Chapter 1, Problem 1.99E

You have 59.95 grams of a compound in 89.35 mL solution. (Hint: write as a fraction of grams per mL) How much is this in moles per liter?28.59 grams = 1 moleRound answer to 2 decimal places.

If 0.276 grams of acetic acid (MM = 60.05 g/mol) are present in your 2.00 mL sample of vinegar, what is the mass/volume percentage of acetic acid in the sample of vinegar?

A chemist adds 1.75 L of a 2.80 × 10 - 5 mol/L mercury(II) iodide (HgI,) solution to a reaction flask. Calculate the micromoles of mercury(II) iodide the chemist has added to the flask. Be sure your answer has the correct number of significant digits. и mol x10

A chemist prepares a solution of mercury(II) iodide (Hgl,) by measuring out 0.0051 µmol of mercury(II) iodide into a 100. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mol/L of the chemist's mercury(II) iodide solution. Be sure your answer has the correct number of significant digits. mol dlo L

Suppose 0.377 g of potassium chloride is dissolved in 100. mL of a 37.0 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 potassium chloride is dissolved in it. Be sure your answer has the correct number of significant digits. M D x10 X S

The mass of acetic acid in a 2.00mL sample of vinegar (density of the vinegar is 0.999g/mL) is determined to be 0.19g. What is the mass % of acetic acid in the vinegar

An aqueous solution of sodium chloride,NaCl , is made by dissolving 1.01 grams of sodium chloride in sufficient water in a 50.0 mL volumetric flask, and then adding enough water to fill the flask to the mark. What is the weight/volume percentage of sodium chloride in the solution? Weight/volume percentage =           %

-1 A geochemist measures the concentration of salt dissolved in Lake Parsons and finds a concentration of 9.0 g·L The geochemist also measures the concentration of salt in several nearby non-isolated lakes, and finds an average concentration of 5.3 g·L *. Assuming the salt concentration in Lake Parsons before it became isolated was equal to the average salt concentration in nearby non-isolated lakes, calculate the percentage of Lake Parsons which has evaporated since it became isolated. Be sure your answer has the correct number of significant digits. x10

A chemist adds 310.0 mL of a 0.045 mmol/L sodium thiosulfate (Na₂S₂03) solution to a reaction flask. Calculate the mass in milligrams of sodium thiosulfate the chemist has added to the flask. Round your answer to 2 significant digits. mg x10 X