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- How many grams of CaF2 (molar mass 78.077) will dissolve in 250 mL of 0.20 M NaF solution? The Ksp for CaF2 is 3.8904e-11.A 50.00 mL solution containing NaBr was treated with excessive AgNO3 to precipitate 0.214 6g of AgBr (FM 187.772). What was the Molarity of NaBr in the solution?A 20 mL volume of 0.015 M KIO3 containing an excess of KI, is added to a 0.312 g sample of a Real Lemon solution containing vitamin C. The Yellow-brown solution, caused by excess I2 is titrated to a colorless starch endpoint with 11.3 mL pf 0.106M Na2S2O3. Question: How many moles of I2 reacted with vitamin C in the Real Lemon sample?
- A 50.00-mL solution containing NaBr was treated with excess AgNO3 toprecipitate 0.214 6 g of AgBr (FM 187.772). (a) How many moles of AgBr product were isolated? (b) What was the molarity of NaBr in the solution?A saturated solutionA.cannot be attainedB. contains no double bondsC. contains as much solvent as it can holdD. will rapidly precipitate if a seed crystal is addedE. contains dissolved solute in equilibrium with undissolved soluteQuestion: How do you expect solubility of potassium bitartrate to vary between solutions with and without KNO3?
- A 0.4671 g sample containg NaHCO₃(Mwt=84.01mg/mmol) was dissolved and titrated with 0.1067 M HCl requiring 40.72 ml, find the percentage of NaHCO₃, in the sampleA 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: 16You have a sample of approximately 100 mg/L of calcium carbonate and the standardized EDTA has a concentration of 0.00085 M. If you only want to spend approximately 15 mL of the titrant and add 25 mL of sample in the Erlenmeyer flask, can you use it or should you dilute it? the sample?, how much? Solution: No, 29 mL would be needed to titrate the sample, you must dilute it approximately 1: 2. Taking, for example, 25 mL of sample and making up to 50 mL.
- The solutbility constant for Ce(IO3)3 is 3.2x10^-10. What is the Ce3+ concentration in a solution prepared by mixing 50 mL of 0.0450 M Ce3+ with 50 mL of: A.) 0.0450 M IO3- ? B.) 0.0500 M IO3- ?To find the Ce4+ content of a solid, 4.37 g were dissolved and treated with excess iodate to precipitate Ce (IO3)4. The precipitate was collected, washed well, dried, and ignited to produce 0.104 g of CeO2 (FM 172.114). What was the weight percent of Ce in the original solid?6. A 100mLSolution containing 0.145g of NiCl2 was supplied in the lab. Students were advised to use 5mL of this solution for gravimetric determination of Ni. The density of solution = 1g/mL Mass of precipitate was calculated to be .0291g and .0353g for two trials of the experiment. Calculate the average amount of Ni in unit ppm (parts per million). Gf = .2031