Question

Calculate the molar concentration of Nitrogen in water at 25oC for the partial pressure of 0.78 atm. The Henry's constant for Nitrogen at this temperature is 6.8x10-4 mol/L.atm

Answer 1

Answer:

S=5.3×〖10〗^(-4)  M

Explanation:

Applying Henry’s equation, S=kP

k=S/P  

k=(6.8×〖10〗^(-4) mol/L)/1

k=6.8×〖10〗^(-4) mol/L∙atm

So, the solubility of N2 at 0.78 atm:

S=(6.8×〖10〗^(-4) mol/L∙atm)(0.78 atm)

S=5.3×〖10〗^(-4)  M

Answer 2

Given: Temperature = 25°C

           Pressure = 0.78 atmospheric pressure

           Henry's constant for Nitrogen at this temperature = 6.8×10 ⁻⁴mole/L. atmospheric pressure  

To find: Molar concentration of Nitrogen

Solution:

Applying Henry's equation, S = kP

k = S/P

Where S is Henry's constant, P is the pressure.

  = (6.8×10 ⁻⁴mole/L. atmospheric pressure  )/1

  = 6.8×10 ⁻⁴mole/L-atmospheric pressure

So, the solubility of Nitrogen at 0.78 atmospheric pressure

S = ( 6.8×10 ⁻⁴mole/L-atmospheric pressure)(O.78atm)

  = 5.3 × 10⁻⁴M

Therefore, the molar concentration of Nitrogen in water at 25°C is 5.3 × 10⁻⁴M

• Molar concentration is the amount of a solute present in one unit of a solution. Its units are mol/L, mol/dm³, or mol/m³.
• Molar concentration, also known as molarity, and can be denoted by the unit M, molar.