७.ग.4.74x 100 = 22.217.4. Bleach products are sold as 5.25-7.5% hypochlorite concentration depending on whether theyare "regular" or "extra-strength"? How do your mass percentages compare to these values?One of my valves falls into that range but theother two fall a little short.5. Bleach products slowly decompose over time eventually rendering them useless. What stepscan be taken to slow this (think back to the chapter on Kinetics) when storing your bleachproduct?The bleach products could be stored at a certaintemperature and kept away from the light. Thiswill help slow the decomposition.6. As mentioned in the introduction, one type of bleach alternative uses hydrogen peroxide toremove stains. The H₂O2 in the product can be titrated with the MnO4 under acidic conditionsby the reaction: 5 H₂O2(aq) + 2 MnO4 (aq) + 6 H* (aq)5 02(g) + 2 Mn+2 (aq) + 8 H₂O(). If a0.505g sample of a product containing H₂O₂ required 16.55mL of a 0.01158M MnO4 solution toreach the end point, then what is the mass percent of hydrogen peroxide in this product+

Given data for Q6 Reaction involved : 5H2O2 (aq) + 2MnO4- (aq) + 6H+ (aq) -------> 5O2 (g) +…

remove stains. The H₂O2 in the product can be titrated with the MnO4 under acidic conditions by the reaction: 5 H₂O2(aq) + 2 MnO4 (aq) + 6 H(aq) 502(g) + 2 Mn+2 (aq) + 8 H₂O). If a 0.505g sample of a product containing H₂O₂ required 16.55mL of a 0.01158M MnO4 solution to point than what is the m percent of hydrogen peroxide in this product ro

remove stains. The H₂O2 in the product can be titrated with the MnO4 under acidic conditions by the reaction: 5 H₂O2(aq) + 2 MnO4 (aq) + 6 H(aq) 502(g) + 2 Mn+2 (aq) + 8 H₂O). If a 0.505g sample of a product containing H₂O₂ required 16.55mL of a 0.01158M MnO4 solution to point than what is the m percent of hydrogen peroxide in this product ro

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Consider the neutralization reaction 2 HNO3(aq) + Ba(OH)2(aq) → 2 H2O(l) + Ba(NO3)2(aq) A 0.105 L sample of an unknown HNO3 solution required 41.1 mL of 0.200 M Ba(OH)2 for complete neutralization. What is the concentration of the HNO3 solution? concentration: Σ
8) What is the molarity of the solution containing 234 g NaCl in 3.00 L of solution? 9) Use the reaction: 2 AgNO3 (aq) + H2SO4 (aq) → Ag2SO4 (s) + 2 H2O (I) What volume of 0.123 M AgNO3 (aq) is needed to form 0.657 g of Ag2SO4 (s)?
23. What volume of 0.250 M KCl(aq) will completely react with 50.0 mL of 0.115 M Pb(NO3 )2 (aq)? Pb2+ (aq)+2Cl- (aq) = PbCl2 (s)
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) The concentration of sulphide ion in the final solution is
Jake carried out three titrations to determine the concentration of unknown nitric acid (HNO3) using 0.1050 M NaOH. He titrated 100.0 mL of the nitric acid sample and obtained the following volumes of NaOH: 20.56, 20.48, and 20.52 mL. The acid-base reaction occurring is NaOH (aq) + HNO3(aq) →→ NaNO3(aq) + H2O(l) Determine the concentration of the acid; report the average molarity with standard deviation. Pay attention to the number of significant figures on the mean and the number of decimal places on the standard deviation.
Complete neutralization of a mixture of magnesium hydroxide and aluminum hydroxide is required 48.5 ml of 0.187M hydrochloric acid. The mixture of dry chloride salts from the reaction has the quantity of 0.420 g. What is the percentage by mass of magnesium hydroxide in the mixture of the above hydroxides for the reaction with HCI? Mg(OH)2 + 2HCI -> MgCl2 + 2H20 Al(OH), + 3HCI -> AICI, + 3H20
Walter White requires a sulfuric acid (Strong acid) solution to use in a very important synthetic reaction. He finds a bottle labeled H2SO4, but by some strange turn of events, he cannot remember the concentration. He decides to perform a titration to determine the concentration of the H2SO4. He pours 22.20 mL of his unknown sulfuric acid solution into a flask and finds that it requires 29.50 mL of 0.57 M KOH (strong base) to reach the endpoint. What is the concentration of Walter White's sulfuric acid solution? (Enter your numeric answer only, do not use scientific notation, enter 2 decimal places with your answer) For reference: KOH = 56.106g/mol H2SO4= 98.079g/mol Avagadro's number 6.022x1023
3. A 4.912-g sample of a petroleum product was burned in a tube furnace, and the SO2 produced was collected in 3% H₂O₂. Reaction: SO2(g) + H₂O2 → H₂SO4. A 25.00-mL portion of 0.00873 M NaOH was introduced into the solution of H₂SO4, following which the excess base was back-titrated with 15.17 mL of 0.01102 M HCI. Calculate the sulfur concentration in the sample in parts per million.
Calculate the number of milliliters of 0.779 M KOH required to precipitate all of the Pb²* ions in 122 mL of 0.541 M Pb(NO3)2 solution as Pb(OH)2. The equation for the reaction is: Pb(NO3)2(aq) + 2KOH(aq) –→Pb(OH)2(s) + 2KNO3(aq) mL KOH
What volume of 0.250 M KCl(aq) will completely react with 50.0 mL of 0.115M Pb(NO3)2(aq)?
Consider the neutralization reaction 2 HNO3(aq) + Ba(OH)2(aq). 2 H2O(l) + Ba(NO3)2(aq) A 0.105 L sample of an unknown HNO3 solution required 42.5 mL of 0.250 M Ba(OH)2 for complete neutralization. Wha the concentration of the HNO3 solution? concentration: .098
A 0.205 g sample of a monoprotic acid was dissolved in 25 mL of water. The acid solution was titrated to its endpoint with 28.1 mL of 0.0788 M NaOH solution. What is the molar mass of the acid?