Calculate the concentration of all the ions in solution after mixing 100.0 mL of 0.0200M KF (aq) with 150.0 mL of 0.0250 M BaCl2 (aq). I know that in the mixture, an insoluble compound forms, BaF2 (s) -> Ba^2+ (aq) + 2F^- (aq), however, Q

Calculate the concentration of all the ions in solution after mixing 100.0 mL of 0.0200M KF (aq) with 150.0 mL of 0.0250 M BaCl2 (aq). I know that in the mixture, an insoluble compound forms, BaF2 (s) -> Ba^2+ (aq) + 2F^- (aq), however, Q

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 14.74QE: Lead poisoning has been a hazard for centuries. Some scholars believe that the decline of the Roman...

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On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate: 2HNO3(aq)+Na2CO3(aq)2NaNO3(aq)+H2O(l)+CO2(g) a. Calculate H for this reaction. Approximately 2.0 104 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 70.0% HNO3 by mass with a density of 1.42 glcm3. What mass of sodium carbonate was required for complete neutralization of the spill, and what quantity of heat was evolved? (Hf for NaNO3(aq) = 467 kJ/mol) b. According to The Denver Post for April 4, 1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of H, what was their major concern?
Lead poisoning has been a hazard for centuries. Some scholars believe that the decline of the Roman Empire can be traced, in part, to high levels of lead in water from containers and pipes, and from wine that was stored in leadglazed containers. If we presume that the typical Roman water supply was saturated with lead carbonate, PbCO3 (Ksp = 7.4 1014), how much lead will a Roman ingest in a year if he or she drinks 1 L/day from the container?
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
You are required to standardize a dilute solution of sulphuric acid, and undertake the following steps:(i) 4.805 g of solid sodium tetraborate (Na2B4O7) are added to a 250 mL volumetric flask, and the solution made up to the mark with distilled water.(ii) 25.00 mL aliquots of the stock solution from (i) are transferred to conical flasks, for titration against the sulphuric acid solution in the burette.(iii) You perform titrations using two different indicators: bromocresol green, and phenolphthalein.With bromocresol green, the average titre volume is 22.50 cm3, while with phenolphthalein, the average volume is 9.50 cm3.(a) Write the balanced equation for the reaction between Na2B4O7 and sulphuric acid
Tartaric 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?…
A solution is prepared by pipetting 25.0 mL of 0.350 M CuCl2 into a 100.0 mL volumetric flask, diluting to the calibration mark on the flask with water and quantitatively mixing the contents of the flask. What is the molar concentration of Cl- in the solution?
Tartaric acid, H2C4H4O6, is a diprotic acid that naturally occurs in the production of apple wine. Emma was tasked to find out the acid content in a 50.0 mL wine sample by titrating it with a standardized solution of NaOH. She was able to establish the working concentration of the NaOH solution by using 17.61 mL of NaOH to titrate a primary standard of KHP that weighed 1.501 g. The grams and %w/w of Tartaric acid present in the 50.0 mL wine sample were then determined by titrating a 12.50 mL aliquot using 21.78 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?…
The tartaric acid, H2C4H4O6 (150.087 g/mol ) concentration in 100.0 mL wine sample was determined using 0.4050 M sodium hydroxide standard solution. In the experiment, the %w/w of tartaric acid present in the wine sample by analyzing and titrating only 25.00 mL aliquot from the 100-ml wine sample. The endpoint of titration was reached upon the addition of exactly 43.56 mL NaOH solution? (Assume the density of the wine sample is 1.000 g/mL) H2C4H4O6 + 2NaOH⟶Na2C4H4O6+2H2O What is the total (%w/w) acid content in the wine sample? 1.324 %w/w 2.648 %w/w 5.296 %w/w 10.59 %w/w
A sample containing NaCl, NaBr, and inert materials weighs 1.000 g. With excess AgNO3 it gives a precipitate of AgCl and AgBr, which weighs 0.5260 g. By heating this precipitate in a current of Cl2 gas, the AgBr is converted to AgCl and the resulting precipitate then weighs 0.4260 g. What is the %NaCl and %NaBr present in the original sample?
Write the balanced NET ionic equation for the reaction when Pb(NO₃)₂ and KI are mixed in aqueous solution. If no reaction occurs, simply write only NR. Be sure to include the proper phases for all species within the reaction.
A student was asked to determine the concentration of ammonia, a volatile substance, in a commercially available cloudy ammonia solution used for cleaning. First the student pipetted 25.00 mL of the cloudy ammonia solution into a 250.0 mL conical flask. 50.00 mL of 0.100 mol L-¹ HCl(aq) was immed added to the conical flask which reactedwith the ammonia in solution. The excess (unreacted) HC1 was then titrated with 21.50 mL 0. 050 M Na2CO3 (aq). Calculate the concentration of the ammonia in the cloudy ammonia solution.
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 / mol