b.löns inhatthe original solution?25. Iron and its compounds make up 5% of Earth's crustMany compounds that contain ferrous ions, Fe2+(a0)are soluble. As a result, ferrous ions are often present inwater supplies, especially from wells. A simple test foriron in water is to fill a large container with a sampleof the water and then leave it exposed to air for a fewdays. If the water contains iron, the ferrous ions willgradually change to ferric ions, Fe3+(aq). The waterwill take on the yellowish colour of ferric compounds,which are insoluble. Explain why ferric compounds aregenerally less soluble than ferrous compounds.26. A student titrated nitric acid, HNO3(aq), withsodium hydroxide, NaOH(aq), using phenolphthaleinindicator. The following data were recorded. Use thedata to calculate the concentration of nitric acid.volume of HNO3(aq) = 25.00 mLconcentration of NaOH(aq) = 0.982 mol/LBurette Readings for the Volume of Sodium Hydroxide%3D%3D31,Reading (mL)Trial 1Trial 2Trial 3Final reading18.2836.4828.44Initial reading0.0018.2810.22

25) In the environment (soil, natural waters, etc.) I think ferric ions tend to be less soluble…

26. A student titrated nitric acid, HNO3(aq), with sodium hydroxide, NaOH(aq), using phenolphthalein indicator. The following data were recorded. Use the data to calculate the concentration of nitric acid. volume of HNO3(aq) = 25.00 mL %3D Concentrati

26. A student titrated nitric acid, HNO3(aq), with sodium hydroxide, NaOH(aq), using phenolphthalein indicator. The following data were recorded. Use the data to calculate the concentration of nitric acid. volume of HNO3(aq) = 25.00 mL %3D Concentrati

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The flask contains 10.0 mL10.0 mL of HClHCl and a few drops of phenolphthalein indicator. The buret contains 0.110 M NaOH.0.110 M NaOH. It requires 31.4 mL31.4 mL of the NaOHNaOH solution to reach the end point of the titration. What is the initial concentration of HClHCl?
Dr. Donwonree tried to determine the vitamin C content in apple juice which he bought at CheMarket. He measured out 50.0 mL of the juice and added the HCl, KI, and starch. Then he started the titration by adding KIO3 solution into the juice. The concentration of the KIO3 solution was 0.200 M and it took only 1.50 mL of KIO3 to reach the endpoint. How much vitamin C (mg) is contained in 1.00 L of this apple juice?
A technician would like to standardize an unknown Ca(OH)2 solution. It takes 18.53 mL of a 0.174 M solution of HCI to titrate 25.00 mL the unknown Ca(OH)2 solution. Calculate the molarity of the Ca(OH)2 solution. Tip: Don't forget to consider the mole ratio between HCl and Ca(OH)2. 2 HCI (aq) + Ca(OH), (aq) CaCl2 (aq) + 2 H2O (1)
You have been provided with a 2.08 x 10-2 L sample of lithium hydroxide (LiOH) of unknown concentration. You perform a titration with 2.19 M nitric acid (HNO3), and find that 24.6 mL are required to reach the equivalence point (as determined using a coloured indicator). What is the concentration of the lithium hydroxide solution in mol L-1?
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. A.) 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!) B.) 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. C.) 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.
Calculate the number of grams of AgCl will precipitate out of solution if 125 mL of 0.500 M AgNO3 is combined with 275 mL of 0.235 M NaCl according to the following AgNO3 (aq) + NaCl (aq) --> AgCl (s) + NaNO3 (aq)
Titration of a 11.0 mLmL solution of HClHCl requires 32.4 mLmL of 0.11 MM NaOHNaOH. What is the molarity of the HClHCl solution? Express your answer using two significant figures.
The total cation content of natural water is often determined by exchanging the cations for hydrogen ions on a strong acid ion-exchange resin. A 25.00 mL sample of a natural water was diluted to 100.00 ML with distilled water, and 2.06 g of a cation - exchange resin was added. After stirring, the mixture was filtered and the solid remaining on the filter paper was washed with three 15.00 mL portions of water. The filtrate and washings required 16.30 mL of 0.0282 M NaOH to give a bromocresol green end point. a) Calculate the number of millimoles of cation present in exactly 1.00 L of sample. b ) Report the results in terms of milligrams of CaCO3 per liter. Only typed solution.
You have been provided with a 30.0 mL sample of hydrochloric acid (HCl) of unknown concentration. You perform a titration with 1.48 M sodium hydroxide (NaOH), and find that 3.81 x 10-2 L are required to reach the equivalence point (as determined using a coloured indicator). What is the concentration of the hydrochloric acid?
You are preparing standard acid and base solutions for the laboratory, using potassium hydrogen phthalate (KHC₈H₄O₄, abbreviated KHP) as the primary standard. KHP (molar mass = 204.22 g/mol) has one acidic hydrogen. You prepared solutions of both NaOH and HCl. It took 22.65 mL of the NaOH solution to titrate (react exactly with) 1.55 g KHP. It then took 32.35 mL of HCl solution to titrate 25.00 mL of the NaOH solution. What is the molarity of the HCl solution?
A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 51 mg of oxalic acid (H2C2O4), a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250 mL of distilled water. The student then titrates the oxalic acid solution with her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 19.2 mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution.
A titration involves adding a reactant of known quantity to a solution of an another reactant while monitoring the equilibrium concentrations. This allows one to determine the concentration of the second reactant. The equation for the reaction of a generic weak acid HA with a strong base is HA(aq) + OH(aq) →A¯(aq) + H₂O (1) A certain weak acid, HA, with a K, value of 5.61 x 10 ", is titrated with NaOH. 6 Part A A solution is made by titrating 9.00 mmol (millimoles) of HA and 2.00 mmol of the strong base. What is the resulting pH? Express the pH numerically to two decimal places. ▸ View Available Hint(s) pH = Submit ▾ Part B pH = IVE] ΑΣΦ Submit A → c More strong base is added until the equivalence point is reached. What is the pH of this solution at the equivalence point if the total volume is 66.0 mL ? Express the pH numerically to two decimal places. ▸ View Available Hint(s) IVE ΑΣΦ A + Ċ ? Doowoon Review | Constants | Periodic Table ?