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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?If I start with 100. mL of a 0.95 M Fe(NO3)3 solution and dilute it until the final volume is 150 mL, what will the concentration of the diluted solution be?Titration of a 25.00 mL sample of acid rain required 12.4 mL of 0.009879 M NaOH to reach the end point. If we assume that the acidity of the rain is due to the presence of sulfuric acid, what was the concentration (in mol/l and %) of sulfuric acid in this sample of rain?
- Titration of a 20.00 mL sample of acid rain required 4.13 mL of 0.08424 M KOH to reach the end point. If we assume that the acidity of the rain is due to the presence of sulfuric acid, what was the concentration (in mol/l and %) of sulfuric acid in this sample of rain?If 0.5693 g of sodium oxalate, Na2C2O4, requiresof a 41.72 mL KMnO4 solution to reach the end point, what is the molarity of the KMnO4.What is the initial molar concentration in moles/L of I - found in 2 mL of 0.060 M KI (mL) with the total volume of the solution being 10 mL?
- CHEMISTRY (Please write the complete solution legibly. No long explanation needed. Answer in 2 decimal places. Box the final answer.) Solve the following: a. Calculate the molarity of hydrochloric acid, HCl, in a solution if 25.00 mL of that solution required35.74 mL of 0.1522 M KOH for complete neutralization in a titration. (Answer: 0.2176 M) b. When aqueous solutions of Ba(NO3)2 and K2SO4 are mixed, a precipitate of BaSO4 results. Writethe molecular, ionic, and net ionic equation for this double displacement reaction. c. 8.50 g of copper (II) sulfate pentahydrate, CuSO4∙5H2O, is dissolved in 250 mL of solution. Whatis the molarity of this solution?Write the balanced neutralization reaction that occurs between H2SO4H2SO4 and KOHKOH in aqueous solution. Phases are optional. neutralization reaction: Suppose 0.250 L0.250 L of 0.500 M H2SO40.500 M H2SO4 is mixed with 0.200 L0.200 L of 0.200 M KOH0.200 M KOH. What concentration of sulfuric acid remains after neutralization?If 0.6546 g of sodium oxalate, Na2C2O4, requiresof a 23.26 mL KMnO4 solution to reach the end point, what is the molarity of the KMnO4 solution?
- What volume of water should be added to 100.0 mL of a 0.500 N Cr2(SO4)3·18H2O solution to obtain a final concentration of 0.075 M? Show complete solution *Also find the number of replaceable ions (n)Following the procedure, a student recorded the initial volume of NaOH in his buret as 1.41 mL. He then titrated a 15.00 mL sample of 0.1027 M HCl until a persistent pale pink appeared. He recorded the final volume of NaOH in his buret as 12.91 mL. What is the concentration (M) of his NaOH solution?Write the balanced neutralization reaction that occurs between H2SO4H2SO4 and KOHKOH in aqueous solution. Phases are optional. Suppose 0.950 L0.950 L of 0.400 M H2SO40.400 M H2SO4 is mixed with 0.900 L0.900 L of 0.300 M KOH0.300 M KOH. What concentration of sulfuric acid remains after neutralization?