Gravimetric Analysis. Please show complete solution. Thank you 1.) A 0.8870 g sample containing only NaCl and KCl was treated with AgNO3. TheAgCl formed had a mass of 1.913 g. Calculate the %Na and %K in the sample.
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Gravimetric Analysis. Please show complete solution. Thank you
1.) A 0.8870 g sample containing only NaCl and KCl was treated with AgNO3. TheAgCl formed had a mass of 1.913 g. Calculate the %Na and %K in the sample.
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- 148. Addition of 50.00 mL of 2.238 m H2SO4 (solution density = 1.1243 g/mL) to 50.00 mL of 2.238 M BaCl2 gives a white precipitate. (a) What is the mass of the precipitate in grams? (b) If you filter the mixture and add more H2SO4 solution to the filtrate, would you obtain more precipitate? Explain.In an impure sample of table salt that weighed 0.8421 g when dissolved in water and treated with excess AgN03 formed 2.044 g of AgCl. Listing the percentage of NaCl is in the impure sample. What is the list of three sources of error in this experiment?Fifty food supplement tablets with a total mass of 66.393 g were crushed into powder to analyse the content of FeSO4·7H2O. 2.988 g of the powder were dissolved in HNO3 and heated to convert all the iron to Fe3+. Addition of aqueous NH3 caused quantitative .precipitation of Fe2O3· X H2O, which was ignited to give 0.0640 g of Fe2O3. Determine the average weight of FeSO4·7H2O in each tablet.
- Fifty food supplement tablets with a total mass of 66.393 g were crushed into powder to analyse the content of FeSO4·7H2O. 2.988 g of the powder were dissolved in HNO3 and heated to convert all the iron to Fe3+. Addition of aqueous NH3 caused quantitative precipitation of Fe2O3·xH2O, which was ignited to give 0.0640 g of Fe2O3. Determine the average weight of FeSO4·7H2O in each tablet.Masses : Ca = 40.08 g S= 32.07 g O= 16.00 g A 35.0 mL sample of CaSO4 was evaporated to dryness, leaving 0.967 g of residue. What was the molarity of the original solution? step by step pleaseShow your complete solution and round-off your answers to four decimal places. A 0.1093-g sample of impure Na2CO3 was analyzed by the Volhard method. After adding 50.00 mL of 0.06911 N AgNO3, the sample was back titrated with 0.05781 N KSCN, requiring 27.36 mL to reach the end point. Calculate the % purity of the Na2CO3 sample. Answer = _% Na2CO3
- Please answer this NEATLY, COMPLETELY, and CORRECTLY for an UPVOTE. Ni(NO3)2From the stock solution (1.0 M), determine the volume needed to prepare 0.00, 0.04, 0.08, 0.12 and 0.16 M Ni(NO3)2 solution in 50 mL volumetric flask. Obtain the calculated amounts, place in corresponding volumetric flasks and dilute to mark.An unknown sample weighing 1.5098 g was acidified with 3.0 M H2SO4 to dissolve the copper compounds and diluted with 30 mL distilled water. This was followed by the addition of excess KI producing I2 and CuI precipitate from Cu2+ (Reaction 1). Then, the liberated I2 reacted with the excess KI forming triiodide anion (Reaction 2), which was then titrated with Na2S2O3 titrant (Reaction 3). This entire solution required 17.60 mL of the titrant to reach the starch end point. What are the balanced chemical equations for reactions 1-3? What is the mole ration between Cu2+ and S2O32-?The ingredients in herbicides and pesticides must be carefully monitored. Arsenic in a pesticide sample was precipitated as MgNH4AsO4 (molar mass = 181.25 g/mol). This was heated to form the more stable Mg2As2O7 (molar mass = 310.45 g/mol). Based on the following data, what is the numeric value of the gravimetric factor for the sample?
- Sample: Saline 0.900% (m/v), in sodium chloride (NaCl). Data: M.A. (g/mol): Na = 22.9898; K = 39.0983; Cr=51.9961; Ag = 107.8682; Cl = 35.453; N=14.0067; O = 15.9994. Material available in the laboratory's warehouse: Reagents: distilled water; standardized solution of silver nitrate (AgNO₃), at a concentration of 0.09980 mols/L; Potassium chromate solution (K₂CrO₄) 1%; ammoniacal ferric alum solution [Fe(NH₄)(SO₄)₂] and; nitrobenzene (or cooking oil, alternatively); 0.1000 mols/L potassium thiocyanate (KSCN) standard solution. Glassware: beakers of all sizes available on the market; 50, 100, 150, 200 and 250 ml Erlenmeyers; 10.00 and 25.00 mL volumetric pipettes; 15.00 mL burette; 30.00, 50.00 and 100.00 mL volumetric flasks Calculate the molarity of saline, in terms of the NaCl concentration (concentration in mols/L). (a) 0.900 mols/L (b) 5.84 mols/L (c) 0.154 mols/L (d) 0.0154 mols/LA stock solution containing Mn2+ ions was prepaned by dissolving 1.584 g pure manganese metal in nitric acid and diluting to a final volume of 1.000 L. The following solutions were then prepared by dilution: For solution A, 50.00 mL of stock solution was diluted to 1000.0 mL. For solution B, 10.00 mL of solution A was diluted to 250.0 mL. For solution C, I 0.00 mL of solution Bwas diluted to 500.0 mL. Calculate the concentrations of the stock solution and solutions A,B, and C.When standardizing two liters of a potassium permanganate solution, approximately 0.0100 M, with a primary standard solution of sodium oxalate, it was planned to use between 30.00 and 45.00 ml of the titrated reagent. In which mass range (in grams) the primary standard should be weighed?