In 1993 the Minnesota Department of Health set a health risk limit for BCME in groundwater of 2.00 ng/L. Suppose an analytical chemist receives a sample of groundwater with a measured volume of 23.0 mL. Calculate the maximum mass in micrograms of BCME which the chemist could measure in this sample and still certify that the groundwater from which it came met Minnesota Department of Health standards. Be sure your answer has the correct number of significant digits. μg x10 x S

In 1993 the Minnesota Department of Health set a health risk limit for BCME in groundwater of 2.00 ng/L. Suppose an analytical chemist receives a sample of groundwater with a measured volume of 23.0 mL. Calculate the maximum mass in micrograms of BCME which the chemist could measure in this sample and still certify that the groundwater from which it came met Minnesota Department of Health standards. Be sure your answer has the correct number of significant digits. μg x10 x S

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter2: Chemical Compounds

Section: Chapter Questions

Problem 105QRT

See similar textbooks

Similar questions

1.87 A solution of ethanol in water has a volume of 54.2 mL and a mass of 49.6 g. what information would you need to look up and how would you determine the percentage of ethanol in this solution?
3.37 If atypical grain of sand occupies a volume of 1.3 × 10-4 cm3, what is the volume (in cm3) of 1 mole of sand (ignoring the space between grains)? What is the volume in liters?
Potassium sulfate has a solubility of 15 g/ 100 g water at 40C. A solution is prepared by adding 39.0 g of potassium sulfate to 225 g of water, carefully heating the solution, and cooling it to 40C. A homogeneous solution is obtained. Is this solution saturated, unsaturated, or supersaturated? The beaker is shaken, and precipitation occurs. How many grams of potassium sulfate would you expect to crystallize out?
3. What volume of 0.250 M KMnO4(aq) contains 0.500 g KMnO4? 0.791 Ml 2.00 mL 127 mL 125 mL
On October 21, 1982, the Bureau of the Mint changed the composition of pennies (see Exercise 120). Instead of an alloy of 95% Cu and 5% Zn by mass, a core of 99.2% Zn and 0.8% Cu with a thin shell of copper was adopted. The overall composition of the new penny was 97.6% Zn and 2.4% Cu by mass. Does this account for the difference in mass among die pennies in Exercise 120? Assume the volume of the individual metals that make up each penny can be added together to give the overall volume of the penny, and assume each penny is the same size. (Density of Cu = 8.96 g/cm3; density of Zn = 7.14 g/cm3).
Suppose that you are closing a cabin in the north woods for the winter and you do not want the water in the toilet tank to freeze. You know that the temperature might get as low as 30. C, and you want to protect about 4.0 L water in the toilet tank from freezing. Calculate the volume of ethylene glycol (density = 1.113 g/mL; molar mass = 62.1 g/mol) you should add to the 4.0 L water.
3.83 For the reaction of nitrogen, N2, and hydrogen, H2, to form ammonia, NH3, a student is attempting to draw a particulate diagram, as shown below. Did the student draw a correct representation of the reaction? If not, what was the error the student made?
A chemist prepares a solution of potassium dichromate (K, Cr,0,) by measuring out 63.7 umol of potassium dichromate into a 450. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in umol/L of the chemist's potassium dichromate solution. Be sure your answer has the correct number of significant digits. H mol L
A chemist prepares a solution of iron(II) bromide (FeBr,) by measuring out 223. umol of iron(II) bromide into a 200. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in umol/L of the chemist's iron(II) bromide solution. Be sure your answer has the correct number of significant digits. H mol L
A chemist must dilute 88.2mL of 6.18mM aqueous copper(II) fluoride CuF2 solution until the concentration falls to 5.00mM. 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.
mol L A chemist must prepare 850. mL of 2.00 M aqueous silver nitrate (AgNO3) working solution. He'll do this by pouring out some 4.47 aqueous silver nitrate stock solution into a graduated cylinder and diluting it with distilled water. Calculate the volume in mL of the silver nitrate stock solution that the chemist should pour out. Be sure your answer has the correct number of significant digits.
A chemist prepares a solution of silver(1) perchlorate (AgC104) by measuring out 817. μmol of silver(1) perchlorate into a 450. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mol/L of the chemist's silver(I) perchlorate solution. Round your answer to 3 significant digits. mol L 0 x10 X