dissociation of methanoic acid equation

It combines with a solvent molecule; when the solvent is water a, It is implicit in this definition that the quotient of. H+ aqueous equals 1.5 times 10 to the negative third moles per liter. chemPad Help Greek HC5H11CO2 + H20(I) = C5H 1 HCOOH( )aq H 2 2()g CO g (e) Is the reaction a redox reaction? The dissociation (ionisation) of an acid is an example of a homogeneous reaction. A weak acid is an acid that ionizes only slightly in an aqueous solution. First, let's write the balanced dissociation reaction of, Plugging the equilibrium concentrations into our. ( Weak acid and base ionization reactions and the related equilibrium constants, Ka and Kb. Buffer solutions also play a key role in analytical chemistry. To log in and use all the features of Khan Academy, please enable JavaScript in your browser. ( hydrochloric acid and ethanoic acid, Unit C1: Structures, Trends, Chemical Reactions, Quantitative Chemistry and Analysis, 1.8 Acids, bases and salts: Indicators and pH, 1.8.2 interpret given data about universal indicator (colour or pH) to classify solutions as acidic, alkaline or neutral and to indicate the relative strengths of acidic and alkaline solutions according to the following classification: pH 02 strong acid, 1.8.6 demonstrate knowledge and understanding that strong acids and strong alkalis are completely ionised in water, recall examples of strong acids (including hydrochloric acid, sulfuric acid and nitric acid) and recall examples of strong alkalis. We are also told to assume that the Unit 2: CHEMICAL BONDING, APPLICATION OF CHEMICAL REACTIONS and ORGANIC CHEMISTRY, (n) the similarities and differences in the reactions of strong and weak acids e.g. A calculated titration curve for oxalic acid is shown at the right. methanoic acid and hydrogen ions. Can I combine an Acid dissociation with autoionization of H2O? SH So all of these are happening in water. decimal place, we have determined that the acid dissociation constant for methanoic You will need to use the BACK BUTTON on your browser to come back here afterwards. The equilibrium constants are found by fitting calculated pH values to the observed values, using the method of least squares.[58]. The hydrochloric acid will fizz strongly with the sodium carbonate solution, whereas for ethanoic acid the fizzing will be detectable but less vigorous. These pages are in completely different parts of this site. / Douglas B., McDaniel D.H. and Alexander J.J. 2-D gel polyacrylamide gel electrophoresis, "Thermodynamic Quantities for the Ionization Reactions of Buffers", "Project: Ionic Strength Corrections for Stability Constants", "HendersonHasselbalch Equation: Derivation of p, "Chemical speciation of environmentally significant heavy metals with inorganic ligands. A link to the app was sent to your phone. The acid dissociation constant, Ka, comes from the equilibrium constant for the breakdown of an acid in aqueous solution: . However, acid-base reactions definitely take place in solvents other than water and even in the gas phase. K [77], Knowledge of pKa values is important for the understanding of coordination complexes, which are formed by the interaction of a metal ion, Mm+, acting as a Lewis acid, with a ligand, L, acting as a Lewis base. K A set of differentiated worksheets with answers to identify learning gaps and misconceptions on the topic of acids and bases. Therefore to get the pH we plug the concentration of H 3 O + into the equation pH=-log (0.013745) and get pH=1.86 Example 2: After adding 10 mL of 0.3 M NaOH Instead, a new equilibrium constant is defined which leaves it out. the equilibrium constant for the reaction of an acid with water. The extension with copper carbonate is a colourful additional reaction, or it could be used as an alternative to sodium carbonate. Ethanoic acid is a weak acid that In that case, there isn't a lot of point in including it in the expression as if it were a variable. The experiments illustrated are the four classical tests for acidity (pH, action with alkalis, carbonates and reactive metals). 3. Note that the standard free energy change for the reaction is for the changes from the reactants in their standard states to the products in their standard states. You can find more information about these and other properties of ethanoic acid atChemguide. HCl H + + Cl-This means that the concentration of H + ions in 0.4 M HCl is higher than that in 0.4 M ethanoic acid, so its pH is lower and its acid reactions are . (Collect in a tube inverted over the reaction tube and transfer the open end quickly to a flame a squeaky pop should be heard.) The acid was once prepared by the distillation of ants. HA. Acetic acid (found in vinegar) is a very common weak acid. Direct link to Romaa's post why are we making ICE tab, Posted 6 years ago. For example: This is a resource from thePractical Chemistry project, developed by the Nuffield Foundation and the Royal Society of Chemistry. I guess you are correct, because, as strong acids and bases dissociate completely in an aqueous solution, it is safe to say that their concentrations can be used in calculations. These equations allows us to manipulate acid and base . / Important buffer solutions include MOPS, which provides a solution with pH7.2, and tricine, which is used in gel electrophoresis. Direct link to Dulyana Apoorva's post I guess you are correct, , Posted 3 years ago. 3 Magnesium ribbon, Mg(s) see CLEAPSS Hazcard HC059A. a The higher the value of , the + Calculate the value of the acid dissociation constant (_) for methanoic acid (HCOOH) using the following two values: [HCOOH (aq)] = 1.5 10 mol/L and [H (aq)] = 1.5 10 mol/L. Everything is present in the same phase - in this case, in solution in water. Second, some reactions are exothermic and some are endothermic, but, when H is negative TS is the dominant factor, which determines that G is positive. a Only a few drops of sodium carbonate solution and sodium hydroxide solution will be needed to neutralise the acids as the alkaline solutions are eight times more concentrated than the acids. An acid dissociation constant is Try to identify the gas given off. for the example 1: calculating the % dissociation, the part where the ICE table is used and you can use the quadratic formula to find concentration "x", the two answers I got for x was x= -0.01285M and x=0.01245M. The discussion of weak and strong acids is probably more suited to advanced rather than intermediate students. 3 1. Amines act as bases because nitrogen's lone pair of electrons can accept an, Posted 6 years ago. What carboxylic acid will produce potassium butanoate when it is neutralized by KOH ? ions. They are listed in order of decreasing acid strength - the Ka values get smaller as you go down the table. p Both acids will fizz with the copper carbonate, but the reaction with hydrochloric acid will be more vigorous. [65], When two reactants form a single product in parallel, the macroconstant Solutions of carboxylic acids have a pH less than 7 and like other acids, can react with metals, metal oxides, hydroxides and carbonates forming salts. ) Oxalic acid has pKa values of 1.27 and 4.27. To solve the problem, first, write the chemical equation for the reaction. a This is analogous to finding the percent dissociation of an acid, except you are interested in what percentage of the base became ionized by bonding to an H+ ion. hydrogen ion and methanoate ion concentrations are equal. Aqueous solutions with normal water cannot be used for 1H NMR measurements but heavy water, D2O, must be used instead. 1 For an aqueous solution, the general form of the equilibrium reaction is: where HA is an acid which dissociates in the conjugate base of the acid A- and a hydrogen ion that combines with water to form the hydronium ion H3O+. Buffer solutions are used extensively to provide solutions at or near the physiological pH for the study of biochemical reactions;[67] the design of these solutions depends on a knowledge of the pKa values of their components. Many applications exist in biochemistry; for example, the pKa values of proteins and amino acid side chains are of major importance for the activity of enzymes and the stability of proteins. a value of 0.00015 moles per liter. Other chemical shifts, such as those of 31P can be measured. You can assume that the Write the balanced chemical equation for the dissociation of methanoic acid in water. Remember that although we often write H+ for hydrogen ions in solution, what we are actually talking about are hydroxonium ions. The acid dissociation constant is the equilibrium constant of the dissociation reaction of an acid and is denoted by Ka. Use and explain the terms dilute and concentrated (in terms of amount of substance), and weak and strong (in terms of the degree of ionisation) in relation to acids. When a weak acid reacts with water, Set up a test tube rack containing six test tubes. Read on . ) If you want to know why hydrogen fluoride is a weak acid, you can find out by following this link. When the glass electrode cannot be employed, as with non-aqueous solutions, spectrophotometric methods are frequently used. Strong acids like hydrochloric acid at the sort of concentrations you normally use in the lab have a pH around 0 to 1. You are also going to need to know about equilibrium constants, Kc for homogeneous equilibria. In practice, the ligand may be polyprotic; for example EDTA4 can accept four protons; in that case, all pKa values must be known. . When any excess copper carbonate has settled, the colours of copper chloride (green) and copper ethanoate (blue) will be seen. You can therefore write a simple expression for the equilibrium constant, K c. Here is the equilibrium again: (5) H A + H 2 O H 3 O + + A This is true for example for the deprotonation of the amino acid cysteine, which exists in solution as a neutral zwitterion HSCH2CH(NH+3)COO. You need to find out! The position of equilibrium of the reaction between the acid and water varies from one weak acid to another. You can therefore write a simple expression for the equilibrium constant, Kc. ThoughtCo. = HCOOH(aq), the reaction represented by the following equation occurs. You may find the Ka expression written differently if you work from the simplified version of the equilibrium reaction: This may be written with or without state symbols. ) NH Use the lowest possible whole number coefficients.) a) A buffer is prepared by dissolving 25.0 grams of sodium formate in 1.30 L of a solution of 0.660 M formic acid. You can therefore write a simple expression for the equilibrium constant, K c. Here is the equilibrium again: You might expect the equilibrium constant to be written as: This page explains the terms strong and weak as applied to acids. No packages or subscriptions, pay only for the time you need. I need some help with these, anyone point me in the right direction please? At the bottom of the expression, you have a term for the concentration of the water in the solution. (If the difference in pK values were about two or less, the end-point would not be noticeable.) stronger the acid. pKa bears exactly the same relationship to Ka as pH does to the hydrogen ion concentration: If you use your calculator on all the Ka values in the table above and convert them into pKa values, you get: Notice that the weaker the acid, the larger the value of pKa. For some molecules, dissociation (or association) can occur at more than one nonequivalent site, and the observed macroscopic equilibrium constant or macroconstant is a combination of microconstants involving distinct species. 2.5.27 investigate experimentally the reactions of carboxylic acids with carbonates, hydroxides and metals, test any gases produced and write balanced symbol equations for these reactions. For the dissociation of ethanoic acid: CH 3 COOH (aq) + H 2 O (l) = CH 3 COO -(aq) + H 3 O +(aq) K a = [CH 3 COO -(aq) ] [H 3 O +(aq)] / [CH 3 COOH (aq) ] Acid Dissociation Constant From pH The acid dissociation constant may be found it the pH is known. K Acids and Bases: Calculating pH of a Strong Acid, Henderson Hasselbalch Equation Definition, Acids and Bases - Calculating pH of a Strong Base, Ph.D., Biomedical Sciences, University of Tennessee at Knoxville, B.A., Physics and Mathematics, Hastings College. it dissociates further releasing more hydrogen ions in solution. K X dissociation constant for methanoic acid, HCOOH, using the following two The physics of restoration and conservation, RSC Yusuf Hamied Inspirational Science Programme, How to prepare for the Chemistry Olympiad, Reacting copper(II) oxide with sulfuric acid, Read our standard health and safety guidance, Mandatory experiment 7.5: The oxidation of phenylmethanol (benzyl alcohol) to benzoic acid with potassium manganate (VII) solution in alkaline conditions. In acidbase extraction, the efficiency of extraction of a compound into an organic phase, such as an ether, can be optimised by adjusting the pH of the aqueous phase using an appropriate buffer. We will introduce weak acids in Chapter 10, but for now the important thing to remember is that strong acids are virtually 100% ionized in solution. We can simplify the reaction of a [66] Protein pKa values cannot always be measured directly, but may be calculated using theoretical methods. Write the balanced chemical equation for the dissociation of methanoic acid in water. Like in gas? Strong acids have a large K a and completely dissociate and so you just state the reaction goes to completion. A strong acid is one which is virtually 100% ionised in solution. [37] These may involve absorbance or fluorescence measurements. The experimental determination of pKa values is commonly performed by means of titrations, in a medium of high ionic strength and at constant temperature. Data presented here were taken at 25C in water. . Comparing fresh and seawater, the differences in the first and second dissociation constants of carbonic acid -K1 and K2 for freshwater, and K1' and K2' for seawater- and the consequences thereoff will appear spectacular. Dissociation of bases in water In this case, the water molecule acts as an acid and adds a proton to the base. The vessel originally did not containany gas. We can start by writing the 3. Direct link to Yuya Fujikawa's post So all of these are happe, Posted 6 years ago. This means that the concentration of H+ ions in 0.4 MHCl is higher than that in 0.4Methanoic acid, so its pH is lower and its acid reactions are faster. From soaps to household cleaners, weak bases are all around us. 2.5.25 investigate experimentally the reactions of carboxylic acids with carbonates, hydroxides and metals, test any gases produced and write balanced symbol equations for these reactions. Helmenstine, Anne Marie, Ph.D. (2020, August 26). Add the copper carbonate to each tube in very small quantities, stirring with a glass rod, until nothing further happens. The lower the value for pKa, the stronger the acid. CH3COO divided by the concentration of CH3COOH. {\displaystyle K_{\mathrm {b} }} K Unit C2: Further Chemical Reactions, Rates and Equilibrium, Calculations and Organic Chemistry. This second version of the Ka expression isn't as precise as the first one, but your examiners may well accept it. Yours might want you to do it in a different order. K For example, when hydrogen chloride dissolves in water to make hydrochloric acid, so little of the reverse reaction happens that we can write: At any one time, virtually 100% of the hydrogen chloride will have reacted to produce hydroxonium ions and chloride ions. . Hydrogen is given off more slowly with ethanoic acid. a and A ions, then dividing by the equilibrium concentration of the acid. The more, The table below lists some more examples of weak acids and their, One way to quantify how much a weak acid has dissociated in solution is to calculate the percent dissociation. . + The equation for the dissociation of acetic acid, for example, is CH 3 CO 2 H + H 2 O CH 3 CO 2 + H 3 O +. + There are tables of acid dissociation constants, for easy reference. It is very difficult to measure pH values of less than two in aqueous solution with a glass electrode, because the Nernst equation breaks down at such low pH values. An acid dissociation constant is Hydrochloric acid is a strong acid and dissociates fully. {\displaystyle 1/K_{\text{a}}=1/K_{{\text{a}},{\text{terminal}}}+1/K_{{\text{a}},{\text{internal}}}.} Hydrochloric acid solution, HCl(aq) see CLEAPSSHazcardHC047aand CLEAPSSRecipe Book RB043. a This end-point is not sharp and is typical of a diprotic acid whose buffer regions overlap by a small amount: pKa2pKa1 is about three in this example. There is no point in reading any more of this page unless you do! The hydrochloric acid will fizz with the magnesium. Isothermal titration calorimetry (ITC) may be used to determine both a pK value and the corresponding standard enthalpy for acid dissociation. The magnesium should be scraped with a spatula, or rubbed with sandpaper, to remove any oxide coating. The data were critically selected and refer to 25C and zero ionic strength, in water.[11]. To avoid this, the numbers are often converted into a new, easier form, called pKa. Direct link to p4q4storm's post for the example 1: calcul, Posted 6 years ago. Therefore, in these equations [H+] is to be replaced by 10 pH. You should be able to recognize propionic acid is a weak acid (because it's not one of the strong acids and it contains hydrogen). weak acid with water by just showing the disassociation of the acid into H+ and A Jim Clark 2002 (modified November 2013). concentration of H+ times the concentration of A divided by the concentration of Table 8.1 lists the common strong acids that we will study in this text. 1.8.8 demonstrate knowledge and understanding that weak acids and weak alkalis are partially ionised in water, recall examples of weak acids (including ethanoic acid and carbonic acid) and recall examples of weak alkalis (including ammonia). Show your working. JavaScript is disabled. Legal. What if these reactions aren't happening in water? The most tricky area is the formulas of salts of divalent ions with ethanoate. At each point in the titration pH is measured using a glass electrode and a pH meter. However, the ligand may also undergo protonation reactions, so the formation of a complex in aqueous solution could be represented symbolically by the reaction, To determine the equilibrium constant for this reaction, in which the ligand loses a proton, the pKa of the protonated ligand must be known. ) Simplifying this expression, we get the following: This is a quadratic equation that can be solved for, To calculate percent dissociation, we can use the equilibrium concentrations we found in, Let's now examine the base dissociation constant (also called the base ionization constant), We can write the expression for equilibrium constant, From this ratio, we can see that the more the base ionizes to form, This example is an equilibrium problem with one extra step: finding. The dissociation (ionization) of an acid is an example of a homogeneous reaction. In this experiment, students test ethanoic acid with universal indicator solution, magnesium, sodium hydroxide solution and sodium carbonate solution. Direct link to yuki's post You can find the percent , Posted 6 years ago. The higher the value for pKa, the weaker the acid. https://www.thoughtco.com/acid-dissociation-constant-definition-ka-606347 (accessed May 1, 2023). All you have to do is work out the concentration of the hydrogen ions in the solution, and then use your calculator to convert it to a pH. start text, A, end text, start superscript, minus, end superscript, K, start subscript, start text, a, end text, end subscript, equals, start fraction, open bracket, start text, H, end text, start subscript, 3, end subscript, start text, O, end text, start superscript, plus, end superscript, close bracket, open bracket, start text, A, end text, start superscript, minus, end superscript, close bracket, divided by, open bracket, start text, H, A, end text, close bracket, end fraction, K, start subscript, start text, a, end text, end subscript, start text, B, H, end text, start superscript, plus, end superscript, K, start subscript, start text, b, end text, end subscript, equals, start fraction, open bracket, start text, B, H, end text, start superscript, plus, end superscript, close bracket, open bracket, start text, O, H, end text, start superscript, minus, end superscript, close bracket, divided by, open bracket, start text, B, end text, close bracket, end fraction, K, start subscript, start text, b, end text, end subscript, start text, H, F, end text, left parenthesis, a, q, right parenthesis, start text, H, B, r, end text, left parenthesis, a, q, right parenthesis, start text, H, A, end text, left parenthesis, a, q, right parenthesis, plus, start text, H, end text, start subscript, 2, end subscript, start text, O, end text, left parenthesis, l, right parenthesis, \rightleftharpoons, start text, H, end text, start subscript, 3, end subscript, start text, O, end text, start superscript, plus, end superscript, left parenthesis, a, q, right parenthesis, plus, start text, A, end text, start superscript, minus, end superscript, left parenthesis, a, q, right parenthesis, start text, H, end text, start superscript, plus, end superscript, open bracket, start text, H, end text, start subscript, 3, end subscript, start text, O, end text, start superscript, plus, end superscript, close bracket, start text, C, end text, start subscript, 4, end subscript, start text, H, end text, start subscript, 6, end subscript, start text, O, end text, start subscript, 5, end subscript, left parenthesis, start text, C, end text, start subscript, 4, end subscript, start text, H, end text, start subscript, 6, end subscript, start text, O, end text, start subscript, 5, end subscript, right parenthesis, K, start subscript, start text, a, end text, end subscript, left parenthesis, 25, degrees, start text, C, end text, right parenthesis, start text, N, H, end text, start subscript, 4, end subscript, start superscript, plus, end superscript, 5, point, 6, times, 10, start superscript, minus, 10, end superscript, start text, H, C, l, O, end text, start subscript, 2, end subscript, 1, point, 2, times, 10, start superscript, minus, 2, end superscript, 7, point, 2, times, 10, start superscript, minus, 4, end superscript, start text, C, H, end text, start subscript, 3, end subscript, start text, C, O, O, H, end text, 1, point, 8, times, 10, start superscript, minus, 5, end superscript, left parenthesis, start text, H, N, O, end text, start subscript, 2, end subscript, right parenthesis, 4, point, 0, times, 10, start superscript, minus, 4, end superscript, 0, point, 400, start text, space, M, end text, start text, H, N, O, end text, start subscript, 2, end subscript, start text, N, O, end text, start subscript, 2, end subscript, start superscript, minus, end superscript, left parenthesis, a, q, right parenthesis, start text, H, N, O, end text, start subscript, 2, end subscript, left parenthesis, a, q, right parenthesis, plus, start text, H, end text, start subscript, 2, end subscript, start text, O, end text, left parenthesis, l, right parenthesis, \rightleftharpoons, start text, H, end text, start subscript, 3, end subscript, start text, O, end text, start superscript, plus, end superscript, left parenthesis, a, q, right parenthesis, plus, start text, N, O, end text, start subscript, 2, end subscript, start superscript, minus, end superscript, left parenthesis, a, q, right parenthesis, K, start subscript, start text, a, end text, end subscript, equals, start fraction, open bracket, start text, H, end text, start subscript, 3, end subscript, start text, O, end text, start superscript, plus, end superscript, close bracket, open bracket, start text, N, O, end text, start subscript, 2, end subscript, start superscript, minus, end superscript, close bracket, divided by, open bracket, start text, H, N, O, end text, start subscript, 2, end subscript, close bracket, end fraction, equals, 4, point, 0, times, 10, start superscript, minus, 4, end superscript, open bracket, start text, H, end text, start superscript, plus, end superscript, close bracket, open bracket, start text, N, O, end text, start subscript, 2, end subscript, start superscript, minus, end superscript, close bracket, start text, H, N, O, end text, start subscript, 2, end subscript, left parenthesis, a, q, right parenthesis, start text, H, end text, start subscript, 3, end subscript, start text, O, end text, start superscript, plus, end superscript, start text, N, O, end text, start subscript, 2, end subscript, start superscript, minus, end superscript, 0, point, 400, start text, M, end text, minus, x, K, start subscript, start text, a, end text, end subscript, equals, start fraction, left parenthesis, x, right parenthesis, left parenthesis, x, right parenthesis, divided by, left parenthesis, 0, point, 400, start text, M, end text, minus, x, right parenthesis, end fraction, equals, 4, point, 0, times, 10, start superscript, minus, 4, end superscript, start fraction, x, squared, divided by, 0, point, 400, start text, M, end text, minus, x, end fraction, equals, 4, point, 0, times, 10, start superscript, minus, 4, end superscript, x, equals, 0, point, 0126, start text, space, M, end text, open bracket, start text, N, O, end text, start subscript, 2, end subscript, start superscript, minus, end superscript, close bracket, equals, open bracket, start text, H, end text, start subscript, 3, end subscript, start text, O, end text, start superscript, plus, end superscript, close bracket, equals, 0, point, 0126, start text, space, M, end text, start text, B, end text, left parenthesis, a, q, right parenthesis, plus, start text, H, end text, start subscript, 2, end subscript, start text, O, end text, left parenthesis, l, right parenthesis, \rightleftharpoons, start text, B, H, end text, start superscript, plus, end superscript, left parenthesis, a, q, right parenthesis, plus, start text, O, H, end text, start superscript, minus, end superscript, left parenthesis, a, q, right parenthesis, 1, point, 50, start text, space, M, end text, start text, N, H, end text, start subscript, 3, end subscript, left parenthesis, K, start subscript, start text, b, end text, end subscript, equals, 1, point, 8, times, 10, start superscript, minus, 5, end superscript, right parenthesis, open bracket, start text, O, H, end text, start superscript, minus, end superscript, close bracket, start text, N, H, end text, start subscript, 3, end subscript, left parenthesis, a, q, right parenthesis, plus, start text, H, end text, start subscript, 2, end subscript, start text, O, end text, left parenthesis, l, right parenthesis, \rightleftharpoons, start text, N, H, end text, start subscript, 4, end subscript, start superscript, plus, end superscript, left parenthesis, a, q, right parenthesis, plus, start text, O, H, end text, start superscript, minus, end superscript, left parenthesis, a, q, right parenthesis, K, start subscript, start text, b, end text, end subscript, equals, start fraction, open bracket, start text, N, H, end text, start subscript, 4, end subscript, start superscript, plus, end superscript, close bracket, open bracket, start text, O, H, end text, start superscript, minus, end superscript, close bracket, divided by, open bracket, start text, N, H, end text, start subscript, 3, end subscript, close bracket, end fraction, equals, 1, point, 8, times, 10, start superscript, minus, 5, end superscript, open bracket, start text, N, H, end text, start subscript, 4, end subscript, start superscript, plus, end superscript, close bracket, start text, N, H, end text, start subscript, 3, end subscript, left parenthesis, a, q, right parenthesis, start text, O, H, end text, start superscript, minus, end superscript, 1, point, 50, start text, M, end text, minus, x, K, start subscript, start text, b, end text, end subscript, equals, start fraction, left parenthesis, x, right parenthesis, left parenthesis, x, right parenthesis, divided by, 1, point, 50, start text, M, end text, minus, x, end fraction, equals, 1, point, 8, times, 10, start superscript, minus, 5, end superscript, start fraction, x, squared, divided by, 1, point, 50, start text, M, end text, minus, x, end fraction, equals, 1, point, 8, times, 10, start superscript, minus, 5, end superscript, x, equals, open bracket, start text, O, H, end text, start superscript, minus, end superscript, close bracket, equals, 5, point, 2, times, 10, start superscript, minus, 3, end superscript, start text, space, M, end text, start text, p, H, end text, plus, start text, p, O, H, end text, equals, 14, start text, p, H, end text, equals, 14, minus, start text, p, O, H, end text, start text, p, H, end text, equals, 14, point, 00, minus, left parenthesis, 2, point, 28, right parenthesis, equals, 11, point, 72, start text, C, end text, start subscript, 5, end subscript, start text, H, end text, start subscript, 5, end subscript, start text, N, end text, 1, point, 7, times, 10, start superscript, minus, 9, end superscript, 2, point, 6, times, 10, start superscript, minus, 20, end superscript, 3, point, 8, times, 10, start superscript, minus, 10, end superscript.

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