table of bases with kb and pkb values
Understanding Kb and pKb in detail. Table 17.3 on page 808 of your text is your new best friend! It is called slaked lime because it is made by treating lime (CaO) with water. The pKa values for organic acids can be found in Appendix II of Bruice 5th Ed. pKb = - log (10) Kb One should always know which source to use. What is the KB value for acetic acid? PDF TABLE OF CONJUGATE ACID-BASE PAIRS Acid Base Ka (25 C) We can also calculate the (or ) of a weak acid . These tables are compiled in PDF . What would be the concentration of OH - be at equilibrium? How would you find the appropriate buffer with given pKa's - Socratic Calculation of the pH of a weak base: Find the [OH-] from the pKb value (in the same way as for weak acid type calculations) From the [OH-] find the pOH. The corresponding expression for the reaction of cyanide with water is as follows: \[K_b=\dfrac{[OH^][HCN]}{[CN^]} \label{16.5.9}\]. They describe the degree of ionization of an acid or base and are true indicators of acid or base strength because adding water to a solution will not change the equilibrium constant. There is virtually no undissociated NaOH left in the solution as it is almost entirely ionized to ions. If we add Equations \(\ref{16.5.6}\) and \(\ref{16.5.7}\), we obtain the following (recall that the equilibrium constant for the sum of two reactions is the product of the equilibrium constants for the individual reactions): \[\cancel{HCN_{(aq)}} \rightleftharpoons H^+_{(aq)}+\cancel{CN^_{(aq)}} \;\;\; K_a=[H^+]\cancel{[CN^]}/\cancel{[HCN]}\], \[\cancel{CN^_{(aq)}}+H_2O_{(l)} \rightleftharpoons OH^_{(aq)}+\cancel{HCN_{(aq)}} \;\;\; K_b=[OH^]\cancel{[HCN]}/\cancel{[CN^]}\], \[H_2O_{(l)} \rightleftharpoons H^+_{(aq)}+OH^_{(aq)} \;\;\; K=K_a \times K_b=[H^+][OH^]\]. This calculated value checks well with our initial guess. Acid/Base Ionization Constants. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.48 M in this salt. This acids and bases chemistry video tutorial provides a basic introduction into the calculation of the pH and pOH of a solution. A lower pKb value indicates a stronger base. It is represented as H+(aq) or H 3O +(aq). pKa and pKb are common terms in chemistry that are known as dissociation constants. A significant Kb value implies a strong base's high amount of dissociation. arrow_forward. 0000006813 00000 n
At 25C, pKa+pKb=14.00. Table of Acids with Ka and pKa Values* CLAS Acid HA A - Ka pKa Acid Strength Conjugate Base Strength Hydroiodic HI I . Browse e12806.pkb resources on Teachers Pay Teachers, a marketplace trusted by millions of teachers for . For reference or additional information, please contact websupport@aatbio.com Use Ka = 1.8 x 10-5 and Kb = 1.5 x 10-14 for your calculations. 10081 views around the world You can reuse this answer Creative Commons License iOS . The strong bases are listed at the bottom right of the table and get weaker as we move to the top of the table. And since the NH 2- accepted that proton, NH 3 is the conjugate acid. These as well, are types of acid-base reactions where the base is the oxide ion (O2-) and water is the acid. The lesser the pKb is, the more potent the base will be. BPP Marcin Borkowskiul. Dalslands Kanal Paddla, Their licenses helped make this book available to you. This is related to K a by pK a + pK b = pK water = 14.00 (at 25C) Compounds are listed by molecular formula in Hill order. Ph(RS. Understanding Kb and pKb. The value of the pK a changes with temperature and can be understood qualitatively based on Le Chtelier's principle: when the reaction is . What is the Ka of a solution whose known values are given in the table: pH = 1.7 HA A-H+ . The difference between pKa and pKb is that pKa is the negative logarithm of Ka whereas . Use table search to locate desired compound in database. K14KcqT FaV1! pKb = 14 - pKa. The pKb of pyrldlne Is 8.77 . Once again, the concentration does not appear in the equilibrium constant expression.. 0000000916 00000 n
- FindAnyAnswer.com, 7.12: Relationship between Ka, Kb, pKa, and pKb, Solved Table 10.2: pKa and pKb values at 25 C for some - Chegg, pH, pKa, Ka, pKb, Kb - Organic Chemistry | Socratic, pH, pKa, Ka, pKb, and Kb Explained - ThoughtCo, Equilibria of Weak Bases, K b - Purdue University, Solved Using your knowledge of equilibrium, pH, Ka and Kb | Chegg.com, Acid-Base Equilibrium Part 1: How to Use the pKa Table, Relationship between Ka and Kb (article) - Khan Academy, Acidity-Basicity Data (pKa Values) in Nonaqueous Solvents - ut, How would you find the appropriate buffer with given pKa's - Socratic. Theoretical background. Please note: Although these values are common (and published) values associated with the substances given, there are many possible sources for these values. This table is part of our larger collection of acid-base resources. This is Appendix D: Dissociation Constants and pKb Values for Bases at 25C, appendix 4 from the book Principles of General Chemistry (v. 1.0). What is pKb? RbOH. 7.12: Relationship between Ka, Kb, pKa, and pKb is shared under a not declared license and was authored, remixed, and/or curated by LibreTexts. Determine the K b of a weak base if a 0.30 M solution of the base has a pH of 11.98 at 25 C. (Kb > 1, pKb < 1). What is a KB value? 0000013626 00000 n
Based on theKbvalues, NH3 is the strongest base, and it has a smaller pKb value. Below are tables that include determined pKa values for various acids as determined in water, DMSO and in the gas Phase. The values of \(K_a\) for a number of common acids are given in Table \(\PageIndex{1}\). pH, pKa, Ka, pKb, and Kb Explained - ThoughtCo 2) 1.8 10 -5. The table below gives the value of the base dissociation constant, K b, for aqueous solutions of different weak bases at 25C: base formula K b : phosphine: PH 3: 1.0 10-14: smaller K b: PKb = -log [Kb] A large Kb value and small PKb value gives the strongest base Compound Kb PKb (A) C6H5NH2 - 4 x 10^-10 9.349 . The equilibrium constant for this dissociation is as follows: \[K=\dfrac{[H_3O^+][A^]}{[HA]} \label{16.5.2}\]. No pKb value given. So, just like the acids, the trait is that a stronger base has a lower pKb while the Kb increases with the acid strength. The \(pK_a\) of butyric acid at 25C is 4.83. It explains how to calculate the percent ionization of a weak acid usi. Consequently, aqueous solutions of acetic acid contain mostly acetic acid molecules in equilibrium with a small concentration of \(H_3O^+\) and acetate ions, and the ionization equilibrium lies far to the left, as represented by these arrows: \[ \ce{ CH_3CO_2H_{(aq)} + H_2O_{(l)} <<=> H_3O^+_{(aq)} + CH_3CO_{2(aq)}^- }\]. Butyric acid is responsible for the foul smell of rancid butter. Equilibrium problems involving bases are relatively easy to solve if the value of Kb for the base is known. The larger the \(K_a\), the stronger the acid and the higher the \(H^+\) concentration at equilibrium. Occasionally we will find that the approximation, is not valid, in which case we must use a series of successive approximations similar to that outlined above for acids. As a general reaction, this can be shown as: where, B is the weak base, and is its conjugate acid BH+. . A pKb3.0 and Kb1103 B pKb5.8 and Kb2106 C pKb11.0 and Kb11011 D pKb12.5 and Kb3102 You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.62 M in this salt. Notice the inverse relationship between the strength of the parent acid and the strength of the conjugate base. Problems calculation of acid-pKa and base-pKa values - ChemAxon Kb's negative log base ten is equal to pKb, it works the same as pKa expect that it's for bases. 2) 1.8 10 -5. Additionally, if an acid or base is known to be strong then the Ka/Kb value is not necessary because we can assume 100% depronation. Legal. The larger the Kb, the stronger . For details on it (including licensing), click here. Using the value for Kb listed in the table, find the pH of 0.100 M NH3. The lesser the pKb is, the more potent the base will be. arrow_forward Literature guides Concept explainers Writing guide Popular textbooks Popular high school textbooks Popular Q&A Business Accounting Economics Finance Leadership Management Marketing Operations Management Engineering Bioengineering Chemical Engineering Civil Engineering Computer Engineering Computer Science Electrical Engineering . Chem1 Virtual Textbook. Chemistry questions and answers. Acids and bases are symbolized by pH, pKa, Ka, pKb, and Kb. A significant Kb value implies a strong base's high amount of dissociation. Vrdintyg Socialstyrelsen. Additionally, the death density in the RS group was later and more concentrated than in the . Pkb Values Of Bases Table. If we are given any one of these four quantities for an acid or a base (\(K_a\), \(pK_a\), \(K_b\), or \(pK_b\)), we can calculate the other three. pKa is given for acid dissociations. A weak acid has a Ka of 2.510^-5. For example, nitrous acid (\(HNO_2\)), with a \(pK_a\) of 3.25, is about a 1000 times stronger acid than hydrocyanic acid (HCN), with a \(pK_a\) of 9.21. A stronger base is indicated by a lower pKb value. Acid: a substance that, when dissolved in water, increases the concentration of H + ions 2. pKa Values of Common Bases Values in H 2O as much as possible, so common comparisons (i.e., H 2OpK a = 15.7) can still be used Note; The pK a values associated with bases is normally meant to refer to the true pK a's of their conjugate acids; i.e., pK a associated with HO-is 15.7, which is the pK a of H 2O. xref
theoretical ph calculator At equilibrium, the concentration of each individual ion is the same as the concentration of the initial reactant . HVMoFWq 'qLE
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'C%{1;hlvxa],5z:81\c5w(}|uY)imF+_1.ltIyk()U5vv-]&CYnUOQ.To9]/wTJ9WE1mTYHZA/-7 Using Equation \ref{4} we have, \[\begin{align*} [\text{ OH}^{-}] &=\sqrt{K_{b}c_{b}} \\[4pt] & =\sqrt{\text{1.8 }\times \text{ 10}^{-\text{5}}\text{ mol L}^{-\text{1}} \times \text{ 0.100 mol L}^{-\text{1}}} \\[4pt] &=\sqrt{\text{1.8 }\times \text{ 10}^{-\text{6}}\text{ mol}^{\text{2}}\text{ L}^{-2}} \\[4pt] &=\text{1.34 }\times \text{ 10}^{-\text{3}}\text{ mol L}^{-\text{1}} \end{align*} \nonumber \], Checking the accuracy of the approximation, we find, \(\dfrac{ [\text{ OH}^{-} ]}{c_{\text{b}}}=\dfrac{\text{1.34 }\times \text{ 10}^{-\text{3}}}{\text{0.1}}\approx \text{1 percent}\). For example, ammonia is a weak base because it produces a hydroxide ion and its conjugate base ammonium ion: \[{K_{\rm{b}}}\;{\rm{ = }}\;\frac{{\left[ {{\rm{N}}{{\rm{H}}_{\rm{4}}}^{\rm{ + }}} \right]\left[ {{\rm{O}}{{\rm{H}}^{\rm{ }}}} \right]}}{{\left[ {{\rm{N}}{{\rm{H}}_{\rm{3}}}} \right]}}\]. Chemistry questions and answers. Additionally, per the publisher's request, their name has been removed in some passages. Introduction i. Acids have sour tastes and cause certain dyes to change color, whereas bases taste bitter 1. BH B- + H+. It has a negative pka value. Postby Evan L 2B Mon Jan 31, 2022 4:46 am. Acid-Base Equilibrium | Calculating the Ka or Kb of a Solution - Video Amine Basicity Is Measued By The pKa Of Its Conjugate Acid (pKaH), Crc handbook ka values - yptbaltimore.org, Bordwell pKa Table - Organic Chemistry Data. (16.7.2) K b = BH + OH B. The relative strengths of some common acids and their conjugate bases are shown graphically in Figure 16.5. 0000007819 00000 n
16.7: Weak Bases is shared under a CC BY-NC-SA 3.0 license and was authored, remixed, and/or curated by LibreTexts. This table is part of our larger collection of acid-base . Because of the use of negative logarithms, smaller values of \(pK_a\) correspond to larger acid ionization constants and hence stronger acids. A statistical difference was significant when the p-value was less than 0.05. Because of the use of negative logarithms, smaller values of \(pK_a\) correspond to larger acid ionization constants and hence stronger acids. Strength of Bases based on their Kb values | Yeah Chemistry You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.48 M in this salt. Note: This expression, K b, is based on the general form for K c. The designation K b is used to indicate that it is the equilibrium constant for the reaction of a base with water.
General Ka expressions take the form Ka = [H3O+][A-] / [HA]. Calculate \(K_b\) and \(pK_b\) of the butyrate ion (\(CH_3CH_2CH_2CO_2^\)). PDF Ka values of some weak acids - Palomar College The difference between pKa and pKb is that pKa is the negative logarithm of Ka whereas . Acid dissociations are given a pKa value. It helps you see the H+ concentration more easily. Ephedrine, a central nervous system stimulant, is used in nasal sprays as . For any conjugate acidbase pair, \(K_aK_b = K_w\). Chapter 16- Acid-Base Equilibria I. Acids and Bases a. The pKbvalues of most common acids are given next to the correspondingKavalues in the table we have shown above. This equation is used to find either K a or K b when the other is . Here's a video on pKa and pKb. It is related to the acid dissociation constant, K a, by the simple relationship pK a + pK b = 14, where pK b and pK a . )%2F16%253A_AcidBase_Equilibria%2F16.07%253A_Weak_Bases, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), equation 4 in the section on the pH of weak acids, equation 6 in the section on the pH of weak acids, status page at https://status.libretexts.org, \(NH_3 + H_2O \rightleftharpoons NH^+_4 + OH^\), \(C_6H_5NH_2 + H_2O \rightleftharpoons C_6H_5NH^+_3 + OH^\), \(CO_3^{2} + H_2O \rightleftharpoons HCO^-_3 + OH^\), \(N_2H_4 + H_2O \rightleftharpoons N_2H^+_5 + OH^\), \(PO_4^{3} + H_2O \rightleftharpoons HPO^{2-}_4 + OH^\), \(C_5H_5N + H_2O \rightleftharpoons C_5H_5NH^+ + OH^\). Group II metal hydroxides (Mg(OH)2, Ba(OH)2, etc.) Architektw 1405-270 MarkiPoland. NaOH and KOH values agree with Kristi Lew, Acids and Bases (Essential Chemistry) KOH. Therefore, a large Kb value can be characterized by a small pKb value with small decimal places. One should always know which source to use. All Rights Reserved. Conjugate acids (cations) of strong bases are ineffective bases. Message of the colors is simple: The blue pKa is a measure of the base strength, the largest the blue pKa value the stronger the base. x Choose weak acid-base pairs to make a buffer based on desired pH and pKa values of the . The strong bases are listed at the bottom right of the table and get weaker as we move to the top of the table. deprotonated). Using the table of the weak base below, you have chosen Methylamine as your weak base in the buffer solution. NH 3 (aq) <> NH 4 + (aq) + OH - (aq) Then set up the ICE table and fill in the information from the . Relationship between \(pK_a\) and \(pK_b\) of a conjugate acidbase pair. In an aqueous solution, a weak base ionizes just minimally. pKa and pKb Table - Microbiology Note Strong Acids & Bases: Table & Examples - Study.com Its called acetic acid because it is an acid therefore it is not a base. The pH of a solution of a weak base can be calculated in a way which is very similar to that used for a weak acid. Because \(pK_a\) = log \(K_a\), we have \(pK_a = \log(1.9 \times 10^{11}) = 10.72\). Acid and Base Chart Table of Acids & Bases - Sigma-Aldrich Also to know is, what is the formula for KB? - Rehabilitationrobotic.net, Acids, Bases, Ka, Kb Equilibrium Law Flashcards - Quizlet. The greater the value of Kb, the stronger the base. Table of Contents show. At equilibrium, the concentration of each individual ion is the same as the concentration of the initial reactant. . These terms are used to make it easy to work with very large or very small values. pKa is given for acid dissociations. * Compiled from Appendix 5 Chem 1A, B, C Lab Manual and Zumdahl 6. th. 0000003232 00000 n
obtain Kb from Ka or Ka from Kb using Kw; determine pKa from Ka and pKb and Kb (or vice versa) and relate pKa or pKb values to the strength of the acid or base compound; calculate the pH of salt solutions; Topic 5: Polyprotic Acids and Bases. pH calculator program - Base Acid Titration and Equilibria - dissociation constants pKa and pKb. trailer
Group II metal hydroxides (Mg(OH)2, Ba(OH)2, etc.) Ka and Kb values are used to represent the percentage deprotonation and protonation respectively. Calculating K b. Kb and pKb As with acids, bases can either be strong or weak, depending on their extent of ionization. Kb values of some weak bases . Learn common examples of acids and bases, and explore the tables of strong acids and bases. To download a .zip file containing this book to use offline, simply click here. * Compiled from Appendix 5 Chem 1A, B, C Lab Manual and Zumdahl 6th Ed. Re: Strength of Bases. Again, for simplicity, \(H_3O^+\) can be written as \(H^+\) in Equation \(\ref{16.5.3}\). Acidic and Basic Salt Solutions - Purdue University . Here we have a buffer solution because it consists of a weak base ( N 3) and its salt ( N H 4 C l). - Rehabilitationrobotic.net As a table above that fluorometry can occur in the base pkb values of bases table as religion and. That means that the bases are getting stronger. Strong bases generally have a pH between 13 and 14. If either the pH or the pOH value of a solution is known, the other can be calculated. Aside from these, the carbonates (CO32-) and bicarbonates (HCO3) are also considered weak bases. Kontakta Tv4 Nyhetsmorgon, For an aqueous solution of a weak acid, the dissociation constant is called the acid ionization constant (Ka). We are given the \(pK_a\) for butyric acid and asked to calculate the \(K_b\) and the \(pK_b\) for its conjugate base, the butyrate ion. . 1 A). This order corresponds to decreasing strength of the conjugate base or increasing values of \(pK_b\). Conversely, smaller values of \(pK_b\) correspond to larger base ionization constants and hence stronger bases. Equilibrium Constants Ka And Kb Pka Pkb - Acid Base Equilibria - MCAT Ka and Kb - Chemistry Video | Clutch Prep, Table of Acids with Ka and pKa Values* CLAS Acid HA A - academia.edu, Strong Acids & Bases: Table & Examples - Study.com, Weak base equilibrium (video) | Khan Academy. This is what we also saw when introducing thepHto quantify the acidity of the solution. A year ago I bought a license for the CASC concentration calculator. Notice that the reaction is shown with a double arrow as it proceeds to a little extent until an equilibrium is established. Applications and skills. Answer (1 of 2): This could be a trick question, but according to two tables of Ka values that I checked, the Ka for H2O is 1.0 x 10^-14 which is the same as the Kw. The value of Ka or Kb is the strength of the acid or base. BASE: proton acceptor 2 In this context we are always looking at aqueous solutions in which the 'proton' is extensively hydrated. Strong bases completely dissociate in aq solution (Kb > 1, pKb < 1). 1 Answer anor277 Jan 6, 2016 #pK_a# #=# #-log_(10)K_a# Explanation: #H_3PO_4 + H . 1, we get: We can use these equations to determine (or ) of a weak base given of the conjugate acid. Pkb Values Of Bases Table Using the table of the weak base below, you have chosen Methylamine as your weak base in the buffer solution. VIDEO Solving Ka, Kb ICE Tables Demonstrated Example 1: If the initial concentration of the base NH 3 was 0.7M, and the Kb is 4.3 * 10-5. Use this acids and bases chart to find the relative strength of the most common acids and bases. pKa and pKb values have been taken from various books and internet sources. So, in an ionic form, the reactions can be shown as: Now, because acid-base reactions always occur in the direction of forming a weaker acid and a base, the oxide ion (O2-) must be a stronger base than the hydroxide ion. Please note: Although these values are common (and published) values associated with the substances given, there are many possible sources for these values. It's simply going to become A minus times H3O+ over HA. Acids. First week only $4.99! (16.7.1) B + H 2 O BH + + OH . How gen chem to a table by an pkb values of bases table search for bases of acids are dissolved in. For more information on the source of this book, or why it is available for free, please see the project's home page. Hence this equilibrium also lies to the left: \[H_2O_{(l)} + NH_{3(aq)} \ce{ <<=>} NH^+_{4(aq)} + OH^-_{(aq)}\]. VIDEO Solving Ka, Kb ICE Tables Demonstrated Example 1: If the initial concentration of the base NH 3 was 0.7M, and the Kb is 4.3 * 10-5. The conjugate base of H2O is OH- Now Ka Kb (for any conjugate acid/conjugate base pair) = 1.0 x 10^-14 So 1.0 x 10^-14 Kb = 1. Acid-base chemistry of aliphatic amines weak bases pKb Kb values why pH of Weak Acids and Bases - Percent Ionization - Ka & Kb, Acid/Base Ionization Constants - Chemistry 301, Understanding pKa Values: Information to Know - Night Helper, How do you find pKa from pKb? How do you find the Ka of an acid from pKa? If a weak base B accepts protons from water according to the equation. NaOH is classified as a strong base, which completely ionizes or dissociates in a solution into Na + and OH - ions. Because \(pK_b = \log K_b\), \(K_b\) is \(10^{9.17} = 6.8 \times 10^{10}\). 0000014076 00000 n
The magnitude of the equilibrium constant for an ionization reaction can be used to determine the relative strengths of acids and bases. This is related to K a by pK a + pK b = pK water = 14.00 (at 25C) Compounds are listed by molecular formula in Hill order. pKb = -log 10 K b. . To calculate the ionization . Transcribed Image Text: Using the table of the weak base below, you have chosen Pyridine as your weak base in the buffer solution. table of bases with kb and pkb values - vizits2netz.com The Kb value for a weak acid can be derived from the following formula: Kb = Kw/Ka To find the Kb for any weak base, identify its conjugate acid on the table of Relative Strengths of Aqueous Acids and Bases and divide Kw (1.0 x 10^-14) by the Ka value for that particular conjugate acid. Instead, they produce it by reacting with water. Determine the following. In this case, we are given \(K_b\) for a base (dimethylamine) and asked to calculate \(K_a\) and \(pK_a\) for its conjugate acid, the dimethylammonium ion. A significant Kb value implies a strong base's high amount of dissociation. Large numbers are strong acids, small numbers are weak acids --A strong acid has a stronger tendency to donate a proton --A strong base has a greater tendency to accept a proton. . This book is licensed under a Creative Commons by-nc-sa 3.0 license. name. The greater the value of Kb, the stronger the base. { "7.01:_Arrhenius_Acids_and_Bases" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.
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