Knowing that at 0 oC and an oxygen pressure of 1.00 atm, the aqueous solubility of O2 (g) is 48.9 mL O2 per liter. The approximate values for the molarity of O2 (g) in solution and the partial pressure of O2 above a 8.23 x 10-4 M O2 (g) saturated aqueous solution at 0 oC are respectively:
A. 2.18 M and 3.78 x 10-4 atm
B. 2.18 x 10-3 M and 0.378 atm
C. 0.0446 M and 0.0179 atm
D. 44.6 M and 1.84 x 10-5 atm
Knowing that at 0 oC and an oxygen pressure of 1.00 atm, the aqueous solubility of...
For the saturated aqueous solution of O2(g) at 20 C and 1 atm
with the solubility increase, decrease or stay no charge when the
indicated change occurs?
For a saturated aqueous solution of O2(3) at 20 °C and 1 atm, will the solubility increase, decrease or stay no change when the indicated change occurs? (1) The solubility of O23) [Select] when pressure increases. (2) The solubility of O2(s) [ Select ] when temperature increases.
The solubility of CO in water at 0°C and 1 atm CO pressure is 0.0354 mg of CO in 1 mL of water. Calculate the molarity of aqueous CO solution at the normal partial pressure of CO of 0.00036 atm? A)3.2×10-3M B)2.9×10-4M C)1.6×10-3M D)1.3×10-5M E)4.5×10-7M
The partial pressure of O2 in air at sea level is 0.21 atm. The solubility of O2 in water at 20 ∘C , at 1 atm gas pressure, is 1.38×10−3 M. Using Henry's law and the data in the introduction, calculate the molar concentration of O2 in the surface water of a mountain lake saturated with air at 20 ∘C and an atmospheric pressure of 660 torr .
What pressure of O2 is required to keep the [O2] = 0.065 M in aqueous solution at 25°C kH O2 @ 25°C =1.3 x 10-3 M/atm
need #7-10 answered
6. The solubility of nitrogen gas at 25°C and a nitrogen pressure of 522 mmHg is 4.7 x 10 mol/L. What is the value of the Henry's Law constant in mol/L-atm? A) 6.8 × 10-4 mol/L-atm B) 4.7 x 10 mol/L-atm C) 3.2 × 104 moVL-atm D) 9.0 x 10 mol/L atm E) 1.5 x 10mol/L atm 7. According to Raoult's law, which statement is false? A) The vapor pressure of a solvent over a solution decreases...
#12
atm. pressure? a) 104.2 °C (b) 101.68 °CC ) 100.42 °Cd ) 101.26 °C 11. A diver has a breathing mixture of air that has a partial pressure of N2 of 1.44 atm. and O2 of 0.36 atm at a total pressure of 1.8 atm when he dives. Determine the solubility of nitrogen in his blood at this pressure, assuming his blood behaves like water. The Henry's Law constant for nitrogen in water is 6.1 x 10mol.L'atm"! a) 8.8...
The solubility product constant for La(IO3)3 is 1.00×10-11 at 25 oC. What is the molar concentration of IO3- ions in a saturated solution of La(IO3)3? Assume an ideal solution at 25 oC. How many grams of La(IO3)3 (663.6 g/mol) can be dissolved in 900 mL of pure water at 25 oC? How many grams of La(IO3)3 can be dissolved in 900 mL of a 0.100 M KIO3 solution at 25 oC? Use activities for this calculation. Activity coefficients can be found...
If the Henry’s law constant for oxygen in water is 1.3 x 10-3 M/atm at 25 oC. What pressure of oxygen is required to produce an aqueous solution that is 0.25M in oxygen?
Thank you for your help! 1. If an ideal gas has a pressure of 9.239.23 atm, a temperature of 55.2855.28 °C, and a volume of 97.8997.89 L, how many moles of gas are in the sample? Moles: 2.The balanced equation for the neutralization reaction of aqueous H2SO4H2SO4 with aqueous KOHKOH is shown. H2SO4(aq)+2KOH(aq)⟶2H2O(l)+K2SO4(aq)H2SO4(aq)+2KOH(aq)⟶2H2O(l)+K2SO4(aq) What volume of 0.4100.410 M KOHKOH is needed to react completely with 15.315.3 mL of 0.1700.170 M H2SO4H2SO4? volume:____ mL 3.How many grams of solute are present...
An aqueous CaCl2 solution has a vapor pressure of 80.2 mmHg at 50 ∘C. The vapor pressure of pure water at this temperature is 92.6 mmHg. What is the concentration of CaCl2 in mass percent? A hypothetical solution forms between a solid and a liquid. The values of the thermodynamic quantities involved in the process are shown in the following table. Action Enthalpy separation of solute 11.5 kJ/mol separation of solvent 21.8 kJ/mol formation of solute-solvent interactions -86.7 kJ/mol solute...