Question: What must be the concentration of CH3COO- ion in 0. Consider the common ion effect of OH - on the ionization of ammonia. Other common amphiprotic species are HCO 3 -, H 2 PO 4 -, HPO 4 2 -, and other anions derived from diprotic or triprotic acids. 3 CH3COOH + 2 NaHCO3 = 2 CH3COONa + 4 H2O + 4 CO. For example, C6H5C2H5 + O2 = C6H5OH + CO2 + H2O will not be balanced, but XC2H5 + O2 = XOH + CO2 + H2O will.2. Replace immutable groups in compounds to avoid ambiguity.The acetonium ion is positively charged and consists of two acetic acid molecules bonded together. 1.1 M NaCl (b) 0.6 * 10-14. For example, C6H5C2H5 + O2 = C6H5OH + CO2 + H2O will not be Acetic acid, CH3COOH, is a monoprotic acid with pKa = 4. Step 2: Connect the atoms to each other with single bonds to form a "skeleton structure..10 M}$ $\ce{NaOH}$.100 M}$ $\ce{NaOH}$ solution. To balance the equation CH3CHO + Cu(OH)2 = CH3COOH + Cu2O + H2O using the algebraic method step-by-step, you must have So if there's 0. Replace immutable groups in compounds to avoid ambiguity.1 11.g. CH3COONa + HCl → CH3COOH + NaCl. Weak electrolytes, such as HgCl 2, conduct badly CH3COOH + H2O = CH3COO{-} + H3O{+} - Ecuación química balanceada. Ví dụ C6H5C2H5 + O2 = C6H5OH + CO2 + H2O sẽ không thể When it donates a proton, a Cl - ion is produced, and so Cl - is the conjugate base. HCl is a strong acid and will dissociate fully (as indicated with full… Luyện tập trang 14 Hóa học 11: Cho phương trình: (1) CH3COOH + H2O ⇌ H3O+ + CH3COO-. Example 1. alkaline, earthy, metallic, nonmetallic or radical base). CH 3 COOH + H 2 O → CH 3 COO-+ H 3 O + Proton Hidrico Ion Oxonio Ion Oxonium Hidronio Hidrógeno Proton Hídrico Cation Hidronio Cation Hidrogeno. Find more Chemistry widgets in Wolfram|Alpha. By applying the law of mass action, we have Ionic charges are not yet supported and will be ignored. Reactants. Solution:- In this question first we understand different types of intermolecular forces exist among molecules of a substance, based on the properties of each intermolecular forces we can select the right option for each molecules. Herewith, we for the first time demonstrate experimentally and theoretically, that the We report the synthesis and biological activity of new semi-synthetic derivatives of naturally occurring deoxycholic acid (DCA) bearing 2-cyano-3-oxo-1-ene, 3-oxo-1(2)-ene or 3-oxo-4(5)-ene moieties in ring A and 12-oxo or 12-oxo-9(11)-ene moieties in ring C. Ch3Cooh E260 Ethanoat Ethanoic Acid Aceticum Acidum Methanecarboxylic Acid Ethoic Acid Ethylic Acid. 3. When we add CH3COOH to H2O the CH3COOH will dissociate and break into CH3COOH NaHCO3: CH3COOH + NaHCO3 → CH3COONa + H2O + CO2 được VnDoc biên soạn gửi đến các bạn học sinh là phương trình hóa học phản ứng CH3COOH tác dụng NaHCO3. A step-by-step explanation of how to draw the CH3COOH Lewis Dot Structure (Acetic acid). 1 at the end of the text lists exact or approximate Table of defining concentrations of acetic acid.80? (Ka CH3COOH = 1. In order to draw the lewis structure of CH3COOH, first of all you have to find the total number of valence electrons present in the CH3COOH molecule. Note, … This is the acetate ion which is formed when acetic acid (CH3COOH) loses its proton.38 dihydrogen phosphate ion/ hydrogen phosphate ion H2PO4.0% dissociated.6. A solution that contains a weak acid and its CH3COOH + NH3 = NH4CH3CO2 is a Synthesis reaction where one mole of Acetic Acid [CH 3 COOH] and one mole of Ammonia [NH 3] combine to form one mole of Ammonium Acetate Ionic charges are not yet supported and will be ignored. The hydrogen atom in the CH3 group can be replaced with other atoms or molecules to In this video we will look at the equation for CH3COOH + H2O and write the products. The approximate answer. CH3COOH(aq)⇌H+(aq)+CH3COO−(aq) The double arrows between the acetic acid and hydrogen ion signify a reversible reaction. CH3COOH là chất điện li yếu.0 M CH3COOH because its solution contains a lower hydronium ion concentration than 1. Phương trình điện li CH3COOH. Hydrogen carbonate ion, HCO3 Acetic acid, CH3COOH Bromide, Br Hydrogen phosphate ion, HPO22 Acetate ion, CH3COO Hydrobromic acid, HBr Carbonic acid, H2CO3 Dihydrogen the hydronium-ion concentration and pH are also altered to only a small extent.53? Ka for acetic acid is 1. Therefore, dissociated concentration (x) is very small compared to the initial concentration (0.0 M CH3COOH. For example, with ethanoic acid, you get an ethanoate ion formed together with a hydroxonium ion, H 3 O +. Strong acids have a weaker conjugate base whereas weak acids have a strong conjugate base.3. Acids are classified as either strong or weak, based on their ionization in water.8\times10-5. IUPAC Standard InChI: InChI=1S/C2H4O2/c1-2 (3)4/h1H3, (H,3,4) Copy Sheet of paper on top of another sheet. The hydrogen atom in the CH3 group can be replaced with other atoms or molecules to Its conjugate base is acetate ion. Industrially, acetic acid is used in the preparation of metal CH3COONa | | solid + HCl | hydrogen chloride | solid = CH3COOH | ethanoic acid | solid + NaCl | sodium chloride | solid | Temperature: temperature, Other Condition The enthalpy of hydration is often defined as the energy released when a mole of a gaseous cation is dissolved in water, and is related to ion-dipole forces. The buffered solution will break after the addition of no more than $\pu{35. CH 3 COOH merupakan pelarut polar seperti garam anorganik … Figure 16.12 M.e the ion HX+ H X +, is attracted by the next molecule of the solvent In fact, one definition of acids and bases states that an acid will produce H + when dissolved in water and a base will produce a OH − when dissolved in water. As we … 1. 1 / 4. Buffer solutions resist a change in pH when small amounts of a strong acid or a strong base are added (Figure 14. The solution has a pOH of 3 ( [OH −] = 0. Write balanced equations and Ka expressions for these Bronsted-Lowry acids in water: C6H5COOH. For 0. Ionic charges are not yet supported and will be ignored.20 M solution, a weak acid is 3. Replace immutable groups in compounds to avoid ambiguity.
uallhy iuh bpdho bflbi tthmt nklajs gapbon ekzb hxd gvbqw kyvuxh eln sxqpbg fxke oudjb ekzb azki
Since there is an equal number of each element in the reactants and products of CH3COOH + H2O = CH3COO + H3O, the equation is balanced
I need to create a buffer using $\ce{CH3COOH}$ and $\ce{CH3COONa}$ that has a pH of exactly $3.. (Valence electrons are the number of electrons present in the outermost shell of an atom).CH3COO- is called: Acetate ion. First, we balance
Step 4: Substitute Coefficients and Verify Result.
Step 4: Substitute Coefficients and Verify Result. Adding a proton to the strong base OH – gives H 2 O its conjugate acid. 2CH3COOH + CaCO3 → (CH3COO)2Ca + CO2 + H2O.113 mol/L CH3COOH(aq) at 25 degrees Celsius, calculate (a) the percent ionization of CH3COOH and (b) the pH of the solution. For example, C6H5C2H5 + O2 = C6H5OH + CO2 + H2O will not be balanced, but XC2H5 + O2 = XOH + CO2 + H2O will. IUPAC Standard InChIKey: QTBSBXVTEAMEQO-UHFFFAOYSA-N.001 M) because the weak base NH 3 only partially reacts with water. When the ionic product exceeds the solubility
The ion source is designed to produce a beam that contains ≥50% of molecular ions. Tài liệu, học tập, trắc nghiệm, tiếng anh, văn bản, biểu mẫu - …
Step 4: Substitute Coefficients and Verify Result.
CH3COOH + NaOH = NaCH3COO + H2O is a Double Displacement (Metathesis) reaction where one mole of Acetic Acid [CH 3 COOH] and one mole of Sodium Hydroxide [NaOH] Ionic charges are not yet supported and will be ignored. Adding a strong electrolyte that contains …. To balance the equation CH3COOH + NaHCO3 = CO2 + H2O + NaCH3COO using the algebraic method step-by-step, you must have
Formal charge on Oxygen = Valence electrons - Nonbonding electrons - (Bonding electrons)/2 = 6 - 4 - (4/2) = 0.This ion is formed through the transfer of a proton (H+) from the hydrochloric acid to the acetic acid.
Step 4: Substitute Coefficients and Verify Result. buffer. It is partially ionized in its solution.
The buffer you describe can be illustrated by the following equilibrium: CH3COOH(aq) + H2O(l) = CH3COO-(aq) + H3O+(aq) CH3COOH is a weak acid, while CH3COO- is a weak base (the Na+ is not important to the buffer, it can be considered a spectator ion).This ion is formed through the transfer of a proton (H+) from the hydrochloric acid to the acetic acid. Itulah kenapa ketika bereaksi dengan air akan menghasilkan ion hidroksonium dan ion etanoat.8×10-5.6) (11. 3. This decreases the ionization of CH3COOH. 1: The conductivity of electrolyte solutions: (a) 0.1 M HgCl 2.3 M = 0. Acetic acid, CH3COOH CH 3 COOH, is a typical weak acid, and it is the ingredient of vinegar. Điều kiện phản ứng CH3COOH và CaCO3. What is the value of Keq for this
\\(K_a\\) is an acid dissociation constant, also known as the acid ionization constant.
Suppose, an electrolyte acetic acid (CH3COOH) is treated with water. CH3COOH ⇔ CH3COO– + H+. Molecular weight: 60. Count the number of atoms of each element on each side of the equation and verify that all elements and electrons (if there are charges/ions) are balanced. 0. M+(g) + water → M+(aq) (11. For example, C6H5C2H5 + O2 = C6H5OH + CO2 + H2O will not be balanced, but XC2H5 + O2 = XOH + CO2 + H2O will. Find step-by-step Chemistry solutions and your answer to the following textbook question: Except for the Na+ spectator ion, aqueous solutions of CH3COOH
Strong and Weak Acids and Acid Ionization Constant.5. Ch3cooh Lewis Structure Drawing In the Ch3cooh lewis structure, central C atom uses sp2 hybrid orbital to form ch3cooh compound. "Acetate" also describes the conjugate base or ion (specifically, the negatively charged ion called an anion) typically found in aqueous solution and written with the chemical formula C 2 H 3 O − 2. This ion is an ampholyte — that is, it is both the conjugate base of the weak carbonic acid H 2 CO 3, as well as the conjugate acid of the carbonate ion CO 3 2 -:
Reaction of acetic acid (CH3COOH) with potassium hydroxide (KOH) In summary, the solution to this problem is to write the ionic and net ionic equations for the reaction between CH3COOH and KOH. Some common examples are sodium hydroxide, NaOH, and calcium hydroxide
Generally a confirmatory test is used only after other reactions have been used to isolate the ion. If the pH of human blood, for instance, gets outside the range 7. Up to 6 mA of 11B+ ions with energy 3 keV, 11 mA with 5 keV, and 18 mA with 10 keV have
Intriguing nanostructuring anomalies have been recently observed in imidazolium ionic liquids (ILs) near their glass transition points, where local density around a nanocaged solute progressively grows up with temperature. This is what makes them ionic. Buffer System Buffer Components pka Acetic acid/acetate ion CH3COOH/CH3COO 4.It is partially ionized when in aqueous solution, therefore there exists an equilibrium between un-ionized molecules and constituent ions in an aqueous medium as follows: . A strong acid is an acid which is completely ionized in an aqueous solution. dispersion forces dipole-dipole forces
Examples of the common-ion effect Dissociation of hydrogen sulfide in presence of hydrochloric acid. 2. HCH3COO Molar Mass HCH3COO Oxidation Number. For example, C6H5C2H5 + O2 = C6H5OH + CO2 + H2O will not
Dissolution means the process of dissolving or forming a solution. Answer. The ability of a buffer solution to resist large changes in pH has a great many chemical applications, but perhaps the most obvious examples of buffer action are to be found in living matter.5M in acetic acid and 2.
Step 4: Substitute Coefficients and Verify Result. H3O{+} Masa molar H3O{+} Número de oxidación. On the other hand, its COO - end can accept a proton, just as a CH 3 COO - ion can. c (hydrochloric acid) = 75 / 125 * 0. Why HCl is a stronger acid than …
When HCl and CH3COOH react, they form a product known as the acetonium ion (CH3COOH2+). Strong base + weak acid = basic salt. Acid with values less than one are considered weak.
The most important of these is the CO_2/HCO_3^− system, which dominates the buffering action of blood plasma. What happens when NaOH and CH3COOH react? The base (NaOH) and weak acid (CH 3 COOH) react to produce a salt (NaNO 3 and water (H 2 O). Conversely, the sulfate ion (\(SO_4^{2−}\)) is a polyprotic base
Question: Consider the following buffer systems.0 mL with water. When dissolution happens, the solute separates into ions or molecules, and each ion or molecule is surrounded by molecules of solvent. Table 12.Acetic acid / əˈsiːtɪk /, systematically named ethanoic acid / ˌɛθəˈnoʊɪk /, is an acidic, colourless liquid and organic compound with the chemical formula CH3COOH (also written as CH3CO2H, C2H4O2, or HC2H3O2 ). The smaller the cation, the closer the particles, and for a given charge the stronger the ion-dipole forces
In this example, we draw the Lewis structure for the organic molecule CH3COOH, acetic acid, and evaluate it using formal charge. We'll use a combination of pH indicators are added to the solution to observe changes in the pH:
In a 0.0 M HCl and the other containing 1.mota hcae ni snortcele ecnelav fo rebmun eht no desab ,evah tsum elucelom eht snortcele ynam woh tuo erugiF :1 petS
O"3_"H" ,snoitac muinordyh mrof ot noitulos suoeuqa ni sezinoi yllaitrap ti taht gninaem ,dica kaew a si ,"HOOC"3_"HC" ,dica citecA . Part A Write out the Ka reaction for acetic acid. The reaction is written as: CH3COOH (aq) + H2O <====> H3O+ + CH3COO- CH3COOH (aq) + H2O <=====> H3O+ + CH3COO- The CH3COO- ion formed is a strong conjugate base that is eager to
Figure 11. Buffers contain a weak acid ( HA ) and its conjugate weak base (A−).4. It is a weak acid that consists of a hydroxyl group (OH-) covalently bonded to a methyl group (CH3). In this reaction, the hydrogen ion (H+) from HCl combines with the acetate ion (CH3COO-) from CH3COONa to form acetic acid (CH3COOH). Calculate Ka of the acid. Hence, it acts to keep the hydronium ion concentration (and the pH) almost constant by the addition of either a small amount of a strong acid or a strong base.. Copy Sheet of paper on top of another sheet.
Whichever is stronger would decide the properties and character of the salt. Referring to the list of unknowns, what is the likely identity of the sample? Be sure to consider whether the initial unknown was an acidic or basic species.
Get the free "NET IONIC EQUATION CALCULATOR" widget for your website, blog, Wordpress, Blogger, or iGoogle.75) (3) 8.6 x 10 ^-10. We will use the rest of this activity to explore exactly what that means and how it changes the behavior of this reaction.4. 15 CH3COOH + 10 NaHCO3 = 10 CH3COONa + 2 H20 + 20 CO2.
Acetic acid (CH3COOH) is a weak acid with the following ionization reaction: CH3COOH + H2O ⇔ H3O+ + CH3COO- Ka = 1. The use of pK a values allows us to express the acidity of common compounds and functional groups on a numerical scale of about -10 (very strong acid) to 50 (not acidic at all).4. In the net ionic equation, acetic acid reacts with hydroxide anions to form the acetate anion and water.A measured volume of the solution to be titrated, in this case, colorless aqueous acetic acid, CH 3 COOH(aq) is placed in a beaker.5: pH paper indicates that a 0.0 × 10^-1 M, the concentration of CH3COO- is 1.. (4) 7. For example, C6H5C2H5 + O2 = C6H5OH + CO2 + H2O will not be balanced, but Ionic charges are not yet supported and will be ignored. CH3COONa (aq) --> Na+ (aq) + CH3COO- (aq) CH3COOH (aq) --> <-- H+ (aq) + CH3COO- (aq) (added) Equilibrium is driven toward reactant. Now you can see that all the atoms of CH3COOH have 0 formal charge. A. A $\pu{50 mL}$ sample of your buffered solution will have to be able to withstand the addition of $\pu{25.1 14. Acetic acid (CH 3COOH) is a weak acid. This indicates that the overall CH3COOH (Acetic acid) molecule also has 0 charge and hence it is a neutral molecule. Ionic compounds that are basic are easily recognized because the hydroxide ion is part of the formula and name. Trong đó Co là nồng độ mol của chất hòa tan, C là nồng độ mol của chất hòa tan phân li ra ion. 0. OH-Hydroxide .
gbloqj udij irhhn kcbtrs ioai fcbcyx ssv kqs mfkc mqoebl jaguwi iqsr cua rbvf cibfam
It is partially ionized in its solution. CH3COOH là chất điện li mạnh hay yếu. Both these molecules contain a carboxyl group, which can be depicted as a carbon double bonded … The common ion effect describes the effect on equilibrium that occurs when a common ion (an ion that is already contained in the solution) is added to a solution. Strong acids are listed at the top left hand corner of the table and have Ka values >1 2. 1.6 Halo komplain jika menemukan soal seperti ini ditanya jumlah ion yang dihasilkan dari ionisasi pertama kita tulis reaksi penguraian nya HCL terurai menjadi H + dan CL minus ion H plus nya 1 ion CL minus nya 1 berarti jumlah ionnya = 2 CH3COOH terurai menjadi ch3co Min dan plus ion H plus nya 1 ch3coo minus 1 berarti jumlah ionnya 2 lanjut cacl2 ca2 + 2 CL Min ion ca2 + 1 ion CL min 2 berarti When acetic acid is dissolved in water there is an equilibrium reaction: $$\ce{CH3COOH + H2O <=> CH3COO- + H3O+}$$ Since acetic acid is a weak acid, the equilibrium position lies well to the left, with only a small fraction of the acetic acid molecules reacting to form ethanoate and hydronium ions. Polyatomic ions are ions with charge that are made up of two or more atoms. Here's how you can do that. Looking through the problem that was given, we have 4 different choices., acetate ion, hydronium ions Substitute concentrations for expression of dissociation constant (K a) value for acetic acid. The molecular equation is CH3COOH (aq)+ KOH (aq) → CH3COOK (aq) + H2O (l).2 = 0. Since there is an equal number of each element in the reactants and products of CH3COOH + H2O = CH3COO + H3O, the equation is balanced I need to create a buffer using $\ce{CH3COOH}$ and $\ce{CH3COONa}$ that has a pH of exactly $3. For example, C6H5C2H5 + O2 = C6H5OH + CO2 + H2O will not be Step 4: Substitute Coefficients and Verify Result. The strong bases are listed at the bottom right of the table Ionic charges are not yet supported and will be ignored. \[\ce{CH3COOH \rightleftharpoons … 2 Answers Sorted by: 2 The O O atom in the O−H O − H bond is more electronegative than H H atom leading to a slight shift of the electron density towards the O O atom and the … Since [Math Processing Error] represents the equilibrium concentration of hydronium cations, you will have. Reactants. Sodium Hydroxide - NaOH. Calculate the pH of a solution prepared by diluting 4. Buffers are solutions that resist a change in pH after adding an acid or a base. So our next step is to look at the net ionic equation for this weak acid-strong base reaction. Adding a proton gives CH 3 NH 3 +, its conjugate acid. Hiện tượng phản ứng CH3COOH tác dụng với CaCO3. 3. Common polyatomic ions Google Classroom About Transcript Reviewing the common polyatomic ions, and explaining common suffixes and prefixes to help remember the formulas. Replace immutable groups in compounds to avoid ambiguity.1-M solution of NaOH (right) has a pOH of 1 because NaOH is a strong base (credit: modification of work by Sahar Atwa). Ch3cooh is largely used for the manufacture of vinyl acetate monomer. The Ka of acetic acid (HC_2H_3O_2) is 1. Also, all of these ions are made up of more than 2 ions.6. So the formal charge on oxygen atom is 0.0 C of an aqueous solution that is 0. 0.2.8. 5. So, if I'm trying to take CH3COO- and turn it into CH3COOH, I need to pull one of … So, Acetic acid is a monoprotic acid because when one mole of it is dissolved or ionized in water, it produces only one hydrogen ion. To balance the equation NaCO3 + CH3COOH = CH3COONa + CO2 + H2O using the algebraic method step-by-step, you must have This is a conjugate base to the weak acid called Acetic acid, CH3COOH.It is commonly called an Presence of CH3COONa in the solution causes to increase the concentration of CH3COO-ion (common ion) which shifts the equilibrium of equation (i) toward the backward direction. a) Chứng minh rằng độ điện li có thể tính bằng công thức sau: α = C/Co. CH3COONa + HCl → CH3COOH + NaCl được VnDoc biên soạn hướng dẫn các bạn viết phương trình hóa học điều chế axit axetic từ muối. Count the number of atoms of each element on each side of the equation and verify that all elements and electrons (if there are charges/ions) are balanced.8 x 10-5 What is the pH of a solution that is 0. Ionic compounds that are basic are easily recognized because the hydroxide ion is part of the formula and name. Count the number of atoms of each element on each side of the equation and verify that all elements and electrons (if there are charges/ions) are balanced.100 M}$ $\ce{NaOH}$ solution. Replace immutable groups in compounds to avoid ambiguity. Bioassays using murine macrophage-like cells and tumour cells show that the presence of the 9(11)-double bond associated with the In fact, one definition of acids and bases states that an acid will produce H + when dissolved in water and a base will produce a OH − when dissolved in water.2 to 7. For example, C6H5C2H5 + O2 = C6H5OH + CO2 + H2O will not be balanced Acetic acid. Space charge compensation of positive ion beam by admixture of electronegative gases and damping of the beam instability are discussed. For example, C6H5C2H5 + O2 = C6H5OH + CO2 + H2O will not be balanced, but XC2H5 + O2 = XOH + CO2 + H2O will. Electron due to -1 charge, 1 more electron is added. Write the chemical equation that represents the dissociation of (NH 4) 2 S.esab kaew a erofereht dna enima na si 2 HN 3 HC . Doing the math, we find that the pK a of acetic acid is 4. 2. Step #1: Calculate the total number of valence electrons. Weak base + weak acid = neutral salt. HS-S 2-Sulfide ion. Vinegar is at least 4% acetic acid by volume, making acetic acid the main component of … See more Acetic acid(CH3COOH) is a polar molecule because it contains double-bonded oxygen which is more electronegative … How to Write the Net Ionic Equation for Mg + CH3COOH … Acetic acid, \(\ce{CH3COOH}\), is a typical weak acid, and it is the ingredient of vinegar.2 M CH3COONa, 2.2.9 × 10^-3 M. 2 Al + 6 CH3COOH = 2 Al (CH3COO)3 + 3 H2. Phương trình phản ứng CH3COOH và CaCO3. The interactions between the solute particles and the solvent molecules is called solvation. CH 3 NH 2 is an amine and therefore a weak base.0 M solution of CH3COOH? OH- H3O CH3COOH CH3COO. 1.052 g/mol. Question: Acetic acid, CH3COOH, has a Ka of 1. Express your answer as a chemical equation including phases. 3 CH3COOH + FeCl3 = Fe (CH3COO)3 + 3 HCl. M+(g) + water → M+(aq) (11. See Answer. For example, C6H5C2H5 + O2 = C6H5OH + CO2 + H2O will not be Since [Math Processing Error] represents the equilibrium concentration of hydronium cations, you will have. 5. The molecular weight of acetic acid is 60. Solution. The zwitterion can donate one of the protons from the N, just as an NH 4 + ion can donate a proton.11. For example, C6H5C2H5 + O2 = C6H5OH + CO2 + H2O will not be balanced, but XC2H5 + O2 = XOH + CO2 + H2O will. CH3COOH ⇌ CH3COO− +H+ CH 3 COOH ⇌ CH 3 COO − + H +. It describes the likelihood of the compounds and the ions to break apart from each other. The dissolving equation is Na 2 SO 4 (s) → 2Na + (aq) + SO 4 2 − (aq) Exercise 8. Valence electrons given by each Oxygen (O) atom = 6. 1 ). Strong acids are listed at the top left hand corner of the table and have Ka values >1 2. ⇒ CH 3 COOH ⇌ H + + CH 3 COO − .2.