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1. Use the Nernst Equation (Box 3.2, Ch. 3) to determine the equilibrium potential for each...
Nernst Equilibrium Equation Problem Use the information in the table below to answer the questions. Ion...
Nernst Equilibrium Equation Problem Use the information in the table below to answer the questions. Ion ECF ICF X+ 120 mM 30 mM A- 100 mM 100 mM B- 140 mM 30 mM a) Calculate the Nernst Equilibrium potential for EACH ion. b) Which ion(s) have a net chemical force acting to move the ion(s) into the cell? c) Which ion(s) have a net electrical force acting to move the ion(s) into the cell? d) If the plasma membrane had...
According to the Nernst equation, the equilibrium potential for any ion, Ejon, distributed across a membrane...
According to the Nernst equation, the equilibrium potential for any ion, Ejon, distributed across a membrane is dependent on the internal, [lon]in, and external, [lon]out, concentrations of the ion (in moles or grams/liter); the valence of the ion, z (an integer); the absolute temperature, K; Faraday's constant, F; and the universal gas constant, R. Eion = ( R ) 2.303 log10 (Ionlout Tomlin If Faraday's constant is approximately 96,500 coulombs/mole, and the equilibrium potential for sodium ions across a skeletal...
15. Given the following concentrations of ions in the intracellular and extracellular fluids of a cell;...
15. Given the following concentrations of ions in the intracellular and extracellular fluids of a cell; inside the cell: Na+ 12mM. K+ 150mM, CI-9mm, Ca2+0.0001mM and outside the cell: Na+ 145mM, K+ 5mM, CI- 125mM, and Ca2+ 2.5mM. Calculate the equilibrium potential for K+ (Ek) if its extracellular concentrations rise from 5 mM to 10 mM. Use the Nernst equation and the ion concentration to perform the following calculation. Comparing this to the normal Ek, is the change a depolarization...
Questions: 1. Nerves: Get your calculators out! As expected, you are about to experience the deep...
Questions: 1. Nerves: Get your calculators out! As expected, you are about to experience the deep satisfaction of solving the Goldman equation to predict the axon membrane potential, as presented in your book and lecture notes. Nernst (cations only): V (MV) = 61 log(CIC) P Na+PK)-PaC). Goldman: V (mV) = 61 log P [Na]. + P (K). + PCI)- To solve this equation, you will need to use the following concentrations inside (i) and outside (o) the cell and permeabilities...
for each, what is the right answer? B) iris 19. The Nernst Equation predicts that the...
for each, what is the right answer?
B) iris 19. The Nernst Equation predicts that the equilibrium potential for an ion is proportional to where "in" means "inside the cell" and "out" means "outside the cell" (pick the answer that most closely matches the Nemst equation). A) log ([ion in x [ionout) B) bg ([on]out [onlin) C) log (ionin) D) bg (ion)in Vlog ([ion)out) E) log (ion)in) x log (ionout) 20. The eustachian tube connects the and the A) middle...
1. If the membrane potential of sodium ions in a cell is equal to +60 mV,...
1. If the membrane potential of sodium ions in a cell is equal to +60 mV, what is its membrane potential for chloride ions if they are found in the exact same concentrations as sodium? Give your answer in mV. 2. Given a cell membrane with the following parameters- Ion Extracellular concentration (mmol/L) Intracellular concentration (mmol/L) Permeability K+ 10 150 1 Na+ 140 15 0.04 Cl- 100 7 0.45 calculate the membrane potential of the cell in mV. (Round your...
please write thorough answers thanks PART 1 Answer ONLY ONE of the following TWO questions of...
please write thorough answers thanks
PART 1 Answer ONLY ONE of the following TWO questions of Part 1 ie a) OR b) a) A typical, healthy nerve cell in the body has intracellular and extracellular Na, K and Cl' concentrations as shown below. Na concentration: Extracellular: = 150 mm K concentration: Extracellular: = 4 mm Ci concentration: Extracellular: = 100 mm Temperature = 37°C (303.3K) R (the Universal Gas constant) = 8.315 VCmol'k F (Faraday's constant) = 96,485 Cmol Intracellular:...
Review equation 16.10 and step B2. Ag+1(aq) and NH3(aq) will form a soluble complex ion. Use...
Review equation 16.10 and step B2. Ag+1(aq) and NH3(aq) will form a soluble complex ion. Use rule 3 of Water-Insoluble Salts in Appendix E to determine what would happen if Ag+1(aq) was combined with KOH instead of NH3. Write the net ionic equation with phase subscripts, where K+1 is a spectator ion which is cancelled out. Equation 16.10: Ag^+(aq) + Cl^-(aq) ⇄ AgCl(s) ⇅ 2NH3(aq) [Ag(NH3)2]^+(aq) Step B2: Silver Chloride equilibrium. To the clear solution from part B.1, add 5...
pages 2-4 please! its equilibrium worksheet 2. A sample of gaseous BrCl is allowed to decompose...
pages 2-4 please! its equilibrium worksheet
2. A sample of gaseous BrCl is allowed to decompose in a closed container at 25C according to the equation below: 2BrCl(g) Bra(g) + Cl2(g) When the reaction reaches equilibrium, the following concentrations were obtained: [BrCl] = 0.38 M, [Cl:] = 0.26 M & [Br2] = 0.26 M. Determine the equilibrium constant for the reaction 3. A mixture of gases NOCI, Cl and NO was allowed to reach equilibrium at a particular temperature. The...
When dealing with buffer systems, we often use the acid reaction to determine the equilibrium and...
When dealing with buffer systems, we often use the acid reaction to determine the equilibrium and set up the ICE table. The most common experimental method used to study acid-base systems is titration, which studies the stoichiometric addition of the acid to a base solution or the base to an acid solution to determine the value of K, or K, The value of the pK, or pK, is essential to the understanding of the buffer system, where pK, = -log...
According to the Nernst equation, the equilibrium potential for any ion, Ejon, distributed across a membrane is dependent on the internal, [lon]in, and external, [lon]out, concentrations of the ion (in moles or grams/liter); the valence of the ion, z (an integer); the absolute temperature, K; Faraday's constant, F; and the universal gas constant, R. Eion = ( R ) 2.303 log10 (Ionlout Tomlin If Faraday's constant is approximately 96,500 coulombs/mole, and the equilibrium potential for sodium ions across a skeletal...
15. Given the following concentrations of ions in the intracellular and extracellular fluids of a cell; inside the cell: Na+ 12mM. K+ 150mM, CI-9mm, Ca2+0.0001mM and outside the cell: Na+ 145mM, K+ 5mM, CI- 125mM, and Ca2+ 2.5mM. Calculate the equilibrium potential for K+ (Ek) if its extracellular concentrations rise from 5 mM to 10 mM. Use the Nernst equation and the ion concentration to perform the following calculation. Comparing this to the normal Ek, is the change a depolarization...
Questions: 1. Nerves: Get your calculators out! As expected, you are about to experience the deep satisfaction of solving the Goldman equation to predict the axon membrane potential, as presented in your book and lecture notes. Nernst (cations only): V (MV) = 61 log(CIC) P Na+PK)-PaC). Goldman: V (mV) = 61 log P [Na]. + P (K). + PCI)- To solve this equation, you will need to use the following concentrations inside (i) and outside (o) the cell and permeabilities...
for each, what is the right answer?
B) iris 19. The Nernst Equation predicts that the equilibrium potential for an ion is proportional to where "in" means "inside the cell" and "out" means "outside the cell" (pick the answer that most closely matches the Nemst equation). A) log ([ion in x [ionout) B) bg ([on]out [onlin) C) log (ionin) D) bg (ion)in Vlog ([ion)out) E) log (ion)in) x log (ionout) 20. The eustachian tube connects the and the A) middle...
please write thorough answers thanks
PART 1 Answer ONLY ONE of the following TWO questions of Part 1 ie a) OR b) a) A typical, healthy nerve cell in the body has intracellular and extracellular Na, K and Cl' concentrations as shown below. Na concentration: Extracellular: = 150 mm K concentration: Extracellular: = 4 mm Ci concentration: Extracellular: = 100 mm Temperature = 37°C (303.3K) R (the Universal Gas constant) = 8.315 VCmol'k F (Faraday's constant) = 96,485 Cmol Intracellular:...
pages 2-4 please! its equilibrium worksheet
2. A sample of gaseous BrCl is allowed to decompose in a closed container at 25C according to the equation below: 2BrCl(g) Bra(g) + Cl2(g) When the reaction reaches equilibrium, the following concentrations were obtained: [BrCl] = 0.38 M, [Cl:] = 0.26 M & [Br2] = 0.26 M. Determine the equilibrium constant for the reaction 3. A mixture of gases NOCI, Cl and NO was allowed to reach equilibrium at a particular temperature. The...
When dealing with buffer systems, we often use the acid reaction to determine the equilibrium and set up the ICE table. The most common experimental method used to study acid-base systems is titration, which studies the stoichiometric addition of the acid to a base solution or the base to an acid solution to determine the value of K, or K, The value of the pK, or pK, is essential to the understanding of the buffer system, where pK, = -log...
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