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Calcium chloride is used to melt ice and snow on roads and sidewalks and to remove water from organic liquids. Calculate the molarity of a solution prepared by diluting 165 mL of 0.688 M calcium chloride to 925.0 mL.a. 3.86 M b. 0.743 M c. 0.222 M d. 0.123 M e. 0.114 M
what adjustment should be made to the mobile phase to bring the compound off sooner? why?
How many grams of precipitate will form from 100mL solution that is both 0.90 M in Na2S and 0.20 M in PbCl2?
Calculate the concentrations of NH4+ and NH3 and the pH in a solution prepared by mixing 22.0g of NaOH and 0.500L of 1.5 M NH4Cl. Assume that the volume remains constant.
A compound contains 69.94 percent iron and 30.06 percent oxygen. What is its molecular formula if the molar mass of the compound is 199.55 grams per mole?
A solution of a protein contains 0.382 grams of the material in 1.00 L of solution. At a temperature of 25°C,this solution has an osmotic pressure of 1.07 torr. Calculate the molar mass of the protein.
How many milliliters of 0.200 M NaOH would be neutralized by the HCl produced after 60 minutes? After 90 minutes? After 120 minutes?
A 25.0 g sample of pure iron at 91°C is dropped into 57 g of water at 15°C. What is the final temperature of the water-iron mixture?
Any help on how to do or start this problem? Suppose the gas above the soda in a bottle of a soft drink is pure CO2 at a pressure of 2 atm. a. Estimate the pH of the soda. b. Calculate CT, the total dissolved inorganic carbon.
2.00 moles of a gas occupies 62.2 L at a particular temperature and pressure. Its density is 0.900 g/L. The standard molar volume is 22.4 L/mole. What is the molar mass.
Why are fluorescence measurements made at 90 degrees from the incident beam in most cases? 3. What is the ideal cuvette placement to avoid pre- and post-filter effects?
A sample of copper was pretreated and diluted to 500mL and portions of this solution were analyzed by measuring the absorbance of a copper (I) complex of 1, 20 phenanthroline using a standard addition technique.
An unknown noble gas effuses through a tiny hole into an evacuated space with a rate that is 0.578 times the rate of N2(g): rateunk/raten2=0.578. calculate the molar mass of the noble gas in g/mol using Gtaham's law of effusion (N=14.0)
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