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 for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter4: Stoichiometry

Section: Chapter Questions

Problem 4.98PAE

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The iron content of hemoglobin is determined by destroying the hemoglobin molecule and producing small water-soluble ions and molecules. The iron in the aqueous solution is reduced to iron(II) ion and then titrated against potassium permanganate. In the titration, iron(ll) is oxidized to iron(III) and permanganate is reduced to manganese(II) ion. A 5.00-g sample of hemoglobin requires 32.3 mL of a 0.002100 M solution of potassium permanganate. The reaction with permanganate ion is MnO4(aq)+8H+(aq)+5Fe2+(aq)Mn2+(aq)+5Fe3+(aq)+4H2O What is the mass percent of iron in hemoglobin?
4.112 A metallurgical firm wishes to dispose of 1300 gallons of waste sulfuric acid whose molarity is 1.37 M. Before disposal, it will be reacted with calcium hydroxide (slaked lime), which costs $0.23 per pound. (a) Write the balanced chemical equation for this process. (b) Determine the cost that the firm will incur from this use of slaked lime.
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 2.00 mL aliquot of reagent grade HCl was diluted to 250.0 mL. The diluted solution was standardized using sodium carbonate, and the concentration of the prepared solution was determined to be 0.09606 M HCl. What is the concentration of reagent HCl (in %w/w)? Note: the specific gravity of the reagent HCl was 1.18 g/mL.
By pipet, 5.00 mLmL of a 0.823 MM stock solution of potassium permanganate (KMnO4) was transferred to a 50.00-mL volumetric flask and diluted to the calibration mark. Determine the molarity of the resulting solution.
In the standardization of HCl using pure anhydrous sodium carbonate as the primarystandard for methyl orange as an indicator, 1.0 mL HCl was found to be equivalent to 0.05gof sodium carbonate (MW =106). The normality of HCl is:
KHP (aq)+NaOH (aq)-->NaKHP (aq)+H2O(l) Trial Vi (mL) Vf (mL) 1 36.19 48.56 2 3 A student masses out 1.096 grams of KHP, which is dissolved in 25.00 mL of DI water. This KHP solution is titrated with NaOH, as shown in the equation above. Calculate the molarity of the NaOH solution.
By pipet, 19.00 mL of a 0.823 M stock solution of potassium permanganate (KMnO4) was transferred to a 50.00-mL volumetric flask and diluted to the calibration mark. Determine the molarity of the resulting solution.
Concentration of NaOCl in Full-strength Commercial Bleach: A diluted bleach solution was found to have a concentration of 0.0284 M. It was originally prepared by diluting 3.0 mL of full-strength commercial bleach, with water, to a total volume of 100.00 mL. What is the molar concentration of NaOCl in the full-strength commercial bleach solution?
To prepare a very dilute solution of K2Cr2O7 (294.18 g/mol), 0.661 g of K2Cr2O7 was transferred to a 250.0-mL volumetric flask and adding water to the mark. A sample of this solution of volume 1.000 mL was then transferred to a 500.0-mL volumetric flask and diluted to the mark with water. Subsequently, 10.0 mL of the diluted solution was transferred to a 250.0-mL flask and diluted to the mark with water. What is the final concentration of K2Cr2O7 in this last solution?
The Bayer process is the formation of aluminum hydroxide from metallic aluminum and sodium hydroxide heated to high temperatures. Al(s)+ 3NaOH(aq) -->Al(OH)3(s) + 3Na A manufacturing chemist observes that two distinctly different solids are present in the solutions after the reaction has come to completion. The chemist collected the following data: data table From the above information, identify the limiting and excess reagent, the supporting evidence, and suggest a method to increase the amount of product produced.
An analyst is planning to standardize a 0.200 mol/L NaOH solution for use in neutralization. For this, he chose to standardize the NaOH solution using potassium hydrogen phthalate. (KHC8O4H4, molecular mass 204.22 g mol/L) - Knowing that potassium hydrogen phthalate is a solid, what is the mass of potassium hydrogen phthalate in grams, the analyst should weigh to standardize the NaOH, anticipating spending 15 mL of NaOH solution approximately 0.200 mol/L ? [Answer; m=0.6123 g] NaOH + KHC8O4H4 → KNaC8O4H4 + H2O(Neutralization reaction in standardization) - Why you need to standardize the NaOH solution and why use potassium hydrogen phthalate?