$$\begin{array} { | l | l | l | }
\hline & \begin{array} { l }
\bf{ Extracellular-concentration } \
( \bf { mM } )
\end{array} & \begin{array} { l }
\bf { Intracellular-concentration } \
( \bf { mM } )
\end{array} \
\bf{ Inn }\
\hline \mathbf { Na } ^ { + } & 300 & 50 \
\hline \mathbf { K } ^ { + } & 40 & 350 \
\hline
\end{array}$$
-Calculate the equilibrium potential for potassium. Assume a temperature of 37°C.
A) +48.2 mV
B) 0.0 mV
C) -58.4 mV
D) -80.0 mV

Question

$$\begin{array} { | l | l | l | } 
\hline & \begin{array} { l } 
\bf{ Extracellular-concentration } \
( \bf { mM } )
\end{array} & \begin{array} { l } 
\bf { Intracellular-concentration } \
( \bf { mM } )
\end{array} \
\bf{ Inn }\
\hline \mathbf  { Na } ^ { + } & 300 & 50 \
\hline \mathbf { K } ^ { + } & 40 & 350 \
\hline
\end{array}$$
-Calculate the equilibrium potential for potassium. Assume a temperature of 37°C.
A) +48.2 mV
B) 0.0 mV
C) -58.4 mV
D) -80.0 mV

Quizplus · Accepted Answer

The equilibrium potential for potassium can be calculated using the Nernst equation:E = (RT/zF) * ln([K+]o/[K+]i)where:E is the equilibrium potential in voltsR is the ideal gas constant (8.314 J/mol*K)T is the absolute temperature in Kelvin (37°C = 310K)z is the valence of the ion (+1 for potassium)F is the Faraday constant (96,485 C/mol)[K+]o is the extracellular potassium concentration (40 mM)[K+]i is the intracellular potassium concentration (350 mM)Plugging in these values, we get:E = (8.314 J/mol*K * 310K) / (1 * 96,485 C/mol) * ln(40 mM / 350 mM)E = -58.4 mVTherefore, the equilibrium potential for potassium is -58.4 mV.

-Calculate the Equilibrium Potential for Potassium