Chemistry: An Atoms-Focused Approach
14th Edition
ISBN: 9780393600681
Author: Gilbert
Publisher: W. W. Norton & Company
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4. Calculate the molar concentration of oxygen in water at 25°C for a
partial pressure of 0.22 atm. The Henry's law constant for oxygen is 1.3
x 103 mol/L. atm.
If 108.2 mL of water is shaken with oxygen gas at 1.6 atm, it will dissolve 0.0036 g O₂. Estimate the Henry's law constant for the
oxygen gas in water in units of g mL-¹ atm-¹.
KH= i
g mL-¹ atm-¹
Calculate the mass of oxygen (in mg) dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air. Assume the mole fraction of oxygen in air to
be 0.21 and the Henry's law constant for oxygen in water at this temperature to be 1.3 x 103 M/atm.
49.4 mg
13.7 mg
23.5 mg
9.87 mg
O 27.3 mg
Chapter 10 Solutions
Chemistry: An Atoms-Focused Approach
Ch. 10 - Prob. 10.1VPCh. 10 - Prob. 10.2VPCh. 10 - Prob. 10.3VPCh. 10 - Prob. 10.4VPCh. 10 - Prob. 10.6VPCh. 10 - Prob. 10.7VPCh. 10 - Prob. 10.8VPCh. 10 - Prob. 10.9VPCh. 10 - Prob. 10.10VPCh. 10 - Prob. 10.11VP
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- Calculate the mass of oxygen (in mg) dissolved in a 2.50 L bucket of water exposed to a pressure of 2.13 atm of air. Assume the mole fraction of oxygen in air to be 0.21 and the Henry's law constant for oxygen in water at this temperature to be 1.3 × 10-3 M/atm. Molar mass for oxygen (O2) is 31.9988 g/mol. A. 46.5 mg B. 27.0 mg C. 13.7 mg D. 23.5 mg E. 9.87 mgarrow_forwardExplain the composition and properties of water, the types of bonds between the atoms, characteristics of hydrophilic and hydrophobic molecules.arrow_forwardCalculate the mass of oxygen (in mg) dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air. Assume the mole fraction of oxygen in air to be 0.21 and the Henry's law constant for oxygen in water at this temperature to be 1.3 × 10-3 M/atm. Calculate the mass of oxygen (in mg) dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air. Assume the mole fraction of oxygen in air to be 0.21 and the Henry's law constant for oxygen in water at this temperature to be 1.3 × 10-3 M/atm. Calculate the mass of oxygen (in mg) dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air. Assume the mole fraction of oxygen in air to be 0.21 and the Henry's law constant for oxygen in water at this temperature to be 1.3 × 10-3 M/atm.arrow_forward
- Calculate the mass of oxygen (in mg) dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air. Assume the mole fraction of oxygen in air to be 0.21 and the Henry's law constant for oxygen in water at this temperature to be 1.3 × 10-3 M/atm. A) 49.4 mg B) 23.5 mg C) 9.87 mg D) 27.3 mg E) 13.7 mgarrow_forwardWater’s highly polar character is responsible for its exceptional ability to dissolve a wide range of ionic and polar-covalent substances?arrow_forwardExplain the meaning of ‘Equilibrium lattice constant’.arrow_forward
- Which of the following should have the largest Henry's law constant (kH) in water? CO2 HCl CH4 Ar Xearrow_forwardX 19. Calculate the mass of oxygen (in mg) dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air. Assume the mole fraction of oxygen in air to be 0.21 given that kH for O2 is 1.3 × 10-3 M/ atm at this temperature. 23.5 mg a b) 27.3 mg c) 49.4 mg d) 13.7 mg e) 9.87 mgarrow_forward3. Maximum solubility of an ionic compounds in water depend on different sets of conditions. Out of five sets of conditions (given below), which one is the best for getting maximum solubility? A. The magnitude of the lattice energy should be large, and the enthalpy of hydration of the ions should be large. B. The enthalpy of hydration (Delta H) of the cation should be equal to the enthalpy of hydration of the anion, regardless of the magnitude of the lattice energy C. The magnitude of the lattice energy should be small, and the enthalpy of hydration of the ions should be small. D. The magnitude of the lattice energy should be small, and the enthalpy of hydration of the ions should be large. E. The magnitude of the lattice energy should be large, and the enthalpy of hydration of the ions should be small.arrow_forward
- In an ionic compound, the size of the ions affects the internuclear distance (the distance between the centers of adjacent ions), which affects lattice energy (a measure of the force needed to pull ions apart); the lattice energy, in turn, affects the enthalpy of solution. Based on ion sizes, arrange these compounds by their expected heats of solution. RbCl RbBr Rbl RbF Most exothermic AH soln Most endothermic AH soln Answer Bankarrow_forwardComplete combustion of 8.653 g of a compound of carbon, hydrogen, and oxygen yielded 21.83 g CO₂ and 3.831 g H₂O. When 18.00 g of the compound was dissolved in 288 g of water, the freezing point of the solution was found to be -0.952 °C. For water, Kfp = = 1.86 °C/m. What is the molecular formula of the compound? Enter the elements in the order C, H, O molecular formula =arrow_forwardDetermine the partial pressure of oxygen necessary to form an aqueous solution that is 6.5 × 10-4 M O2 at 25°C. The Henry's law constant for oxygen in water at 25°C is 1.3 x 10-3 M/atm. O 0.77 atm O 0.50 atm O 0.54 atm O 1.2 atm 2.0 atmarrow_forward
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Solutions: Crash Course Chemistry #27; Author: Crash Course;https://www.youtube.com/watch?v=9h2f1Bjr0p4;License: Standard YouTube License, CC-BY