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describe how you can prepare 500mL of 0.10 M Fe2O3 (159.69g/mol) from the primary-standard-grade solid.
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- 3.A sample is known to contain NaOH, Na2CO3 NaHCO3 or compatible mixture of these together with inert matter. With methyl orange, a 1.100 g sample requires 31.40 mL of HCl ( 1.00 mL is equivalent to 0.0140g CaO). With phenolphthalein indicator, the same weight of sample requires 13.30mL of the acid. What is the percent composition of the sample? ww ww3.A sample is known to contain NaOH, NA2CO3 NaHCO3 or compatible mixture of these together with inert matter. With methyl orange, a 1.100 g sample requires 31.40 mL of HCI ( 1.00 mL is equivalent to 0.0140g CaO). With phenolphthalein indicator, the same weight of sample requires 13.30mL of the acid. What is the percent composition of the sample?Iron (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.…
- If 0.750 L of a 0.0010 M of AgNO3 is added to 0.500 litre of a 0.00050 M solution of CaF2, what is the concentration of each ion after mixing? A solution of Ca (NO) is added to a solution of NazCO. Write down the balanced 3 reactions showing what happens in solution. What is the precipitate? A solution of Pb(CH COO) is added to a dilute solution of MgSO4. Write down the balanced 3 reactions showing what happens in solution. What is the precipitate?What mass of NaOHNaOH is needed to precipitate the Cd2+ ions from 30.0mL of 0.500 M Cd(NO3)2 solution?The apparent solubility products of AgCN and PBF2 at 25°C are 6.0x10¬1/ and 3.3x10-8, respectively. Calculate the solubility (g/100. g of solution) of these compounds. (Assume each solution has a density of 0.99705 g·cm-3.) solubility of AgCN 4.0 g/100. g of solution solubility of PbF2 4.0 g/100. g of solution
- A buffer is prepared using lactic acid (HLac) and sodium lactate (NaLac). 0.300 dm3 of the 0.500 mol·dm–3 HLac solution is mixed with 0.300 dm3 of the 0.300 mol·dm–3 NaLac solution to prepare the buffer. Ka for lactic acid (HLac) is 1.4 x 10-4 a) Calculate the pH of the lactic acid before it is mixed with the NaLac to form the buffer. b) Calculate the pH of the sodium lactate solution before it is mixed with the HLac to form the buffer. c) Calculate the pH of the buffer solution.1. Determine the mass of CaCl2·2H2O (MW 147.02 g/mole) to weigh out using a four- place analytical balance to prepare 100 mL of a 0.1005 M solution of Ca2+. 2. Determine the mass of KCI to weigh out using a four-place analytical balance to prepare 100 mL of a 1 M solution of KCI (MW 74.5513 g/mole). 3. Record the solubility of calcium carbonate in water (mg/L) in your notebook. 4. Calculate the amount of calcium carbonate (mg) not in solution if a tablet is dissolved in 250 mL of water and the tablet's label claim is 600 mg calcium / tablet.A buffer is prepared using lactic acid (HLac) and sodium lactate (NaLac). 0.300 dm3 of the 0.500 mol·dm–3 HLac solution is mixed with 0.300 dm3 of the 0.300 mol·dm–3 NaLac solution to prepare the buffer. Ka for lactic acid (HLac) is 1.4 x 10-4 a) Calculate the pH of the lactic acid before it is mixed with the NaLac to form the buffer. b) Calculate the pH of the sodium lactate solution before it is mixed with the HLac to form the buffer. c) Calculate the pH of the buffer solution. d) What will the pH of the above solution be after 5.0 cm3 of 0.200 mol·dm–3 NaOH has been added to only 100.0 cm3 of this buffer?
- The apparent solubility products of AgCN and PbF2 at 25°C are 6.0x10-1/ and 3.3×10¬8, respectively. Calculate the solubility (g/100. g of solution) of these compounds. (Assume each solution has a density of 0.99705 g·cm-3.) 4.0 solubility of A9CN g/100. g of solution solubility of PBF2 4.0 g/100. g of solutionSolution 1) 50.00mL of a solution containing 0.15M malonic acid, CH2(CO2H)2, and 0.020M manganese (II) sulfate, MnSO4. Calculate the mass (in grams) of manganese(II) sulfate monohydrate required to prepare solution 1. Your answer should have 2 sig figs.A mixture containing only KCl and NaBr is analyzed by the Mohr method. A 0.3172-g sample is dissolved in 50 mL of water and titrated to the Ag,CrO4 end point, requiring 36.85 mL of 0.1120 M AgNO3. A blank titration requires 0.71 mL of titrant to reach the same end point. Report the %w/w KCl and NaBr in the sample.
