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Successive dilution problem. A 10-mL transfer pipet and a 200-mL volumetric flask are used to make 0.100 M and 0.0050 M solutions from a stock solution of 2.000 +/_ 0.005 M. Calculate the percent relative error for the three solutions if perfect technique is used. Report the two new molarities. (The error in a 10-mL transfer pipet is 0.02, and the error in the 200-mL volumetric flask is 0.1)
What is the recommended daily allowance (RDA) of calcium, in mg, assuming a 2000 calorie diet for a 25 year old adult? A student carries out part 1 of this experiment and finds the equation for his/her calibration curve to be
You have 500 mL of a 5.0 M solution of nitric acid HNO3 (63.01 g /?mol) dissolved in water. How many grams of nitrogen does the solution contain.
A certain element consists of two stable isotopes. The first has atomic mass of 7.02 amu and a percent natural abundance of 92.6%.
If 2 volumes of 0.1 M monobasic potassium phosphate, KH2PO4, are mixed with 1 volume of 0.1 M dibasic sodium phosphate, Na2HPO4, what will be the pH of the mixture?
Further studies will refine how much water is needed for endangered species protection. States hope it will be the 130-150 KAF initially agreed upon rather than the 415 KAF the FWS thinks it is. What happen if cooperative agreement fails?
Write a balanced chemical equation for the reaction of chlorine with thiosulfate ion, assuming an acidic solution.
how many grams of zinc must react with sulfuric acid in order to obtain 500mL of hydrogen at 20 deg c and 770 mm hg?
What is the volume in mL of 0.833 M HCl(aq) needed to reach halfway to the equivalence (stoichiometric) point in the titration of 23.5 mL of 0.270 M ethylamine
the solubility reaction of interest in this solution? (b) Is a precipitate expected in the solution (Yes, No, or Not Enough Information to Know)?
the freezing point of the resulting solution is 3.77*C. The freezing point of pure benzine is 5.48*C. Calculate the molar mass of the compound.
Determine E° for the reduction half-reaction Ce4+(aq) + e- → Ce3+(aq), given that the cell voltage for the following voltaic cell is E°cell = 1.887 V:
How many liters of N2 (at STP) form when 1.0 kg of N2H4 react with 1.0 kg of O2?
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