2. The hydrogen sulfide in a 50.0 g sample of crude petroleum was removed by distillation and collected in a solution of CdCl2. The precipitated CdS was then filtered, washed, and ignited to CdSO4. Calculate the percentage of H₂S in the sample if 0.1080 g of CdSO4 was recovered.

0.753-g sample of a chlorocarbon compound was analyzed by burning it in oxygen and collecting the evolved gases in a solution of NaOH.  After neutralizing, the sample was treated with 25.74 mL of a 0.264 M AgNO3 solution.  This precipitated the chloride (Cl-) out as AgCl and left an excess of AgNO3.  The excess AgNO3 was titrated with 0.1 M KSCN and required 16.47 mL to reach the endpoint in a Volhard titration. Calculate the % w/w Cl– (35.45 g/mol) in the sample.  Provide your answer to 2 places after the decimal point and without units. Reactions: Cl– + Ag+  →  AgCl(s)                             Reaction 1                   Ag+ + SCN–  →   AgSCN(s)                    Reaction 2 HINT: This is an example of a back-titration.  Steps to success: First, calculate the TOTAL amount (in moles) of Ag+ added from the volume and molarity of the silver nitrate solution. Second, determine the EXCESS amount of Ag+ from the reaction with thiocyanate (Reaction 2 above).  Third, calculate the…

6. In an experiment, the molecular formula for calcium hydroxide was determined to be Ca(OH)2. In this experiment, 0.050 g of Ca (s) was added to 150. mL of DI water. After adding 10 drops of 0.1% thymol blue indicator, the solution was titrated with 0.30 M HCl. a. Write the balanced equation for the net ionic reaction that occurred during the titration. b. Calculate the volume of 0.30 M HCl required to reach the end point of the titration. C. If the initial reading of HCl in the burette was 25.60 mL, what was the final reading of HCl in the burette at the end point of the titration?

Write the balanced equation for the reaction of aqueous Pb(ClO3)2Pb(ClO3)2 with aqueous NaI.NaI. Include phases. chemical equation:   What mass of precipitate will form if 1.50 L1.50 L of highly concentrated Pb(ClO3)2Pb(ClO3)2 is mixed with 0.500 L 0.300 M NaI0.500 L 0.300 M NaI? Assume the reaction goes to completion.

100.0 mL of 0.60 M aqueous Pb(NO3)2 is mixed with excess aqueous KI. What mass of precipitate is formed?

A 150.0 mL solution of 3.011 M strontium nitrate is mixed with 210.0 mL of a 3.176 M sodium fluoride solution. Calculate the mass of the resulting strontium fluoride precipitate. mass: Assuming complete precipitation, calculate the final concentration of each ion. Ksp values can be found in the table of solubility product constants. [Na] = [NO₂] = [SP²+] = [F] = M M M M

In a titration lab determining the salt content of potato chips, silver nitrate, potassium chromate, and calcium carbonate were used. Explain the purpose of each chemical.

100.0 cm3 of a 1.234 mol.dm-3 solution of nickel(II) nitrate was added to 150.0 cm3 of a 1.178 mol.dm-3 solution of sodium carbonate.   Calculate the concentration of nitrate ions in the solution at the completion of the reaction.

A 12.63 g sample of calcium ore was dissolved in HCl and gravimetrically analyzed, through the precipitation of calcium into CaC2O4 · H2O. The precipitate was filtered, washed, dried, and ignited at 500 oC until the weight was constant, giving a final mass of 2.35 grams pure CaCO3 (100.087 g/mol). Calculate the % Calcium (40.078 g/mol) in the sample.

1. A 0.4126-g sample of primary-standard Na2CO3 was treated with 40.00 mL of dilute perchloric acid. The solution was boiled to remove CO2, following which the excess HClO4 was back-titrated with 9.20 mL of dilute NaOH. In a separate experiment, it was established that 26.93 mL of the HClO4 neutralized the NaOH in a 25.00-mL portion. Calculate the molarities of the HClO4 and NaOH.     2. A 0.5002-g sample that assayed 96.4% Na2SO4 required 48.63 mL of a barium chloride solution. Reaction: Ba2+ + SO42+ → Ba SO4 (s) Calculate the analytical molar concentration of BaCl2 in the solution.     3. A solution was prepared by dissolving 367 mg of K3Fe(CN)6 (329.2 g/mol) in sufficient water to give 750.0 mL. Calculate: (a) the molar analytical concentration of K3Fe(CN)6. (b) the molar concentration of K+.     Using step-by-step process