(a)
Interpretation:
The solution in which the greater volume of titrant is required for titration of a particular sample of Fe2+(aq) should be explained.
Concept introduction:
Redox reactions or oxidation reduction reactions are a type of
(b)
Interpretation:
Volume of 0.1000 M MnO4- which is required for a titration when the same titration requires 24.50 mL of 0.1000 M Cr2O72- should be determined.
Concept introduction:
Redox reactions or oxidation reduction reactions are a type of chemical reaction which involves transfer of electrons between chemical species. Here oxidation state of a chemical state is changed by gaining or removing electrons.
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EBK GENERAL CHEMISTRY
- Assume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO2H, in enough water to make 1.00 102 mL of solution and then titrate the solution with 0.108 M NaOH. C6H5CO2H(aq) + OH(aq) C6H5CO2(aq) + H2O() (a) What was the pH of the original benzoic add solution? (b) What are the concentrations of all of the following ions at the equivalence point: Na+, H3O+, OH, and C6H5CO2? (c) What is the pH of the solution at the equivalence point?arrow_forwardCalculate the solubility in grams per 100 mL of BaF2 in a 0.10 M BaCl2 solution.arrow_forwardOne half liter (500. mL) of 2.50 M HCl is mixed with 250. mL of 3.75 M HCl. Assuming the total solution volume after mixing is 750. mL, what is the concentration of hydrochloric acid in the resulting solution? What is its pH?arrow_forward
- A student is given 0.930 g of an unknown acid, which can be either oxalic acid, H2C2O4, or citric acid, H3C6H5O7. To determine which acid she has, she titrates the unknown acid with 0.615 M NaOH. The equivalence point is reached when 33.6 mL are added. What is the unknown acid?arrow_forwardPhosphate ions are abundant in cells, both as the ions themselves and as important substituents on organic molecules. Most importantly, the pKa for the H2PO4 ion is 7.20, which is very close to the normal pH in the body. H2PO4(aq) + H2O() H3O+(aq) + HPO42(aq) 1. What should the ratio [HPO42]/[H2PO4] be to control the pH at 7.40?arrow_forwardin the titration of 50.0 mL of 0.0200 M C6H5COOH(aq) with 0.100 M NaOH(aq), what is/are the major species in the solution after the addition of 5.0 mL of NaOH(aq)?arrow_forward
- 134 grams of potassium sorbate KCH3 (CH)4CO2 is fully dissolved in 100.00 mL of water, which is carefully transferred to a conical flask. Then 100.00 mL of 0.240 M HNO3 is added dropwise to this solution from a burette. Given: Ka (sorbic acid) = 1.7 × 1O^-5 Showing all your calculations and reasoning, determine the pH of the solution that results after the addition of all the acid mentioned above. Suppose that the titration continues. Determine the pH of the solution in the flask at theequivalence pointarrow_forward1) Potassium permanganate solutions used in oxidation-reduction titrations are often standardized against sodium oxalate, Na₂C₂O₄, used as a primary standard. The reaction involved is 5C₂O₄²⁻(aq) + 2MnO₄⁻(aq) + 16 H⁺(aq) → 2Mn²⁺(aq) + 8H₂O(l) + 10CO₂(g) A 0.2452 g sample of sodium oxalate is dissolved in 100 mL of acid solution, and the permanganate solution is added slowly from a buret. The endpoint is reached when 15.85 mL of the permanganate solution has been added. The molar mass of sodium oxalate is 134.00 g/mol. Calculate [MnO₄⁻], the molar concentration of the permanganate solution. 2) Potassium permanganate solutions used in oxidation-reduction titrations are sometimes standardized against Fe²⁺ ion. The reaction involved is 8H⁺(aq) + MnO₄⁻(aq) + 5Fe²⁺(aq) → 5Fe³⁺(aq) + Mn²⁺(aq) + 4H₂O(l) .A convenient source for Fe²⁺ ion is ammonium iron(II) sulfate, (NH₄)₂Fe(SO₄)₂(H₂O)₆ (FW = 392.14), also known as Mohr's salt, which is readily crystallized, and the crystals resist oxidation…arrow_forwardAssume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO₂H, in enough water to make 5.00 x 10² mL of solution and then titrate the solution with 0.168 M NaOH. C6H5CO₂H(aq) + OH(aq) → C₂H₂CO₂ (aq) + H₂O(l) What are the concentrations of the following ions at the equivalence point? 0.0033722 1.39e-8 Na+, H3O+, OH- C6H5CO₂ X M Na+ X MH₂0+ 7.21e-7 X MOH™ 0.0033722 XM C6H5CO₂ What is the pH of the solution? 7.86arrow_forward
- The ionization constant of lactic acid, CH,CH(OH)CO,H, an acid found in the blood after strenuous exercise, is 1.36 x 10-4. What is the concentration of hydronium ion in the solution of 0.102 M lactic acid? CH;CH(OH)CO,H (aq) + H,O (1) → H;O• (aq) + CH;CH(OH)CO, (aq) O 0.00372 M O 0.0165 M O 0.00549 M O 0.227 Marrow_forwardConsider a flask containing 25.00 mL of 0.100 M sodium benzoate (NaC6H5COO). This is titrated with a 0.110 M nitric acid solution from a burette. Given: Kb of C6H5COO− is 1.6 × 10−101 Determine the pH of the solution in the flask after 32.00 mL of the acid has been added? 1. 2 Determine the pH of the solution in the flask at the half-way point of the titration.arrow_forwardGiven the equation Ag(aq)+ + 2NH3(aq) ----> [Ag(NH3)2]+(aq), determine the concentration of NH3(aq) that is required to dissolved 261mg of AgCl in 100 ml of solution. The Ksp of AgCl is 1.77 x 10-10 Kf = 2 x 107.arrow_forward
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