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The arsenic in a 1.223 g sample of a pesticide was converted to H3AsO4 by suitable treatment. The acid was then neutralized, and 40.00 ml of 0.07891 M AgNO3 was added to precipitate the arsenic quantitatively as Ag3AsO4. The excess Ag+ in the filtrate and washings from the precipitate was titrated with 11.27 ml of 0.1000 M KSCN; the reaction is: Ag+ + SCN- => AgSCN(s) Calculate the percent As2O3 in the sample. (F.W. As2O3 = 197.84 g/mol)
the structure they gave me already has two nonbonding electrons on Bromine with no formal charge
Explain briefly why CuSO4 is more soluble in water than in organic (nonpolar) solvent.
Use Charles's law to calculate the volume the gas will occupy if the temperature is increased to 170.5^circ C while the pressure is held constant.
If a solution of sodium chloride contains 5.2 NaCl in 900 grams of water. What is the concentration of the solution in parts per million?
If 0.80g of gas occupies 295 mL at 25 degrees celsius and 680 mm Hg of pressure, what is the molar mass of the gas?
The reactant concentration in a zero-order reaction was 7.00×10-2 after 105 and 1.50×10-2 after 350 . What is the rate constant for this reaction.
The correct name for FeO is iron(II) oxide is it a poyatomic or binary ion? What is the rule for naming FeO?
How much of the solution is needed?
What is the fate of acetyl CoA in the mitochondria in the presence of the following? (a) high ADP levels? (b) high NADH/NAD+ ratio? (c) low levels of oxaloacetate
How much energy (heat) is released when 1.9 moles of H2 reacts with 0.7 moles of Cl2 to create HCl(g) if the ΔHrxn = -184.6 kJ.
Calculate the mass percent of a NaCl solution in which 110 g of NaCl is dissolved in 2.41 L of water at 25 0C (density = 0.997 rm g/mL).
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.
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