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A 8.76 g sample of impure CsF was dissolved in 100 mL of water. The sample was mixed with excess aqueous calcium nitrate solution to precipitate insoluble calcium flouride. The precipitate was filtered, dried, and weighed. A total of 1.55 g calcium flouride was collected. What was the percentage of CsF in the original sample.
Buffers are important physiological compounds that resist a change in pH. Calculate the pH of system that is 0.25 M benzoic acid and 0.75 M benzoate if the pKa = 4.2.
A gas mixture composed of helium and argon has a density of 0.853g/L at a 745mmHg and 298K .What is the composition of the mixture by volume?
Calculate the pH of a solution prepared by dissolving .370 mol (HCO2H) and .230 mol (NaCO2H) in H2O sufficent to yeild 1.00L of solution. Ka=1.77x10^-4
Zn + 2HCl → ZnCl2 + H2 If 0.600 gram of zinc is used, what is the amount of zinc chloride that is produced in the above reaction?
there is no measurable difference between final and initial pH - that is why it is called a buffer E. final pH is 0.16 pH units lower than original pH
Identify each of the following unbalanced aqueous reactions as an acid/base reaction (a), a redox reaction (r) or a precipitation reaction (p).
0.375 kg of water are in a well insulated container at 21.3 c. After 4.184kj of heat are added to the water, what is the final water temperature ?
Calculate the length in km of a row containing 1 mole of hydrogen atoms laid side to side if diameter of a hydrogen atom =.212 nm?
A sample containing 0.0250 M concentration of a dye in a cell of 1 cm^2 cross section has a measured absorbance of 1.012 at 650 nm.
Express the concentration of a 0.0460 M aqueous solution of fluoride, F-, in mass percentage and in parts per million. Assume the density of the solution is 1.00g/mL.
what is the equation for gypsum when it is heated below 220 degrees celsius and also when it is heated to red heat?
A reaction 3A2+ + 2B --> 3A + 2B3+ is used to make a battery. The standard Gibbs free energy change for the given reaction is -690 kJ. What is the standard potential (E ) for the battery.
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