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A: The number of moles of AgNO3 is calculated as shown below. The number of moles of AgNO3 is 0.03 mol.
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A: Welcome to bartleby ! Number of moles = 0.031 moles Volume = 5.97 ml or 5.97 ×10-3 L
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- The aluminum in a 1.200-g sample of impure ammonium aluminum sulfate was precipitated with aqueous ammonia as the hydrous Al2O3.xH2O. The precipitate was filtered and ignited at to give anhydrous Al2O3, which weighed 0.2001 g. Express the result of this analysis in terms of %NH4Al(So4)2 %Al2O3 %AlA plant manufacturing nails and screws uses a large pool (volume = 10,000 L) to collect and treat its residual wastewater before discharging it in a nearby stream. The manufacturing process makes use of a strong acid (HCl) and a weaker one (phosphoric acid, H3PO4; pKa1 = 2.148, pKa2 = 7.20, pKa3 = 12.15), before discharging them in the pool for treatment (neutralization). Once the pool is filled to its maximum capacity, a technician measures the chlorine and phosphorus concentrations in the wastewater to be 0.5 M and 1.0 M, respectively. Assume (i) that chlorine and phosphorus come only from HCl and phosphoric acid, respectively, and (ii) that no H+ was consumed (or neutralized) in the manufacturing process. (a) Knowing that the technician has to bring the pH of the waste water back to a minimum of 7.2 before discharging it in the stream, what is the minimum amount (in kg) of NaOH(s) (40 g/mol) that he has to add to the pool before discharging the waste water in the stream? (b) What…A plant manufacturing nails and screws uses a large pool (volume = 10,000 L) to collect and treat its residual wastewater before discharging it in a nearby stream. The manufacturing process makes use of a strong acid (HCl) and a weaker one (phosphoric acid, H3PO4; pKa1 = 2.148, pKa2 = 7.20, pKa3 = 12.15), before discharging them in the pool for treatment (neutralization). Once the pool is filled to its maximum capacity, a technician measures the chlorine and phosphorus concentrations in the wastewater to be 0.5 M and 1.0 M, respectively. Assume (i) that chlorine and phosphorus come only from HCl and phosphoric acid, respectively, and (ii) that no H+ was consumed (or neutralized) in the manufacturing process.(a) Knowing that the technician has to bring the pH of the waste water back to a minimum of 7.2 before discharging it in the stream, what is the minimum amount (in kg) of NaOH(s) (40 g/mol) that he has to add to the pool before discharging the waste water in the stream?(b) What will…
- Malic acid (C4H6O5) is a dicarboxylic acid that naturally occurs in the production of bignay wine. Maria was tasked to find out the acid content in a 200.0 mL wine sample by titrating it with a standardized solution of KOH. He was able to establish the working concentration of the KOH solution by using 39.12 mL of it to titrate a primary standard of KHP that weighed 3.021 g. The grams and %w/w of Malic acid present in the 200.0 mL wine sample were then determined by titrating a 20.00 mL aliquot using 48.95 mL of the standardized KOH solution. C4H6O5 (aq) + 2KOH (aq) ↔ K2C4H4O5 (aq) + 2H2O (l) Assume the density of the wine sample is 1.000 g/mL MM of KHP = 204.22 g/mol MM of C4H6O5 = 134.0874 g/mol ? What is the molar concentration of the prepared KOH solution?…Malic acid (C4H6O5) is a dicarboxylic acid that naturally occurs in the production of bignay wine. Maria was tasked to find out the acid content in a 200.0 mL wine sample by titrating it with a standardized solution of KOH. He was able to establish the working concentration of the KOH solution by using 39.12 mL of it to titrate a primary standard of KHP that weighed 3.021 g. The grams and %w/w of Malic acid present in the 200.0 mL wine sample were then determined by titrating a 20.00 mL aliquot using 48.95 mL of the standardized KOH solution. C4H6O5 (aq) + 2KOH (aq) ↔ K2C4H4O5 (aq) + 2H2O (l) Assume the density of the wine sample is 1.000 g/mL MM of KHP = 204.22 g/mol MM of C4H6O5 = 134.0874 g/mol What is the molar concentration of the prepared KOH solution?…Write the balanced equation for the reaction of aqueous Pb(ClO3)2Pb(ClO3)2 with aqueous NaI.NaI. Include phases. What mass of precipitate will form if 1.50 L1.50 L of highly concentrated Pb(ClO3)2Pb(ClO3)2 is mixed with 0.100 L 0.250 M NaI0.100 L 0.250 M NaI? Assume the reaction goes to completion.
- 25.0mL of a 0.515 M K2S solution is mixed with 30.0 mL of 0.833 M HNO3 acid solution to give the following reaction: K2S(aq) + 2HNO3(aq) → 2KNO3(aq) + H2S(g) H2S is an unwanted by-product in a pulp and paper industry. To capture H2S gas, it is bubbled through a NaOH solution to produce Na2S with a yield of 94%. H2S(g) + 2NaOH (aq) → Na2S (aq) + 2H2O(l) The mass of H2S(g) that was processed (in kg) if 10.76 kg of Na2S was collected isIf 30.0 mL of an unstandardized NaOH solution is required to react completely with 1.00 g of KHC8H4O4 (KHP), what is the normality of the base?To determine , by gravimetric analysis, the concentration of barium ions (Ba2+) in a given solution, 25.00cm3 of it are pipetted into a beaker and an excess of dilute sulphuric acid is added to it. The precipitate then obtained (BaSO4) is filtered, dried and weighed. The mass of the precipitate is found to be 1.167g Calculate the concentration of barium ions in the solution? (only 2 decimal places). _________Mol/L
- Q3/ The normality of (100 ml) and (1.5 gm) from AgNO3 solution is -------, if you know the atomic weight of Ag=107.8, N=14, O=16.The concentration of arsenic in an insecticide can be determined gravimetrically through its precipitation as MgNH4AsO4. After the formation of the precipitate, it must be ignited for total conversion to Mg2As2O7, which is then cooled and weighed. Considering that a sample of 1,627 g of the insecticide produced 106.5 mg of Mg2As2O7, determine the% (m/m) As2O3 in the insecticide. Given the molar masses: Mg2As2O7 = 310.447 g / mol and As2O3 = 197.841 g / molTartaric acid, H2C4H4O6, is a diprotic acid that naturally occurs in the production of wine. Jose was tasked to find out the acid content in a 100.0 mL wine sample by titrating it with a standardized solution of NaOH. He was able to establish the working concentration of the NaOH solution by using 35.21 mL of it to titrate a primary standard of KHP that weighed 3.001 g. The grams and %w/w of Tartaric acid present in the 100.0 mL wine sample were then determined by titrating a 25.00 mL aliquot using 43.56 mL of the standardized NaOH solution. H2C4H4O6 (aq) + 2NaOH (aq) ↔ Na2C4H4O6 (aq) + 2H2O (l) Assume that the density of the wine sample is 1.000 g/mL MM of KHP = 204.22 g/mol MM of H2C4H4O6 = 150.087 g/mol What is the molar concentration of the prepared NaOH solution?…