Question

Assuming that the NaCl is completely ionized, calculate how much it will lower the solute potential of the soil at 20°C using the solute potential equation: ѰS = –iCRT where i is the ionization constant (2 for NaCl), C is the molar concentration (in mol/L), R is the pressure constant [R = 0.00831 L • MPa/(mol • K)], and T is the temperature in Kelvin (273 + °C). How much will the solute potential of the soil be lowered at 20°C?

Answer 1

The solute potential of the soil can be calculated using the solute potential equation. At 20°C, assuming complete ionization, a 1.0 molar solution of NaCl would have a solute potential of approximately -5.2 MPa.

Step-by-step explanation:

The solute potential of the soil can be calculated using the solute potential equation: ѰS = –iCRT. In this equation, i represents the ionization constant, which is 2 for NaCl. C is the molar concentration of the solution, R is the pressure constant, and T is the temperature in Kelvin. At 20°C (or 293K), assuming complete ionization, a 1.0 molar solution of NaCl would have a solute potential of approximately -5.2 MPa.

Answer 2

Ѱ
`S=-4.872MPa`

Step-by-step explanation:

Hello,

For this exercise, it must be clear that the concentration is not given, nonetheless, one can assume it arbitrarily as 1M, thus, the solute potential turns out into:

Ѱ
`S=-iCRT=-2*1(mol)/(L) *0.00831(MPa*L)/(mol*K) *293.15K\\`

Ѱ
`S=-4.872MPa`

Nevertheless, if you have a different concentration, you just must change the 1M concentration by the one you're given and subsequently modify the answer.

Best regards.