ACTIVITY 2 ACIDIC OR BASIC Like all equilibrium reactions, this reaction has an equilibrium constant. Because this is a special equilibriumconstant, specific to the self-ionization of water, it is denoted Kw, it hasa value of 1.0 x 10-14. If we write out theactual equilibrium expression for Kw, we get the following:Kw = [H+][OH-] = 1.0 x 10-14%3DHowever, because H* and OH are formed in a 1:1 molar ratio, we have:[H+] = [OH-] = V1.0 x 10-14 1.0 x 10-7M%3D%3DNow, note the definition of pH and pOH:[+H]601- = HdHd-%3D%3DHod-=[-HO][-HO]B01- = HOd[H30+]The term pH refers to the "potential of hydrogen ion." It was proposed by Danish biochemist Soren Sorensen in1909 so that there could be a more convenient way to describehydronium and hydroxide ion concentrations in aqueoussolutions since both concentrations tend to be extremely small.If we plug in the above value into our equation for pH, we find that:pH = - log(1.0 x 107) = 7.0pOH =-log(1.0 x 107) = 7.0Here we have the reason why neutral water has a pH of 7.0; it represents the condition at%3D%3Dwhich the concentrations of H and OH are exactly equal in solution.Since how the equilibrium constant can be expressed was already established, if we takethe negative logarithm of both sides of this equation, we get the following:= (*y)= - log[H+] +-log[OH-]-log (Kw)([-HO][+H]) 801--log (Kw)pKw = pH + p0H%3DHowever, because we know that pKw= 14, we can establish the following relationship:|3DThis relationship always holds true for any aqueous solution, regardless of its level ofacidity oralkalinity. Utilizing this equation is a convenient way to quickly determine pOH frompH and vice versa, aswell as to determine hydroxide concentration given hydrogen concentration, or vice versa.Activity 1: Solving Time!Directions: Solve the following problem. Show your complete solutions.1. Calculate the hydronium ion concentration of a solution with a pH of-1.07.2. What are the pOH and the pH of a 0.0125M solution of potassium hydroxide, KOH?3. The hydronium ion concentration of vinegar is approximately 4 x 10 M.Activity 2: Is it Acidic or Basic?Directions: Complete the table by identifying whether the sample solution mentioned is either acidic or basic and rank itall from the most acidic to most basic (1-5), with 5 as the most basic.SOLUTIONSAcidic or BasicRank1.1 М HCI1.2. Ocean Water3.1 M NAOH4. Rainwater2.5. Baking soda

Answered: Image /qna-images/answer/321bfbc5-9877-4c5b-9192-98abacffc116.jpg

Activity 2: Is it Acidic or Basic? Directions: Complete the table by identifying whether the sample solution mentioned is either acidic or basic and rank it all from the most acidic to most basic (1-5), with 5 as the most basic. SOLUTIONS Acidic or Basic Rank 1.1 М НCI 2. Ocean Water 3.1 M NAOH 4. Rainwater 5. Baking soda

Activity 2: Is it Acidic or Basic? Directions: Complete the table by identifying whether the sample solution mentioned is either acidic or basic and rank it all from the most acidic to most basic (1-5), with 5 as the most basic. SOLUTIONS Acidic or Basic Rank 1.1 М НCI 2. Ocean Water 3.1 M NAOH 4. Rainwater 5. Baking soda

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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