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Chemistry: The Molecular Nature of Matter
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- The amount of oxygen, O2, dissolved in a water sample at 25 C can be determined by titration. The first step is to add solutions of MnSO4 and NaOH to the water to convert the dissolved oxygen to MnO2. A solution of H2SO4 and KI is then added to convert the MnO2 to Mn2+, and the iodide ion is converted to I2. The I2 is then titrated with standardized Na2S2O3. (a) Balance the equation for the reaction of Mn2+ ions with O2 in basic solution. (b) Balance the equation for the reaction of MnO2 with I in acid solution. (c) Balance the equation for the reaction of S2O32 with I2. (d) Calculate the amount of O2 in 25.0 mL of water if the titration requires 2.45 mL of 0.0112 M Na2S2O3 solution.arrow_forwardWhen 85.0 mL of 0.250 M Ba(OH)2 solution is added to 85.00 mL of 0.250 M Al (NO3)3 solution, a white gelatinous precipitate of Al(OH)3; is formed. Assuming 100% yield, (a) what mass (in grams) of Al(OH)3 is formed? (b) what is the molarity of each of the ions Ba2+, OH-, Al3+, NO3- in the resulting solution?arrow_forwardUsing circles to represent cations and squares to represent anions, show pictorially the reactions that occur between aqueous solutions of (a) Fe3+ and OH-. (b) Na+ and PO43-.arrow_forward
- Calculate the concentration of all ions present in each of the following solutions of strong electrolytes. a. 0.100 mole of Ca(NO3)2 in 100.0 mL of solution b. 2.5 moles of Na2SO4 in 1.25 L of solution c. 5.00 g of NH4Cl in 500.0 mL of solution d. 1.00 g K3PO4 in 250.0 mL of solutionarrow_forwardStrong acid solutions may have their concentration determined by reaction with measured quantities of standard sodium carbonate solution. What mass of Na2CO3 is needed to prepare 250. mL of 0.0500 M Na2CO, solution?arrow_forwardThe presence of arsenic in a sample that may also contain another Group 5A element, antimony, can be confirmed by first precipitating the As3+ and Sb3+ ions as yellow solid As2S3 and orange solid Sb2S3. If aqueous HCI is then added, only Sb2S3 dissolves, leaving behind solid As2S3. The As2S3 can then be dissolved using aqueous HNO3. 3 As2S3(s) + 10 HNO3(aq) + 4 H2O() 6 H3AsO4(aq) + 10 NO(g) + 9 S(s) Finally, the presence of arsenic is confirmed by adding AgNO3 to the solution of H3AsO4 to precipitate a reddish brown solid AgxAsOy The composition of this solid is As, 16.199% and Ag, 69.964%. (a) What are the oxidation numbers of As, S, and N in the reaction of As2S3 with nitric acid? (b) What is the formula of the reddish brown solid AgxAsOy?arrow_forward
- The blood alcohol (C2H5OH) level can be determined by titrating a sample of blood plasma with an acidic potassium di-chromate solution, resulting in the production of Cr3+ (aq) and carbon dioxide. The reaction can be monitored because the dichromate ion (Cr2O72) is orange in solution, and the Cr3+ ion is green. The balanced equations is 16H+(aq) + 2Cr2O72(aq) + C2H5OH(aq) 4Cr4+(aq) + 2CO2(g) + 11H2O(l) This reaction is an oxidationreduction reaction. What species is reduced, and what species is oxidized? How many electrons are transferred in the balanced equation above?arrow_forwardA mountain lake that is 4.0 km × 6.0 km with an average depth of 75 m has an H+(aq) concentration of 1.3 × 10−6 M. Calculate the mass of calcium carbonate that would have to be added to the lake to change the H+(aq) concentration to 6.3 × 10−8 M. Assume that all the carbonate is converted to carbon dioxide, which bubbles out of the solution.arrow_forwardThe molarity of iodine in solution can be determined by titration with arsenious acid, H3AsO4. The unbalanced equation for the reaction is H3AsO3(aq)+I2(aq)+H2O2 I(aq)+H3AsO4(aq)+2 H+(aq)A 243-mL solution of aqueous iodine is prepared by dissolving iodine crystals in water. A fifty-mL portion of the solution requires 15.42 mL of 0.134 M H3AsO3 for complete reaction. What is the molarity of the solution? How many grams of iodine were added to the solution?arrow_forward
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