In a whole-cell patch-clamp experiment at 32 degrees C, the intracellular solution contains 16 mM NaCl, 150 mM K-gluconate, and 1µM Ca(NO3)2, and the extracellular solution contains 150 mM NaCl, 3 mM KCI, 25 mM NaHCO3, 2 mM MgCl2, and 1.5 mM CaCl2. The below graph is a current-voltage (I-V) curve generated by measuring the current fluy thrOUgh a spocific jon chappel over

In a whole-cell patch-clamp experiment at 32 degrees C, the intracellular solution contains 16 mM NaCl, 150 mM K-gluconate, and 1µM Ca(NO3)2, and the extracellular solution contains 150 mM NaCl, 3 mM KCI, 25 mM NaHCO3, 2 mM MgCl2, and 1.5 mM CaCl2. The below graph is a current-voltage (I-V) curve generated by measuring the current fluy thrOUgh a spocific jon chappel over

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

List the sources of error associated with pH measurements made with the glass electrode.
Suppose we have a cell with a resting membrane potential of -70 mV. The Na+ concentrations in the ECF and ICF are as follows: [Na+]ECF = 50 mM and [Na+]ICF = 50 mM. (a) Which direction (into or out of the cell) will Na+ flow if acted on only by its concentration force? Which direction will Na+ flow if acted on only by its electrical force? (b) Under these conditions, what is the equilibrium potential for Na+? (c) If we increase permeability to Na+ (by opening up a pathway in the membrane,) where will Na+ move and why? (d) How will this change Vm? Is this depolarization or hyperpolarization? (e) Please draw a figure of Vm as a function of time in this scenario
An ion-selective electrode (ISE) produces voltage output (mV) proportional to solution pH. You have three standard pH solutions (4, 7, and 10). Assuming that pH 7 buffer solution is used together with pH 4 for calibration prior to measuring acidic solutions and together with pH 10 before measuring alkaline solutions, produce a flowchart of the calibration routine for a single pH ISE.
Describe principle of a glass membrane pH electrode.
14-10. Consider the rechargeable battery: Zn(s)|ZnCl2 (aq) |I Cl (ag)|Cl2(1)|C(s) a. Write reduction half-reactions for each electrode. From which electrode will electrons flow from the battery into a circuit if the electrode potentials are not too different from E° values? b. If the battery delivers a constant current of 1.00 × 10³ A for 1.00 h, how many kilograms of Cl2 will be consumed?
Propose structures for the compounds below: (a) Molecular formula C4H9Br 13. TMS 4.2 4.0 2.0 1.5 1.0 8 7 4 3 1 SH (ppm) (b) Molecular formula C3HĄBR2 TMS 6.0 5.8 5.6 4.4 4.2 4.0 8 7 4 3 1 SH (ppm)
At 25 ºC, the resistance of a cell containing a 0.01 mol.L–1 KCl solution is 525 Ω. The resistance of the same cell containing a 0.1 mol.L–1 solution of NH4OH is 2030 Ω. Which the degree of apparent dissociation of ammonium hydroxide? λ0KCl = 14.99 mS.m2mol–1; NH+ 4 = 7.35 mS.m2mol–1; λOH - = 19.91 mS.m2mol–1)
The concentration of Ca2* in the endoplasmic reticulum (outside) is 1 mM, and the concentration of Ca2* in the cytosol (inside) is 0.1 uM. Calculate AG at 37°C when the membrane potential is -50 mV (cytosol negative). Express your answer in units of kJ mol using 3 significant figures. kJ mol1 the tolerance is +/-2% Calculate AG at 37°C when the membrane potential is +50 mV. Express your answer in units of kJ mor using 3 significant figures. kJ mol1 the tolerance is +/-2%
Salstrom and Hildebrand reported the following data for the cell Ag(s)|AgBr(s)||HBr(aq)|Br2(g, 1 atm)|Pt 442.3 456.0 490.9 521.4 538.3 556.2 0.8031 0.7989 0.7887 0.7803 0.7751 0.7702 T/°C E/V The charge number of the reaction is 1. What is the entropy change (in J K-¹ mol-¹) for the cell reaction? Express your answer in four significant figures. * = 96,485 C mol-¹
14-21. Suppose that the concentrations of NaF and KCl were each 0.10 M in the cell Pb(s)|PbF2(s)|F (ag)||Cl (ag)|AgCl(s)|Ag(s) a. Using the half-reactions 2A£C1(s) + 2e PbF2(s) + 2e = Pb(s) + 2F , calculate the cell voltage. F 2Ag(s) + 2CI¯_and b. In which direction do electrons flow? c. Now calculate the cell voltage by using the reactions 2Ag† + 2e¯ = 2Ag(s) and Pb²+ + 2e¯ = Pb(s). For this part, you will need the solubility products for PbF2 and AgCl.
12-6. Calculate the potential of the following cells: (a) a galvanic cell consisting of a lead electrode immersed in 0.0848 M Pb2 and a zine electrode in contact with 0.1364 M Zn+. (b) a galvanic cell consisting of a standard hydrogen electrode and a platinum elec- trode immersed in a solution that is 1.46 X 10- M in TiO+,0.02723 M in Ti-, and buffered to a pH of 3.00.
Suppose you are given 0.0856ppm to be the concentration of dissolved lead found in pond water after dilution factor of 1:100 in 100ml volumetric flask and the other sample is diluted at the dilution factor of 1:2 and the concentration is 2.14ppm. How would you comment on the amount of lead in pond water