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A solution is prepared by dissolving 11.60g of a mixture of sodium carbonate and sodium bicarbonate in 1.00 L of water. A 300.0-cm^3 sample of the solution is then treated with excess HNO3 and boiled to remove all the dissolved gas. A total of 0.955 L of dry CO2 is collected at 298 K and 0.972 atm.
Find the molarity of the carbonate in the solution.
Find the molarity of the bicarbonate in the solution.
One mole of an ideal gas is expanded from a volume of 1.00 liter to a volume of 4.90 liters against a constant external pressure of 1.00 atm. How much work (in joules) is performed on the surroundings?
Assume complete combustion occurs. Determine the dew point temperature of the flue gas.
Differentiate between alkenes and alkynes, cis isomers and trans isomers. Describe how cis- trans isomers
The goal of the recrystallization procedure is to obtain purified material with a maximum recovery. For each of the following situations, explain why this goal would be adversely affected.
A solution of ethanol (C2H5OH) in water is prepared by dissolving 67.5 mL of ethanol (density = 0.79 g/cm3) in enough water to make 250.0 mL of solution. What is the molarity of the ethanol in this solution?
An underground reservoir contains natural gas at a pressure of 425 kPa and a temperature of 15 °C. If the volume of the reservoir is 1.3 x 104 kL
At a certain temperature, the pH of a neutral solution is 7.72. What is the value of Kw at that temperature
Explain for which of the following species resonance is an important property: HONO, HONO2, N3-, NO2-, NO2.
The critical constants of ethane are Pc= 48.20 atm, Vc= 148 cm3mol-1, and Tc= 305.4 K. Calculate the van der Waals parameters of the gas and estimate the radius of the molecules.
What mass of silver was in the original solution? (Assume that all of the silver was precipitated out of solution by the reaction.)
what mass of Na2SO4 is needed to prepare 350. ml of a solution having a sodium ion concentration of 0.125 M.
Cassify these compounds by whether they behave as strong acids, weak acids, strong bases, or weak bases in aqueous solution.
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