copper(II) fluoride  CuF2 . Be sure your answer has the correct number of significant digits.

An aqueous solution at 25 °C has a H₂O concentration of 6.2 × 10¯M. Calculate the OH concentration. Be sure your answer has the correct number of significant digits. -7 1.61 × 10 M x10 X Ś

Suppose 4.20 g of iron(II) chloride is dissolved in 300. mL of a 75.0 m M aqueous solution of silver nitrate. Calculate the final molarity of chloride anion in the solution. You can assume the volume of the solution doesn't change when the iron (II) chloride is dissolved in it. Be sure your answer has the correct number of significant digits. M x10

A chemist must prepare 300. mL of 1667. µM aqueous copper(II) fluoride (CuF₂) working solution. She'll do this by pouring out some 0.00374 M aqueous copper(II) fluoride stock solution into a graduated cylinder and diluting it with distilled water. Calculate the volume in mL of the copper(II) fluoride stock solution that the chemist should pour out. Be sure your answer has the correct number of significant digits.

Deionized water is added to 138.0 mL sample of 1.103 M oxalic acid to dilute it to 0.436M. What volume of water, in milliliters, was added to dilute the sample? Enter your answer in the box, rounded to the correct number of significant figures. 

You are a researcher working in a famous molecular biology lab. You will be doing a very important experiment tomorrow and need to get ready by preparing several solutions. One of the solutions you will need to make is a stock solution of 3M magnesium chloride. Since you will need to use this solution many times, you decide to make 350 mL of this solution. You take out your container of magnesium chloride solid and take it to the balance. How many grams would you weigh to make 300 ml of this 3M stock solution? Atomic weight of Mg = 24.31 Atomic weight of Cl = 35.45 Write your answer with two digits past the decimal point.  (Important - Trailing zeroes count as digits - (e.g. 12.00 counts as two digits past the decimal point). The answer is ___________________________ grams 85.5 g is not the correct answer