A hammer can be used to put and also remove nails, depending on the need. Similarly, amphiproticsubstances can act both as an acid and as a base.!Water accepts aproton, and is actingWater loses aproton, and is actingas an acid.H3O+H20OH-as a base.How can this equation be related to the hammer previously discussed?"Water, like the hammer, can serve two purposes: as a proton donor and as proton acceptor.The auto-ionization of water molecules follows the reaction below:OHH20H*"From the equation, what are the products of the auto-ionization of water?""How to simplify this equation further?"The products of the ionization of water molecules include a hydrogen ion and a hydronium ion.The reaction can also be written as:2H20H3O*OHExercise 21.1 Give what is asked for.1. Write the equilibrium constant expression (K reaction).Tips: Recall the following points in writing equilibrium constant expression:a. Solutes enter as their molarity, [].b. Terms for pure liquids need not appear in the expression. Its concentration is the samefor all dilutes.The equilibrium constant expression can be written as: KExperimentally, the hydronium ion and the hydroxide ion is present at almost exactly0.0000001 molar at 25."Why do yo'u think these two ions are present in equal amounts?"> They must be equal since ionization of water molecule produces equal number of Lesson 21. Acid -Base Equilibria and Salt Equilibria: Bronsted Acids &Bases and Acid-Base Property of Water21INTRODUCTION:This lesson introduces you to the concept of acids and bases which havechemical equilibrium in solution. At chemical equilibrium, the products andreactants have reached a state of balance. Reactions may still be taking place withinthe sample, but the forward and reverse reactions are taking place at the same rate,so the concentrations of the products and reactants are not changing with time.Concepts related to acid base equilibrium include designing buffers andplotting pH curves.Additionally, determining the acid base equilibrium can help in predicting theproducts of a reaction and the relative concentration of the products, as well asaiding in the identification of the weaker acid and base.fficeOBJECTIVES/LEARNING COMPETENCIESLearning Competency:• Define Bronsted acids and bases. (STEM_GC11ABIVF-g-153)• Discuss the acid-base property of water. (STEM_GC11ABIVF-g-154)Specific Learning Outcomes:WPSAt the end of the lesson, the learners will be able to:explain the acid-base property of water;write the equilibrium constant expression for the auto-ionization of water; anddescribe how Bronsted acids and bases act in a chemical reaction.EXPLOREKey ConceptsHow can a substance, like water, show its amphiprotic nature?What information can be derived from the auto-ionization of water?Water molecules exhibit their amphiprotic property even in trace amounts.Consider this example!

Equilibrium is a condition at which all the species involved are at constant concentration over…

Answered: 2H20 H3O* OH Exercise 21.1 Give what is…

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Chemistry

2H20 H3O* OH Exercise 21.1 Give what is asked for. 1. Write the equilibrium constant expression (K reaction).

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...

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6.B Consider the chemical equation A(aq) + 3B(aq) 5 2C(aq) with an equilibrium constant equal to 4.00 at a certain temperature. Each chemical is initially present at a concentration of 0.25 molar. (a) Set up a simple* expression for the equilibrium constant. (*freshman level) (b) Determine whether the forward or reverse reaction is occurring. (c) Set up an 1CE table to begin a calculation of the equilibrium composition. (d) Without a better calculator or resources on the internet, you cannot solve for the equilibrium composition. Which value for "x" works: 0.0261, 0.0315, or - 0.0129. If they all fail, then one of us did something wrong.
II. WHAT I HAVE LEARNED EVALUATION/POST TEST: I. Directions: Write the equilibrium constant expression, Kc, for the following reactions. Indicate also if the equilibrium is homogeneous or heterogeneous.
Question 2, part c: please see attached Part a answer: if an initial concentration before equilibrium of c2h4o2 is 0.080 M, what are the equilibrium conc of the three species in the equilibrium: [H3O+]=[C2H3O2-]=1.20x10^-3M Part b answer: a solution in which this reaction takes place is analyzed and found to have [C2H4O2]=0.073M and [C2H3O2-]=0.251M and pH 2.131. Is the system and equilibrium? Calculate Q Qc=2543.0 x 10^-5 Kc=1.81 x 10^-5 not at equilibrium
Dinitrogen tetraoxide and nitrogen dioxide are two gases that exist in equilibrium at a range of temperatures. NO2 is a reddish brown gas while N2O4 is colorless. ... At High Temperature the red color is strong. ... ... At Low Temperature the gas has less color. ... If we represent the equilibrium as:... 2 NO2(g) N2O4(g)We can conclude that: fill in the blank 1 1. This reaction is: A. Exothermic B. Endothermic C. Neutral D. More information is needed to answer this question. fill in the blank 2 2. When the temperature is decreased the equilibrium constant, K: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question. fill in the blank 3 3. When the temperature is decreased the equilibrium concentration of NO2: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question.
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Q1) For the equilibrium: A B, if [A].0.569, [B].0.162, and Kea 47.8, what are [A]es and [B]ea? algebraic expression: [A]eq= Q2) For the equilibrium: 1221, if [2]. 1.26, [1].0, and Keq = 1.14 x10, what are [12]eg and [lleg? E algebraic expression: [H₂leq_ [12]eg [B]ea. algebraic expression: [12]ea. [eq M Q3) For the equilibrium: H₂ + 1₂2H1, if [H₂lo=0.546, [b]o 1.26, [HI].0, and Kea 45.3, what are [Halea, [lzles and [HI]eq? =0 [HI] eq = 0 0
II. Calculate the value of the equilibrium constant. 1) 1.60 moles CO, 1.60 moles H,O, 4.00 moles CO,, 4.00moles H, are found in a 8.00L container at 690°C at equilibrium. CO (g) + H,O (g)2 CO, (g) + H, (g) 2) 2.00 moles of NO, and1.60 moles of N,O, are present in a 4.00 L flask at equilibrium at 20°C. Calculate the Kc at 20°C. NO29) 3) At equilibrium at 100°C, a 2.0L flask contains: 75.1 of PCI5 0.050 mol of H,O 0.750 mol Of HCl 0.500mol of POC1, Calculate the Kc for the reaction: PCl, (s) + H,O (g) 2 HC1 (g) + POCI, (g)
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Carbon monoxide may be reacted with hydrogen to yield solid carbon and water vapor according to the reaction below. When the contents of a 1.000L reaction vessel are at equilibrium the components have the following amounts: 14.5mol C, 12.9mol H₂O, 3.52mol CO, and 2.43mol H₂ H₂ and H₂O Calculate Ke What are the concentrations of CO the new equilibrium? CO +Huy… CHỌ at
Dinitrogen tetraoxide partially decomposes according to the following equilibrium: N2Oatg) 2NO219) A 1.00L flask is charged with 0.479 moles of N204. At equilibrium at 380K, 0.176 moles of N204 remains. K. for this reaction is Write your answer to 3 Sig Figs (ie. 1.23EO)
III O Kinetics and Equilibrium Writing the concentration equilibrium expression for a heterogeneous... Write the concentration equilibrium constant expression for this reaction. Cr₂0 (aq)+61 (aq)+14 H(aq)-31,(s)+2 Cr (aq)+7H₂O(1) 号 G 0/5