Question 8.
According to Henry's law:
The equilibrium concentration of dissolved oxygen * Henry's constant (KH) = pressure of oxygen
i.e. Equilibrium concentration of dissolved oxygen * 730 atm.L/mol = (21/100) * 0.62 atm
i.e. Equilibrium concentration of dissolved oxygen = 1.7836*10-4 mol/L
= 1.7836*10-4 mol/L * 32 g/mol
= 5.71 mg/L
the equilibrium concentration of dissolved oxygen jn mg/L in Lake Titicaca. The elevation is 3.850 m...
Lake Titicaca is located high in the Andes Mountains between Peru and Bolivia. Its surface is 3811 m above sea level, where the average atmospheric pressure is 0.636 atm. During the summer, the average temperature of the water’s surface rarely exceeds 15°C. What is the solubility of oxygen in Lake Titicaca at that temperature? Express your answer in molarity and mg/L.
Lake Titicaca is situated at an altitude of 3810 m in the Bolivian Andes. Calculate the solubility of oxygen (in mg/L) in this lake at a temperature of 8.47 ºC. The Henry's Law constant at this temperature is 1.90×10-8 mol L-1Pa-1
Lake Titicaca is situated at an altitude of 3810 m in the Bolivian Andes. Calculate the solubility of oxygen in this lake at a temperature of 5C. (The Henry’s law constant at 5C is 1.9x10-8 mol L-1 Pa-1. The vapour pressure of water is approximately 870 Pa at 5C)
Calculate the concentration in units of mg/L for oxygen dissolved in 1050.0 mL of water at 25 °C, if the partial pressure of O2 in gas phase in equilibrium with the water is 238.1 mm Hg. Assume the density of water =1 g/mL
Calculate the theoretical oxygen demand for a 130 mg/L aqueous solution of lactic acid (C3H6O3). Calculate the equilibrium concentration of dissolved oxygen in 25°C water at sea level (p = 1.00 atm), and again at 4000 m elevation in 5°C water. [Use the exponential p vs. z equation, not the empirical formula.]
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 0.41 and the Henry's law constant for oxygen in water at this temperature to be 1.3 × 10-3 M/atm. 96.3 mg 49.4 mg 63.2 mg 48.2 mg
26 Calculate the equilibrium concentration of dissolved oxygen in 15°C water at 1 atm, and again at 2,000 m elevation. Suppose the gas above the soda in a bottle of soft drink is pure CO2 at a pressure of 2 atm. Calculate (CO2) at 25°C. 27
Calculate the equilibrium concentration of dissolved oxygen in 25°C water at sea level (p = 1.00 atm), and again at 4000 m elevation in 5°C water. [Use the exponential p vs. z equation provided in the lectures, not the empirical formula given in the textbook.] P(z)=P(O)exp(-z/H)
The saturation concentration of dissolved oxygen in freshwater can be calculated with the equation, ln Osf = −139.34411 + 1.575701 × 105 Ta − 6.642308 × 107 T2 a + 1.243800 × 1010 T3 a − 8.621949 × 1011 T4 where Osf is the saturation concentration of dissolved oxygen in freshwater at 1 atm (mg/L) and Ta is the absolute temperature in Kelvin (K), where Ta = T + 273.15, where T is the temperature in Celsius (oC). According to...
Find the equilibrium concentration of aluminum ions in pure water at 25 degree C caused by the dissociation of Al(OH)_3. Express the answer both in units of M and mg/L. Find the equilibrium pH value if copper ion (Cu^2+) concentration in water is 1.2 mg/L. The copper ion is dissolved from Cu(OH)_2. Calculate the equilibrium concentration of dissolved oxygen in mg/L in 10 degree C water (a) at msl (mean sea level), and (b) at 600 m elevation.