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Mr. Chemikaze, the stockroom coordinator at Big Chem Co., found an un-labeled bottle that needs to be properly disposed. The liquid in the bottle is clear and colorless, and must be identified before it can be sent to the disposal center. He is fairly certain that the bottle contains an aqueous barium chloride solution. Since it is cheaper to dispose of solids than liquids, Mr. Chemikaze decides to precipitate the two ions separately, as this will help him confirm his initial assumptions.
a. Describe a set of chemical reactions or laboratory procedures that would allow him to confirm that the cation was indeed barium.
b. Describe why barium must be disposed of properly. What are the health effects of excess barium in drinking water? What is the maximum allowable concentration of barium in public water systems?
c. Why aren't we as concerned with the chloride?
A graduated cylinder contains 148 mL of water. A 11.0 g piece of iron (density = 7.86 {g/cm^3}) and a 19.0 g piece of lead are added. What is the new water level in the cylinder? Density of the lead is 11.3g/ml
Name a compound with the formula, C5H12, which will show only one peak in the NMR spectrum.
A buffer is made by mixing HCN and KCN to give a solution whose pH is 9.49. If the KCN molarity is 0.20 M, what is the molarity of the HCN?
Calculate the partial pressure of each gas and the total pressure after the valve between the flasks is opened. P(He) in mmHg P(Ar) in mm Hg Ptotal in mm Hg
A gas sample in a piston assembly expands, doing 588 kJ of work on its surroundings at the same time that 372 kJ heat is added to the gas.
Assuming complete dissociation of the solute, how many grams of KNO3 must be added to 275 mL of water to produce a solution that freezes at -14.5 C?
How many moles of each are present in the eq mixture b)Calculate the equilibrium constant
Calculate the heat required to convert 50.0 g of C2CL3F3 from a liquid at 20.00 degrees celcius to a gas at 75.00 degrees celcius.
calculate the heat released when 176g of water at 23.0 degrees celsius are converted to ice at -10.0 degrees celsius?
Write net ionic equations for the reactions that take place when aqueous solutions of the following substances are mixed.
After the reaction comes to equilibrium, an additional 1.00g of O2(g) is added to the system. What is the expected partial pressure of SO2(g) then?
Suppose 50 mL of 0.020 M Hydhrochloric acid solution was mixed to 50 mL of 0.20 M acetic acid solution (Ka of acetic acid, CH3COOH, = 1.8 x 10-5). Determine the approximate pH of the mixture.
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