Determination of ash content is part of the proximate analysis in food laboratories which provides a measure of the total amount of minerals in the food sample. A 1.068 g as received representative sample of "tunsoy", salted fish. Before ignition, moisture was determined to be 5.65%. After ignition, the ashed sample registered 0.2685 g (ashed sample + crucible). The constant weight of crucible was 0.0178 g. From the data given, calculate % ash in the as received sample. 23.5% 25.1% 24.9% cannot be determined

Determination of ash content is part of the proximate analysis in food laboratories which provides a measure of the total amount of minerals in the food sample. A 1.068 g as received representative sample of "tunsoy", salted fish. Before ignition, moisture was determined to be 5.65%. After ignition, the ashed sample registered 0.2685 g (ashed sample + crucible). The constant weight of crucible was 0.0178 g. From the data given, calculate % ash in the as received sample. 23.5% 25.1% 24.9% cannot be determined

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Chapter6: Chemical Composition

Section6.1: Atoms And Moles

Problem 1RQ

See similar textbooks

Similar questions

If the mass of the original sample of alloy was 0.7459 ± 0.0005 g and the mass of precipitated CuSCN was 0.2275 ± 0.0005 g and the volumetric flasks used had a 0.05% error, what is the error in the calculated percentage mass of Cu in the alloy? Assume no error in the molecular masses. Provide your answer as an absolute error.
7. After performing precipitation gravimetry, Asta placed the weighing form inside the crucible, heated it, cooled it down, and weighed the crucible with the weighing form and obtained a mass of 23.4120 g. Repeating this cycle continuously gave a mass of 23.2125 g, then 23.1136 g, then 23.1139 g. Which among these masses should he use for his calculations?
What is the concentration, in units of grams of dye per liter of solution (g/L), of the dilute dye solution that is produced as follows? Transfer 16.51 mL of the stock solution (6.12 g/L) to a 200.0 mL volumetric flask and dilute to the 200.0 mL line with deionized water. Your answer should be reported to the correct number of significant figures.
As part of the aspirin synthesis lab the orgo students also had to perform the following calculation to demonstrate their knowledge. Are you able to help them work this out? Saponification is a process in which soap is produced from the chemical reaction between animal fat (triglycerides) and a strong base such as KOH. An example of such balanced chemical reaction is shown here: C51H98O6 + 3KOH → C3H5(OH)3 + 3C16H31O2K (Triglyceride) (Soap) if during the saponification reaction 231.5 g of C51H98O6 is mixed with 231.5 g of KOH and 160 g of soap is produced. Calculate the theoretical yield of soap C16H31O2K and indicate who is the limiting reactant. (Provide your answer to 2 decimal places) Calculate the percent yield for this reaction (Provide your answer to 1 decimal place) *Show ALL steps and mathematical equations involved in your calculations to help the orgo students. Remember to label all…
Complete the following statements. You may find the flowchart in section 1.2 of your textbook helpful. In station C.... The provided aqueous KI/I2 was a The provided solid Na2S2O3 was a Options Pure element Pure compound Homogeneous Heterogeneous
One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(I) carbonate, in concentrated sulfuric acid The sulfuric acid reacts with the copper(I) carbonate to produce a blue solution of copper(I) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe(s) + CuSO4(aq) -> Cu(s) + FeSO4(aq) Suppose an industrial quality-control cherist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 300. mL copper(I) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 75. mg Calculate the oriqinal concentration of copper(I) sulfate in the sample. Round your answer to 2 significant digits.
i have hard time geting it stright even after I do the experiment can u help me with the one pls Material ChemicalsSealed NO2 tubes, KSCN solution (0.002 M), acidified Fe(NO3)3 solution (0.2 M), KSCN crystals, Fe(NO3)3 crystals, KOH (concentrated (8 M)), distilled waterApparatus:Bunsen burner, ring stand, wire gauze, matches, thermometer, dropper, test tubes, glass stirring rod, beaker tongs Procedure Part A: Fill a 600 mL beaker to the 3/4 mark with water. Bring to a boil using a Bunsen burner. In another 600 mL beaker, fill to the 1/2 mark with water; add ice in order to lower the temperature to about 0°C. Note the room temperature. Observe the NO2 thoroughly at room temperature. Place the sealed NO2 tube in the cold bath. Note your observations. Remove the test tube from the cold bath. Let the test tube stand until it reaches room temperature. Note your observations. Place the test tube in the hot bath. Note your observations. Remove the test tube from the hot bath. Let the test…
I submitted these responses and they were incorrect. Are there any other suggestions?
After performing precipitation gravimetry, Asta placed the weighing form inside the crucible, heated it, cooled it down, and weighed the crucible with the weighing form and obtained a mass of 23.4120 g. Repeating this cycle continuously gave a mass of 23.2125 g, then 23.1136 g, then 23.1139 g. Which among these masses should he use for his calculations? 23.1136 g 23.2125 g 23.4120 g 23.1139 g
A 1.00 L bottle of wine, labeled as 8.5% (by volume) ethanol, is found to have a defective seal. Analysis of 1.00 mL showed that there were 0.0274 grams of acetic acid in that 1.00 mL. The density of ethanol is 0.816 g/mL and the density of water is 1.00 g/mL. What mass of oxygen must have leaked into the bottle? I'm pretty good with conversions and molarity and stuff but I mainly need to know how to even go about answering this question.
One of the reactions in the Solvay Process involves the reaction of calcium oxide with water toproduce slaked lime (calcium hydroxide).CaO(s) + H O2 (l) - Ca(OH)2 (s)A lab technician performs the experiment and uses 54.8 g of calcium oxide to react with a setamount of water. When the reaction is completed, the technician uses a filtration apparatus tocollect the mass of calcium hydroxide produced. The following data is recorded:Mass of filter paper: 1.24 gMass of filter paper and solid: 68.04 g What is the theoretical mass of calcium hydroxide that is predicted to be produced? What mass of precipitate was collected in this experiment? What is the percent error? Comment on the validity of the results
I just want the Calculation. EXPERIMENT: ESTIMATION OF TOTAL SUSPENDED SOLID AND TOTAL DISSOLVED SOLID IN WATER SAMPLE (TSS) Aim: To determine the amount of Total suspended solid and Total Dissolved Solid in the given water sample. Apparatus & Chemicals: weighing balance, filter paper, heater, oven, glassware, distill water, Chemicals: unknown water samples Theoretical Background: …. Observation table for TSS: Sr no Sample Volume (ml) Weight of Filter paper and dry residue in (mg) [As] Weight of Filter paper in (mg) [Bs] 1 50 133 122 2 50 124 114 Observation table for TDS: Sr no Sample Volume (ml) Weight of Crucible and dry residue in (mg) [Ad] Weight of Crucible in (mg) [Bd] 1 50 7566 7506 2 50 8774 8710 Calculation: TSS in mg / lit or ppm = (As-Bs)*1000 / volume of sample in ml TDS in mg / lit or ppm = (Ad-Bd)*1000 / volume of sample in ml Result & discussion: Precautions: References: