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You need to make a solution of Ca(NO3)2 for a class demonstration. First, you measure a quantity of the solid Ca(NO3)2 by weighing the reagent container before obtaining the sample (4.2540 ± 0.0003 g) and after taking some reagent (3.9440 ± 0.0003 g). You were about to transfer the Ca(NO3)2 into a 100- ml volumetric flask, but notice that you forgot to wash it the previous week and there is something green growing in it. So rather than cleaning the volumetric flask, you instead decide to just use a beaker and fill it to a final volume of 0.100 ± 0.005 L. The molar mass of Ca(NO3)2 is 164.10 g/mol, and its uncertainty is negligible (i.e. treat it as a constant).
a. Calculate the concentration of nitrate ions in the resulting solution (don't forget about the stoichiometry), and determine the uncertainty in that value. What is the primary contribution to the uncertainty?
b. A typical 100-ml volumetric flask has an uncertainty of ± 0.12 ml. If you had made the above solution in a volumetric flask instead of the beaker, what would have been the resulting concentration and uncertainty?
This solution was back-titrated with a 0.0440 M Ga3 solution until all the EDTA reacted, requiring 14.0 mL of the Ga3 solution. What was the original concentration of the V3 solution?
Consider a binary liquid mixture A and B, where A is volatile and B is nonvolatile. The composition of the solution in terms of mole fraction is xA = 0.045 and xB = 0.955
Thomas Jefferson Snodgrass found an unlabelled reagent bottle in his -80 C freezer. The Bottle contained a liquid. He found that the compound( compound 1) quickly evaporated when warmed to room temperature. H-NMR of the compound showed only two pe..
The standard free energy of activation of a reaction A is 76.9 kJ mol-1 (18.4 kcal mol-1) at 298 K. Reaction B is one hundred million times faster than reaction A at the same temperature
Using data from thermodynamic quantities at 298.15K, calculate deltaG^degree for the following reactions. Indicate if each reaction is spontaneous at 298K under standard conditions.
At a given temperature, the equilibrium constant K for the reaction 2SO2(g) + O2(g) 2SO3(g) is 3.0 × 109. If 2.80 mol of SO2 and 4.06 mol of O2 are placed in a 1.78-L container.
Calculate the pH of the solution at the half equivalence point. Explain how the pH at the half equivalence point is related to Ka for the weak acid.
Unlike translational degrees of freedom, the rotational partition function must be evaluated by summation, unless the high-temperature limit is obtained. What is the definition of the high-temperature limit for rotations?
Calculate the number of moles of Ascobic acid in the 50.00 ml Sample. Titration Volumes of KIO3 Initial Buret reading/ml trial 1=12.54 trial 2=8.78 Final buret reading/ trial 1=38.74 trial 2=34.93 Volume of KIO used/ml trial 1=? trial 2=?
A titration of 200.0 mL of 1.00 M H2A was done with 1.10 M NaOH. For the diprotic acid H2A, Ka1 = 2.5 × 10-5, Ka2 = 3.1 × 10-9. Calculate the pH after 600.0 mL of 1.10 M NaOH have been added.
What is the height of the column that contains a solution of Sucrose (C12H22O11) with 21% weight percentage of Sucrose?
an electron is confined to a linear region with a length of the same orderas the diameter of an atom (about 100 pm)
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