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- A 19.51 ݃ sample of impure methylamine, which contains 72.58% (by mass) of CH3NH2 , isreacted with 30.81 ݃ of pure oxygen gas:4CHଷNHଶ(g) + 9Oଶ(g) ⟶ 4COଶ(g) + 10HଶO(ℓ) + 2Nଶ(g) In another experiment, this impure methylamine was used as follows: An unknown mass of the impure compound is dissolved in enough water to make 500.0 ݉ܮof solution. 20 ݉ܮ of this solution was transferred by pipette to a clean 250 mL volumetric flask andmade up to the mark. The molarity of the CH3NH2 in the final solution was determined to be 0.103 M.Determine the mass of CH3NH2 present in the original amount of impure compound used tomake this solution.What is the concentration of a 62.0 % (w/w) concentrated nitric acid (HNO3, Mr = 63.0 g/mol) solution (density: 1.32 g/cm3) in mol/dm3 (molarity) and g/dm3 (mass concentraion) units?Sodium carbonate is a reagent that may be used to standardizeacids in the same way. In such standardization it was found that a 0.432-g sample ofsodium carbonate required 22.3 mL of a sulfuric acid solution to reach the end point forthe reaction.Na2CO3(aq) + H2SO4(aq) -----> H2O(l) + CO2(g) + Na2SO4(aq)What is the molarity of the H2SO4?
- Mg +2HCL > Mg cl2 +H2 If 1.505×10 exponent 23 particles of Mg react with 300ml 0.9mol.dm3 solutions of HCl Determine the limiting reagentTo prepare a very dilute solution of K2Cr2O7 (294.18 g/mol), 0.661 g of K2Cr2O7 was transferred to a 250.0-mL volumetric flask and adding water to the mark. A sample of this solution of volume 1.000 mL was then transferred to a 500.0-mL volumetric flask and diluted to the mark with water. Subsequently, 10.0 mL of the diluted solution was transferred to a 250.0-mL flask and diluted to the mark with water. What is the final concentration of K2Cr2O7 in this last solution?A 25.00 cm3 solution containing Ni2+ was treated with an excess of an ammoniacal solution of dimethylglyoxime (dmgH2) and 0.7223 g of Ni(dmgH)2 was precipitated. What is the molarity of Ni2+ in the solution in mol dm–3? [Mr / g mol–1: Ni(dmgH)2 = 288.9149] a. 1.000 × 10–3 mol dm–3 b. 1.00 × 10–1 mol dm–3 c. 1.0 × 10–1 mol dm–3 d. 1.000 × 10–1 mol dm–3 e. 1.0 × 10–3 mol dm–3
- A sample of pure sodium oxalate weighing 0.1050 g is ignited [Na2C2O4 (s) --> Na2CO3 (s) + CO (g)] and the resulting product requires 15.00 mL of a solution of H2SO4 for complete neutralization. What is the normality of the acid? MM of Na2CO3 = 106.0 g/molMM of Na2C2O4 = 134.0 g/molMM of CO = 28.01 g/molMM of H2SO4 = 98.08 g/molCalculate the limiting and excess reagent of 3I2 + 6KOH → 5KI + KIO3 + 3H2O with solutions. 950g=I2, 1500g=KOH25 ppm of CaCO3 was found in the water sample obtained on the lake in the nearby town.Calculate the moles of CaCO3 having a molar mass of 100.09 g/mol in 10 liters of water samplesolution having a density of 997 kg/m3. (Ans.: 24.95 moles CaCO3)
- 1. What mass of MC| is needed to make 3000g or 109 solution? (MW: H= 1 , Cl= 35)a. 0.09 gb. 90 gc. 900 g d. 0.9 g 2. Detemine the mole faction of the solvent in a solution prepared by dissolving: 36g of CH3OH in 1000 of H2O. a. 55.55molesb. 0.02molesc. 0 98molesd. None of the aboveWhat volume of 0.10 moldm-3 sulphuric acid would be required to neutralise a mixture of 1.06 g of anhydrous sodium carbonate and 4.00 g of sodium hydroxide? (H2SO4 + 2NaOH ---> Na2SO4 + 2H2O) and (H2SO4 + Na2CO3 ® ---> Na2SO4+ H2O + CO2)What mass of Na2SO4 is necessary to fully react with 25 L of .01M of PbCl2 solution? PbCl2(aq)+Na2SO4(s) --> 2NaCl (aq) + PbSO4(aq)