12lon concentrationsIONECFICFK+4 mM145 mMNa+150 mM12 mMCI-108 mM 10 mMGiven the numbers above, which are slightly different from the numbers in the textbook, what is the equilibrium ion concentration for potassium? (do not include units in your finalanswer)Type your answer...lon concentrationsIONECFK+Na+4 mM150 mMCI-108 mMEion =ICF145 mM12 mM10 mMEion =----DUGiven the numbers above, which are slightly different from the numbers in the textbook, what is the equilibrium ion concentration for chloride? (do not include units in your finalanswer)Type your answer...

Eion=2.303 RTZ F log ECFICF WHEREE, R= Universal Gas constant (8.314 J/mol K) T= Human body…

Answered: lon concentrations ION ECF K+ 4 mM Na+…

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lon concentrations ION ECF K+ 4 mM Na+ 150 mM CI- 108 mm ICF 145 mM 12 mM 10 mM Eion =

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 13Q: Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this...

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Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?
. When a chemical system has reached equilibrium, the concentrations of all reactants and products remain _________ with lime.
The experiment in Exercise 12.33 was redesigned so that the reaction started with 0.15 mol each of N2 and O2 being injected into a 1.0-L container at 2500 K. The equilibrium constant at 2500 K is 3.6 X 10“’. What was the composition of the reaction mixture after equilibrium was attained? The following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) *2 2 NO K = 4.1 X IO-4 If the reaction began with 0.100 mol L-1 of N2 and 0.100 mol L-’ ofO2, what were the equilibrium concentrations of all species?
. Hydrogen gas, oxygen gas, and water vapor are in equilibrium in a closed container. Hydrogen gas is injected into the container, and the system is allowed to return to equilibrium. Which of the following occurs? Explain your answer. 2H2(g)+O2(g)2H2O(g)a. The concentration of oxygen gas remains constant. b. The value for K increases. c. The concentration of oxygen gas increases. d. The concentration of water vapor increases. e. The value for K decreases.
The creation of shells by mollusk species is a fascinating process. By utilizing the Ca2+ in their food and aqueous environment, as well as some complex equilibrium processes, a hard calcium carbonate shell can be produced. One important equilibrium reaction in this complex process is HCO3(aq)H+(aq)+CO32(aq)K=5.61011 If 0.16 mole of HCO3 is placed into 1.00 L of solution, what will be the equilibrium concentration of CO32?
Nitrogen, hydrogen, and ammonia are in equilibrium in a 1000-L reactor at 550 K. The concentration of N2 is 0.00485 M, H2 is 0.022 M, and NH3 is 0.0016 M. The volume of the container is halved, to 500 L. (a) Calculate the equilibrium constant. (b) Define y as the change in the concentration of nitrogen in the 500-L container. Is y positive or negative? (c) Write the iCe table and express the equilibrium constant in a polynomial in terms of y.
Calculate the equilibrium concentrations that result when 0.25 M O2 and 1.0 M HCl react and come to equilibrium. 4HCl(g)+O2(g)2Cl2+2H2O(g)Kc=3.11013
Analysis of the gases in a sealed reaction vessel containing NH3, N2, and H2 at equilibrium at 400 C established the concentration of N2 to be 1.2 M and the concentration of H2 to be 0.24 M. N2(g)+3H2(g)2NH3(g)Kc=0.50 at 400 C Calculate the equilibrium molar concentration of NH3.
Because carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that the hydrogen ion concentration she calculated is not correct. She looks up the equilibrium constant for the reaction HCO,-(aq) «=* H+(aq) + COf'(aq) Upon finding that the equilibrium constant for this reaction is 4.8 X 10“H, she decides that her answer in Exercise 12.39 is correct. Explain her reasoning. A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H,CO,(aq) 5=6 H+(aq) + HCO,'(aq) K = 4.4 X 10'7She starts with 0.1000 A1 carbonic acid. W hat are the concentrations of all species at equilibrium?
Hydrogen is prepared commercially by the reaction of methane and water vapor at elevated temperatures. CH4(g)+H2O(g)3H2(g)+CO(g) What is the equilibrium constant for the reaction if a mixture at equilibrium contains gases with the following concentrations: CH4, 0.126 M ; H2O, 0.242 M ; CO, 0.126 M ; H2 1.15 M, at a temperature of 760 C?
For the reaction 2NO(g)+2H2(g)N2(g)+2H2O(g) it is determined that, at equilibrium at a particular temperature, the concentrations are as follows: [NO(g)] = 8.1 103 M, [H2(g)] = 4.1 105 M, [N2(g)] = 5.3 102 M, and [H2O(g)] = 2.9 103 M. Calculate the value of K for the reaction at this temperature.
A sample of gaseous nitrosyl bromide (NOBr) was placed in a container tiued with a frictionless, massless piston, where it decomposed at 25C according to the following equation: 2NOBr(g)2NO(g)+Br2(g) The initial density of the system was recorded as 4.495 g/L. After equilibrium was reached, the density was noted to be 4.086 g/L. a. Determine the value of the equilibrium constant K for the reaction. b. If Ar(g) is added to the system at equilibrium at constant temperature, what will happen to the equilibrium position? What happens to the value of K? Explain each answer