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A 0.250 g sample of a magnesium-aluminum alloy dissolves completely in an excess of HCl (aq). When the liberated hydrogen gas is collected over water at 29 degrees celsius and 752 torr, the volume is found to be 343 mL. The vapor pressure of water at 29 degrees celsius is 30.0 torr. What is the mass percentage of aluminum in this alloy?
What is the pH of a buffer that results when 0.50 mole of Na3PO4 is mixed with 0.75 mole of HCl and diluted with water to 1.00 L? The acid dissociation constants for phosphoric acid
if 0.100 m NaCl is added slowly to a beaker containing both .120m AgNO3 and .150m Pb(NO3)2 at 25 celsius which will precipitate first AgCl or PbCl2?
The cereal sample without adding complexing agent was used as blank when measuring cereal sample. Why cannot we use DI water?
What phase or phases are present when 250. kJ of energy is removed from this sample? Specific heat capacities:
A Solution is made by dissolving 8.5 grams of NaOH in 2.3 L of water. What is the molarity of the solution?
Calculate the molar mass of a gas if 4.40 g occupies 3.50 L at 560 torr and 41°C.
If 69.5 kJ of heat is applied to a 1040. g block of metal, the temperature of the metal increases by 11.4°C. Calculate the specific heat capacity of the metal in J/g°C.
What mass of NaOH is needed to precipitate the Cd2+ ions from 44.0 mL of 0.500 M Cd(NO3)2 solution?
When heating the acetone in a water bath, why must there be a hole in the foil cap
How much potassium nitrate has to dissolve in water to absorb 110 of heat?
One way to isolate metals from their ores is to react the metal oxide with carbon as shown in the following reaction: 2MO(s) + C(s) → 2M(s) + CO2(g)
We add excess Na2CrO4 solution to 16.0 mL of a solution of silver nitrate (AgNO3) to form insoluble solid Ag2CrO4. When it has been dried and weighed, the mass of Ag2CrO4 is found to be 0.380 grams.
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