Why is it less desirable to wash AgCl precipitate with aqueous NaNO3 than with HNO3 solution? (Select all that apply.) A) HNO3 evaporates during drying. B)HNO3 is nonvolatile and will lead to a high mass for the precipitate. C )NNO3 is and will lead to a high mass for the precipitate. D)NaNO3 evaporates during drying.
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- The question is : Using benzoic acid's solubility data in water (found in pre-lab), calculate the amount of hot water needed to dissolve your crude benzoic acid. Based on your data and observation, explain why you may have used more ore less water than the calculated value. Pre lab Question: calculated amount of hot water to dissolve 2.0g of benzoic acid. => (2.0g benzoic acid)/( 68 g/L)(1000ml)/(1L) = 29.4 mL of hot water needed to dissolve 2.0g of benzoic acid. My cruse of benzoic acid is 1.81g.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.…PS. Further values required for the solvings are give in the various situations below. (ANSWER) Situation: A community in a mountainous area of Bohol uses water collected from a nearby natural spring. A sample was submitted to a laboratory for the analysis of its total hardness. Required: SHOW YOUR COMPLETE CALCULATIONS. BASED ON THE IMAGE PROVIDED BELOW FOR THIS QUESTION: Calculate the amount of titrant used in each trial to reach endpoint. Report total hardness of the sample as mean ±sd. a. 250.0 mL of 500.0 ppm of CaCO3 solution from a primary standard (assume solvent is distilled water only). Answer : Mass of CaCO3 = 0.125 g b, The EDTA solution was standardized by titrating it with a 25.0 mL aliquot of the CaCO3 solution. How much of the titrant was consumed. Answer: Volume of EDTA consumed = 12.405 g c. Calculate the average titer (mg CaCO3/mL EDTA). Mass of CaCO3 in 25 mL CaCO3 solution: 0.0125 g Answer: 1.008 mg CaCO3/ mL EDTA
- Solid cobalt (II) acetate is slowly added to 125 mL of 0.0945 M ammonium chromate solution. What is the concentration of cobalt required to just initiate precipitation? The Ksp of CoCrO4 is 7.1 * 10 -4. Report answer in scientific notation to two sig figs.What is observed when equal volumes of 0.1M aqueous HCl and 0.01 M Na2SO3 are mixed? Group of answer choices Colorless solution and a white precipitate. Colored solution and a white precipitate. Colorless solution and a colored precipitate. Colorless solution, no precipitate and gas evolution.A salt is known to have a solubility of 40 g per 100 g of water. 20 g of salt is put in 80 g of pure water. If it takes 10 min to dissolve 5 g of the salt, how much more salt will dissolve in the next 10 min? Topic : Differential Equation : Application : Rate of Dissolution
- 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.NEED HELP PLEASE GRAVIMETRIC ANALYSIS (Exercises) Instructions: Answer each of the problems below by showing your solutions neatly and logically. You may use periodic table for atomic masses of elements. Copy and answer each problem and please box your final answers. 9. What weight of pyrite ore (impure FeS2) must be taken for analysis so that the BaSO4 precipitate weight obtained will be equal to one-half that of the percent S in the sample? NOTE: KINDLY WRITE THE SOLUTIONS ON A SEPARATE SHEET OF PAPERSources 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: Determination of % SO32-Not all solid was transferred during the filtration of the precipitate. EX _____ ET
- Because of the risk of lead poisoning, the exposure of children to lead-based paint is a significant public health concern. Thefirst step in the quantitative analysis of lead in dried paint chips is to dissolve the sample. Corl evaluated several dissolution techniques.24 In this study, samples of paint were collected and pulverized with a Pyrex mortar and pestle. Replicate portions of the powdered paint were then taken foranalysis. Results for an unknown paint sample and for a standard reference material, in which dissolution wasaccomplished by a 4–6-h digestion with HNO3 on a hot plate, are shown in the following table. (a) Determine the overall variance, the variance due to the method, and the variance due to sampling. (b) What percentage of the overall variance is due to sampling? (c) How might the variance due to sampling be decreased?A student was tasked to perform gravimetric analysis of a soluble sulfate. His unknown sample weighed 0.7543 g. The sample underwentprecipitation using BaCl2 and was digested for overnight. The precipitate was then filtered off to obtain white crystalline precipitate that was collected inan ash less filter paper. In performing constant weighing, he obtained a crucible mass that is 29.9442 g. After burning his samples inside the crucible,the obtained mass was 30.3375 g. Compute for the theoretical % SO3 obtained by the student and the theoretical mass (g) of SO3 that should be obtained by the student using his weighed sampleA student was tasked to perform gravimetric analysis of a soluble sulfate. His unknown sample weighed 0.7543 g. The sample underwentprecipitation using BaCl2 and was digested for overnight. The precipitate was then filtered off to obtain white crystalline precipitate that was collected inan ash less filter paper. In performing constant weighing, he obtained a crucible mass that is 29.9442 g. After burning his samples inside the crucible,the obtained mass was 30.3375 g.29. Compute for the mass (g) of BaSO4 from the experiment.A) 0.3933B) 0.3393C) 0.3133D) 0.3951E) 0.359130. Compute for the experimental mass (g) of SO3 in grams obtained by the student.A) 0.1439B) 0.1349C) 0.1943D) 0.1394E) 0.359131. Compute for the experimental % SO3 obtained by the student.A) 73.21B) 56.33C) 17.89D) 56.89E) 72.8032. Compute for the theoretical % SO3 obtained by the studentA) 0.3933B) 56.37C) 17.33D) 17.89E) 0.425233. Compute for the theoretical mass (g) of SO3 that should be obtained by the student…