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A solution of vinegar is 4.68% by mass acetic acid in water. Assuming the density of vinegar is 1.00 g/mL , what is the molarity of the acetic acid.
Calculate the volume of this flask. empty weighed 56.12g , and full of ammonia weighed 87.39g . density of liquid ammonia is 0.625g/l . calculate flask volume in L
The atomic mass of copper is 63.55 amu. Given thatb there are two naturally occuring isotopes of copper, 63Cu and 65Cu, the natural abundance of the 65Cu isotope must be approximately
Which of the following would break apart into free radicals (an atom with one unpaired electron) when a photon promotes one electron to an antibonding orbital. I. B2 II. C2 III. N2 IV. O2 V. F2
When atoms of the hypothetical element X are placed together, they rapidly undergo reaction to form the X2 molecule: Would you predict that this reaction is exothermic or endothermic. Explain.
Write the balance equation and predict the moles of ammonia that can be made using usng 22.4g of nitrogen and an unlimited amount of hydrogen
Which of the following hormones requires selenium for its synthesis?
Draw the most stable form of the major mixed Claisen product formed in the reaction.
whick species is reduced. How many grams of oxygen gas are required to completely react with 77.28g of ethane (C2H6)
Two compounds have the same empirical formula. One substance is a gas, the other is a viscous liquid. How is it possible for two substances with the same empirical formula to have markedly different properties?
An aqueous solution contains 4.90% NH3 (ammonia) by mass. The density of the aqueous ammonia is 0.979 g/mL. What is the molarity of NH3 in the solution?
Air is 21 mole percent oxygen, that is, 0.21 atm oxygen at 1 atm. Suppose the pH of the water is 5.28 and that the concentration of iron(II) in the water is 5.38x 10-5 M, what is the potential of the corrosion reaction under the above conditions a..
An industrial waste from a metals industry contains approximately 5*10^-3 M H2SO4. Before being discharged into the stream, the water is diluted with tap water in order to raise the pH.
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