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(4 أل containing The density of concentrated ammonia, which is 28.0% w/w NH3, is 0.899 g/mL. What volume of this reagent should be diluted to 1.0 x10³ mL to make a solution that is 0.036 M in NH3? nous solution contains 45.1 mg of a pesticide. Express the

(4 أل containing The density of concentrated ammonia, which is 28.0% w/w NH3, is 0.899 g/mL. What volume of this reagent should be diluted to 1.0 x10³ mL to make a solution that is 0.036 M in NH3? nous solution contains 45.1 mg of a pesticide. Express the

Chemistry
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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Homework 1) A solution of 0.10 M SO4 is available. What is the normality of this solution when used in the following reactions? a- Pb²+ (aq) + SO4²- (aq) b. HCl(aq) + SO4² (aq). ← PbSO4(s) →HSO4 (aq) + Cl(aq) H₂SO3(aq) + 5H₂O(1) c. SO42- + 4H3O*(aq) + 2e → 2) The concentration of lead in an industrial waste stream is 0.28 ppm. What is its molar concentration? 3) Commercially available concentrated hydrochloric acid is 37.0% w/w HCl. Its density is 1.18 g/mL. Using this information calculate (a) the molarity of concentrated HCl, and (b) the mass and volume (in milliliters) of solution containing 0.315 mol of HCl. 4 The density of concentrated ammonia, which is 28.0% w/w NH3, is 0.899 g/mL. What volume of this reagent should be diluted to 1.0 x10³ mL to make a solution that is 0.036 M in NH3? 5) A 250.0-mL aqueous solution contains 45.1 mg of a pesticide. Express the pesticide's concentration in weight percent, parts per million, and parts per billion. 6.92x10- 6) What is the pH of a solution for which the concentration of H* is 6M? What is the [H*] in a solution whose pH is 8.923? 7) Calculate the molarity of a potassium dichromate solution prepared by placing 9.67 g of K₂Cr₂O7 in a 100-mL volumetric flask, dissolving, and diluting to the calibration mark. 8) For each of the following, explain how you would prepare 1.0 L of a solution that is 0.10 M in K+. Repeat for concentrations of 1.0 x 102 ppm K and 1.0% w/v Kt. a. KCI b. K₂SO4 c. K3Fe(CN)6
Transcribed Image Text:Homework 1) A solution of 0.10 M SO4 is available. What is the normality of this solution when used in the following reactions? a- Pb²+ (aq) + SO4²- (aq) b. HCl(aq) + SO4² (aq). ← PbSO4(s) →HSO4 (aq) + Cl(aq) H₂SO3(aq) + 5H₂O(1) c. SO42- + 4H3O*(aq) + 2e → 2) The concentration of lead in an industrial waste stream is 0.28 ppm. What is its molar concentration? 3) Commercially available concentrated hydrochloric acid is 37.0% w/w HCl. Its density is 1.18 g/mL. Using this information calculate (a) the molarity of concentrated HCl, and (b) the mass and volume (in milliliters) of solution containing 0.315 mol of HCl. 4 The density of concentrated ammonia, which is 28.0% w/w NH3, is 0.899 g/mL. What volume of this reagent should be diluted to 1.0 x10³ mL to make a solution that is 0.036 M in NH3? 5) A 250.0-mL aqueous solution contains 45.1 mg of a pesticide. Express the pesticide's concentration in weight percent, parts per million, and parts per billion. 6.92x10- 6) What is the pH of a solution for which the concentration of H* is 6M? What is the [H*] in a solution whose pH is 8.923? 7) Calculate the molarity of a potassium dichromate solution prepared by placing 9.67 g of K₂Cr₂O7 in a 100-mL volumetric flask, dissolving, and diluting to the calibration mark. 8) For each of the following, explain how you would prepare 1.0 L of a solution that is 0.10 M in K+. Repeat for concentrations of 1.0 x 102 ppm K and 1.0% w/v Kt. a. KCI b. K₂SO4 c. K3Fe(CN)6
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