Question

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 .Express the result in molarity and ppb

Answer #1

CO2 dissolves in water to produce H2CO3 in the same way that SO2
produces H2SO3. (a) Confirm by calculation that the pH of
CO2-Saturated water at 25 degrees C is 5.6, given that the CO2
concentration in air is 365ppm. For carbon dioxide, the henry's law
constant KH=3.4x10^-2M atm^-1 at 25 degrees C. The Ka for carbonic
acid, H2CO3, is 4.5x10^-7. (b) Recalculate the pH for carbon
dioxide concentration of 560ppm.

Using Raoult's law for water and Henry's law for nitrogen,
calculate the pressure and gas-phase composition (mole fractions)
in a system containing a liquid that is 1.200 mole% N2
and 98.80 mole% water in equilibrium with nitrogen gas and water
vapor at 50.0°C.
The Henry's law constant for nitrogen in water is recommended by
NIST to be well represented by
kH = 0.000625 exp[1300 (1/T –
1/298.15)] mol N2 / (kg H2O bar), where
T is measured in Kelvin
a)...

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.

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

1. The atmospheric concentration of CO2 has exceeded 400 ppm for
most of 2016. Water that is in contact with air will absorb CO2
according to Henry’s Law:
[CO2] = kCO2 ∙ PCO2 with kCO2 = 3.1×10–2M/atm at 25°C
a) Use this information to calculate the molarity of CO2(aq) in
rain water. Assume that the barometric pressure is 1 atm, the
temperature is 25°C, and [CO2] is the equilibrium
concentration.
b) Calculate the pH of the rainwater assuming that all...

Use Henry's law and the solubilities given below to calculate
the total volume of nitrogen and oxygen gas that should bubble out
of 2.0 L of water upon warming from 25 ∘C to 50 ∘C. Assume that the
water is initially saturated with nitrogen and oxygen gas at 25 ∘C
and a total pressure of 1.0 atm. Assume that the gas bubbles out at
a temperature of 50 ∘C. The solubility of oxygen gas at 50 ∘C is
27.8 mg/L...

1) Use Henry's law to determine the molar solubility of helium
at a pressure of 1.9 atm and 25 ∘C. Henry’s law constant for helium
gas in water at 25 ∘C is 3.70⋅10−4M/atm.
2) A 2.800×10−2M solution of NaCl in water
is at 20.0∘C. The sample was created by dissolving a sample of NaCl
in water and then bringing the volume up to 1.000 L. It was
determined that the volume of water needed to do this was 999.2 mL...

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