A solution is prepared by weighing 7.345g of (NH4)2Ce(NO3)6 (548.2 g/mol) and then dissolving it in water to a final volume of 900.0 ml.
a) the concentration of the cerium solution is ________
b) the correction for the indicator is a) subtract 0.05 ml b) add 0.05 ml c) none
c) 12.00 ml of iron (ii) solution is titrated with this cerium solution, and it requires 19.55 ml. the concentration of the Fe(ii) is __________M.
A solution is prepared by weighing 7.345g of (NH4)2Ce(NO3)6 (548.2 g/mol) and then dissolving it in...
Question 2 0/1 pts A solution was prepared by dissolving 8.03 g of (NH4)2SO4 (MW = 132.14 g/mol; specific volume = .565 ml/g) in 35.0 ml of water. The final volume of the solution is __ml. Question 3 0/2 pts A solution was prepared by dissolving 8.03 g of (NH4)2SO4 (MW = 132.14 g/mol; specific volume = .565 ml/g) in 35.0 ml of water. The concentration of (NH4)2SO4 in the solution is ___%(w/v).
A solution is prepared by dissolving 0.300 g Fe(NH4)2(SO4)2*6H2O in sufficient water to produce 250.0 mL of solution. a. What is the molar concentration of Fe2+? b. What is the molar concentration of NH4+? c. What is the concentration of sulfur in mg/L?
What is the pH of a solution that is prepared by dissolving 2.49 g of pyridine (79.10 g/mol) in 100 mL of 0.0550 M HCl and diluting to 900.0 mL?
What is the concentration of NO3-ions in a solution prepared by dissolving 20.0 g of Ca(NO3)2 in enough water to produce 300 mL of solution? 0.406 M 0.537 M 0.813 M. O 0.203 M
A solution is prepared by dissolving 200.0 g of iron (III) chloride (162.2 g/mol) in 200.0 mL of water. What is the molarity of the solution?
3. a) A standard ZnCl2 solution is prepared by dissolving 0.6483 g of Zn in an HCl solution and diluting to volume in a 1.00 L volumetric flask. An EDTA solution is standardized by titrating a 15.00 mL aliquot of the ZnCl2 solution, which requires 16.12 mL of EDTA solution to reach the end point. Determine the concentration of the EDTA solution. (2 pts) b) A 1.5146 g sample of powdered milk is dissolved and the solution titrated with...
14. If a solution is made by dissolving 14.5 g of Fe(NO3)3 in 455 ml of water, what is the mass percent of iron and nitrate in this solution? Assume 1.00 g/ml density of the water. 4 pts
14. If a solution is made by dissolving 14.5 g of Fe(NO3)3 in 455 ml of water, what is the mass percent of iron and nitrate in this solution? Assume 1.00 g/ml density of the water. 4 pts
A solution of iron (II) sulfate was prepared by dissolving 10.00g of FeSO4-7H20 (FW= 277.9) in water and diluting up to a total volume of 250 ml. The solution was left to stand, exposed to air, and some of the iron (II) ions became oxidized to Iron (III) ions. a 25.0 ml sample of this partially oxidized solution required 23.70 ml of 0.0100M potassium dichromate K2Cr2O7 solution for complete reaction in the presence of dilute sulfuric acid. Calculate the percentage...
A solution of F− is prepared by dissolving 0.0744±0.0005 g NaF (molar mass = 41.989±0.001 g/mol) in 157.00±0.07 mL of water. Calculate the concentration of F− in solution and its absolute uncertainty.