Question

The current partial pressure of CO2 in the Earth's atmosphere is 3.9 • 10-4 atm. If the Henry's law constant is 2.3 • 10-2 M/atm, calculate the equilibrium concentration of dissolved CO2 in bodies of water.

Answer #1

The partial pressure of CO2 gas inside a bottle of soda is 3 atm
at 25°C. What mass (in g) of CO2 is dissolved in a 0.56
liter bottle of soda? The Henry's law constant for CO2 in
water is 3.3x 10-2mol/Latm at 25°C. Enter to 1 decimal place.

Henry's law constant for CO2 at 38oC is 2.28 x 10–3
mol/L\cdot⋅atm. Calculate the pH of a solution of CO2 at 38oC in
equilibrium with the gas at a partial pressure of 3.20 atm. Assume
that all dissolved CO2 is in the form of carbonic acid (H2CO3). Ka1
= 4.3 x 10–7 and Ka2 = 5.6 x 10–11 for carbonic acid.

The solubility of CO2 in water at 25C and partial pressure=1 atm
is 0.034M. How high do you have to increase the carbon dioxide
pressure to get a CO2 of 0.15M, assuming that CO2 continues to obey
Henry's law?

The concentration of CO2 in a soft drink under a pressure of 2.3
atm is 0.071 M. Calculate the concentration of CO2 in a soft drink
after the bottle is opened and equilibrates at the same temperature
under a CO2 partial pressure of 3.0 x 10-4atm.
The answer is 9.3 * 10^-6 M but I don't know how to start this
problem. Pls help!

41. Henry's law constant for CO2
at 38°C is 2.28
×10−3 mol / L ·
atm. Calculate the pH of a solution of
CO2 at 38°C in
equilibrium with the gas at a partial pressure of
3.25atm.
A solution of formic acid (HCOOH) has a pH of 2.17. How many
grams of formic acid are there in 100.0 mL of solution? g/100.0
mL

Calculate the concentration of Co2 in rainwater at 25C using
Henry's law. Assume that the water is saturated with air that
contains 350 ppm of CO2. The Henry's law constant for CO2 is
KH=3.4X10-2 MOL/L-ATM at 15C . Express the result in molarity and
ppm. Calculate the concentration of NO in rainwater at 25 C that is
in equlibrium with polluted air where the NO concentration is 10
ppm. The Henry's law constant for No is Kh=2x10-4 mol/l-atm at 25C...

The solubility of CO2 in a salt water lake at 298 K and 750 torr
pressure was found to be 1.0 x 10-5 moles CO2/liter of aqueous
solution. The Henry’s Law constant in this case is 3.0 x 10-2
mol/L.atm. Please find the partial pressure of CO2 (g) (PCO2, in
atm) in the air above the lake (2) Please use your answer to
determine the percentage of CO2 in the atmosphere (2) Given the
percentage of CO2 in the atmosphere...

3. The pressure inside an unopened can of soda is 2.5 atm (you
may assume all of this pressure is from CO2). If the concentration
of CO2 under these conditions is 0.080 M, find the Henry’s law
constant (in M/atm), and use this to calculate how many grams of
CO2 will escape from 355 mL of soda (a 12-oz can) when it is opened
to the atmosphere, where the concentration of CO2 is 41 ppm.

A handbook lists the value of the Henry's Law constant as
1.400 ✕ 10−3 mol L-1 atm-1 for methane, CH4, dissolved in water at
25°C. Calculate the mole fraction of methane in water at an methane
partial pressure of 380. torr.

The solubility of oxygen, O2, in water is 7.20 ✕ 10−4 mol/L at
0°C when the nitrogen pressure above water is 0.554 atm. Calculate
the solubility of oxygen in water when the partial pressure of
oxygen above water is 1.083 atm at 0°C? The Henry's Law constant
for oxygen is 1.30 ✕ 10−3 mol/ L atm.

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