1. A solution containing 50% KOH is fed at a rate of 1000 mol/h to an evaporator to produce a concentrated solution containing 80%mol KOH. The concentrated solution is then fed to a crystallizer to produce a filter cake containing 90% pure KOH and 10% mother liquor (60% KOH solution). The rest of the mother liquor (60% KOH solution) is recycled back to the evaporator. Determine the values of B, C, P and W. Refer to the figure below. H,0 TW F-1000 mole/ B, 8O% KOH P, S0% pure KOH filter 50% by mole KOH 10% (s0s KOH solution) 60% KOH
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- A concentration of toxic metals in plant tissue is often found by combusting the material in a furnace and then dissolving the ash in concentrated acid. A 0.5124-gram sample of leaves was combusted to ash and transferred to a 150-mL beaker. A 25-mL portion of concentrated HCl was added and the mixture was heated on a hot plate. Three 5-mL portions of concentration HCl were added over approximately 10 minutes with continued heating in between additions. The resulting mixture was cooled to room temperature and filtered into a 50-mL volumetric flask, which was brought to volume using distilled water and mixed well. From this stock solution, a 10-mL portion was pipetted into a clean 50-mL volumetric flask, brought to volume with distilled water, and mixed. This final solution was analyzed and found to contain 12.1 ppm lead. What are the mass percent of lead in the original plant tissue?4.0g of potassium hydrogen tartrate was added to 300mL distilled water. The temperature of the solution is 23.1C. The liquid was filtered and 50mL of the filtered solution was transferred to 250mL beaker, two drops of phenolpthalein was added to the 250mL beaker. The concentration of NaOH is 1.0 M that is filled in the 2mL graduate pipette, single drops of NaOH was added to the 250mL beaker until the solution turns pink and the potassium hydrogen tartrate reach the endpoint. The datd of four trials was collected. Please answer the following questions 4) calculate ksp for potassium hydrogen tartrate for each trial and average ksp for thr experiment 5) calculate the percent error in you value of ksp using reference that is found as the theoretical value. 6) why was the temperature of the saturated solution recorded?4.0g of potassium hydrogen tartrate was added to 300mL distilled water. The temperature of the solution is 23.1C. The liquid was filtered and 50mL of the filtered solution was transferred to 250mL beaker, two drops of phenolpthalein was added to the 250mL beaker. The concentration of NaOH is 1.0 M that is filled in the 2mL graduate pipette, single drops of NaOH was added to the 250mL beaker until the solution turns pink and the potassium hydrogen tartrate reach the endpoint. The datd of four trials was collected. Please answer the following questions 1) calculate the total volume and moles of NaOH required to reach the endpoint for each trial. 2) calculate the molar solubility of potassium hydrogen tartate ( in mol/L) for each trial. 3) calculate the average molar solubility of potassium hydrogen tartate for the four trials. What is the average solubility of potassium hydrogen tartrate in g/L? 4) calculate ksp for potassium hydrogen tartrate for each trial and average ksp for thr…
- An aqueous solution of sodium hydroxide contains 30.0% NaOH by mass. It is desired to produce an 10.0% NaOH solution by diluting a stream of the 30% solution with a stream of pure water. Calculate the ratios (liters H2O/kg feed solution) and (kg product solution/kg feed solution).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 sampleA 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.]
- In an experiment, 0.500 grams of sodium bicarbonate were added to an evaporating dish and an excess of 6.0 M hydrochloric acid was added. The bicarbonate bubbled with the addition of the aqueous HCl. The evaporating dish was gently swirled until the bubbling stopped. The evaporating dish was placed on a hot plate and heated carefully to dryness so that it was completely dry and at constant mass. The amount of sodium chloride obtained from the evaporating dish was 0.114 g. The reaction is given below. NaHCO3 (s) + HCl (aq) ---> NaCl (s) + CO2 (g) + H2O (l) Question: Is the reaction balanced?In an experiment, 0.500 grams of sodium bicarbonate were added to an evaporating dish and an excess of 6.0 M hydrochloric acid was added. The bicarbonate bubbled with the addition of the aqueous HCl. The evaporating dish was gently swirled until the bubbling stopped. The evaporating dish was placed on a hot plate and heated carefully to dryness so that it was completely dry and at constant mass. The amount of sodium chloride obtained from the evaporating dish was 0.114 g. The reaction is given below. NaHCO3 (s) + HCl (aq) ---> NaCl (s) + CO2 (g) + H2O (l) Is the reaction balanced? What was in the bubbles? What were the actual, theoretical, and percent yields of sodium chloride (NaCl)? You must show your work to receive credit.In an experiment, 0.500 grams of sodium bicarbonate were added to an evaporating dish and an excess of 6.0 M hydrochloric acid was added. The bicarbonate bubbled with the addition of the aqueous HCl. The evaporating dish was gently swirled until the bubbling stopped. The evaporating dish was placed on a hot plate and heated carefully to dryness so that it was completely dry and at constant mass. The amount of sodium chloride obtained from the evaporating dish was 0.114 g. The reaction is given below. NaHCO3 (s) + HCl (aq) ---> NaCl (s) + CO2 (g) + H2O (l) What were the actual, theoretical, and percent yields of sodium chloride (NaCl)?
- In an experiment, 0.500 grams of sodium bicarbonate were added to an evaporating dish and an excess of 6.0 M hydrochloric acid was added. The bicarbonate bubbled with the addition of the aqueous HCl. The evaporating dish was gently swirled until the bubbling stopped. The evaporating dish was placed on a hot plate and heated carefully to dryness so that it was completely dry and at constant mass. The amount of sodium chloride obtained from the evaporating dish was 0.114 g. The reaction is given below. NaHCO3 (s) + HCl (aq) ---> NaCl (s) + CO2 (g) + H2O (l) Question: What were the actual, theoretical, and percent yields of sodium chloride (NaCl)?A solid sample contains unknown amounts of potassium and magnesium chloride and moisture. 1.193 g of the sample is dissolved in water and the solution is diluted to 250.00 mL. 25.0 mL of the sample is allowed to pass through an H + -saturated cation exchanger, the eluate consuming 22.03 mL of a 0.100 M NaOH solution. The moisture content of the sample was determined to be 5.22%. Calculate the % by weight of potassium and magnesium chloride in the sample.. The total cation content of natural water is often determined by exchanging the cations for hydrogen ions on an ion exchange resin. The cations are adsorbed to the resin which releases H+ (1:1 exchange) which can then be titrated with a base. A 25.0 mL sample of a natural water is diluted to 100 mL with distilled water and 2.0 g of a cation-exchange resin was added. After stirring, the mixture was filtered and the solid remaining on the filter paper was washed with three 15.0 mL portions of distilled water. The filtrate and washing required 15.3 mL of 0.0202 M NaOH to reach the equivalence pt. Calculate the number of moles of cation present in 1.00 L of sample.