A solution was made by mixing benzene ( C6 H6) and carbon tetrachloride ( CCL). Given that the mole fraction of carbon tetrachloride is 0.837 in the solution obtained from 22.9 g CCI4, calculate the mass of benzene used. Mass =
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- A student carried out the synthesis of aspirin as described using 3.00 g of salicylic acid and 6.0 ml. of acetic anhydride and obtained 1.306 g of aspirin. (a) Calculate the amount of salicylic acid used in moles: (salicylic acid molar mass: 138.12 g/mol) (b) Calculate the mass (g) of acetic anhydride used: (acetic anhydride density: 1.08 g/cm³, Molar mass: 102.09 g/mol) (c) Calculate the amount of acetic anhydride used in moles: (d) Which one is the limiting reactant?Mass of Na2CO3=5g Mass of CaCl2=4.98g Mass of filter paper=1.11g Na2CO3 and CaCl2 combined, filtered, and dried overnight. The mass of the solid produced = 2.86g Calculate the theoretical yield of solid expected and the percent yield obtained.Given: 0.35g NaCl, 0.25 g NaHCO3, 0.15 g KCl & 2 g C6H12O6 are present in 100 mL ORS solution (MW: Na: 23, K: 39, Cl: 35, H: 1, C: 12, O: 16) a. Calculate the total amount of glucose expressed in mmol/L present in the prepared solution b. Calculate the total amount of sodium expressed in mmol/L present in the prepared solutionc. c. Calculate the total amount of potassium expressed in mmol/L present in the prepared solution a 111.11 mmol/L b 90.10 mmol/L c 80.61 mmol/L d 60.34 mmol/L e 29.76 mmol/L f 20.27 mmol/L
- 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?Concentrated sulfuric acid has a density of 1.84 g/cm3 and is 95.0% by mass H2SO4. (Hint: assume a basis of 1.00 L of solution) a) What is the mass fraction of sulfuric acid in the solution? b) What is the molarity of this acid?Please answer question 2: Instructions attached below .2. A 48.33-mL sample of 0.150 M NaBr is titrated into 50.00 mL of 0.145 M AgNO3. Bothsolutions had the same initial and final temperatures. The reaction occurred in a calorimeterwith a known heat capacity and produced 1546.03 J of heat.i. Write a balanced equation that is occurring.ii. Determine the theoretical yield of the solid.iii. Calculate the enthalpy of the reaction (kJ/mole of precipitate).
- Recently a team from Clarkson University discovered a porous solid called NU-1000, constructed from Zr, C, O, and H, excels at removing poly- and perfluoroalkyl species (aka PFAS) from water. The density of this material is 0.486 g/cm³ and its surface area is 2255 m²/g. If 50.0 g of this material is placed in water, calculate the total area (in cm²) of this sample. DONT GIVE ANY TYPE OF IMAGE IN ANSWER OTHERWISE I WILL GIVE INCORRECT ANSWER DON'T GIVE HANDWRITTEN SOLUTIONMost to least soluble ba2+ ca2+ mg2+ sr2+Prepare 1500mL of 0.5N H2SO4 solution with specific gravity of 1.84g/mL and assay of 97%. Write the complete formula and solution in a padpaper
- A 0.3000 g of Na3PO4 (163.94 g/mol) is dissolved in water and diluted to 100.0 mL. A. Calculate the ppm Na+ (23.00 g/mol) in the solution B. If 50.00 mL of the Na3PO4 solution is mixed with 50.00 mL solution of 0.0200 M Ca(NO3)2, calculate the mass of Ca3(PO4)2 (310.177 g/mol) that could be obtained.Describe the preparation of a 700 mL of 4.36% (w/v) aqueous ethanol (C2H; OH, 46.1 g/mol). Weigh ___ g ethanol and add enough water to give a final volume of ____ mL. 700 g of 4.36% (w/w) aqueous ethanol. Mix ____ g ethanol with ____ g water. 700 mL of 4.36% (v/v) aqueous ethanol. Dilute ____ mL ethanol with enough water to give a final volume of ____ mL.Give the molar concentration of HCl with a specific gravity of 1.18 and has 37.0 % (w/w) purity. (Atomic mass: H = 1.01 amu; Cl = 35.45 amu)