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classify each of the following acids as strong or weak. If the acid is weak, write an expression for the acid ionization constant (Ka).
a.) HF
b.) HCHO2
c.) H2SO4
d.) H2CO3
Explain why the rates of diffusion of nitrogen gas and carbon monoxide are almost identical at the same temperature.
A quantity of HI was sealed in a tube, heated to 425C, and held at this temperature until equilibrium is reached. The concentration of HI in the tube at equilibrium was found to be 0.0706 moles/liter
A 0.1000 m aqueous solution of a weak acid, HA, is 1.5% ionized. At what temperature does it freeze? Kf for water = 1.86°C/m.
A gas sample containing 1.47 mol at 25°C exerts a pressure of 401 torr. Some gas is added to the same container, and the temperature is increased to 50.°C. If the pressure increases to 800. torr,
Calculate the osmotic pressure of a solution containing 18.55 of hemoglobin in 13.7 of solution at 24. The molar mass of hemoglobin is .
Determine the pressure in a 14.6 L cylinder filled with 0.440mol of N2 gas at a temperature of 327K.
What is the partial pressure of each substance if the total pressure of the mixture is 2.35 atm?
The equilibrium constant for the reaction, 2HI = H2 + I2 is 0.49. Calculate the number of moles of hydrogen produced when one mole of HI
53.5 g of an ideal gas of molecular weight = 30.5 g/mol are confined at a pressure of 133 mmHg. The density of the gas is 0.228 g/L. Compute the temperature of the gas in degrees Celsius.
Assuming the solution has a heat capacity of 4.18 J/°C · g and assuming no heat loss to the calorimeter, calculate the enthalpy change for the dissolution of NH4NO3 in units of kJ/mol.
Compute the vapor pressure at the temperature of 25 degree Celsius of H 2 O above a solution formed by mixing 100.
A standard oxalic acid solution is 0.065 M. It was prepared by dissolving H2C2O4*2H2O in distilled water.
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