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A titration experiment is set up to use .235M bleach (NaOCl) to analyze CrO2^-. If 50mL of the CrO2^-(aq) solution required 28.62mL of bleach to react to completion, what would you calculate as the molarity of the CrO2- solution? Balance the redox rxn first (it is in basic medium).
ClO-(aq) + CrO2^-(aq) --> Cl^-(aq) + CrO4^2-(aq)
Sample has a mass of 0.171 g at a pressure of 761 mm Hg and a temperature of 32oC. What is the molar mass of the gas? R=0.0821 L atm / mol K
How many grams of NaCl must be added to 250g water to lower the vapor pressure by 1.30 mm Hg at 40 degrees C assuming complete dissociation?
A mixture of gases with a pressure of 800.0 mm hg contains 60% nitrogne and 40% oxygen by volume. what is the partial pressure of oxygen in this mixture?
The average pH of precipitation in rural areas is 5.80. Assuming that the pH is controlled by the carbonate system, i.e., no anthropogenic acid gases are present in the atmosphere.
A solution contains 25 mmol of H3PO4 and 10. mmol of NaH2PO4. What volume of 2.0 M NaOH must be added to reach the second equivalence point of the titration of the H3PO4 with NaOH?
Calculate the masses of (a) KNO3 and, separately, (b) Ba(NO3)2 to add to a 0.110 mol kg^-1 solution of KNO3(aq) containing 500 g of solvent to raise its ionic strength
Concentrated hydrochloric acid is 38% HCl by weight and has a density of 1.19 g/mL. A solution is prepared by measuring 25 mL of the concentrated HCl,
What is the concentration of CH3NH2 added to the solution?
What is the pressure (in atm) exerted by a 2.00 mole sample of gas that occupies 2.50 L at 307.15K? The value of R = 0.0821 L atm mol - 1 K - 1 .
A solution is made by mixing equal masses of methanol, CH4O, and ethanol, C2H6O. Determine the mole fraction of each component to at least three significant figures.
A student collected hydrogen in a eudiometer as described above. Barometric pressure is 765.5 Torr, the vapor pressure of water is 22.0 Torr at this temperature and the solution remaining in the eudiometer is 5.75 cm above the water in the beaker
Reaction of 2.042g zinc with 2.005g iodine produces 2.510g zinc iodide, leaving 1.518g of unreacted zinc. According to these data, is the law of mass conservation verified within 1% error?
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