Sample Problem 2 A 5.63 g sample of an impure barium chloride crystals were dissolved in water to make 100 mL aqueous solution. A 20-mL aliquot of this solution was titrated with 0.260 M AgNO3 solution using potassium chromate as indicator. What is the minimum amount of titrant needed to reach the equivalence if the sample is 96.8% pure? FW: BaCl2 = 208.23
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- A 10.00mL sample of alcoholic ethyl acetate was diluted to 100.00 mL. 20.00 mL was aliquoted and mixed with 40.00 mL of 0.04672 M KOH. The resulting mixture was heated for 2 hours. CH3COOC2H5 + OH- → CH3COO- + C2H5OH After cooling, the excess OH was back titrated with 3.41 mL of 0.05042 M H2SO4. Answer the following: Calculate the number of moles of OH- that reacted with ethyl acetate. Calculate the number of moles of ethyl acetate in the 20.00 mL solution. What is the mass of ethyl acetate (FW=88.11 g/mol) in the original 10.00 mL sample?Was wondering how to solve this hw problem? Calcium Flouride (dissociation) K@25 C = 3.94 *10^-11 Calcium fluoride is not very soluble in water. ** Its dissociation is: CaF2 (s) Ca²+ (aq) + 2 F¯ (aq) a. At 25°C, how many milligrams of CaF2 would dissolve in 2.0 L of water? b. What were your initial and final values of Q?A sample weighing 10.91 g containing an unknown amount of H3PO4 was diluted with water and titrated with a standardized concentration of 0.7255 M NaOH. The endpoint was reached after 27.03 mL of the titrant was added. What is the % H3PO4 (97.994 g/mole) in the sample? H3PO4 + 2 NaOH --> Na2HPO4 + 2H2O ROUND OFF FINAL ANSWER TO FOUR (4) SIG FIGS
- What is the molar weight of an unknown monoprotic acid, if 0.2501 g of the acid is titrated with 18.61 mL of0.1100 M NaOH? Show work.Molarity of (NH3) solution (M) from bottle- 5.0 Initial reading of buret (NH3) (mL)- .27 Final reading of buret (NH3) (mL)- 8.25 Volume of Cd(NO3)2 solution (mL)- 10.00 Volume of Na2C2O4 solution (mL)- 10,00 please find Total volume of solution after titration (mL) Total moles of C2O42- (mol) Molarity of C2O42- (M) Total moles of Cd2+ (mol) Moles of [Cd(NH3)4]2+ (mol) Molarity of [Cd(NH3)4]2+ (M) Moles of NH3 added by titration (mol) Moles of NH3 that did not react with Cd2+ (mol) Molarity of NH3 that did not react with Cd2+ (M) Kf for [Cd(NH3)4]2+0.7050-g of pure KHP (FW = 204.2) was dissolved and titrated with 35.00mL of NaOH solution. The excess NaOH was backtitrated with 5.00mL of HCl solution. In a separate titration it was found that 30.00mL of NaOH will react with 28.00mL of HCl. Find the molarity of NaOH and HCl.
- You want to measure the concentration of carbonate (CO32-) in a mildly basic solution by using an EDTA back titration. CaCO3 has a Ksp of 5x10-9. You add 50.00 mL of 0.3484 M CaCl2 to 500.0ml of sample and filter the solution to remove the precipitate. You then take 250.0 mL of the filtered solution and titrate with 0.1786 M EDTA. You require 23.72 mL to reach the endpoint. What is the concentration of carbonate in the original sample?1. A 0.1250-g sample of pure (100%) of K2Cr2O7 was dissolve in 250-mL volumetric flask, and dilute to volume, producing a concentration of 1.700 × 10-3 M. The resulting solution is an example of a standard solution prepared from a primary standard. Select one: a. True b. False 2. Which of the following is not an example of a standard solution? a. 1000 ppm Lead Nitrate solution b. 1.000g pure sodium carbonate dissolved in 1L of solution c. 3:4 nitric acid: hydrochloric acid solution d. NaOH solution standardized using KHP e. 0.104 M NaOHWhat mass of Ba(OH)2 is present in a sample if it is titrated to its equivalence point with 44.20 mL of 0.1000 N H2SO4? Note: Please present complete solution. Express your final answers up to two (2) decimal places.
- A 1.067g sample of magnesium oxide of 84.736% were treated with 50mL of 1.017 N Sulfuric Acid, and a 5.195mL volume of sodium hydroxide is required in the back titration. 1. What is the equivalent weight consumed by the acidic titrant? A. 5.281 g-meq B. 55.150 g-meq C. 5.723 g-meq D. 50.850 g-meq 2. What is the difference of milliequivalent weight consumed in the reaction? A. 45.127g-meq B. 56.573g-meq C. 50.850g-meq D. 55.150g-meq 3. What is the amount (in mg) of the analyte that is equivalent to 1 milliliter of the tirant at its equivalence point? A. 22.060mg B. 40.680mg C. 44.12mg D. 20.340mgTitration of the I2 produced from 0.2645g of primary standard KIO3 required 45.36mL of sodium thiosulfate. Calculate the concentration of the Na2S2O3 in M. IO3- + 5I- + 6H+ --> 3I2 + 3H2O I2 + 2S2O32- --> 2I- + S4O62- KIO3 mw = 214.001g/molTitration of 50.00 mL of 0.04715 M Na2C2O4 required 39.25 mL of a potassium permanganate solution.MnO4- + 5H2C2O4 + 6H+ → 2Mn2+ + 10CO2(g) + 8H2OCalculate the molar concentration of the KMnO4 solution.