500 mL of river water was subjected to sulfate determination by the barium gravimetric method. The final weight of the precipitate was 74.3 mg. What was the sulfate concentration in mg/L?
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500 mL of river water was subjected to sulfate determination by the barium gravimetric method. The final weight of the precipitate was 74.3 mg. What was the sulfate concentration in mg/L?
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- In order for all of the analyte to be consumed completely, an excess of a reagent has to be added. If 10.00 mL of a 0.1000 M HCl is needed in the back titration, what volume of a 0.5000 M NaOH should be added to a sample that contains 2.000 mmol of aspirin1.00 grams of table salt was dissolved in 100 mL water and excess AgNO3 reagent was added and yielded 2.3789 grams of precipitate. Calculate the percentage of NaCl in the table salt.What will be the molar analytical concentration of Na2co3 in the solution produced when 25.0 ml of 0.200 M agno3 is mixed with 50.0 ml of 0.0800 M na2co3 ?
- If the original sodium tartrate solution had a concentration of 1.00 M instead of 0.100 M, what would the concentration of copper be in a solution created by combining 10 mL of it with 10 mL of the 0.100M copper (II)sulfate solution. Ksp = 6.10E-4Iron (55.845 g/mol) can be determined gravimetrically by precipitation as Fe(OH)3 (106.867 g/mol) and subsequent inflammation of the precipitate to convert it to Fe2O3 (159.69 g/mol). A 0.7873 g sample to be analyzed was weighed and transferred to a 400 mL beaker, where it was dissolved in 50 mL of H2O and 10 mL of 6M HCl. Then 2 mL of concentrated HNO3 was added to the solution. After boiling to remove excess HNO3 and nitrogen oxides, the solution was diluted to 200 mL, brought to boiling, and Fe(OH)3 was precipitated by the slow addition of 1:1 NH4OH solution until an odor of NH3 was detected (indicating the presence of excess NH3 in the medium). The solution was left in a water bath at 80 ºC for 30 min at rest. The precipitate was then filtered and washed with several portions of hot 1% m/v NH4NO3 until no Cl– was detected in the wash water. Finally, the precipitate was ignited at 500-550 °C, then left in a desiccator to cool and weighed as Fe2O3, resulting in a mass of 0.4512 g.…Which of the following conditions would lead to an increase in the relative supersaturation of a solution during precipitation gravimetry? a. decrease in temperature b. slow addition of precipitating agent c. precipitation from a hot solution d. vigorous stirring
- 3) When excess sliver nitrate was added to 25.00 ml of barium chloride, a precipitate of sliver chloride formed at the bottom of the beaker. If the mass of the precipitate was 4.30g, calculate the initial concentration of barium chloride.In order to adjust the Potassium Permanganate solution, 0.0544g Na2C2O4 was taken and necessary experimental procedures were performed on it and the titrant consumption was found to be 7.9 mL. What is the KMnO4 concentration?1.00 grams of table salt was dissolved in 100 mL water and excess AgNO3 reagent was added and yielded 2.3789 grams of precipitate. Calculate the percentage of NaCl in the table salt. Answer must be in 2 significant figures.