Sulphuric acid can affect you by breathing in and moving through your skin. The value of Ka for hypochlorous acid HClO is 3.50 x 10-8. III. ncdu: What's going on with this second size column? See Answer Question: write a balanced chemical equation for the first dissociation of the polyprotic acid H2SO3 in water. vegan) just to try it, does this inconvenience the caterers and staff? 1st Equiv Point (pH= 7.1; mL NaOH= 100). For example, the general equation for the ionization of a weak acid in water, where HA is the parent acid and A is its conjugate base, is as follows: \[HA_{(aq)}+H_2O_{(l)} \rightleftharpoons H_3O^+_{(aq)}+A^_{(aq)} \label{16.5.1} \]. - 85.214.46.134. Consider the following reaction: H_2SO_3 + H_3AsO_4 \to H_3AsO_3 + SO_4^(2-) + 2H^+ a) In the above reaction, the oxidation state of sulfur changes from 0 to _____. Millero, F. J., 1983, The estimation of the pK The equations above are called acid dissociation equations. Consequently, it is impossible to distinguish between the strengths of acids such as HI and HNO3 in aqueous solution, and an alternative approach must be used to determine their relative acid strengths. Again, for simplicity, H3O + can be written as H + in Equation ?? There is a simple relationship between the magnitude of \(K_a\) for an acid and \(K_b\) for its conjugate base. Kim, H.-T. and FrederickJr., W. J., 1988, Evaluation of Pitzer ion interaction parameters of aqueous electrolytes at 25 C, I. What is the molarity of the H2SO3 Sulfur dioxide (SO2) is produced during the combustion of fossil fuels containing sulfur. Chem.49, 2934. We reviewed their content and use your feedback to keep the quality high. +4 What are the major and minor products of 2-methylcyclopentanol reacting with concentrated H2SO4? What is the chemical reaction for acid rain? Just like water, HSO4 can therefore act as either an acid or a base, depending on whether the other reactant is a stronger acid or a stronger base. 2 * for the ionization of H2SO3 in marine aerosols. Arrhenius dissociation: $$\ce {H2SO4 <=> H+ + HSO4-}~~~~~~~~~~\ce {K_ {a (1)}}=\ce {large}$$ Brnsted-Lowry Dissociation: In an acid-base neutralization reaction, 20.0 mL of 1.20 M sulfuric acid (H_2SO_4) is added to 25.0 mL of 2.00 M potassium hydroxide (KOH). Find the balanced equation for this reaction (in ionic form) and identify the oxidizing agent and the reducing agent for the reaction. Similarly, the equilibrium constant for the reaction of a weak base with water is the base ionization constant (\(K_b\)). , NO two steps: Sulfurous acid is not a monoprotic acid. Salts such as \(K_2O\), \(NaOCH_3\) (sodium methoxide), and \(NaNH_2\) (sodamide, or sodium amide), whose anions are the conjugate bases of species that would lie below water in Table \(\PageIndex{2}\), are all strong bases that react essentially completely (and often violently) with water, accepting a proton to give a solution of \(OH^\) and the corresponding cation: \[K_2O_{(s)}+H_2O_{(l)} \rightarrow 2OH^_{(aq)}+2K^+_{(aq)} \label{16.5.18} \], \[NaOCH_{3(s)}+H_2O_{(l)} \rightarrow OH^_{(aq)}+Na^+_{(aq)}+CH_3OH_{(aq)} \label{16.5.19} \], \[NaNH_{2(s)}+H_2O_{(l)} \rightarrow OH^_{(aq)}+Na^+_{(aq)}+NH_{3(aq)} \label{16.5.20} \]. Since we have a two substances combining, SO2 + H2O = H2SO3 is a Synthesis Reaction (also called a Combination Reaction" reaction). Thus sulfate is a rather weak base, whereas \(OH^\) is a strong base, so the equilibrium shown in Equation \(\ref{16.6}\) lies to the left. Substituting the values of \(K_b\) and \(K_w\) at 25C and solving for \(K_a\), \[K_a(5.4 \times 10^{4})=1.01 \times 10^{14} \nonumber \]. Is the God of a monotheism necessarily omnipotent? Click Start Quiz to begin! See the answer. What are ten examples of solutions that you might find in your home? The pK 1 * and pK 2 * of H2SO3 have been determined in NaCl solutions as a function of ionic strength (0.1 to 6 m) and temperature (5 and 25 C). Article Solution Chem.12, 401412. Because the \(pK_a\) value cited is for a temperature of 25C, we can use Equation \(\ref{16.5.16}\): \(pK_a\) + \(pK_b\) = pKw = 14.00. What is the product when magnesium reacts with sulfuric acid? It is a sulphur oxoacid, tautomer of a sulfonic acid, and conjugate acid of a hydrogensulfite. However there's no mention of clathrate on the whole page. Equiv Pt Conversely, the sulfate ion (\(SO_4^{2}\)) is a polyprotic base that is capable of accepting two protons in a stepwise manner: \[SO^{2}_{4 (aq)} + H_2O_{(aq)} \ce{ <=>>} HSO^{}_{4(aq)}+OH_{(aq)}^- \nonumber \], \[HSO^{}_{4 (aq)} + H_2O_{(aq)} \ce{ <=>>} H_2SO_{4(aq)}+OH_{(aq)}^- \label{16.6} \]. Solution Chem.3, 539546. It, thus, seems reasonable to assume that the interactions of Mg2+ and Ca2+ with HSO As you learned, polyprotic acids such as \(H_2SO_4\), \(H_3PO_4\), and \(H_2CO_3\) contain more than one ionizable proton, and the protons are lost in a stepwise manner. A 0.144 M solution of a monoprotic acid has a percent dissociation of 1.60%. Latest answer posted September 19, 2015 at 9:37:47 PM. The acid dissociation constant is the equilibrium constant of the dissociation reaction of an acid and is denoted by K a. Done on a Microsoft Surface Pro 3. Difficulties with estimation of epsilon-delta limit proof. Sulfurous acid is a corrosive chemical and until experimental values are available. 1 Millero, F. J. and Thurmond, V., 1983, The ionization of carbonic acid in NaMgCl solutions at 25 C, J. Although \(K_a\) for \(HI\) is about 108 greater than \(K_a\) for \(HNO_3\), the reaction of either \(HI\) or \(HNO_3\) with water gives an essentially stoichiometric solution of \(H_3O^+\) and I or \(NO_3^\). HNO3 - this is a strong acid and dissociation equation is HNO3 (aq) H+ (aq) + NO3- (aq) H2SO4 - This is not so simple: H2SO4 is a diprotic acid . * in artificial seawater were found to be in good agreement with the calculated values using the derived Pitzer parameters. It is a diprotic acid, meaning that it yields two protons (H+) per molecule. 1st Equiv Pt. One method is to use a solvent such as anhydrous acetic acid. How would you balance the equationP + O2 -> P2O5 ? Sulphurous acid is also called Sulphur dioxide solution or dihydrogen trioxosulphate or trioxosulphuric acid. For an aqueous solution of a weak acid, the dissociation constant is called the acid ionization constant (\(K_a\)). Majority of texts (at high school level) say that when $\ce{SO2}$ is dissolved in water sulphurous acid $\ce{H2SO3}$ is formed. What would the numerator be in a Ka equation for hydrofluoric acid? What are the spectator ions in the reaction between KCl (aq) and AgNO_3 (aq)? Data6, 2123. How many grams of sulfuric acid would be needed to make 2.5 x 102 mL of a 0.100 M H2SO4 solution? Pitzer, K. S. and Mayorga, G., 1973, Thermodynamics of electrolytes. Pitzer, K. S. and Kim, J. J., 1974, Thermodynamics of electrolytes. [H3O+][HSO3-] / [H2SO3] By clicking Accept all cookies, you agree Stack Exchange can store cookies on your device and disclose information in accordance with our Cookie Policy. Thus, the ion H. 2. [H3O+][SO3^2-] / [HSO3-]. B.) Acidbase reactions always contain two conjugate acidbase pairs. For example, hydrochloric acid is a strong acid that ionizes essentially completely in dilute aqueous solution to produce \(H_3O^+\) and \(Cl^\); only negligible amounts of \(HCl\) molecules remain undissociated. How many grams of H2SO4 can be found in 750 mL of a 3 M H2SO4? Identify the conjugate acidbase pairs in each reaction. Determine the acid dissociation constant (Ka) for a 0.200 M solution of hydrogen sulfate ion with a pH of 1.35 if the reaction for the dissociation of this acid is HSO4- arrow H+ + SO42-. How many mL of a 0.0500 M H2SO4 solution are needed to exactly neutralize 33.0 mL of 0.760 M KOH? Arena, G., Rizarelli, E., Sammartono, S., and Rigano, C., 1979, A non-linear least-squares approach to the refinement of all parameters involved in acid-base titration, Talanta26, 114. With our Essay Lab, you can create a customized outline within seconds to get started on your essay right away. Therefore, avoid skin contact with this compound. What is the pH of a 0.25 M solution of sulfurous acid? Calculate Ka1 and Ka2 This is a preview of subscription content, access via your institution. The LibreTexts libraries arePowered by NICE CXone Expertand are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. Unfortunately, however, the formulas of oxoacids are almost always written with hydrogen on the left and oxygen on the right, giving \(HNO_3\) instead. Thus acid strength decreases with the loss of subsequent protons, and, correspondingly, the \(pK_a\) increases. Calculate \(K_a\) and \(pK_a\) of the dimethylammonium ion (\((CH_3)_2NH_2^+\)). in NaCl solutions. below. Predict the redox reaction that will take place when a potassium dichromate solution is added to a sulfurous acid solution. How would you prepare a 0.250 L of 0.80 mol/L sulfuric acids, from an 18 mol/L concentrated solution of sulfuric acid? Both are acids and in water will ionize into a proton and the conjugate base. Balance this equation. Sulfurous acid | H2SO3 or H2O3S | CID 1100 - structure, chemical names, physical and chemical properties, classification, patents, literature, biological activities . H2SO4 + H2O = HSO4 (-)+ H3O (+) Here, the HSO4 (-) ion, with a unit negative charge, is the conjugate base of H2SO4. 1 The resultant parameters . Write molar and ionic equations of hydrolysis for FeCl3. The extrapolated values in water were found to be in good agreement with literature data. 7.1, 7.6, 10.1, II. Already a member? where the net photolysis of gaseous sulfurous acid (in addition to SO2) likely proceeds as follows: $\ce{H2SO3 (g) + hv -> .OH (g) + .HOSO (g) }$. The leveling effect applies to solutions of strong bases as well: In aqueous solution, any base stronger than OH is leveled to the strength of OH because OH is the strongest base that can exist in equilibrium with water. Single salt parameters, J. Chem. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. b) How many electrons are transferred in the reaction? pH------ 1.4, 1.8, Butyric acid is responsible for the foul smell of rancid butter. H_2S + H_2O Leftrightarrow Blank + H_3O^{+1}. H2S2O7 behaves as a monoacid in H2SO4. Updated on May 25, 2019. Darzi, M. and Winchester, J. W., 1981, Marine aerosol composition in the Indian Ocean, Symposium on the Role of the Oceans in Atmospheric Chemistry, IAMAP Third Scientific Assembly, Hamburg, FRG. The experimental results have been used to determine the Pitzer interaction parameters for SO2, HSO . Using first-principles simulations, we show that HOSO displays an unforeseen strong acidity (pK = 1) comparable with that of nitric acid and is fully dissociated at the airwater interface. HA How many mL of 2.00 M NaOH are needed to react with 15 mL of 0.400 M H2SO4 solution? For example, propionic acid and acetic acid are identical except for the groups attached to the carbon atom of the carboxylic acid (\(\ce{CH_2CH_3}\) versus \(\ce{CH_3}\)), so we might expect the two compounds to have similar acidbase properties. Disconnect between goals and daily tasksIs it me, or the industry? The equation for this reaction is H_2SO_4(aq) + BaCl_2(aq) + BaSO_4(s) + 2HCl(aq), Balance the following equation: C3H8O (aq) + CrO3 (g) + H2SO4 (aq) Cr2(SO4)3 (aq) + C3H6O(aq) + H2O(l), Write the dissociation equations for the following acids: A. HCl (strong) B. HC2H3O2 (weak). The equilibrium in the first reaction lies far to the right, consistent with \(H_2SO_4\) being a strong acid. A. and Riley, J. P., 1979, Solubility of sulfur dioxide in distilled water and decarbonated sea water, J. Chem. two steps: H2SO3 + H2O <---> H3O+ + HSO3- ; Ka1 = ACID = HI / H2SO3 / H2C2O4 BASE = Sr (OH)3 / LiOH SALT = BaF2 / KNO3 / NH4NO3 Classify the compounds as acids, bases, or salts. Two species that differ by only a proton constitute a conjugate acidbase pair. There are 100 M of 0.765 M sulfuric acid (H2SO4) that reacts with 23.9 grams of barium chloride (BaCl2). H2SO3 + H2O <---> H3O+ + HSO3- ; Ka1 = Screen capture done with Camtasia Studio 4.0. Site design / logo 2023 Stack Exchange Inc; user contributions licensed under CC BY-SA. How many mL of NaOH must be added to reach the first equivalence point? How do you calculate the dissociation constant in chemistry? To learn more, see our tips on writing great answers. eNotes Editorial, 7 May 2013, https://www.enotes.com/homework-help/use-chemical-equation-prove-that-h2so3-stronger-432981. Calculate \(K_a\) for lactic acid and \(pK_b\) and \(K_b\) for the lactate ion. solution? 7, CRC Press, Boca Raton, Florida, pp. Data33, 177184. -3 Why is is that tellurium(VI) fluoride is completely hydrolysed but iodine(III) fluoride isn't, even in hot water? Res.88, 10,72110,732. what is the dissociation reaction of H2SO3 and H2SO4? * for the dissociation of H2S in various media, Geochim. How would one make 250 mL of 0.75 M H2SO4 solution from a 17 M H2SO4 solution? 4 is a very weak acid, and HPO. below. The conjugate acidbase pairs are listed in order (from top to bottom) of increasing acid strength, which corresponds to decreasing values of \(pK_a\). Given the chemical reaction of H2SO4(aq) +BaCl2(s) to BaSO4(s) + 2HCl(aq). , SO What forms when hydrochloric acid and potassium sulfite react? The larger the \(K_b\), the stronger the base and the higher the \(OH^\) concentration at equilibrium. HSO3- + H2O <---> H3O+ + SO3^2- ; Ka2 = H2SO3 + H2O <---> H3O+ + HSO3- ; Ka1 = The equilibrium will therefore lie to the right, favoring the formation of the weaker acidbase pair: \[ \underset{\text{stronger acid}}{NH^+_{4(aq)}} + \underset{\text{stronger base}}{PO^{3-}_{4(aq)}} \ce{<=>>} \underset{\text{weaker base}}{NH_{3(aq)}} +\underset{\text{weaker acid}} {HPO^{2-}_{4(aq)}} \nonumber \]. Consider, for example, the \(HSO_4^/ SO_4^{2}\) conjugate acidbase pair. and SO We can use the relative strengths of acids and bases to predict the direction of an acidbase reaction by following a single rule: an acidbase equilibrium always favors the side with the weaker acid and base, as indicated by these arrows: \[\text{stronger acid + stronger base} \ce{ <=>>} \text{weaker acid + weaker base} \nonumber \]. Use H3O+ instead of H+. Weak bases react with water to produce the hydroxide ion, as shown in the following general equation, where B is the parent base and BH+ is its conjugate acid: \[B_{(aq)}+H_2O_{(l)} \rightleftharpoons BH^+_{(aq)}+OH^_{(aq)} \label{16.5.4} \]. If we add Equations \(\ref{16.5.6}\) and \(\ref{16.5.7}\), we obtain the following: In this case, the sum of the reactions described by \(K_a\) and \(K_b\) is the equation for the autoionization of water, and the product of the two equilibrium constants is \(K_w\): Thus if we know either \(K_a\) for an acid or \(K_b\) for its conjugate base, we can calculate the other equilibrium constant for any conjugate acidbase pair. Synthesis reactions follow the general form of: A + B AB An. 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"license:ccbyncsa", "licenseversion:40" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FBookshelves%2FGeneral_Chemistry%2FMap%253A_A_Molecular_Approach_(Tro)%2F16%253A_Acids_and_Bases%2F16.04%253A_Acid_Strength_and_the_Acid_Dissociation_Constant_(Ka), \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), Example \(\PageIndex{1}\): Butyrate and Dimethylammonium Ions, Solutions of Strong Acids and Bases: The Leveling Effect, Calculating pH in Strong Acid or Strong Base Solutions, status page at https://status.libretexts.org, \(\cancel{HCN_{(aq)}} \rightleftharpoons H^+_{(aq)}+\cancel{CN^_{(aq)}} \), \(K_a=[H^+]\cancel{[CN^]}/\cancel{[HCN]}\), \(\cancel{CN^_{(aq)}}+H_2O_{(l)} \rightleftharpoons OH^_{(aq)}+\cancel{HCN_{(aq)}}\), \(K_b=[OH^]\cancel{[HCN]}/\cancel{[CN^]}\), \(H_2O_{(l)} \rightleftharpoons H^+_{(aq)}+OH^_{(aq)}\). mL NaOH 0, 50, 100, The balanced chemical equation for the dissociation of both acids in water is: {eq}\rm H_2SO_3(aq) + H_2O(l) \rightleftharpoons HSO_3^-(aq) + H_3O^+(aq) \\ a) CaOH and H2SO3 b) CaOH and H2SO4 c) Ca(OH)2 and H2SO3 d) Ca(OH)2 and H2SO4, a. Accessed 4 Mar. The Ka for H2SO3 (sulfurous acid) is 0.016 and for H2S (hydrogen sulfide) it is 6.3x10^-8. Use the relationships pK = log K and K = 10pK (Equations \(\ref{16.5.11}\) and \(\ref{16.5.13}\)) to convert between \(K_a\) and \(pK_a\) or \(K_b\) and \(pK_b\). My code is GPL licensed, can I issue a license to have my code be distributed in a specific MIT licensed project? Trioxosulphuric acid is a liquid without colour and has a pungent burning sulphur smell. a) Write the chemical equation for each dissociation. Notice the inverse relationship between the strength of the parent acid and the strength of the conjugate base. HSO3- + H2O <---> H3O+ + SO3^2- ; Ka2 = Although each of these equations contains three terms, there are only four unknowns [H 3 O +], [H 2 S], [HS-], and [S 2-] because the [H 3 O +] and [HS-] terms appear in both equations.The [H 3 O +] term represents the total H 3 O + ion concentration from both steps and therefore must have the same . 2023. Who are the experts?Our certified Educators are real professors, teachers, and scholars who use their academic expertise to tackle your toughest questions. Hence the ionization equilibrium lies virtually all the way to the right, as represented by a single arrow: \[HCl_{(aq)} + H_2O_{(l)} \rightarrow H_3O^+_{(aq)}+Cl^_{(aq)} \label{16.5.17} \]. The magnitude of the equilibrium constant for an ionization reaction can be used to determine the relative strengths of acids and bases. S + O_2 \rightarrow SO_2, For the titration of sulfuric acid (H_2SO_4) with sodium hydroxide (NaOH), how many moles of sodium hydroxide would be required to react with. Thus the proton is bound to the stronger base. 2nd Write the balanced chemical equation for the first dissociation of the polyprotic acid H_3PO_3 in water. The smaller the Ka, the weaker the acid. Environ.18, 26712684. For any conjugate acidbase pair, \(K_aK_b = K_w\). Understand the Bronsted-Lowry acid definition, the mechanisms, and see Bronsted-Lowry acid and base conjugate examples. Millero, F. J., 1982, Use of models to determine ionic interactions in natural waters, Thalassia Jugoslavica18, 253291. How can you determine whether an equation is endothermic or exothermic? An ionic crystal lattice breaks apart when it is dissolved in water. What is the mass of oxygen in 250 g of sulfuric acid, H2SO4? {/eq}. Because of the use of negative logarithms, smaller values of \(pK_a\) correspond to larger acid ionization constants and hence stronger acids. Once again, the activity of water has a value of 1, so water does not appear in the equilibrium constant expression. Browse other questions tagged, Start here for a quick overview of the site, Detailed answers to any questions you might have, Discuss the workings and policies of this site. 1 What mass (in grams) of H2SO4 would be needed to make 750.0 mL of a 2.00 M H2SO4 solution? Identify the Bronsted acids for the following equilibrium: HClO_{4}(aq) + H_{2}O(l) H_{3}O+(aq) + ClO_{4} (aq) \\ - HClO and HO \\ - HO and ClO \\ - HClO and HO. * and pK (a) H_2SO_4 and HCl are acting as a conjugate acid-base pair (b) HCl is acting as a base (c) Cl^- is acting as a base (d). What is the pH of a 0.05 M solution of formic acid? Start your 48-hour free trial to get access to more than 30,000 additional guides and more than 350,000 Homework Help questions answered by our experts. , NH3 (g), NHO3 (g), Atmos. Res.82, 34573462. 16.4: Acid Strength and the Acid Dissociation Constant (Ka) is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by LibreTexts. In aqueous solutions, \(H_3O^+\) is the strongest acid and \(OH^\) is the strongest base that can exist in equilibrium with \(H_2O\). Write the reaction between formic acid and water. a. By clicking Post Your Answer, you agree to our terms of service, privacy policy and cookie policy. 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: \[ \ce{ CH_3CO_2H_{(aq)} + H_2O_{(l)} <<=> H_3O^+_{(aq)} + CH_3CO_{2(aq)}^- } \nonumber \]. A 150mL sample of H2SO3 was titrated with 0.10M Cosmochim. Let us know your assignment type and we'll make sure to get you exactly the kind of answer you need. Learn about Bronsted-Lowry acid. Latest answer posted December 07, 2018 at 12:04:01 PM. Thanks for contributing an answer to Chemistry Stack Exchange! What is the name of the salt produced from the reaction of calcium hydroxide and sulfuric acid? SO_3(g) + H_2O(l) ---> H_2SO_4(aq), Give the products(s) of the reaction (in H_{2}SO_{4}): CH_{2} CHCH_{3} + H_{2}O \rightarrow product(s) a. CH_{2}OHCH(OH)CH_{3} b. CH_{2}OHCH_{2}CH_{3} c. CH_{2}OHCHOHCH_{3} + H_{2} d. CH_{3}CH_{2}CH_{3} + H_{2}O_{2} e. CH_{3}CH(OH)CH_{3}.

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