The arsenic in a 1.203 g sample of a pesticide was converted to H3AsO4 by reaction with concentrated nitric acid. The acid was then neutralized, and 40.00 mL of 0.05871 M AgNO3 was added to precipitate the arsenic quantitatively as silver arsenate, Ag3AsO4 (FM 462.52 g/mol) 3 Ag+ + AsO43-→ Ag3AsO4 (s) The excess Ag in the filtrate and in the washings from the precipitate was titrated with 9.63 mL of 0.1000 M KSCN.Ag+ + SCN-→ AgSCN (s)Find the weight percent of arsenic trioxide, As2O3 (FM 197.841 g/mol), in the sample.

2.00 g calcium tablet sample is determined by precipitating CaC2O4, dissolving this in acid, and titrating the oxalate with 0.0200 M KMnO4. The formula reaction is 5 H2C2O4 + 2 MnO4- + 6 H+ ->10 CO2 + 2 Mn2+ + 8 H2O What percent of CaO is in the sample, if 35.6 ml KMnO4 is required for the titration?

A 65.0 mL sample of a 0.110 M potassium sulfate solution is mixed with 36.5 mL of a 0.114 M lead(II) acetate solution and the following precipitation reaction occurs: K2SO4(aq)+Pb(C2H3O2)2(aq)→2KC2H3O2(aq)+PbSO4(s) The solid PbSO4 is collected, dried, and found to have a mass of 1.01 g . Determine the limiting reactant, the theoretical yield, and the percent yield.

A stock solution of Cu(C2H302)2 has a concentration of 0.270 M. If 6.00 mL of this solution is transferred to a 50.00 mL flask and then diluted with distilled water, what is the final concentration of Cu2+ ions?

What is the maximum mass (in grams) of each of the following soluble salts that can be added to 310 mL of 0.050 M BaCl2 without causing a precipitate to form? (Assume that the addition of solid causes no change in volume.) (a) (NH4)2SO4  ____ × 10___g (Enter your answer in scientific notation.) b) Pb(NO3)2 ______g  c) NaF ______g

The antacid found in Tums™ has the active ingredient calcium carbonate, which undergoes a reaction when mixed with hydrochloric acid to produce water, calcium chloride and carbon dioxide. A tablet of this antacid had a mass of 1.774g and was dissolved completely in an excess of 30.0mL of 0.794M HCl. The resulting solution was then titrated with 0.995M NaOH. The initial buret reading was 11.05mL and the final buret reading was 28.52mL. The listed mass of active ingredient on the bottle is 325mg. a. What is the calculated mass of active ingredient in this tablet? b. What is the percent error from the listed mass? c. What percent of the tablet is inert (non-active) ingredients? explain in detail

15. Iron(II) can be oxidized by an acidic K2C12O7 solution according to the net ionic equation Cr2072 + 6FE2+ + 14H* → 2Cr3+ + 6Fe3+ + 7H2O If it takes 26.0 mL of 0.0250 M K2Cr2O7 to titrate 25.0 mL of a solution containing Fe2*, What is the molar concentration of Fe2*?

Calculate the grams of precipitate formed if you react 38.9 g AgNO3 with 30.2 g of Na2S according to the following reaction: 2AgNO3 (aq) + Na2S (aq) -> Ag2S (s) + 2NaNO3 (aq)

The zinc content of a 1.55 g ore sample was determined by dissolving the ore in HCl, which reacts with the zinc. The excess HCl is then neutralized with with NaOH. The reaction of HClHCl with Zn is shown.   Zn(s)+2HCl(aq)⟶ZnCl2⁢(aq)+H2⁡(g)   The ore was dissolved in 150 mL of 0.600 M HCl  and the resulting solution was diluted to a total volume of 300 mL. A 20.0 mL aliquot of the final solution required 8.92 mL of 0.548 NaOH to neutralize the excess HCl. What is the mass percentage (%w/w) of Zn in the ore sample?

In the following balanced reaction: Pb(NO3)2(aq) + 2KI(aq) → PbI2(s) + 2KNO3(aq) 10.9 g of KI react with a 0.193 mol L-1 solution of Pb(NO3)2. The total solution volume is 0.200L Calculate the number of moles of Pb(NO3)2.