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A current of 0.500 A flows through a cell containing Fe2+ for 10.0 min. Calculate the maximum number of moles of Fe that can be removed from solution. Assume the current is constant over time.

Calculate pBa2+ when 25.00 mL of 0.200 0 M EDTA is added to 50.00 mL of 0.100 0 M Ba2+ in the presence of 0.100 M nitrilotriacetate.  = 1.48 × 10−4.  = 0.30 at pH 10. Kf = 7.59 × 107 for BaY2−.

A 15.3-g sample of an organic compound is completely combusted in air, producing 21.0 g CO2 and 8.61 g H2O. What is the weight percent of C in the organic compound? (answer to 1 decimal place)

Calculate the pH of a 0.340 M NaO2CCO2H solution. pK1 = 1.250 and pK2 = 4.266 for HO2CCO2H.

Which of the following statement(s) is/are TRUE regarding the properties of the limiting reagent in a chemical reaction?

A(n) ______________ is a compound with a physical property that changes abruptly near the equivalence point.

Which is NOT an end point detection method used with EDTA titrations?

A current of 3.56 A is passed through an Fe(NO3)2 (FM 179.855) solution for 1.60 h. How many grams of Fe(s) (FM 55.845) will be deposited? (report to 2 decimal places)

Calculate pMn2+ when 50.00 mL of 0.100 0 M Mn2+ is titrated with 17.00 mL of 0.200 0 M EDTA. The titration is buffered to pH 11, for which  = 0.81. Kf = 7.76 × 1013 for MnY2−.

The Cl− concentration of a solution was determined by coulometric titration. Ag+ generated at the anode reacts with the Cl− in solution, forming the precipitate AgCl(s). The end point is determined when an increase in current is detected due to excess Ag+ in solution. A current of 0.500 A was applied for 17.55 min through a 25.00-mL solution containing an unknown Cl− concentration. Calculate the Cl− concentration. (Report to 4 decimal places)