A chemist adds 55.0 mL of a 4.75M silver perchlorate (AgCIO,) solution to a reaction flask. Calculate the mass in grams of silver perchlorate the chemist has added to the flask. Round your answer to 3 significant digits. の

Suppose 4.47 g of barium acetate is dissolved in 350. mL of a 69.0 m M aqueous solution of ammonium sulfate. Calculate the final molarity of barium cation in the solution, You can assume the volume of the solution doesn't change when the barium acetate is dissolved in it. Round your answer to 3 significant digits. | M

A chemist adds 280.0 mL of a 1.32M iron(III) bromide (FeBr,) solution to a reaction flask. Calculate the millimoles of iron(III) bromide the chemist has added to the flask. Round your answer to 3 significant digits. mmol x10

Suppose 2.72 g of potassium bromide is dissolved in 200. mL of a 0.20 M aqueous solution of silver nitrate. Calculate the final molarity of bromide anion in the solution. You can assume the volume of the solution doesn't change when the potassium bromide is dissolved in it. Round your answer to 3 significant digits. ?

A chemist must dilute 99.9 mL of 161. mM aqueous silver perchlorate (AgClio,) solution until the concentration falls to 117. 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. Round your answer to 3 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. 

A chemist adds 435.0 mL of a 0.0630 mmol/L potassium permanganate (KMnO4) solution to a reaction flask. Calculate the mass in milligrams of potassium permanganate the chemist has added to the flask. Round your answer to 3 significant digits.

A chemistry student must write down in her lab notebook the concentration of a solution of sodium thiosulfate. The concentration of a solution equals the mass of what's dissolved divided by the total volume of the solution. Here's how the student prepared the solution: • The label on the graduated cylinder says: empty weight: 5.0 g She put some solid sodium thiosulfate into the graduated cylinder and weighed it. With the sodium thiosulfate added, the cylinder weighed 61.167 g. • She added water to the graduated cylinder and dissolved the sodium thiosulfate completely. Then she read the total volume of the solution from the markings on the graduated cylinder. The total volume of the solution was 10.64 mL. What concentration should the student write down in her lab notebook? Be sure your answer has the correct number of significant digits. - 1 g•mL х10

Suppose 1.70 g of sodium chloride is dissolved in 50. mL of a 0.50 Maqueous solution of silver nitrate. Calculate the final molarity of sodium cation in the solution, You can assume the volume of the solution doesn't change when the sodium chloride is dissolved in it. Round your answer to 2 significant digits. do

a. A 250.0-mL solution of sodium hydroxide was prepared by dissolving pure NaOH(s) in deionized water. It required 21.37 mL of 0.1127 M sulfuric acid to completely neutralize 39.29 mL of this sodium hydroxide solution. Calculate the mass, in units of g, of NaOH(s) that was dissolved to make the 250.0-mL solution. Enter your answer in decimal notation using 3 significant figures; i.e., enter 0.03478 as 0.0348   b. In an experiment, 23.24 mL of 0.235 mM silver nitrate are mixed with 9.12 Ml of 0.205 mM sodium phosphate. Assuming 100% yield, what is the concentration, in units of μM, of phosphate in the solution. Assume that the volume of the solid formed is negligible. Enter your answer in decimal notation using 3 significant figures; i.e. enter 2.579 as 2.58.