An aqueous ethylene glycol (HOCH₂CH₂OH, FW = 62.07 g/mol) solution with a mass of 214.3 mg is titrated with 61.9 mL of 0.0867 M Ce in 4 M HCIO. The solution is held at 60 °C for 15 min to oxidize the ethylene glycol to formic acid (HCO,H) and carbon dioxide. The excess Cet is titrated with 10.57 mL of 0.0479 M Fe²+ to a ferroin end point. What is the mass percent of ethylene glycol in the unknown solution?

A permanganate solution is prepared by dissolving 20.0123 g KMNO4 in 500 mL of distilled water and boiled for 1 hour to remove any organic material. Following sintered-glass filtration, the solution is quantitatively transferred to a 1.0 L volumetric flask and diluted to volume with distilled water. The permanganate solution was titrated against 0.1023 M oxalic acid prepared in sulfuric acid solution. A 50.00 mL aliquot of oxalic acid solution required 16.68 mL of permanganate solution. A titration blank required 0.04 mL of permanganate. What is the permanganate molarity? 5 H2C204 + 2 MnO4 + 6H* s 10 CO2 + 2 Mn²* + 8 H2O

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

4. A certain barium halide exists as the hydrated salt BaX2.2H2O, where X is the halogen. The barium content of the salt can be determined by gravimetric methods. A sample of the halide (0.2650 g) was dissolved in water (200 cm3) and excess sulfuric acid added. The mixture was then heated and held at boiling for 45 minutes. The precipitate (barium sulfate) was filtered off, washed and dried. Mass of precipitate obtained = 0.2533 § Determine the identity of X. 3 g.

A student weights out 1.118g of impure KHP, dissolves the sample in deionized water and titrate it with 0.1001 M NaOH solution. If the titration requires 27.10 mL of the NaOH solution, and none of the impurities react with NaOH, what is the percent KHP in the sample?

The calcium (40.078 g/mol) in a 500.0 mL sample of natural water was determined by precipitating the cation as CaC2O4. The precipitate was filtered, washed, and ignited in a crucible with an empty mass of 32.3555 g. The mass of the crucible plus CaO (56.077 g/moI) was 33.1471 g. A. Calculate the concentration of Ca in water in units of grams per 100 mL of the water. B. What is the molarity of Ca in the water sample?

A 59.0 mLmL sample of a 0.122 MM potassium sulfate solution is mixed with 34.5 mLmL of a 0.130 MM lead(II)(II) acetate solution and the following precipitation reaction occurs: K2SO4(aq)+Pb(C2H3O2)2(aq)→2KC2H3O2(aq)+PbSO4(s)K2SO4(aq)+Pb(C2H3O2)2(aq)→2KC2H3O2(aq)+PbSO4(s) The solid PbSO4PbSO4 is collected, dried, and found to have a mass of 0.991 gg . Determine the limiting reactant, the theoretical yield, and the percent yield.

If 20.0 g of LiOH is added to 0.750 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.

An aqueous ethylene glycol (HOCH, CH, OH, FW = 62.07 g/mol) solution with a mass of 220.9 mg is titrated with 33.7 mL of 0.0839 M Ce+ in 4 M HCIO,. The solution is held at 60 °C for 15 min to oxidize the ethylene glycol to formic acid ( HCO,H) and carbon dioxide. The excess Ce+ is titrated with 11.03 mL of 0.0447 M Fe2+ to a ferroin end point. What is the mass percent of ethylene glycol in the unknown solution? 9.2 mass percent = |% Incorrect