In the Flint Water Crisis, trihalomethanes were produced in the new water supply due to the mixing of _________ with ________ water. Ferric chloride then was added, which fortunately worked to _________ , but unfortunately also worked to ___________ , resulting in lead-contaminated water. Orthophosphates would have helped to prevent this problem by specifically creating a _________ , which would work to keep ________ .

In the Flint Water Crisis, trihalomethanes were produced in the new water supply due to the mixing of _____ with water. Ferric chloride then was added, which fortunately worked to _ , but unfortunately also worked to ___ , resulting in lead-contaminated water. Orthophosphates would have helped to prevent this problem by specifically creating a _ , which would work to keep ____ .

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter13: Titrations In Analytical Chemistry

Section: Chapter Questions

Problem 13.27QAP

See similar textbooks

Similar questions

Bleach (sodium hypochlorite, NaOCl, a strong oxidizing agent) neutralizes and inactivates mustard gas. Bleach is also effective on organic stains because it oxidizes coloredcompounds to colorless compounds. Propose products that might be formed by thereaction of mustard gas with bleach
Where does the strongest IMF occur in liquid water?
why does enrgy have to be supplied to a chemical in order to break the IMFs between the molecules in that chemical?
(a) Write the principle of electrolytic refining.(b) Why does copper obtained in the extraction from copper pyrites have a blistered appearance?(c) What is the role of depressants in the froth floatation process?
What is chemical reduction (only reduction, not redox) and chemical dechlorination in chemical treatment of hazardous waste? What are their processes?
Consider the reaction of pyruvate with NADH and the standard reduction potentials, ?′°,E′°, of pyruvate and NAD+. Redox pair E'°, V pyruvate/lactate –0.19 NAD+/NADH –0.32 pyruvate+NADH↽−−⇀lactate+NAD+ Assuming that the concentrations of each reactant and product are 1 M and that the reaction is performed at pH 7 and 25 °C, determine the Δ?′°Δ⁢E′° for the reaction.
Calculate the time, in minutes, needed to plate 17.697 g of metal M at 43 Amps. The molar mass of metal M is 57.915 g/mol. M6+ + 6 e– → M Recall that, C = A*s, and Faraday’s constant, F, is 96,485 C/mole of electrons.
A hard water sample was found to have an equivalent of 0.1598 g CaCO3 (mw =100g/mol). What volume of 0.05M EDTA would be required to remove the calcium from the water sample?
In determining the manganese dioxide content of a pyrolusite mineral. A sample of 0.5261 g of pyrolusite was treated with 0.7149 g of 97.98% sodium oxalate in an acid medium. After the reaction was complete, 30.47 mL of a 0.02160 M potassium permanganate solution was required to titrate for excess unreacted oxalic acid. Calculate the percentage of manganese dioxide in the pyrolusite.
Why alkali is added to the nitrification tank？ A. to provide electron donors B. to provide alkalinity for the nitrification reaction C. to acidify the reaction solution D. to provide nutrients for the nitrifier bacteria
1. Why is the KMnO4 solution filtered? KMnO4 doesn't need to be filtered prior to use. Most commercial samples of KMnO4 contain some manganese dioxide that must be removed prior to use to avoid further decomposition. KMnO4 is very stable, but the unstable ions in the commercial packaging materials must be removed prior to use. Most commercial samples contain inorganic matter that will react slowly with the KMnO4 and cause its decomposition. 2. Why is the KMnO4 not stored in a rubber-stoppered bottle? Rubber doesn't make a good seal with the plastic bottles in which permanganate is usually stored. Rubber is made of inorganic matter and will reduce the permanganate solution. Rubber is made of organic matter and will reduce the permanganate solution. Rubber can oxidize the permanganate solution.
Write the balanced net ionic equations to describe the oxidation of Mn2+ to MnO4- by ammonium peroxydisulfate.