Reaction 5FeCl,(aq):NaOH(aq):Balance equation:FeCl,(aq) +NAOH(aq)→Observations:Type of Reaction:Reaction 6NaHCO,(aq):HCI(aq):Balance Equation:NaHCO,(aq) +HCl(aq) →Observations:Type of Reaction:Reaction 7(1) Pb(NO3),(aq): .(2) KI(aq):Balance equation:Pb(NO,),(aq) +KI(aq) →Mass of test tube 1 and test tube 2 + beaker:Mass of the test tube that contains products + an empty test tube + a beaker:58

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Answered: Reaction 5 FeCl,(aq): NAOH(aq): Balance…

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Reaction 5 FeCl,(aq): NAOH(aq): Balance equation: FeCl,(aq) + NAOH(aq) Observations: Type of Reaction:

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 14.97QE: According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as...

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North of Kingston you discover a hidden mountain and name it Mt. Kevinmanjaro, which weighs 1x1012 kg and is made entirely of CaCO3(s) (MW = 100 g/mol, Ksp = 3.3×10–9). Each year the mountain received approximately 1×106 L of rainfall, which flow from the mountain completely saturated with Ca2+(aq). How many years will it take to entirely dissolve Mt. Kevinmanjaro?
Because barium sulfate is opaque to X-rays, it is suspended in water and taken internally to make the gastrointestinal tract visible in an X-ray photograph. Although barium ion is quite toxic, barium sulfate’s Ksp of 1.1 x 10–10 gives it such low solubility that it can be safely consumed. (a) What is the molar solubility of BaSO4? (b) What is its solubility in grams per 100 g of water?
A student is asked to perform a neutralization reaction between hydrochloric acid, HCl and sodium hydroxide, NaOH. The student transfers 5.00 mL of HCl solution to the titration flask and then adds 25.0 mL of distilled water and 3 drops of phenolphthalein indicator to the solution. The resulting solution uses 35.5 mL of 0.125M NaOH solution to reach the end point.a. Write a balanced chemical equation for the neutralization process.b. What will be the color of solution at the end point?c. Calculate the number of moles of NaOH used for complete neutralization.d. Calculate the strength in terms of molarity for HCl solutione. Calculate the m/v percent strength of the HCl solution
A student prepares a dilute solution of sodium hydroxide, NaOH (aq), starting with 6 M sodium hydroxide. She then titrates a 1.372 g sample of KHP with the dilute sodium hydroxide solution, NaOH (aq), to a phenolphthalein end point. 1. If the titration required 21.84 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of the sodium hydroxide solution, NaOH (aq). (Remember that KHP is potassium hydrogen phthalate, KHC8H4O4, NOT potassium hydrogen phosphorus!) 2.The student uses the same sodium hydroxide to titrate 10.00 mL of vinegar to a phenolphthalein end point. If the titration required 27.48 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of acetic acid, HC2H3O2 (aq), in the vinegar. 3. Calculate the mass percent of acetic acid, HC2H3O2 (aq), in the vinegar using the molar concentration for acetic acid, HC2H3O2 (aq), determined in part b and assuming the density of the solution is 1.01 g/mL.
Volume Acid: 20.0 mL Volume of Base added: 14.20 mL Molarity of Base: 0.10 M 1) From the volume and molarity of NaOH solution used and the stoichiometry of the reaction, HCl (aq) + NaOH (aq) --> H2O (l) + NaCl (aq) calculate the molarity of the HCl solution for the two precise trials.
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?