Six 50.0 ml volumetric flask 1-6 are labeled. 10.00 ml of 2.00 x 101 M Fe(NO3)3 solution was then pipet into each volumetric flask. A 1.00,2.00,3.00,4.00 and 5.00ml of 2.00 x 10-3M NaSCN solution was then pipetted to flask 2 through 6 respectively. A sufficient 0.10 M nitric acid was then added to each flask to make them total volume of 50.00ml. 1.a)Calculate the final Fe(NO3)3 concentrations for each. 1.b)Also how would you find the initial  concentration of SCN- for each flask? Please show calculations to solutions.Thanks

Calcium carbonate is used as an antacid to relieve heartbum, acid indigestion, and upset stomach. You have intake 6.088g CaCO3 with empty stomach and reacted with 2.852g Hydrochloric acid (HCl) present in the stomach. What mass of CaCO3 remains unreacted? Show the complete solution. CaCO3 +2HCl -> CaCl2 + CP2 +H2O a. What is the limiting reagent? b. What is the excess reagent? c. How much is leftover in the excess reagent?

What is the solubility (in mol/L) of PbCl2 in a 1.150 M solution of NaCl? Use Ksp = 9.60 x 10-6 for PbCl2. Express your answer to 4 significant figures and do not use scientific notation. Your Answer:

< Question 12 of 17 A 25.0 mL solution of HNO3 is neutralized with 25.4 mL of 0.250 M Ba(OH)2. What is the concentration of the original HNO3 solution? Tap here or pull up for additional resources 1 4 7 +/- M 2580 3690 . X C x 10

2.23 gr sample taken from a bleaching powder is dissolved and completed to 250 ml. Taken from here 25One ml of sample is titrated with 33.02 ml of 0.1158 N Na2S2O3 solution after the necessary procedures. Bleachingactive chlorine in powder (OClCalculate the amount and percentage. (OCl: 51.5 g / mol)

A dried sample of commercial salt was prepared by a coning and quartering. A 0.911-g sample of the salt was dissolved and diluted to 250.0 mL in a volumetric flask.  Repeat 10.00-mL aliquots of this solution were titrated with a 0.054 M silver nitrate solution, requiring 9.68 mL to reach equivalence. Calculate the %(w/w) NaCl in the original sample.

ma 12. 3.000 g BaCl₂.H₂O (molar mass=244.263 g/mol) was added to a solution of 100 mL of 0.050 M Na₂CO3. BaCl₂ (aq) + Na₂CO3 (aq) → BaCO3 (s) + 2NaCl Ksp for BaCO3 = 1.1 x 10-15 Calculate the concentration of CO32 in the resulting solution. a) 5M b) 0.050 M c) 0.072 M d) 1.5 x 10-¹3 M e) 1.5 x 10-¹4 M

Group I Cations of 6 M HCI; centrifuge for ~1 minute. Decant the solution and add an additional one or two drops of 6 M HCI; if no additional precipitate forms, the precipitation is complete. If it was incomplete, centrifuge to obtain the additional solid; then decant the liquid, add 1 or 2 drops of 6 M HCI, and repeat the procedure until no precipitate forms. Discard the supernatant into the appropriate waste container or keep for later experiments if your instructor so indicates. Add 1.5 mL of cold deionized or distilled water to the precipitate to wash; agitate, centrifuge, and discard the water to the appropriate waste container. Repeat the wash procedure. The solid contains Pb2*, Ag*, and/or Hg22*. Step 2. Separation of Pb2*. Add 1 mL of boiling water to the solid from step 1. Agitate, centrifuge, and decant the liquid. Repeat the extraction, combining the supernatant. The liquid should contain Pb?* if any is present. Step 3. Testing for Pb2*. Add 2 or 3 drops of 0.2 M K2CRO4…

What is the mass percent of Fe for each trial ?   Mass of (NH4)2Ce(NO3)6 (in 100.00 mL) =   4.5038 g             Mass of unknown (in 250.00 mL) = 10.000 g     Trial # Volume of unknown solution (mL) Titration Volume (mL of Ce4+) Mass Percent(% Fe) 1 25.00 mL 7.20 mL   2 25.00 mL 7.40 mL   3 25.00 mL 7.60 mL   4 25.00 mL 7.50 mL