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At room temperature (25.0 degrees Celsius) the Ksp for Copper (II) hydroxide is 2.2x10-20. Determine the molar solubility for Copper (II) hydroxide in (a) a water solution at 25 degrees Celsius, and (b) in a solution having a pH of 8.75 at 25 degrees Celsius.
2.0 moles of a gas was collected in the lab at a temperature of 1.1 degrees C and a pressure of 9.5 atm. What volume will the gas occupy under these conditions.
If the diameter of a sodium atom is 3.14×10-8 , how many sodium atoms would fit along a line exactly 2.00 inch long?
a sample of oxygen that occupies 1.00X 10^6 ml at 575 mm hg is subjected to a pressure of 1.25 atm. what will the final volume of the sample be if the temperature is held constant?
calculate the pH and concentration of all species present assuming that the activity coefficients are equal to 1.0 for all species
A 38.8 L volume of methane gas is heated from 25°C to 72°C at constant pressure. What is the final volume of the gas
Draw the amine from the following: A Hofmann degradation of a primary amine forms an alkene that gives butanal
When equilibrium is established, it is found that the partial pressure of ammonia has increase by 12.4%. Calculate K for the decomposition of NH4HS at 25 degrees C.
You have a 100.0- mL graduated cylinder containing 50.0 mL of water. you drop a 115-g piece of brass into the water. To what height does the water rise in the graduated cylinder.
A certain substance has a heat of vaporization of 69.66 kJ/mol. At what Kelvin temperature will the vapor pressure be 4.50 times higher than
Tablets from a bottle of commercial aspirin gave a negative test with FeCl3. Several months later, tablets from the same bottle gave a positive test with FeCl3. How do you account for this result? Why?
Explain why a determination of the rate law can never prove a proposed reaction mechanism but can sometimes disprove
Aspirin is an organic acid with formula C8H7COOH and molar mass 180.16171 g/mol. A 1.30 g tablet is titrated with 0.1500 M HCl and the endpoint is reached
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