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a 1.00 L buffer solution is 0.250 m in HF and 0.250 m in NaF. 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
It requires 251 J to melt 2.22 g of sodium metal at its normal melting point of 98°C. Calculate the molar heat of fusion of sodium.
Calculate the Gibbs energy of the reaction (delta G rxn) at 25'C for the above rxn when all three gases are at 0.0010 atm. Kp = 1.8 x 10 ^ - 18
Low concentration replicate samples of Cd-EDTA gave the following counts in a mass spectral measurement: 178.3, 131.2, 144.3, 159.3, 128.3, 197.7, 149.3, 153.9, 143.3, 160.9. Ten measurements of a blank had a mean of 27.7 counts
estimate the enthalpy change for the combustion of hydrogen gas in the presence of oxygen gas.
Calculate the final temperature that results when a 13.0 -g sample of water at 23.1C absorbs 870 J of heat.
A calorimeter containing 200.0 mL of water was calibrated by carrying out a reaction which released 15.6 kJ of heat. If the temperature rose 3.25 degrees celcius then the heat capacity of the calorimeter inclusing the water is?
A copper wire (density = 8.96 g/cm3) has a diameter of 0.41 mm. If a sample of this copper wire has a mass of 12 g, how long is the wire?
Suppose the pH of the water is 3.88 and that the concentration of iron(II) in the water is 2.30x 10-5 M, what is the potential of the corrosion reaction under the above conditions at 298 K?
Help me understand specifically why the dissociated phosphate ion would prefer to bond with cations like Al and Zn. I think I know why but help me better understand.
20.00mL of radiator liquid, ethylene glycol has a mass of 20.85 g. What is the density of the liquid?
At equilibrium, it is found that .25 moles of COCl2 remain. What is the equilibrium concentration of CO?
The mass of the tablet was 0.162 g. What percent of calcium carbonate was in the tablet?
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