Question

Calculate the successive equilibrium potentials for Na⁺, K, and Cl⁻ at 20°C given the following outside and inside concentrations of the ions: Na+: inside= 145 mM; outside= 12mM K+: inside= 5 mM; outside= 150mM Cl-: inside= 110 mM; outside= 10mM.

Answer 1

To calculate the successive equilibrium potentials for Na⁺, K, and Cl⁻, we can use the Nernst equation. The Nernst equation is given by Ecell = E°cell - (RT/nF) * ln(Q), where Ecell is the cell potential, E°cell is the standard cell potential, R is the gas constant, T is the temperature in Kelvin, n is the number of moles of electrons transferred in the reaction, F is Faraday's constant, and Q is the reaction quotient.

Step-by-step explanation:

To calculate the successive equilibrium potentials for Na⁺, K, and Cl⁻, we can use the Nernst equation. The Nernst equation is given by Ecell = E°cell - (RT/nF) * ln(Q), where Ecell is the cell potential, E°cell is the standard cell potential, R is the gas constant, T is the temperature in Kelvin, n is the number of moles of electrons transferred in the reaction, F is Faraday's constant, and Q is the reaction quotient.

For Na⁺, the equilibrium potential can be calculated using the following equation:

Ecell = E°cell - (RT/nF) * ln(Q) = E°cell - (RT/nF) * ln([Na⁺]ₒ/[Na⁺]ᵢ)

Similarly, for K, the equilibrium potential can be calculated using the equation:

Ecell = E°cell - (RT/nF) * ln(Q) = E°cell - (RT/nF) * ln([K⁺]ₒ/[K⁺]ᵢ)

And for Cl⁻, the equilibrium potential can be calculated using the equation:

Ecell = E°cell - (RT/nF) * ln(Q) = E°cell - (RT/nF) * ln([Cl⁻]ₒ/[Cl⁻]ᵢ)

Substituting the given concentrations and E°cell values into the respective equations will give the successive equilibrium potentials for Na⁺, K, and Cl⁻.