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Using the Extended DH Equation, we calculate the activity coefficient, ?, of an ion in solution as, -log ? = [ 0.253 ± 0.008]/ [ 3.50 ± 0.03]. What is the error in ? if the principal uncertainties are in the ionic size and the ionic strength. The errors above are ? values
How many equivalents of electrons were delivered to the unknown soln. What is the normality of the unknown solution
A student has prepared a 0.309 M solution of Barium hydroxide and a 0.443M solution of hydrochloric acid for you. Determine the volume of the hydrochloric acid solution will be needed to exactly neutralize 10.0 mL of the Barium chloride solution.
Determine the mass of snow that can be completely melted - Determine the mass of snow (frozen water) that can be completely melted with the application
Aspirin that has been stored for a long time may give a vinegar odor and give a purple color with FeCl3, what reaction would cause this to happen
If 29.1 mL of 0.4 M NaOH is used to reach the endpoint when titrating 20.1 mL of acetic acid, what is the concentration of the acetic acid in moles/L
Calculate H per mole of CaCl2 (in kJ) for the reaction under the above conditions. Aside, the ?H per mole for dilution depends on the process.
Tell what type of chemical reaction is represented by the following chemical equation.
Suppose that each of the following pairs of compounds are being used as reactants in this experiment. Draw structures of the intermediate imines formed,
a bomb clorimeter contains 2.5 liters of water if the combustion of .175 moles causes the temperature of the water to rise 45 degrees celsius, what is the molar heat of combustion.
Copper dissolved in nitric acid, producing copper (II) nitrate. After reaction with sodium hydroxide and heating, copper nitrate changed to coper (II) oxide. Calculate the percent yield of this process if 1.075 g of copper produced 1.075 g of copp..
Calculate the pH of the solution after the addition of 100mL of 1.00 M HCL. the Ka for Hf is 3.5*10-4
A mixture of Ar and N2 gases has a density of 1.592 g/L at STP. What is the mole fraction of each gas?
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