Contamination of precipitate by co-precipitation can be minimized by (tick all that may apply) A. Digestion B. Peptization C. Washing D. Re-precipitation
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Contamination of precipitate by co-precipitation can be minimized by (tick all that may apply)
A. Digestion
B. Peptization
C. Washing
D. Re-precipitation
Step by step
Solved in 2 steps
- Sources of Error Determine the relationship between the observed/apparent value (EX) VERSUS that of the true value (ET) for the quantity being sought by writing either <, >, or = on the space provided. TOPIC: Measured mass of the precipitate 1. Overignition which causes the conversion of BaSO4 precipitate to BaO. EX _____ ET2. Precipitate was not washed thoroughly. Ex _____ ET TOPIC: Standardization of Titrant 3.Distilled water was not equilibrated to room temperature before the preparation of NaOH titrant. EX _______ ETWhich among these is/are properties for the type of precipitate required in gravimetric analysis? Hygroscopic Known composition Reactive with atmospheric constituents Large particlesWhile working in a metal processing facility, Letlen had accidentally mixed two metal vatstogether creating an alloy. One vat was labeled for cadmium, while the other was not. It canbe assumed that these are of pure metal composition. To identify this metal, Letlen took 1.000 g of the homogenous alloy sample composed ofcadmium and the unknown metal, dissolved, and diluted it to exactly 100.0 mL in avolumetric flask. A 20.00-mL aliquot was taken and titrated this using 22.82 mL of 0.05000M EDTA. In a second 20.00-mL aliquot, the Cd was masked through the addition of HCN/NaCN buffer.The titration of the unknown metal in the aliquot required 15.13 mL of EDTA.MW: Cd (112.411 g/mol) a. Calculate the moles of Cd and the moles of unknown metal in the 20.00-mL aliquot.b. Calculate the moles of Cd and the moles of unknown metal in the sample.
- If you want to dissolve 0.225 grams of AgBr, what volume of 0.0138M Na2S2O3 in mililiters, should be usedIt 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.Make an schematic diagram for procedure below: B. %SO3 determination Transfer all precipitate to the filter paper avoiding any loses during the filtration procedure. One may use a rubber policeman to scrape remaining precipitate in the beaker. Wash the precipitate in the beaker 3x with hot water before transferring to the filter paper. Test the washings with 0.1 M AgNO3 Cloudiness indicates presence of chloride ions; therefore there is a need to wash more the precipitate. Carefully lift the paper out of the funnel, fold it as demonstrated by your instructor and transfer it onto the constant weighed crucible. Dry the crucible cautiously with a small flam, as instructed by your instructor. The flame should be directed at the top of the container, and the lid should be off. Avoid spattering. After drying, char the filter paper by increasing the flame temperature. The crucible should have free access to air. The lid should be kept handy to smother the filter paper in case it catches fire.…
- 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?25 mL of a saturated solution of K2Cr2O7 was cooled from 90oC to 50oC, how many moles solid will precipitate from solution?The concentration of CO in the air can be determined by passing a known volume of air through a tube containing I2O5, resulting in the formation of CO2 and I2. I2 is removed from the tube by distillation and collected in a solution containing excess KI, producing I3-. I3- is titrated with a standard solution of Na2S2O3. A 4.79 L air sample was sampled as described here, requiring 7.17 ml of 0.00329 M Na2S2O3 to reach the endpoint in a typical analysis. If the density of the air is 1.23×10^-3 g/ml, what is the amount of CO in the air in ppm? (CO: 28 g/ml)
- Which characteristic of a precipitate doesn’t do well for gravimetric analysis. a Readily filtered and washed free of contaminants b Of sufficiently high solubility (Ksp) c Unreactive with constituents of the atmosphere and high purity d Of known composition after it is dried or, if necessary, ignited. e None of the aboveTrue or False: Blank titration is indicated for the determination of the concentration of a sample. Can you please expound why?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.
