BPHY102 Biophysics Course Work 2.Last submitting date: 07.06.2021Q1. Use the Nernst equation to calculate the equilibrium potential for the following distribution of ionsmeasured in squid and mammalian neuron.Concentration (mM)lonIntracellularExtracellularEquilibrium potentialSquid neuronPotassium (K*)40020Sodium (Na*)50440Chloride (Cl)95560Calcium (Ca2")0.000110Mammalian neuronPotassium (K*)140Sodium (Na+)10145Chloride (Cl-)17110Calcium (Ca2+)0.00011

Answered: Image /qna-images/answer/64eec69e-64c1-48f3-992e-97c5180475b1.jpg

Q1. Use the Nernst equation to calculate the equilibrium potential for the following distribution of ions measured in squid and mammalian neuron. lon Squid neuron Potassium (K) Sodium (Na+) Chloride (Cl-) Calcium (Ca²+) Mammalian neuron Potassium (K) Sodium (Na+) Chloride (Cl-) Calcium (Ca2+) Intracellular 400 50 95 0.0001 Concentration (mm) 140 10 17 0.0001 Extracellular 20 440 560 10 5 145 110 1 Equilibrium potential

Q1. Use the Nernst equation to calculate the equilibrium potential for the following distribution of ions measured in squid and mammalian neuron. lon Squid neuron Potassium (K) Sodium (Na+) Chloride (Cl-) Calcium (Ca²+) Mammalian neuron Potassium (K) Sodium (Na+) Chloride (Cl-) Calcium (Ca2+) Intracellular 400 50 95 0.0001 Concentration (mm) 140 10 17 0.0001 Extracellular 20 440 560 10 5 145 110 1 Equilibrium potential

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter22: Bulk Electrolysis: Electrogravimetry And Coulometry

Section: Chapter Questions

Problem 22.28QAP

See similar textbooks

Similar questions

Q1. Use the Nernst equation to calculate the equilibrium potential for the following distribution of ions measured in squid and mammalian neuron. Concentration (mM) lon Intracellular Extracellular Equilibrium potential Squid neuron Potassium (K) 400 20 Sodium (Na*) 50 440 Chloride (CI) 95 560 Calcium (Ca) 0.0001 10 Mammalian neuron Potassium (K*) 140 Sodium (Na+) 10 145 Chloride (CI-) 17 110 Calcium (Ca2+) 0.0001
Calculate the equilibrium electrical membrane potentials corresponding to the following extracellular and intracellular concentrations of ions at 20 °C. Assume permeability of the 2+ membrane for one type of ion only (e.g. K* for V, Ca for V and H for V) K' Са lonic Species Intracellular Extracellular Equilibrium Potential Potassium (K ) 150 mM 4 mM V, = ?mV K 2+ Calcium (Ca) 2 mM V = ? mV 70 nM %3D Са Hydrogen ion (proton, H) pH 7.2 pH 7.4 V, = ? mV
Subject Year Month, 58 Discuss the mechanism by which the potential of a platinum electrode becomes poised by immer- sion into a solution of Fe(II) and Fe(III) in 1 M HCl. Approximately how much charge is required to shift the electrode potential by 100 mV? Why does the potential become uncertain at low concentra- tions of Fe(II) and Fe(III), even if the ratio of their concentrations is held near unity? Does this ex- perimental fact reflect thermodynamic considerations? How well do your answers to these issues apply to the establishment of potential at an ion-selective electrode? Date. فصل دوم مراجع استاد
Determine the potential of a platinum electrode (vs. SHE) when placed in a mixture of 0.00207 M TICI, and 0.0362 M TICI at 25 °C. T13+ (aq) + 2e- = TIt (aq) E° = 1.25 V EPt = V Determine the potential of a platinum electrode when placed in a mixture of 0.0137 M potassium permanganate (KMNO,) and 0.0667 M manganese chloride (MnCl,) at pH 5.46 and 25 °C. Mno, (aq) + 5e- + 8 H* (aq) = Mn²+ (aq) + 4 H, O(1) E° = 1.51 V Ept = V
An electrode is immersed in a solution containing 0.1 mol dm-3 Cu2+ and 0.05 mol dm-3 Zn2+ at 298 K. The current is recorded as a function of the applied potential. Draw the current-potential plot for this system, indicating the order in which the solution species are reduced. E o Zn2+|Zn = -0.76 V E o Cu2+|Cu = 0.34 V %3D
https://chem.libretexts.org/Ancillary_Materials/Reference/Reference_Tables/Electrochemistry_Tables/P1%3A_Standard_Reduction_Potentials_by_Element https://chem.libretexts.org/Ancillary_Materials/Reference/Reference_Tables/Thermodynamics_Tables/T1%3A_Standard_Thermodynamic_Quantities
1) Calculate the mass of metal that is plated when an electrolytic cell consisting of aqueous tantalum(III) chloride and a tantalum electrode runs for 16.00 h with at current of 200.5 A. 2)A chemical reaction at standard thermodynamic temperature with a rate constant of 6.13×10−2 M−1 s−1 and an initial reactant concentration of 0.446 M, is heated to 414.3 ∘C. If the activation energy of the reaction is 32.76 kJ mol−1, how many times faster is the reaction at the higher temperature with the same initial concentration?
use the Nernst eqaution to determine the equilibrium potential (relative to SHE) for the oxygen evolution reaction (OER) in alkaline medium (0.1M KOH =pH= 14)
A conductivity cell filled with a 0.01 M KCl solution was found to have a resistance of 189 ohms at 25oC. When filled with 0.01 M HCl solution, the cell gave a resistance of 64.8 ohms at the same temperature. At 25oC, the conductivity of 0.01 M KCl solution was 1.4088 x 10-3 S cm-1. Calculate (a) the cell constant and (b) the conductivity of the HCl solution. answer is [0.266; 4.105 x 10-3] please explain. thank you!
A 25.00cm of potassium dichromate(K,Cr,CH so lution aretadded to an acidified aqueous solution of potassium lodide(present in excess). The lodine was then liberated according to the equation K-Cr.O;(aq) +14- (aq) + KI(ag) K(aq) + Cr (aq) + H;O(1) + 12(aq) Required 19.63cm of a 0.1478M Na S,O for complete reaction. The equation for the reaction of between Na S;03 and I2 is 2(aq)+ Na;S;SO;(aq)-Na S4O6(aq) + Nallac) Calculate the concentration of potassium dichromate (only 4 decimal places) mol/L
116.In a conductivity cell of a cell constant 0.003 cm³¹ concentration of 0.01 M solution of acetic acid, the resistance against ionic mobility is 20 ohm at 25 °C. the degree of dissociation of the acid is (where the molar conductance at infinite dilution = 390 x 104 2¹¹ m² mol¹ at 25° C) a) 0.015 b) 0.027 c) 0.038 d) 0.047
LUse the table ot standard reduction potentiais to select a reduding agent that converts Ni' to NI but not Fet to Fe Standard Reduction Potentials in Aqueous Solution at 25 °C Acidic Solution B* (V) H0;{ag) +3H*(eg) +2e +2 H,0(4) 1.77 Au (ag) + Au(s) 1.68 Au*(ug) +1e Au(a) 1.50 Brslé) + 2e+2 Br (ag) 1.08 NO, (E) +4H' (uq) + ** - NOlg) + 2 H,0(4) 0.96 Ag* (ag) +e- Agts) 0.7994 Hg."(ag) +2e + 2 Hgle) 0.789 Cu" (ag) +2 - Cnla) 0337 Hg, Cls (s) +2e+ 2 Hg() 0.27 2H (ug) +2 - H(g) 0.00 Sa* (ag) +24- Sn(a) -0.14 N*(a9) + 2e- Na) -0.25 Ca* (agi +2- Co(a) -0.28 ca* (ag) + 2 - Oda) -0.40 C"(ag) +- C ( -0.41 Fe* (ag) + 1e + Fen) -0.44 Za* (aq) + 2e + Zn(a) -0.763 * (ag) +24 Ca(a) -0.91 A*(eg) +3e - Alja) -1.66 Mg*(aq) +2e + Mgla) -2.37 O zn O sn