An attempt is made to analyse barium gravimetrically by precipitating of BaF, with NaF2. Assuming that 200 mg sample of Ba2+ in 100 mL of solution is to be precipitated and the precipitation must be 99.9% completed. The solubility product of BaF, is 1.7 x 10-6. i. Determine the amount of Ba2+ that must remain in 100 mL of solution so that the precipitation 99.9% is completed (in mg mL-1). ii. Based on the following balanced chemical equation, calculate the concentration of F after the precipitation of BaF2. BaF, (s) == Ba?* (aq) + 2F¯(aq)

An attempt is made to analyse barium gravimetrically by precipitating of BaF, with NaF2. Assuming that 200 mg sample of Ba2+ in 100 mL of solution is to be precipitated and the precipitation must be 99.9% completed. The solubility product of BaF, is 1.7 x 10-6. i. Determine the amount of Ba2+ that must remain in 100 mL of solution so that the precipitation 99.9% is completed (in mg mL-1). ii. Based on the following balanced chemical equation, calculate the concentration of F after the precipitation of BaF2. BaF, (s) == Ba?* (aq) + 2F¯(aq)

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter20: Applications Of Oxidation/reduction Titrations

Section: Chapter Questions

Problem 20.26QAP

See similar textbooks

Similar questions

What wt of magnetite should be taken for analysis in order that after converting to a precipitate of Fe2O3.xH2O, the percentage of Fe3O4 in the sample can be found by multiplying the wt in grams of the ignited precipitate (Fe2O3) by 100.
What is the maximum solid solubility of Mg in Al? At what temperature does it occur? e. An Al-Mg alloy (10 wt% Mg, 90 wt% Al) is heated slowly (to insure equilibrium) from a temperature of 200 C: i. At what temperature does the first liquid phase form? ii. What is the composition of the liquid phase at the temperature in part i.? iii. At what temperature does complete melting (no solid phase remaining) occur? iv. What is the composition of the last solid remaining prior to complete melting? f. Using the equilibrium phase diagram of Figure 1, identify the phases present, their compositions, and their relative mass fractions at equilibrium for a 70 wt% Mg – 30 wt% Al alloy held at 300 C.
The chloride in the sample is to be determined gravimetrically by precipitating and weighing AgCl. What weight in grams of sample should be taken so that the percentage of Cl is obtained by simply multiplying the weight of the AgCl precipitate by 10?
It is required to know the concentration of an aqueous solution of H2SO4 that appeared in the laboratoryChemistry III and it's unlabeled. To this end, a student of analytical chemistry carried out the followingProcedure: He took 5.00 mL of a fresh and standardized solution of 0.525M NaOH and brought them to a250.0 mL balloon to be completed with distilled water. Subsequently, he poured 15.00 mL of the solutionH2SO4 of unknown concentration in an Erlenmeyer flask and added 2 drops of phenolphthalein.Using a burette filled with the last NaOH solution, he noticed that when adding 39.40 mL of the hydroxidethe Erlenmeyer solution reached a faint but permanent pink. With the above dataDetermine the concentration and pH of the H2SO4 solution.
The molar solubility of CuCO3 at 298K is 1.5811×10-5 M. Determine the Ksp of this salt.
The compound lead(II) sulfate has a solubility of 4.824E-3 g/100mL at 25 degC.What is the molar solubility of this solution at saturation? 0.0002 mol/L What is the Ksp at 25 degC for lead(II) sulfate? What is the molar solubility of lead(II) sulfate in 0.28 M lead(II) nitrate ?
What is the molar solubility of a. As2Cd3O8 (Ksp = 2.2E-33) b. Be(OH)2 (Ksp = 6.9E-22) c. Cu3(AsO4)2 (Ksp = 8.0E-36) in pure H2O at 25 deg C?
(a) I f t he molar solubilit y o f CaF2 at 35 °C i s1.24 x 10-3 mol/L, what is Ksp at this temperature? (b) It isfound that 1.1 x 10-2 g SrF2 dissolves per 100 mL of aqueoussolution at 25 °C. Calculate the solubility product forSrF2. (c) The Ksp of Ba(IO3)2 at 25 °C is 6.0 x 10-10. What isthe molar solubility of Ba(IO3)2?
123 mL of a 0.352 M Ca(NO3)2 solution is mixed with 251 mL of a 0.254 M solution of NaF at 25ºC. Calculate Qsp for the precipitate formed.
Will Mn(OH)2 precipitate from a 0.01 M solution of MnCl2 at pH = 9? Ksp(Mn(OH)2) = 1,0 x 10-13. Discuss from solubility diagrams and prove by calculation.calculation. Co is a metal that is present in every lithium battery to stabilize its charge and toincrease stability. Every cell phone, tablet and electric car relies on the availability ofcobalt, 97% of which is extracted from mines in places like the Congo, where essentially slave labor is used.Cobalt ions form complexes with e.g. CN- . You see solubility diagrams and fraction diagrams for CoCO3 with and without the addition of 10 mM CN- .. Explain whythe solubility of cobalt carbonate increases at high pH when cyanide ions are present.Write reaction formulas for the formation of the dominant cobalt cyanide complexes.
Q: The concentration of the sulphate ion in a mineral water can be determinedby the turbidity which results from the addition of excess BaCl2, to a quantityof measured sample. A turbidometer used for this analysis has been standardisedwith a series of standard solutions of NaSO4. The following resultswere obtained:Standard solution Conc. (SO4)2− (mg/L) Reading of turbidometerS0 0.00 0.06S1 5.00 1.48S2 10.00 2.28S3 15.00 3.98S4 20.00 4.61i. In supposing that a linear relationship exists between the readings takenfrom the apparatus and the sulphur ion concentration, derive an equationrelating readings of the turbidometer and sulphate concentration(method of least squares).ii. Calculate the concentration of sulphate in a sample of mineral waterfor which the turbidometer gives a reading of 3.67.
Solubility tests of benzoic acid with a dissolution enthalpy of -32kJ / mol were performed at 2 different temperatures. In the first experiment carried out at 27 ° C, 5 mL of the sample taken from the benzoic acid solution is taken into 25 mL of water and titrated with 0.02M NaOH. As a result of the titration, there is a consumption of 8 mL, respectively. In the second experiment performed at a different temperature under the same conditions, 22 mL was consumed. Taking advantage of these results a) Solubility of benzoic acid at 27 ° C .................................................; b) solubility of benzoic acid at different temperature ................................................; c) second test temperature ....................................................... (M (benzoic acid): 122.12 g / mol) Note: enter only required numerical values and units in the spaces in the question.