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The initial SCN-1 concentration is constant at 0.0010 M in all samples. Yet the stock bottle clearly reads 0.0020 M. Why? Similarly, why is the initial concentration of iron (III) ion 0.10 M when the stock bottle contained 0.20 M iron (III) nitrate?
A certain gaseous oxide of sulfur has an effusion rate that is 0.707 times the effusion rate of oxygen gas. What is the most likely molecular formula of this oxide?
A student adds an excess (more than she needs to react completely) of solid sodium hydrogen carbonate to a beaker containing exactly 675 mL of 0.220M coper(II)nitrate aqueous solution.
An empty graduated cylinder weighs 82.450 g. Whe filled to 50.0 mL with an unknown liquid it weighs 110.810 g. What is the density of the unknown liquid?
The specific rate constant at 293 K is found to be 2.35 x 10^-4 s^-1 and at 303 K the specific rate constant is found to be 9.15 x 10^-4 s^-1. Calculate the frequency factor for the reaction at 303 K.
Calculate the pH of the solution after the addition of 0.100 mL NaOH. The Ka for HC2H3O2 is 1.8x10^-5.
Calculate the molarity of a solution made by dissolving 0.850 grams of Na2SO4 in enough water to form exactly 930 mL of solution.
A 2.00-L flask is filled with propane gas (C3H8) at 1.00 atm and -15.0 degree C. What is the mass of the propane in the flask?
Calculate the molar concentration of uncomplexed Zn2+ in a solution that contains 0.20 mole of Zn(NH3)42+ per liter and 0.0116 M NH3 at equilibrium.
Calculate the number of moles of Br2 that would react with 0.793 moles of AI to form AIBr3?
Which ions were present in the original solution? What are the net ionic equations for each reaction that occured?
If the titration required 23.95 mL of 0.2556 M HCl to reach the endpoint, calculate the equilibrium molar concentration of B4O5(OH)4 2- in the saturated solution.
Suppose that coal of density 1.5 g/cm3 is pure carbon. (It is, in fact, much more com- plicated, but this is a reasonable ?rst ap proximation.)
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