Calculate the ionic strength of a solution that is 0.060 M in FeSO4. Ionic strength =  0.60 M in (NH4)2CrO4. Ionic strength = 0.60 M in FeCl3 and 0.50 M in FeCl2. Ionic strength = 0.060 M in La(NO3)2 and 0.040 M in Fe(NO3)2. Ionic strength =

An equimolar solution of ammonium sulfate, sodium chloride and magnesium nitrate has an ionic strength of 0.14 M. What is the molar concentration of the solution with respect to each solute? O 0.020 M O 0.025 M O 0.10 M O 0.015 M

The solubility-product constant for Ce(IO3)3  is 3.2x10-10 . What is the Ce3+ concentration in a solution prepared by mixing 40.00 mL of 0.0420 M Ce3+ with 40.00 mL of  water?  M  0.0420 M IO3-?  M  0.260 M IO3-?  M  0.0470 M IO3-?  M

A standardized iodine solution is used to titrate hydrazine sulfate in a sodium bicarbonate- buffered solution. The reactions that occur are I2 + 2e- = 2I     N2H4 .H2SO4 → N2 + SO4 2- + 6H+ + 4e- What is the molarity of a solution of hydrazine sulfate when 27.29 mL of 0.100 N iodine is required to titrate 25.00 mL of the hydrazine sulfate to the equivalence point?

1.Calculate the normality of the solutions containing 5.267g/L K2Cr2O7 (the Cr is reduced to Cr3+).(FW=294.19 g/mol) 2.A and B react as follows: A + B 2C. The equilibrium constant is 5.0 x 106. If 0.40 mol of Aand 0.70 mol of B are mixed in 1L, what are the concentrations of A, B and C after reaction? 3. The following data is given at a certain temperature:(1) 2N2 (g) + O2 (g) 2N2O (g) K1 = 1.2 x 10-35(2) N2O4 (g) 2NO2 (g) K2 = 4.6 x 10-3(3) ½N2 (g) + O2 (g) NO2 (g) K3 = 4.1 x 10-9Calculate the molar equilibrium constant, K for the reaction:2N2O (g) + 3O2 (g) 2N2O4 (g)

HBR, O2, CH3OH all have comparable molecular masses. List the dominant type of IMF for the pure substances, then rank the strength of each compound based on IMFs within the samples. (1 = strongest 2= in between 3 = weakest ) Substance IMF Relative Strength HBR     O2     CH3OH

A 0.2585 gram amount of H₂C₂O4 is dissolved in approximately 100 mL of 0.5 M H₂SO4. A KMnO4 solution is added to a burette and added to the H₂C₂O₂ solution. A faint colour persists when 22.35 mL of KMnO solution has been added. slowly Calculate the molarity of the KMnO4 solution. A) 0.2294 M B) 0.02235 C) 0.05139 M 0.02927 M

Parts 6A and 6B

A solution of 0.10 M Sulfate ion is available. What is the normality of this solution when used in the given reaction?

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