2:02 AM Thu Dec 5 60 Done AA A www-awu.aleks.com O SIMPLE REACTIONS Jaquesha Determining the volume of base needed to titrate a given mass of acid A chemistry student weighs out 0.0614 g of phosphoric acid (H,PO4), a triprotic acid, into a 250. mL volumetric flask and dilutes to the mark with distiller water. He plans to titrate the acid with 0.1200 M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the final equivalence point. Be sure your answer has the correct number of significant digits. mL x10 Check Explanation Ise Privacy 2019 McGraw-Hill Education. A

2:02 AM Thu Dec 5 60 Done AA A www-awu.aleks.com O SIMPLE REACTIONS Jaquesha Determining the volume of base needed to titrate a given mass of acid A chemistry student weighs out 0.0614 g of phosphoric acid (H,PO4), a triprotic acid, into a 250. mL volumetric flask and dilutes to the mark with distiller water. He plans to titrate the acid with 0.1200 M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the final equivalence point. Be sure your answer has the correct number of significant digits. mL x10 Check Explanation Ise Privacy 2019 McGraw-Hill Education. A

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter3: Statistical Tests With Excel

Section: Chapter Questions

Problem 5P

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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?
According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?
When jump-starting a car with a dead battery, the ground jumper should be attached to a remote part of the engine block. Why?
The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)
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:
What volume of 0.10 moldm-3 sulphuric acid would be required to neutralise a mixture of 1.06 g of anhydrous sodium carbonate and 4.00 g of sodium hydroxide? (H2SO4 + 2NaOH ---> Na2SO4 + 2H2O) and (H2SO4 + Na2CO3 ® ---> Na2SO4+ H2O + CO2)
Ca2+ in a drinking water sample was analyzed by the following reactions below: Ca2+(aq) + C2O42-(aq) → CaC2O4 (s) → CaO(s) + CO(g)+ CO2(g) First an excess of C2O42- was added to 0.10 L of the Ca2+ water sample. Then CaC2O4 was precipitated, which was demcomposed into CaO with filtering and some heat. The CaO was measured to be 5.61 mg. What is the concentration of Ca2+ in the original water sample? The MW of CaO is 56.1 g/mol. 0.0100M 0.0010 M 1.00 M 0.100 M The partition coefficient (K) of methylamine (CH3NH2) is 4.50, preferring the organic layer over the aqueous layer in this extraction. The Ka of methylammonium (CH3NH3+) is 2.00 x 10-11. If 10 mL aqueous methylamine solution at pH 11.0 is extracted with 20.0 mL organic solvent, what is the fraction of solute remaining in the water (q)? HINT: methylamine is a weak base. 14.3% 10.0% 18.2% 81.8%
A commercial vinegar was analyzed by titration to determine the percent acetic acid. Briefly, 10.00 mL of vinegar sample was diluted to 100. mL solution in volumetric flask. A 25.00 mL aliquot from the diluted vinegar required 25.55 mL of 0.1005 M NaOH to reach the phenolphthalein endpoint. Which is the correct equation between the analyte and titrant reaction? CH3COOH + NaOH → NaCH3COO + H2O 2CH3COOH + NaOH → NaCH3COO + H2O C20H14O4 + NaOH → NaC20H14O4 + H2O CH3COOH + 2NaOH → NaCH3COO + H2O
and Employees CH STATE GE 90 ENDULERSE IS FOREVER "ON-Tame Name Jodi Rayal Molarity = wt. x1000 3. Calculate the massof Potassium hydrogen phthalate (KHP) to prepare a 250.0 mL solution of 0.1000 M KHP solution. Mol ut. x Voluse the 2500×1000 204.22250 mass Initial Buret Reading Final Buret Reading Vol NaOH Added Moles of NaOH Moles of HCI Volume of unknown HCI solution Concentration of HCI Average concentration of HCI of KHP = 5.11g 4. Complete the table below for the following neutralization reaction of an unknown concentration of hydrochloric acid with 0.100 M sodium hydroxide: Mu spate solution Trial 1 0 11.15 го data and calculate the concentration 15 Trial 2 11.15 22.15 Trial 3 22.15 33.25 abyh 067 LANDINUKASHU TROWTHCENTISSATE ARAD Ma That par މއކނި REMURNAR MISAMARALISERDRY Tile
Marble, a material used in buildings and statues, has the chemical composition CaCO₃. CaCO₃ reacts with acid (H₃O⁺), dissolving the solid through the reaction: CaCO₃(s) + 2H₃O⁺(aq) → Ca²⁺(aq) + CO₂(g) + 3 H₂O(l) In 1985, rain water in central Pennsylvania had an approximate H₃O⁺ concentration of 8.0 × 10⁻² mM. What volume of rain would be needed to dissolve a small statue made of 4.50 kg of marble?
A commercial research organization is planning to develop a sensor to detect methyl parathion that may be injected into a water supply by terrorists. The LD50 for methyl parathion is reported to be as low as 6 mg ・ kg−1 for rats. They are assuming a safety factor of 1 × 105 and a volume of liquid ingested equal to a cup of coffee (about 250 mL) in the design of the instrument. What concentration (in mg ・ L−1) must their instrument be able to detect? Using Equation 6–10, the concentration you have calculated, the ingestion rate of 250 mL, an exposure frequency of one day, and exposure duration of one day, an adult malebody weight, and an averaging time of 1 day, estimate the hazard index. The RfD for methyl parathion is 2.5 × 10−4 mg ・ kg−1 ・ d−1 .
The solubility of borax, which is made up of sodium tetraborate (Na2B4O5(OH)4 8H2O), was analyzed. The dissolution of borax is: Na2B4O5(OH)4 • 8H2O(s) ⇌ 2 Na+(aq) + B4O5(OH)42–(aq) + 8 H2O(l) A 50 mL saturated solution was prepared. After filtration of solution, 5 mL aliquot was transferred to a flask and titrated using 0.432 M HCl. The endpoint was found to be 4.73 mL of the titrant. Tetraborate anion (B4O5(OH)42-) is a weak base which reacts with HCl like the following reaction: B4O5(OH)42–(aq) + 2 H+(aq) + 3 H2O(l) ⇌ 4 H3BO3(aq) What is Ksp expression for the dissolution? What is the tetraborate ions concentration in the filtrate? What is the molar solubility and Ksp of borax if the titration was done at room temperature (298 K)?