Computer 16 DATA TABLE Equivalence point (mL) Mass of filter paper + precipitate (g) Mass of filter paper (g) Mass of precipitate (g) Molarity of H₂SO. (M) Trial 1 4.997mL 0.6825 0.5200 0.1m Trial 2 8861mL 0.6757 0.5175 Trial 3 DATA ANALYSIS 1. Use the titration results to calculate the moles of H₂SO, that were used to reach the equivalence point in each trial. Conductimetric Titration and Gravimetric Determination of a Precipitate 3. Convert the mass of the barium sulfate precipitate, formed in each trial, to moles.

Computer 16 DATA TABLE Equivalence point (mL) Mass of filter paper + precipitate (g) Mass of filter paper (g) Mass of precipitate (g) Molarity of H₂SO. (M) Trial 1 4.997mL 0.6825 0.5200 0.1m Trial 2 8861mL 0.6757 0.5175 Trial 3 DATA ANALYSIS 1. Use the titration results to calculate the moles of H₂SO, that were used to reach the equivalence point in each trial. Conductimetric Titration and Gravimetric Determination of a Precipitate 3. Convert the mass of the barium sulfate precipitate, formed in each trial, to moles.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter21: Potentiometry

Section: Chapter Questions

Problem 21.22QAP

See similar textbooks

Similar questions

The value of Ksp for Mg3(AsO4)2 is 2.1 * 10-20. The AsO43- ion is derived from the weak acid H3AsO4 (pKa1 = 2.22; pKa2 = 6.98; pKa3 = 11.50). (a) Calculate the molar solubility of Mg3(AsO4)2 in water.
If 500mL of 0.10M Ca2+ is mixed with 500mL of 0.10M SO42-, what mass of calcium sulfate will precipitate? Ksp for CaSO4 is 2.40 • 10-5. express answer to 3 significant figures. And include units.
9. An aqueous solution of sulfuric acid is prepared by mixing a secondary standard of sulfuric acid with deionized water. The aforementioned acid is to be used as a titrant hence its concentration must be accurately determined. To do this, Engr. Polinar, standardized the titrant by titrating two liters of ammonia at 0.90 atm and 30 deg C. From the experiment, 134 mL of the titrant was necessary to neutralize the ammonia. Determine the concentration of the acid in terms of normality? 10. Engr. Forcadela is optimizing a plastic formulation by manipulating the phosgene concentration injected as a gas during the reaction. To obtain credible results, he considered the propensity of phosgene to dissociate into carbon monoxide and chlorine gas at 395 deg C. Performing an experiment at the aforementioned temperature, an equilibrium is reached amongst the species where the total pressure is at 3 atm. If the equilibrium constant expression in terms of concentration for the reaction at 395 deg C…
What molar ratio of base/salt is required to prepare an ammoniaammonium chloride buffer solution having a pH of 11.0? The Kbvalue of ammonia ammonia is 1.80 x 10-5 at 250C. Also express theresult in mole percent. The molar ratio of Sodium acetate to acetic acid in a buffer solutionhaving a pH of 5.76 is 10:1. Assuming that the total bufferconcentration is 2.2 x 10 -2 mole /liter, how many grams of sodiumacetate (MW=82g/mole) and how many grams of acetic acid(MW=60g/mole) should be used in preparing a liter of the solution?
1.10 M Acetic acid 0.900 M Sodium acetate Solution (mL) |(mL) [H3o*1 (M) 1 8.00 2.00 8.71e-5M 2 7.00 3.00 5.13e-5M 3 6.00 4.00 3.24e-5M 4 5.00 5.00 4.00 6.00 6. 3.00 7.00 7 2.00 8.00 8 1.00 9.00
P Chemical eg X P Chemical eq X P Chemical ec X P Chemical ec X P Chemical ec x P Chemi View?assignmentProblemlD=144082837&offset%3Dnext CHE154-H Gen Chem II Bronikowski S20 Part A sp Use the molar solubility, 1.08 × 10-5 M, in pure water to calculate K, for BaCrO4. Express your answer using three significant figures. . ΑΣφ Ksp
Calculate: 1)mean Experimental solubility of calcium hydroxide 2)Standard deviation 3)RSD(pph)
The chloride in a sample containing approximately 3.5 % NaCl is to be determined gravimetrically as AgCl. What weight of sample must be taken to obtain a precipitate that will weigh about 0.10 g?
A solution of NaF is added dropwise to a solution that is 0.0483 M in Mg2+ and 1.23e-08 Min Y³+. The Ksp of MgF2 is 5.16e-11. The Ksp of YF3 is 8.62e-21. (a) What concentration of is necessary to begin precipitation? (Neglect volume changes.) 71-3.0863 [F] = XM. (b) Which cation precipitates first? O Mg2+ y²+ (c) What is the concentration of F when the second cation begins to precipitate? [F]-1436-4 XM.
A suitable target for the titration is 30.0 cm3 of 0.025 moldm-3 Br2(aq) Justify why a much smaller target titre would not be appropriate Calculate the amount in moles of bromine in the target titer Justification? calculate a suitable massof alive oil to transfer to the volumetric flask using your answer to of above question and the structure of Y Assume that the olive oil contains 85/- of Y by mass (If you were unable to calculate the amount of bromine in the target titer,you should assume it is 6.25×10^-8 mol .this in not the correct amount)
What is the solubility (in mol/L) of PbCl2 given that the Ksp is 1.69⋅10-13.
True or False Very Insoluble precipitates are not the best candidates for gravimetric analysis.