6. The purity of a sample of sodium oxalate, Na2C2O4, is determined by titrating with a standard solution of KMnO4. If a 0.5116-g sample requires 35.62 mL of 0.0400 M KMNO4 to reach the titration's end point, what is the %w/w Na2C2O4 in the sample.

4. The concentration of a NaOH solution is determine by using the solution to titrate a sample of potassium hydrogen phthalate (C8H5O4K, M = 204.22 g/mol). In the titration 34.67 mL of NaOH solution is required to react with 0.1082 g C8H5O4K to reach the equivalence point. a) Calculate the concentration of the sodium hydroxide solution. Potassium hydrogen Phthalate = 0-10829, Molar mass of KMP=204-22 Hales of KMP = Mass 0.10829 g/mol Mm 6.000529 mal 204229/Mal Concentration of NaOH = Males = = of volume of Naot (L) = 0-000529 mal 34-67 mе onl ها NaOH (mal) = 0.000015258 mal/L 0.015M b) This solution of sodium hydroxide is used for another titration. A sample of 10.0 mL of HCI is neutralized using 22.1 mL of sodium hydroxide solution. Calculate the concentration of the HCI solution. sodium hydroxide 222.1 ml, Nal100

1.

B. A solution was prepared by dissolving 5.76 g of KCI .MgCl2. 6H2O (277.761 g/mol) in sufficient water to give 2 L. Calculate i) ii) The molar analytical concentration of KCI.MgCl26H2O in this solution. The molar concentration of Mg²+ The molar concentration of Cl iii)

Initial Cu2+ Concentrations of 0.16 M, 0.080 M, 0.040 M, and 0.016 M. 1.00 mL of each solution is in a beaker After the addition of 4.00 mL of 0.5 M NH3 and 3.00 mL of distilled water, based on the dilutions calculate the concentration of Cu2+ in each of the respective beakers

Solid potassium sulfite is slowly added to 75.0 mL of a 0.0373 M barium nitrate solution. The concentration of sulfite ion required to just initiate precipitation is M.

If 30.0 g of LiOH is added to 0.650 L of 1.00 M Cd(NO₃)₂, how many grams of precipitate will be formed in the following precipitation reaction?    a) Write a balanced equation. Identify a precipitate. Include states of matter.  b) Determine how much precipitate would form if all reactant 1 ( LiOH) would be used up.  c) Determine how much precipitate would form if all reactant 2 ( Cd(NO3 )2 would be used up.  d) State Limiting reactant , and theoretical yield ( in grams) of the precipitate that would form from the given amounts.

Sodium oxalate, Na2C2O4Na2C2O4, in solution is oxidized to CO2(g)CO2(g) by MnO−4MnO4− which is reduced to Mn2+Mn2+. A 50.3 −mL−mL volume of a solution of MnO−4MnO4− is required to titrate a 0.342 −g−g sample of sodium oxalate. This solution of MnO−4MnO4− is then used to analyze uranium-containing samples. A 4.60 −g−g sample of a uranium-containing material requires 33.0 mLmL of the solution for titration. The oxidation of the uranium can be represented by the change UO2+→UO2+2UO2+→UO22+.     Part A Calculate the percentage of uranium in the sample.

A solid sample containing some Fe2+ion had a total mass of .9791 g. It required 18.2 ml of 0.02304 M KMnO4 to titrate the Fe2+ in the dissolved sample to a pink endpoint.  How many moles of  Fe2+ were in the the sample? How many grams of irion were present in the sample and what was the mass percent iron in the sample?

A 2.45 g mixture of BaCl2 and Ba(NO3)2 is dissolved in water.  Excess AgNO3 is added and all of the dissolved chloride ion is precipitated. The resulting precipitate weighs 0.845 g.  Use the following Molar Masses (in g mol−−1) as required: Ba: 137.3 Cl:  35.45 Ag: 107.9 N: 14.01 O: 16.00   What is the mass of Ba(NO3)2 in the original mixture?  Enter a mass accurate to three significant figures.  g