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Antimony has two stable isotopes, 121^Sb and 123^Sb. The 121^Sb isotope has a natural abundance of 57.21% and an atomic mass of 120.90382 amu. Calculate the percent abundance and atomic mass of the 123^Sb isoyope.
Provide structures consistent with the following molecular formulae and spectral data, and assign spectral peaks. Write your structures and tables on a sheet of paper.
Calculate the molarity of a solution made by adding 44.4 mL of concentrated ammonia (28% by mass, density 0.880 g/mL) to some water to some water in a volumetric flask
The atomic radius of O is smaller than the atomic radius of Se. What is the effective nuclear charge for the valence electron(s) in O and Se
Blending of two wines with different concentrations of acid, Two wines are available for blending: One tank of 1000 L has a Titratable Acidity of 9.0 g/L and another tank containing 2000 L has a Titratable Acidity of 0.6 g/L.
Which statement best desrcibes the energy change as bonds are formed and broken in this reaction ?
What is the ratio of the conjugate base concentration to the acid concentration, that is, [B-]/[HB] when the indicator switches to the acidic color?
If a 100.0 g sample of water at 60.0 degreesC is added to a 100.0 g sample of water at 10.0 degrees C, determine the final temperature of the water.
A test solution contained 2 mL of 0.10 M Ag+. A silver strip was dipped into the test solution, and a cell potential of 0.0592 V was measured against an Ag/Ag+(1.0M) reference half-cell.
One molecular form of elemental sulfur is a ring of eight sulfur is a ring of eight sulfur atoms. As one molecule of this element is burned to make sulfur trioxide, how many oxygen molecules are used?
Calculate the hydronium ion concentration and the pH when 25.0 mL of 0.50 M NH3 is mixed with 65.0 mL of 0.19 M HCl.
what is a detailed mechanism for the formation of dibenzalacetone? This reaction is beginning with acetone and benzaldehyde and is treated with NaOH and then forms dibenzalacetone.
A compound is constituted by mass of 52.1% carbon and 13.1% hydrogen, the rest being oxygen. Given that a volume of 5.33 L of this gas has a mass of 11.5 g at 13 °C and 110 kPa, find the molecular formula for this compound.
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