Q3/A 0.80868 gm sample of a commercial phosphate detergent was ignited at a red heat to destroy the organic matter the residue was then taken up in hot HCl, which converted the P to H3PO4. The phosphate was precipitated as MgNH.PO4.6H₂O by addition of Mg¹2 followed by aqueous NH3. after being filtered and washed. The precipitate was converted to Mg₂P₂0 (222.57gm mol) by ignition at 1000 Cº this residue weighed represent 61.5% of the total sample mass. Calculate the percent P(30.974gm mol),0 (16 gm/mol) and Mg (24.3 gm/mol) in the sample.

Q3/A 0.80868 gm sample of a commercial phosphate detergent was ignited at a red heat to destroy the organic matter the residue was then taken up in hot HCl, which converted the P to H3PO4. The phosphate was precipitated as MgNH.PO4.6H₂O by addition of Mg¹2 followed by aqueous NH3. after being filtered and washed. The precipitate was converted to Mg₂P₂0 (222.57gm mol) by ignition at 1000 Cº this residue weighed represent 61.5% of the total sample mass. Calculate the percent P(30.974gm mol),0 (16 gm/mol) and Mg (24.3 gm/mol) in the sample.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter31: Introduction To Analytical Separations

Section: Chapter Questions

Problem 31.19QAP

See similar textbooks

Similar questions

Calcium fluoride is considered as a relatively insoluble compound and therefore lime or slakedlime has been considered as a possible material to remove excess fluoride in water of boreholesin certain parts of the country. The solubility product of CaF2 is Ksp = 3 x 10 – 11 and that ofCa(OH)2 isKsp =8x10-61. How much lime can be added to the water to remove 10 mg of F- ion per litre ofborehole water?(The atomic masses are Ca: 40.08; F: 19.00; O: 16; H: 1)
0.1 g of the mixture of na2so4 and k2so4 is taken and 100 ml of solution is prepared. 10 ml of this prepared solution is placed in a beaker and some distilled water is added. A mass of 15.5 mg is obtained by precipitation with Bacl2 at PH=5, then filtering and bringing to a constant weight at 800 °C. Calculate the percentages of Na2so4 and K2so4 in the mixture accordingly.
Q1. Dissolved 0.273 grams of pure sodium oxalate (Na,C,O.) in distilled water and added sulfuric acid and titration the solution at 70 ° C by using 42.68 ml of KMNO, solution and has exceeded end point limits by using 1.46 ml of standard oxalic acid (H; C;O.) with 0.1024 N. Calculate the normlity of KMN0.. Note that the molecular weight of sodium oxalate (Na,C,O.) = 134 and its equivalent weight = 67
Hexanoic acid was added to an immiscible biphasic solvent sysem, water and CCl4 at 20.0OC and the equilibrium concentrations of hexanoic acid were determined to be 3.66 g/L in H2O and 67.0 g/L in CCl4. Caluclate the distrubution coeffiecent (D1) of hexanoic acid in CCl4 with respect to water.
One litre of a saturated aqueous solution of Ag2SO4 (MW = 311.79 g mol- 1) at 25 °C is evaporated to dryness. 4.844 g of Ag2SO4 residue was produced. What is the solubility product (Ksp)?
Hexanoic acid was added to an immiscible biphasic solvent system, water and CCl4 at 20.0OC and the equilibrium concentrations of hexanoic acid were determined to be 3.66 g/L in H2O and 67.0 g/L in CCl4. Caluclate the distrubution coeffiecent (D2) of hexanoic acid in water with respect to CCl4.
Dissolved 0.273 grams of pure sodium oxalate (Na2C204) in distilled water and added sulfuric acid and titration the solution at 70 °C by using 42.68 ml of KMNO4 solution and has exceeded end point limits by using 1.46 ml of standard oxalic acid (H2 C204) with 0.1024 N. Calculate the normlity of KMNO4. Note that the molecular weight of sodium oxalate (Na2C204) = 134 and its equivalent weight = 67 * %3D
what is the purpose of preparing of a standard sodium hydroxide solution in determination of purity of impure KHP?
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.
A 0.512 g sample of a commercial phosphate detergent was ignited at a red heat to destroy the organic matter. The residue was taken up in hot HCl, which converted the P to H3PO4. The phosphate was precipitated as MgNH4PO4.6H2O by addition of Mg2+ followed by aqueous NH3. After being filtered and washed the precipitate was converted to Mg2P2O7 by ignition at 1000 0C and the residue weighed 0.1151g. (a) What is the Gravimetric Factor to convert Mg2P2O7 to P? (b) Calculate the percent P in the sample could you type it out please
To determine the fluoride content in an aqueous and chloride-containing preparation of ammonium fluoride, the following analysis was performed. 105.2 mg of the preparation was dissolved in 100.0 mL of water. Then a 300 mL 40 mM lead chloride solution was added, whereby all fluoride ions were precipitated out of the solution in the form of the sparingly soluble salt PbClF (s). The precipitate was separated and washed at 15 degrees with a lead fluoride chloride saturated solution and dried at 130 degrees. The precipitate weighed 651.3 mg. a) Calculate the fluoride content (as % by weight F) in the preparation.b) Determine the purity of the ammonium fluoride preparation
Q1. Dissolved 0.273 grams of pure sodium oxalate (Na2C0.) In distilled water and added sulfuric acid and titration the solution at 70 ° C by using 42.68 ml of KMnO, solution and has exceeded end point limits by using 1.46 ml of oxalic acid (H , C, 0.) With 0.1024 N. Calculate the normlity of KMnO .. Note that the molecular weight of sodium oxalate (Na, C, 0.) = 134 and its equivalent weight = 67