EXPERIMENT : GRAVIMETRIC ANALYSIS OF PHOSPHORUS IN PLANT FOODAim: To determine the amount of phosphorus in a commercial plant food I want the Calculations for this experiment and complete the table Observations:Mass of plant food (original sample) = 2 gWeight of Filter Paper = W1 = 0.87 gWeight of Filter paper + Precipitate = W2 = 2.85 gWeight of Precipitate Wz - Wi = 2.85 – 0.87 = 1.98Table 1: Measurement of Conductance.TrialPlant Food (g)Amount of P (g)% PCalculations:2 g of soluble plant food yields (W2-W:) g of MGNH4PO4.6H2O[M9NH4PO4.6H2O]245 g31 g(Wz-W1) g of MGNH4PO4.6H2O = 'X'g of PAmount of P =Percent phosphorous in the original sample:gP% P = (-x 100'g original samnple

The amount of MgNH4PO4.6H2O in 2 g plant food =1.98 g Calculate amount of P present in 1.98 g as…

Observations: Mass of plant food (original sample) = 2 g Weight of Filter Paper = W1 = 0.87 g Weight of Filter paper + Precipitate = W2 = 2.85 g %3D Weight of Precipitate W - Wi = 2.85 – 0.87 = 1.98 Table 1: Measurement of Conductance. Trial 1 Plant Food (g) Amount of P (g) % P Calculations: 2 g of soluble plant food yields (W2-W:) g of MGNH4PO4.6H2O [M9NH«PO4.6H2O] E P 245 g 31 g (Wz-Wi) g of MGNHPO4.6H2O = X' g of P Amount of P = Percent phosphorous in the original sample: % P ( gP 'g original sample x 100

Observations: Mass of plant food (original sample) = 2 g Weight of Filter Paper = W1 = 0.87 g Weight of Filter paper + Precipitate = W2 = 2.85 g %3D Weight of Precipitate W - Wi = 2.85 – 0.87 = 1.98 Table 1: Measurement of Conductance. Trial 1 Plant Food (g) Amount of P (g) % P Calculations: 2 g of soluble plant food yields (W2-W:) g of MGNH4PO4.6H2O [M9NH«PO4.6H2O] E P 245 g 31 g (Wz-Wi) g of MGNHPO4.6H2O = X' g of P Amount of P = Percent phosphorous in the original sample: % P ( gP 'g original sample x 100

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

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
20 aspirin tablets labeled 80mg were dissolved in 100mL of 90% ethanol. A 10mL aliquot was taken and was used for assay. The analyte followed usual process and was treated with 50mL of 0.1000N NaH and was titrated with 35mL 0.1050N H2O4 until the solution achieved completion. Calculate the % content of the total aspirin capsules and the actual label claim
A 0.1 M solution of acid was used to titrate 10 ml of 0.1 M solution of alkali and thefollowing volumes of acid were recorded: 9.88 10.18 10.23 10.39 10.21 Calculate the 95% confidence limits of the mean and use them to decide whetherthere is any evidence of systematic error.
A 1.000-gram sample of NaOH (39.997 g/mol) which has been exposed to the air for some time (NaOH will adsorb water and CO2 from the ambient air) is dissolved in water and then diluted to 500.00 mL. 100.0 mL of this solution required 38.60 mL of 0.1062 M HCl to be titrated to the endpoint (~pH 3). A second 100.00 mL portion is treated with excess BaCl2 and then diluted to 250 mL and filtered. 200 mL of the filtrate required 29.62 mL of HCl to titrate to the (~pH 8-9) endpoint. Calculate the mass percentage of NaOH and Na2CO3 (105.9898 g/mol) in the original sample. The adsorbed CO2 is converted to Na2CO3. The Ksp for BaCO3 (s) is 2.58 x 10-9.
A 18 g of unknown organic sample was dissolve in 756 mL of benzene. The boiling point of benzene was increased by 3.36oC. As the first step of analysis, determine the moecular weight of the unknow sample? Kb of benzene= 2.64oC/m Bb of benzene = 80.09 oC density of benzene = 0.874 g/mL at 25 °C Answer in whole number, no units required.
A 25.00mL wastewater sample was analyzed for its Mg2+ content using a standard gravimetric method. the sample was diluted to 3.00L and an 11.00mL aliquot was treated to precipitate magnesium as MgNH4PO4.6H2O using (NH4)2HPO4 as the precipitating agent. the precipitate was then filtered, washed, dried, and ignited resulting in a 0.1325mg Mg2P2O7 residue. How much Mg (in ppm) is present in the original sample
detailed calculations on how to prepare the solutions listed below, Solution 1) 25 mL 7 M sulfuric acid and the respective dilution of this solution to prepare 50 mL 2 M sulfuric acid in deionised water. Sulfuric acid Mw = 98.079 g mol-1 Sulfuric acid density = 1.84 g mL-1 Sulfuric acid purity = 98%
Solid Na2S is slowly added to a solution of 1.0 x 10-3 M Cr3+ (with no change in volume). At what [S2-] will Cr2S3 start to ppt? For Cr2S3, Ksp = 1.0 x 10-20
The buret was filled with 0.100 M HCl solution. Then was transferred in a 25.0 mL of saturated calcium hydroxide solution (2g of calcium hydroxide per 100 ml of water) in two separate E-flasks. Then 2 drops of phenolphthalein was added to each flask Titration data for the determination of solubility and Ksp of calcium hydroxide: Trial 2: Final Buret reading (ml)-26.10; Initial Buret reading (ml)- 19.80; Temperature (Celcius)- 25 Voume of HCl used: Trial 2- 6.30mL 1. Compute for the moles of H+ used and the moles of OH- present. moles of H+ used = (concentration of HCl) × (volume of HCl used)moles of OH- = moles of H+ used 2. Construct an ICE table for the reaction.3. Calculate the molar solubility (in mol/L) of OH- and Ca2+.4. Determine the solubility of Ca(OH)2 in g/L. (MM of Ca(OH)2 = 74.096 g/mol). 5. Calculate the Ksp of Ca(OH)26. Compute for the percent error of the experimental value for Ksp of Ca(OH)2 with the literature…
Suppose you have a soil that is made up of 10% organic matter with CEC = 200 cmol/kg, 40% kaolinitewith CEC = 10 cmol/kg, and 50% vermiculite with CEC = 100 cmol/kg.1- Calculate the overall CEC of the soil by taking a weighted average of the three soil components.2- What percentage of the overall CEC is contributed by the organic matter? How does that numbercompare to the 10% of the soil itself that is organic?
You are given a container with Na3PO3 that is reportedly contaminated. You are asked by your supervisor to determine the percent purity of that sample in order to know the next measures to be taken by the plant. The following are the procedures that you need to do: a. Dissolve sample weighing 1 g in 35 mL water. b. Prepare solution with 45 mL 3% w/v HgCl2, 30 mL 10% w/v C2H3NaO2 and 10 mL CH3COOH. c. Digest sample then filter then rinse the precipitate that weighs 0.2857 g. d. Compute for the % purity.
A 100 g soil containing 20% smectitie mineral matter was mixed with 150 mL solution containing 0.10 M Pb. CEC of pure smectitie is 110 emol(+)/kg. CEC of the soil (cmol(+)/kg) is: