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A 85.2 g sample of compound X4O10 contains 48.0 g of oxygen atoms. what is the molar mass of element x?
How many grams of MgO are produced when 40.0 grams of O2 react completely with Mg
Aqueous solutions of nickel(II) sulfate and mercury(I) nitrate react to give aqueous nickel(II) nitrate and a mercury(I) sulfate precipitate
The compound ZnI4 is best described as anions in a face-centered cubic unit cell with the cations in the tetrahedral holes. What is the density of this compound?
What must be the velocity, in meters per second, of a beam of electrons if they are to display a de Broglie wavelength of 83.7 ?m?
When a sucba diver goes to a dive shop to have her scuba tanks filled with air, the tank is connected to a compressor and filled to about 2100 psia while immersed in a tank of water (so that the compression of air into the tank will be approximate..
The vapor pressure of water at 20.0 °C is 17.5 mm Hg. If the pressure of a gas collected over water was measured to be 453.0 mm Hg. What is the pressure of the pure gas
Bromine can be obtained from the decomposition of calcium bromide by means of electrolysis. If 10.0 g of calcium bromide are dissolved in water
Draw a mechanism to demonstrate how pyridine catalyzes the hydrolysis of acetic anhydride to two molecule of acetic acid. Is this reaction reversible? why or why not? Show all non-bonding electrons on each atom, circle positive charges
Vitamin C (L-ascorbic acid; MW = 176.0 g/mol) is a weak acid (pKa = 4.863). Suppose a 500.0 mg tablet is dissolved in water and titrated with 0.100 M NaOH. How many mL of NaOH are required to reach the equivalence point?
If 29.7 mL of 0.0205 M KOH us required to completely neutralize 25.0 mL of a HC2H30 solution. What is the molarity of the acetic acid solution
the pka of benzoic acid is 4.2 show mathematically that this acid is 50% ionized at ph 4.2? Part B is Use this result to explain why precipitation of benzoic acid is incomplete if the pH of an aqueos solution of benzoate ion is lowered to Ph 7 by ..
Methyl red (Ka = 7.9 x 10^-6 is added to a buffered solution of unknown pH. Spectrophotometric measurements show the ratio of the basic to the acidic form of the indicator to be 2.57 to 1.000. Calculate the pH of the buffer solution.
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