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An unknown gas has been determined to have the empirical formula CH2. At 27°C and 0.966 atm, the gas has a density of 1.65 g/L. What is the molecular formula of this gas
What is the pH of a buffer that consists of 0.20 M NaH2PO4 and 0.40 M Na2HPO4? Ka = 6.2 × 10-8
Calculate the concentrations of all species at equilibrium for the following case.
What mass of NaCl must be dissolved in 65.0 grams of water to lower the freezing point by 7.50 °C? The freezing point depression constant, Kfp, for water is -1.86 °C/m.
How much PV work is done, if 90 grams of ethylene and 120 grams of HCl are allowed to react at atmospheric pressure and the volume change is -71.2 liters?
Compute the mass of Trisodium phosphate required to remove all Ca^2+ ions from 2.50 Litres of the H 2 O sample?
Aerosol cans carry clear warnings against incineration because of the high pressures that can develop upon heating. Suppose a can contains a residual amount of gas at a pressure of 755mm Hg and a temperature of 25 C
A 20.0-mL sample of 0.25 M HNO3 is titrated with 0.15 M Na OH. What is the pH of the solution after 30.0 mL of NaOH have been added to the acid?
If 122 mL of a 1.2 M glucose solution is diluted to 550.0 mL, what is the molarity of the diluted solution?
Determine how would you compare the escape velocity of asteroid Y as compare to the escape velocity of asteroid X?
Suppose that in changing samples, a portion of the water in the calorimeter weere lost. In what way, if any, would this change the heat capacity of the calorimeter?
Calculate the pH at the equivalence point in a titration between 10.00 mL of acetic acid(0.100 mol/L) and sodium hydroxide (0.100 mol/L).
A buffer is made by dissolving H3PO4 and NaH2PO4 in water. Write and equation that shows how this buffer neutralizes added bases.
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