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A solution is initially 0.050M in acetate, CH3COO- (Kb = 5.6 x 10^-10). 10.0mL of 0.10 M HCl is added to 50.0mL of the acetate solution. The Ka for the conjugate weak acid of CH3CHOO- is 1.8 x 10^-5. Calculate the pH for this solution at equilibrium.
calculate the wavelength of the photon emitted when an electron drops from 4d obital to a 2p orbital in a hydrogen atom using Rydberg constant as 1.097 x 10-2 pm-1 .
If 12.5 g of magnesium nitride is treated with water, what volume of ammonia gas would be collected at 28°C and 753 mm Hg?
If 5.36 103 kg each of NH3, O2, and CH4 are reacted, what mass of HCN and of H2O will be produced, assuming 100% yield?
what is the chloride concentration ppt (W/V) of you sample? (include a standard deviation in your result) The standard deviation for the electronic balance used to weigh the AgCl is 0.15 mg.
When the following reaction is balanced in basic solution using the lowest possible whole number coefficients, the coefficient of H2O will be: CN-(aq) + MnO4-(aq) --> CNO-(aq) + MnO2(s)
A thief plans to steal a gold sphere with a radius of 28.8 cm from a museum. If the gold has a density of 19.3 {rm g/cm}^3, what is the mass of the sphere? [The volume of a sphere is V = (4/3)pi r^3.]
Copper (II) sulfate dissolve sin water to form a blue solution. What species are present in the solution, ie, what is actually swimming around in the solution? Write the formulas.
A reaction takes place at a constant pressure of 1.10 atm with an internal energy change of 71.5 kJ and a volume decrease of 13.6 L.
How is concentration an intensive property? I mean if you add more amount of a substance(mass), the number of moles increase and so the concentration increases.
when the base was 0.292 M and the cation was 1.89 M. Calculate the equilibrium dissociation constant (Kb).
What is the pH at the equivalence point? (Kb of NH3 = 1.8 A 20.0 mL sample of 0.20 M sodium acetate is titrated with 0.11 M HCl(aq). What is the pH after the addition of 50.0 mL HCl(aq)?
The gas with an initial volume of 24.0 L at a pressure of 565 mmHg is compressed until the volume is 16.0 L. What is the final pressure of the gas, assuming the temperature does not change?
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