Organic carbon in seawater can be measured by oxidation to CO2 with K2S2O8, followed by gravimetric determination of CO2 trapped by a column of Ascarite. Water weighing 6.234 g produced 2.378 mg of CO2 (FM 44.010). Find ppm carbon in the seawater.
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Organic carbon in seawater can be measured by oxidation to CO2 with K2S2O8, followed by gravimetric determination of CO2 trapped by a column of Ascarite. Water weighing 6.234 g produced 2.378 mg of CO2 (FM 44.010). Find ppm carbon in the seawater.
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- Organic carbon in seawater can be measured by oxidation to CO2 with K2S2O8, followed by gravimetric determina- tion of CO2 trapped by a column of Ascarite. Water weighing 6.234 g produced 2.378 mg of CO2 (FM 44.010). Find ppm carbon in the seawater.4) How would your calculated value of Kup be affected by errors introduced from the following sources? Be specific in your answer. State whether Ksp would be too large, too small, or not affected, and explain why that error would have that effect on Ksp c. Although the KIOs used to standardize the Na2S20s is labeled as 0.0100 M, its actual concentration is somewhat higher than 0.0100 M. d. Extraneous water is introduced from wet filter paper or wet funnels, or by washing the precipitate during the final filtration of Ca(IOs)2.A weight of 0.50 g was taken impure container containing sodium carbonate and bicarbonate. Dissolved in water and then crushed with hydrochloric acid (0.1 N), the burette reading game was at the endpoint of phenolphthalein of 10.5 ml and at the end point of the orange methylation point 30.1 ml. The percentage of sodium carbonate was in ................. knowing that the weights are: Na: 23, C: 12, O: 16
- Consider the titration illustrated in Figure 8.] Anhydrous sodium carbonate (Na₂CO₃) is a primary standard. When 0.364 grams of the substance is placed in a conical flask, then 20.00 cm³ of sulphuric acid (H₂SO₄) solution is required to reach the end point of the titration. What is the concentration in mol·dm⁻³ of the sulphuric acid solution? [Give the answer to 3 decimal places. Do not type in the unit. Use a decimal point.] *1. What is the MW of the analyte?2. What is the meq of the analyte?3. What is the weight (in grams) of the analyte?4. What will be the percentage purity of the sample if 43mL of the titrant was consumed?5. Did the sample conform to the USP requirement? Yes or No?one or more answers Which of the following will result in an increase in the calculated Ksp of Ca(OH)2? Receiving flask used during filtration was contaminated with HCl The Na2CO3 primary standard solution was overtitrated The saturated Ca(OH)2 solution was overtitrated Some Ca(OH)2 solid passed through the filter paper during filtration The water used to dissolve Ca(OH)2 solid was greater than the required amount
- 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.Laura and Sebastian create an aqueous solution of Ba(OH)2 by pipetting 25.00 mL of 0.0970 M Ba(NO3)2 into an Erlenmeyer flask and that contains 25.00 mL of 0.105 M KOH. a) Calculate the molar concentrations of Ba2+(aq) and OH1-(aq) in their 50.00 mL solution. b) Use the molar concentrations of Ba2+(aq) and OH1-(aq) as determined above and the Ksp to show why a precipitate does not form. You must include a calculation as part of your answer. The value of Ksp for Ba(OH)2, is 5.0 x 10-3. c) Laura adds solid KOH to their solution of Ba(OH)2 until the hydroxide concentration, [OH1-], becomes 0.200 M. Assuming that the volume of the solution does not change, does the molar concentrations of Ba2+(aq) increase, decrease or remain the same? justify your answer.Chemistry 1. If your 10 g sample contains 200 µg H2O, calculate the water concentration of your sample in ppm (i.e., µg water per g of sample)? Do not include units in your numeric answer. 2. Calculate the water content of your tablet sample (specimen) as a % wt/ wt: Given: 4g tablet sample was weighed, and S (= KFR volume consumed by sample during titration) = 6.00 mL Submit your answer to 2 decimal places. Do not include the % symbol; only numeric values allowed in your answer.
- Chemistry One litre of aqueous sample containing the organic pollutant, polychlorinated biphenyl (PCB), was brought to a lab for analysis. Two extractions each with 50 ml of fresh organic solvent were performed. On analysis of the aqueous phase after the first extraction, the concentration of PCB was 10 µg/ml. After the second extraction with fresh organic solvent, the concentration of PCB in the aqueous phase was 0.6 µg/ml. Determine the distribution ratio of PCB under these conditions2 what is the purpose of BSC Level 1 & 2, proper layout, performance, and its application in biosafety assessmentChemistry The levels of an organic pollutant (P) in the groundwater at the perimeter of a plant were a cause for concern. A 10 mL sample of the water was taken and the pollutant was extracted with 95% efficiency using 25 mL of diethyl ether. GC was used to analyse the concentration of P in diethyl ether. A calibration curve was plotted for a series of standards of P which yielded the following results: Peak Area Toluene Conc. (µg/ml) 12,000 2.6 23,700 5.0 35,500 7.7 46,800 9.9 31,250 Sample Determine the concentration of P in ppb in the initial groundwater sample.