Q1. A 100 g soil containing 20% smectitie mineral matter was mixed with 150 mL solution containing 0.10 M Pb2+. CEC of pure smectitie is 110 cmol(+)/kg. CEC of the soil (cmol(+)/kg) is:
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- A 100 g soil containing 20% smectitie mineral matter was mixed with 150 mL solution containing 0.10 M Pb. CEC of pure smectitie is 110 emol(+)/kg. CEC of the soil (cmol(+)/kg) is:The %purity of a powdered crude sample of Na2CO3 containing only inert impurities is to be determined by reacting 225.0 mg of the crude sample to 10.0 mL of 3.00 M HCl solution, and bubbling the resulting CO2(g) product in water that is at exactly 29 °C. After the reaction has completed, the level of the liquid inside the eudiometer rests 4.30 cm above the water level in the beaker. The graduation on the eudiometer indicates that the trapped gas is 44.37 mL. The experiment was done under a barometric pressure of 755.2 torr. a. How many moles of CO2 were collected? b. What is the percent purity of the sample? Round off to the nearest whole numberThe %purity of a powdered crude sample of Na2CO3 containing only inert impurities is to be determined by reacting 225.0 mg of the crude sample to 10.0 mL of 3.00 M HCl solution, and bubbling the resulting CO2(g) product in water that is at exactly 29 °C. After the reaction has completed, the level of the liquid inside the eudiometer rests 4.30 cm above the water level in the beaker. The graduation on the eudiometer indicates that the trapped gas is 44.37 mL. The experiment was done under a barometric pressure of 755.2 torr. What CASE does this experiment satisfy?
- A 25.00mL wastewater sample was analyzed for its Mg2+ content using a standard gravimetric method. the sample was diluted to 3.00L and an 11.00mL aliquot was treated to precipitate magnesium as MgNH4PO4.6H2O using (NH4)2HPO4 as the precipitating agent. the precipitate was then filtered, washed, dried, and ignited resulting in a 0.1325mg Mg2P2O7 residue. How much Mg (in ppm) is present in the original sampleThe % purity of a powdered crude sample of Na^2CO^3 containing only inert impurities is to be determined by reacting 225.0 mg of the crude sample to 10.0 mL of 3.00 M HCl solution, and bubbling the resulting CO2(g) product in water that is at exactly 29 °C. After the reaction has completed, the level of the liquid inside the eudiometer rests 4.30 cm above the water level in the beaker. The graduation on the eudiometer indicates that the trapped gas is 44.37 mL. The experiment was done under a barometric pressure of 755.2 torr. Write the balanced chemical equation of the reaction in your solutions sheet. What is the sum of all the coefficients of the balanced chemical equation? Determine the pressure of the trapped gas inside the eudiometer in mmHg. Determine the partial pressure of the collected CO^2 in mm Hg. How many millimoles of CO^2 was collected? What is the % purity of the sample to the nearest whole number?The % purity of a powdered crude sample of Na^2CO^3 containing only inert impurities is to be determined by reacting 225.0 mg of the crude sample to 10.0 mL of 3.00 M HCl solution, and bubbling the resulting CO2(g) product in water that is at exactly 29 °C. After the reaction has completed, the level of the liquid inside the eudiometer rests 4.30 cm above the water level in the beaker. The graduation on the eudiometer indicates that the trapped gas is 44.37 mL. The experiment was done under a barometric pressure of 755.2 torr. What is the % purity of the sample to the nearest whole number?
- Prepare 1500mL of 0.5N H2SO4 solution with specific gravity of 1.84g/mL and assay of 97%A empty evaporating dish weighs 30.56g. You place 20.0mL of an NaCl solution in the dish plus the solution weighs 53.31g. You evaporatorate the solution to dryness ant find that the evaporatoring dish plus the residue weighs 32.25g. What is the w/v%? What is the w/w%? What is the molarity?Suppose you have a soil that is made up of 10% organic matter with CEC = 200 cmol/kg, 40% kaolinitewith CEC = 10 cmol/kg, and 50% vermiculite with CEC = 100 cmol/kg.1- Calculate the overall CEC of the soil by taking a weighted average of the three soil components.2- What percentage of the overall CEC is contributed by the organic matter? How does that numbercompare to the 10% of the soil itself that is organic?
- 20 aspirin tablets labeled 80mg were dissolved in 100mL of 90% ethanol. A 10mL aliquot was taken and was used for assay. The analyte followed usual process and was treated with 50mL of 0.1000N NaH and was titrated with 35mL 0.1050N H2O4 until the solution achieved completion. Calculate the % content of the total aspirin capsules and the actual label claimThe concentration of purified OXA-M290 is tested with a BCA assay. Serial dilutions of a bovine serum albumin (BSA) stock solution are prepared, then pipetted into a 96-well plate; each dilution of the BSA standard is tested in triplicate. Then, bicinchoninic acid and Cu2+ ions are added to all of the wells of the plate. After incubating the plate for 1 hour, a microplate reader is used to measure the absorbance of all of the wells in the plate at 560 nm. This generates the following data: BSA conc. (μg/mL), Replicate 1 Absorbance, Replicate 2 Absorbance, Replicate 3 Absorbance 40, 1.360, 1.403, 1.481 20, 0.750, 0.745, 0.810 10, 0.380, 0.344, 0.398 5, 0.198, 0.160, 0.183 2.5, 0.090, 0.100, 0.085 1.25, 0.038, 0.043, 0.051 0.625, 0.024, 0.028, 0.019 Prepare a calibration curve using these data. You can use Excel, R, SPSS or an equivalent graphing software. In this graph, plot absorbance (y-axis) against the concentration of the protein standard (x-axis). Calculate and plot…A spent 1.0 percent caustic soda solution (ρNaOH = 8.42 lb/gal) with a volumetric flow rate of 3.0gpm is to be neutralized using either sulfuric acid or hydrochloric acid. First, determine the massflow rate (lb/day) of NaOH in the spent caustic soda solution, and then use that value todetermine the stoichiometric amounts (lb/day) of:1. H2SO4 required for neutralizing the OH− ions contributed by the spent caustic soda.[Hints: (1) write the balanced chemical equation for the acid-base reaction betweenNaOH and H2SO4, and use it to establish the stoichiometric weight ratio H2SO4 : NaOH.]2. HCl required for neutralizing the OH− ions contributed by the spent caustic soda. [Hints:(1) write the balanced chemical equation for the acid-base reaction between NaOH andHCl and use it to establish the stoichiometric weight ratio HCl : NaOH.]
