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An aqueous stock solution is 28.0% NH3 by mass and its density is 0.9 g/mL. What volume of this solution is required to make 1.50 L of 2.75 mol/L NH3(aq)? Give your answer in millilitres, accurate to three significant figures.
Cyanogen is a gas which contains 46.2 % C and 53.8 % N by mass. At a temperature of 25oC and a pressure of 750 mmHg, 1.50 g of cyanogen occupies 0.714 L.
What is the equation for the reaction of cyclohexene wtih MnO4- to form 1,2-cyclohexanediol and MnO2 in a basic medium.
what hybrid orbitals are used about the central atom of each of the angles.
Calculate the following to determine Kc for FeSCN2+. a,) moles Fe3+ initially present. b.) moles SCN- initially present
Determine the molar mass of aspartame and How many moles of molecules are in 10.0g of aspartame?
Calculate the average formal charge on an oxygen atom in the structure of the phosphate ion that minimizes formal charges, such as demonstrated in Part A.
Mercaptoacetic acid and NH3 were introduced, production of the complex with the former resulted in the release of an equivalent amount of EDTA, which required a 22.85-mL titration with 0.07238 M Mg2+. Calculate the percent Cu and Ni in the alloy.
A student who suspected he had a carbonyl compound for an unknown dissolved his solid unknown compound in acetone and the solution was analyzed by IR
Combustion of a 0.1000 g sample of a compound containing only carbon, hydrogen, and oxygen in excess yields 0.1953 g CO2, and 0.1000 g H2O. A separate experiment shows that the molar mass is 90 Daltons. Calculate the mass percent composition.
How many milliliters of 0.100 M NaOH(aq) would be needed to completely neutralize 50.0 milliliters of 0.300 M HCl(aq)
For restriction digestion, how would you dilute the 10X buffer so that it was at the correct concentration (1X) in the reaction solution
If a solution containing 30.87 g of mercury(II) chlorate is allowed to react completely with a solution containing 5.102 g of sodium sulfide,
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