5. An accurately measured 2g sample of hydrogen peroxide (H₂O₂-34g/mol) was dissolved in a mixture of 20mL water and 20mL diluted sulfuric acid. Sample is titrated with 0.1N potassium permanganate consuming 30mL to reach the endpoint. Compute for the percentage of hydrogen peroxide. 2KMnO4 + 5H₂O₂ + 3H₂SO4Ⓡ 2MnSO4 + K₂SO4 +50₂ + 8H₂O

5. An accurately measured 2g sample of hydrogen peroxide (H₂O₂-34g/mol) was dissolved in a mixture of 20mL water and 20mL diluted sulfuric acid. Sample is titrated with 0.1N potassium permanganate consuming 30mL to reach the endpoint. Compute for the percentage of hydrogen peroxide. 2KMnO4 + 5H₂O₂ + 3H₂SO4Ⓡ 2MnSO4 + K₂SO4 +50₂ + 8H₂O

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter9: Complexometric And Precipitation Titrations

Section: Chapter Questions

Problem 13P

See similar textbooks

Similar questions

Sulfide ion (S2- ) is formed in wastewater by the action of an aerobic bacteria on organic matter. Sulfide can be readily protonated to form volatile, toxic H2S. In addition to the toxicity and noxious odor, sulfide and H2S cause corrosion problems because they can be easily converted to sulfuric acid when conditions change to aerobic. One common method to determine sulfide is by coulometric titration with generated silver ion.At the generator electrode, the reaction is Ag Ag+ + e-. The titration reaction is S2- + 2Ag+ Ag2S(s). (a) A digital chloridometer was used to determine the mass of sulfide in a wastewater sample. The chloridometer reads out directly in ng Cl-.In chloride determinations, the same generator reaction is used,but the titration reaction is Cl- + Ag+ AgCI(s). Derive an equation that relates the desired quantity, mass S2- (ng), to the chloridometer readout in mass Cl- (ng). (b) A particular wastewater standard gave a reading of 1689.6 ng Cl-. What total charge in coulombs was required to generate the Ag+ needed to precipitate the sulfide in this standard? (c) The following results were obtained on 20.00-mL samples containing known amounts of sulfide.17 Each standard was analyzed in triplicate and the mass of chloride recorded. Convert each of the chloride results to mass S2- (ng). (d) Determine the average mass of S2- (ng), the standard deviation, and the %RSD) of each standard. (e) Prepare a plot ofthe average mass of S2- determined (ng) versus the actual mass (ng). Determine theslope, the intercept, the standard error, and the R2 value. Comment on the fit of the data to a linear model. (f) Determine the detection limit (ng) and in parts per million using a k factor of 2 (see Equation 1-12). (g) An unknown wastewater sample gave an average reading of 893.2 ng Cl. What is the mass of sulfide (ng)? If 20.00 mL of the wastewater sample was introduced into the titration vessel, what is the concentration of S2- n parts per million?
Calculate the solubility at 25°C of CaF2 in pure water and in a 0.0060M NaF solution. You'll find Ksp data in the ALEKS Data tab. (CaF2 Ksp is 3.45×10−11 Round both of your answers to 2 significant digits. solubility in pure water: ? gL? solubility in 0.0060 M NaF solution:? gL?
Calculate the solubility of lead(II) sulfate (Ksp = 2.53x10-8) in a 0.0034 M solution of sodium sulfate. Give your answer to three sig. figs. and in exponential form (e. g. 1.23E-3).
An experiment to observe the effect of ionic strength on the solubility of Ca(OH)2 was conducted. Ca(OH)2 was added to 250 mL 0.01 M KCl, stirred until equilibrium. This was then filtered, and 50 mL of the filtrate was measured out. The 50 mL filtrate was then titrated with standardized 0.13 M HCl solution until phenolphtalein endpoint (11 mL). How do I solve for the solubility s of Ca(OH)2? Please provide an explanation of the process (do I multiply ionic strength μ to the solubility [where s = [Ca(OH)2) = [Ca2+] = 1/2[OH-]?)
An experiment to observe the effect of ionic strength on the solubility of Ca(OH)2 was conducted. Ca(OH)2 was added to 250 mL 0.01 M KCl, stirred until equilibrium. This was then filtered, and 50 mL of the filtrate was measured out. The 50 mL filtrate was then titrated with standardized 0.13 M HCl solution until phenolphtalein endpoint (11 mL). How do I solve for the solubility s of Ca(OH)2? Please provide an explanation of the process (do I multiply ionic strength μ to the solubility [where s = [Ca(OH)2) = [Ca2+] = 1/2[OH-]?) I would like to know how the diverse ion effect would affect the solubility of Ca(OH)2. How does the ionic strength μ of KCl affect this?
The buret was filled with 0.100 M HCl solution. Then was transferred in a 25.0 mL of saturated calcium hydroxide solution (2g of calcium hydroxide per 100 ml of water) in two separate E-flasks. Then 2 drops of phenolphthalein was added to each flask Titration data for the determination of solubility and Ksp of calcium hydroxide: Trial 1: Final Buret reading (ml)-19.80; Initial Buret reading (ml)- 13.00; Temperature (Celcius)- 25 Trial 2: Final Buret reading (ml)-26.10; Initial Buret reading (ml)- 19.80; Temperature (Celcius)- 25 Voume of HCl used: Trial 1- 6.80ml; Trial 2- 6.30mL 1. Compute for the moles of H+ used and the moles of OH- present. moles of H+ used = (concentration of HCl) × (volume of HCl used)moles of OH- = moles of H+ used 2. Construct an ICE table for the reaction.3. Calculate the molar solubility (in mol/L) of OH- and Ca2+.4. Determine the solubility of Ca(OH)2 in g/L. (MM of Ca(OH)2 = 74.096 g/mol). 5.…
The compound lead(II) sulfate has a solubility of 4.824E-3 g/100mL at 25 degC.What is the molar solubility of this solution at saturation? 0.0002 mol/L What is the Ksp at 25 degC for lead(II) sulfate? What is the molar solubility of lead(II) sulfate in 0.28 M lead(II) nitrate ?
The solubility of Fe(OH)2 is measured and found to be 1.15×10-3 g/L. Use this information to calculate a Ksp value for iron(II) hydroxide.
00 mL of a diprotic acid primary standard solution was accurately prepared to a concentration of 0.1431 M. Three samples of this primary standard solution were used as samples in a titration to standardize an aqueous solution of sodium hydroxide, NaOH, which would be used as a titrant. Using the following table of data for the titration of the primary standard acid with NaOH, calculate the average concentration of NaOH. Trial # Volume of primary standard Initial titrant volume Final titrant volume 1 10.00 mL 8.21 mL 27.22 mL 2 10.00 mL 27.22 mL 46.23 mL 3 10.00 mL 30.28 mL 49.29 mL 0.1506 M 0.0753 M 0.0376 M 0.1431 M 0.0526 M
The buret was filled with 0.100 M HCl solution. Then was transferred in a 25.0 mL of saturated calcium hydroxide solution (2g of calcium hydroxide per 100 ml of water) in two separate E-flasks. Then 2 drops of phenolphthalein was added to each flask Titration data for the determination of solubility and Ksp of calcium hydroxide: Trial 2: Final Buret reading (ml)-26.10; Initial Buret reading (ml)- 19.80; Temperature (Celcius)- 25 Voume of HCl used: Trial 2- 6.30mL 1. Compute for the moles of H+ used and the moles of OH- present. moles of H+ used = (concentration of HCl) × (volume of HCl used)moles of OH- = moles of H+ used 2. Construct an ICE table for the reaction.3. Calculate the molar solubility (in mol/L) of OH- and Ca2+.4. Determine the solubility of Ca(OH)2 in g/L. (MM of Ca(OH)2 = 74.096 g/mol). 5. Calculate the Ksp of Ca(OH)26. Compute for the percent error of the experimental value for Ksp of Ca(OH)2 with the literature…
Calculate the solubility at 25°C of BaCrO4 in pure water and in a 0.0180M BaCl2 solution. You'll find Ksp data in the ALEKS Data tab. ksp for Ba Cr04 =1.17×10−10 Round both of your answers to 2 significant digits. solubility in pure water: gL solubility in 0.0180 M BaCl2 solution: gL
a 10g soil sample was gently stirred with 250 ml of 1.0 M CH3COO(NH4) solution for 24 h and centrifuged to separate the solution. The solution recovered after centrifugation was titrated with distilled water to a volume of 1 liter and analyzed for cations. Analytical results showed that the solution contained 20 mg/L Ca, 2 mg/L Mg, 1 mg/L K, and 0.5 mg/L Na. Calculate the number of cation exchange equivalents and express it in meq/100 g of soil