h2so3 dissociation equation

Does there exist a square root of Euler-Lagrange equations of a field? The magnitude of the equilibrium constant for an ionization reaction can be used to determine the relative strengths of acids and bases. where the net photolysis of gaseous sulfurous acid (in addition to SO2) likely proceeds as follows: $\ce {H2SO3 (g) + hv -> .OH (g) + .HOSO (g) }$ Supporting source: See Page S6,Table S2, Eq (1), Eq (2), Eq (5) and Eq (12) in this available supplement. Dissociation is the separation of ions that occurs when a solid ionic compound dissolves. Because acetic acid is a stronger acid than water, it must also be a weaker base, with a lesser tendency to accept a proton than $H_2O$. ?. Pitzer, K. S. and Mayorga, G., 1974, Thermodynamics of electrolytes. Single salt parameters, J. Chem. two steps: H2SO3 + H2O <---> H3O+ + HSO3- ; Ka1 = Harvie, C. E., Moller, N., and Weare, J. H., 1984, The prediction of mineral solubilities in natural waters: the NaKMgCaHClSO4OHHCO3CO3CO2H20 systems to high ionic strengths at 25 C, Geochim. of water produces? Part AGiven that sulfurous acid dissociates in water in two stepsAccording to given data First equivalence point is at 100mL and Half equivalence for. Eng. The best answers are voted up and rise to the top, Not the answer you're looking for? The reaction produces methylammonium sulfate (CH3NH3)2SO4, In which of the following reactions is the species on the left side acting as an acid? , SO Tanner, R. L., 1982, An ambient experimental study of phase equilibrium in the atmospheric system: aerosol H+, NH Acta47, 21212129. Learn more about the Structure, physical and chemical properties of H2SO3 from the experts at BYJUS. Other examples that you may encounter are potassium hydride ($KH$) and organometallic compounds such as methyl lithium ($CH_3Li$). Unfortunately, however, the formulas of oxoacids are almost always written with hydrogen on the left and oxygen on the right, giving $HNO_3$ instead. 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: \[ \ce{ CH_3CO_2H_{(aq)} + H_2O_{(l)} <<=> H_3O^+_{(aq)} + CH_3CO_{2(aq)}^- } \nonumber \]. Thus the conjugate base of a strong acid is a very weak base, and the conjugate base of a very weak acid is a strong base. Learn about Bronsted-Lowry acid. What is the concentration of OH. Because of the use of negative logarithms, smaller values of $pK_a$ correspond to larger acid ionization constants and hence stronger acids. What is the name of the acid formed when H2S gas is dissolved in water? Because $pK_a$ = log $K_a$, we have $pK_a = \log(1.9 \times 10^{11}) = 10.72$. -4 Hence the ionization equilibrium lies virtually all the way to the right, as represented by a single arrow: \[HCl_{(aq)} + H_2O_{(l)} \rightarrow H_3O^+_{(aq)}+Cl^_{(aq)} \label{16.5.17} \]. Thus propionic acid should be a significantly stronger acid than $HCN$. Majority of texts (at high school level) say that when $\ce{SO2}$ is dissolved in water sulphurous acid $\ce{H2SO3}$ is formed. {/eq} and {eq}\rm H_2SO_4 Dissociation. What type of reaction is a neutralization reaction? This problem has been solved! Calculate the pH of a 4mM solution of H2SO4. H2SO4 (aq) + 2NaOH (aq) 2H2O (l) + Na2SO4 (aq) Suppose a beaker contains 34.9 mL of 0.164 M H2SO4. 150, 200, 300 The experimental results have been used to determine the Pitzer interaction parameters for SO2, HSO The implication for acid rain formation has previously been noted, for example, in an MIT article, with cited Reactions (1) to (3) below: However, in this recent 2019 work: A New Mechanism of Acid Rain Generation from HOSO at the AirWater Interface, some important chemistry: The photochemistry of SO at the airwater interface of water droplets leads to the formation of HOSO radicals. What concentration, Consider the following reaction between sulfur trioxide and water: SO_{3 (g)} + H_2O_{(l)} \to H_2SO_{4 (aq)} A chemist allows 61.5 g of SO_3 and 11.2 g of H_2O to react. For example, nitrous acid ($HNO_2$), with a $pK_a$ of 3.25, is about a million times stronger acid than hydrocyanic acid (HCN), with a $pK_a$ of 9.21. How would you balance the equationP + O2 -> P2O5 ? b. The Ka for H2SO3 (sulfurous acid) is 0.016 and for H2S (hydrogen sulfide) it is 6.3x10^-8. In an acidbase reaction, the proton always reacts with the stronger base. Conversely, smaller values of $pK_b$ correspond to larger base ionization constants and hence stronger bases. To know the relationship between acid or base strength and the magnitude of $K_a$, $K_b$, $pK_a$, and $pK_b$. What is the molecular mass of sulfuric acid? 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. However, such solutions do show spectra of the hydrogen sulfite ion, $\ce{HSO3}$, by reaction with water, and it is in fact the actual reducing agent present: ions and pK Again, for simplicity, $H_3O^+$ can be written as $H^+$ in Equation $\ref{16.5.3}$. Write the reaction between formic acid and water. Consider $H_2SO_4$, for example: \[HSO^_{4 (aq)} \ce{ <=>>} SO^{2}_{4(aq)}+H^+_{(aq)} \;\;\; pK_a=-2 \nonumber \]. You will notice in Table $\PageIndex{1}$ that acids like $H_2SO_4$ and $HNO_3$ lie above the hydronium ion, meaning that they have $pK_a$ values less than zero and are stronger acids than the $H_3O^+$ ion. b) 250 mL of a 0.67 M solution of sulfurous acid is titrated with a solution of 0.1 M NaOH. Sulfur dioxide is fairly soluble in water, and by both IR and Raman spectroscopy; the hypothetical sulfurous acid, $\ce{H2SO3}$, is not present to any extent. Sulfurous acid, H2SO3, dissociates in water in Pitzer, K. S. and Mayorga, G., 1973, Thermodynamics of electrolytes. [H3O+][SO3^2-] / [HSO3-]. (a) NH_3 leftrightharpoons NH_4^+ + OH^- (b) H_2SO_4 leftrightharpoons H^+ + HSO_4^- (c) NaOH leftrightharpoons Na^+ + OH^- (d) H_2C_2O_4 leftrightharpoons H^+ + HC_2O_, Which is a conjugate acid base pair in the following equation? With our Essay Lab, you can create a customized outline within seconds to get started on your essay right away. The equilibrium constant is a way to measure what percentage of each acid is in the dissociated state (products) versus the associated state (reactant). A 0.144 M solution of a monoprotic acid has a percent dissociation of 1.60%. 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. Predict whether the equilibrium for each reaction lies to the left or the right as written. The resultant parameters for NaHSO3 and Na2SO3 were found to be in reasonable agreement with the values for NaHSO4 and Na2SO4. Predict the redox reaction that will take place when a potassium dichromate solution is added to a sulfurous acid solution. Two species that differ by only a proton constitute a conjugate acidbase pair. 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. A 150mL sample of H2SO3 was titrated with 0.10M The equations for that are below. A Video Calculating pH in Strong Acid or Strong Base Solutions: Calculating pH in Strong Acid or Strong Base Solutions [youtu.be]. What is the theoretical yield of sodium sulfate formed from the reaction of 42.2 g of sulfu. What is the net ionic equation for the reaction between aqueous sodium fluoride and aqueous hydrobromic acid, which yields sodium bromide and hydrofluoric acid ? Ionization equation: H2SO4 (arrow pointing right) 2H + SO4 The concentration of sulfuric acid is .004M a. In fact, all six of the common strong acids that we first encountered in Chapter 4 have $pK_a$ values less than zero, which means that they have a greater tendency to lose a proton than does the $H_3O^+$ ion. See Answer Question: write a balanced chemical equation for the first dissociation of the polyprotic acid H2SO3 in water. What is the formula for salt produced from the neutralization reaction between sulfuric acid and sodium hydroxide? and SO Created by Yuki Jung. S + HNO3 --%3E H2SO4 + NO2 + H2O. HSO3- + H2O <---> H3O+ + SO3^2- ; Ka2 = The relative order of acid strengths and approximate $K_a$ and $pK_a$ values for the strong acids at the top of Table $\PageIndex{1}$ were determined using measurements like this and different nonaqueous solvents. 209265. Complete the reaction then give the expression for the Ka for H2S in water. H_2SO_4 + H_20 \to HSO_4^{-1} + H_3O^{+1}. Get access to this video and our entire Q&A library, Bronsted-Lowry Acid: Definition & Examples. What is acid dissociation reaction for CH_3CO_2H? In order to balance H2SO3 = H2O + SO2 you'll need to watch out for two things. b) How many electrons are transferred in the reaction? Difficulties with estimation of epsilon-delta limit proof. Cosmochim. Again, for simplicity, H3O + can be written as H + in Equation ?? Transcribed Image Text: O ACIDS AND BASES Writing the dissociation reactions of a polyprotic acid Sulfurous acid (H2SO3) is a polyprotic acid. Substituting the values of $K_b$ and $K_w$ at 25C and solving for $K_a$, \[K_a(5.4 \times 10^{4})=1.01 \times 10^{14} \nonumber \]. 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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)}} $, $K_a=[H^+]\cancel{[CN^]}/\cancel{[HCN]}$, $\cancel{CN^_{(aq)}}+H_2O_{(l)} \rightleftharpoons OH^_{(aq)}+\cancel{HCN_{(aq)}}$, $K_b=[OH^]\cancel{[HCN]}/\cancel{[CN^]}$, $H_2O_{(l)} \rightleftharpoons H^+_{(aq)}+OH^_{(aq)}$. Determine the. 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. Rank the following items in order from largest to smallest: cell, chromosome, gene, DNA, organism, nucleus. What type of reaction occurs during an acid-base titration. How many grams of H2SO4 can be found in 750 mL of a 3 M H2SO4? Connect and share knowledge within a single location that is structured and easy to search. Douabul, A. Substituting the $pK_a$ and solving for the $pK_b$. Article Pitzer, K. S., 1979, Theory: ion interaction approach, in R. M., Pytkowicz (ed. Conversely, the sulfate ion ($SO_4^{2}$) is a polyprotic base that is capable of accepting two protons in a stepwise manner: \[SO^{2}_{4 (aq)} + H_2O_{(aq)} \ce{ <=>>} HSO^{}_{4(aq)}+OH_{(aq)}^- \nonumber \], \[HSO^{}_{4 (aq)} + H_2O_{(aq)} \ce{ <=>>} H_2SO_{4(aq)}+OH_{(aq)}^- \label{16.6} \]. 2 In its molten form, it can cause severe burns to the eyes and skin. 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. Arrhenius dissociation: $$\ce {H2SO4 <=> H+ + HSO4-}~~~~~~~~~~\ce {K_ {a (1)}}=\ce {large}$$ Brnsted-Lowry Dissociation: Required fields are marked *. Part of Springer Nature. Write ionic equations for the hydrolysis reactions. a. a) CaOH and H2SO3 b) CaOH and H2SO4 c) Ca(OH)2 and H2SO3 d) Ca(OH)2 and H2SO4, a. The magnitude of the equilibrium constant for an ionization reaction can be used to determine the relative strengths of acids and bases. {/eq}. What is the formula mass of sulfuric acid? Don't forget the H2O in SO2 on the product side of the chemical equation!Drawing/writing done in Adobe Illustrator 6.0. Updated on May 25, 2019. The larger the $K_a$, the stronger the acid and the higher the $H^+$ concentration at equilibrium. Write the net ionic equation for the reaction between hypochlorous acid and sodium hydroxide? -3 Its $pK_a$ is 3.86 at 25C. Give the net ionic equation for the reaction that occurs when aqueous solutions of H_2SO_4 and KOH are mixed. Daum, P. H., Kelly, T. J., Schwartz, S. E., and Newman, L., 1984, Measurements of chemical composition of stratiform clouds, Atmos. What am I doing wrong here in the PlotLegends specification? 1 Johansson, T. B., Van, Grieken, R. E., and Winchester, J. W., 1974, Marine influences on aerosol composition in the coastal zone, J. Rech. Similarly, Equation $\ref{16.5.10}$, which expresses the relationship between $K_a$ and $K_b$, can be written in logarithmic form as follows: The values of $pK_a$ and $pK_b$ are given for several common acids and bases in Tables $\PageIndex{1}$ and $\PageIndex{2}$, respectively, and a more extensive set of data is provided in Tables E1 and E2. eNotes.com will help you with any book or any question. According to Table $\PageIndex{1}$, HCN is a weak acid (pKa = 9.21) and $CN^$ is a moderately weak base (pKb = 4.79). It only takes a minute to sign up. III. How do you ensure that a red herring doesn't violate Chekhov's gun? Use H3O+ instead of H+. This equilibrium constant is a quantitative measure of the strength of an acid in a solution. * and pK Lantzke, I. R., Covington, A. K., and Robinson, R. A., 1973, Osmotic and activity coefficients of sodium dithiorate and sodium sulfite at 25 C, J. Chem. with possible eye damage. Find the balanced equation for this reaction (in ionic form) and identify the oxidizing agent and the reducing agent for the reaction. * and pK [H3O+][HSO3-] / [H2SO3], HSO3- + H2O <---> H3O+ + SO3^2- ; Ka2 = 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. The equations above are called acid dissociation equations. Since H2SO3 has the higher Ka value, it is the stronger acid of the two. 2nd Equiv Point (pH= 10.1 ; mL NaOH = 200) For any conjugate acidbase pair, $K_aK_b = K_w$. 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 $NO_3^$. Thus acid strength decreases with the loss of subsequent protons, and, correspondingly, the $pK_a$ increases. Butyric acid is responsible for the foul smell of rancid butter. 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 _____. Sulfurous acid is not a monoprotic acid. Write the ionic equation for the following reaction: H_2SO_4 (aq) + Ca (NO_3)_2 (aq) to CaSO_4(s) + 2 HNO_3 (aq). The conjugate acidbase pairs are listed in order (from top to bottom) of increasing acid strength, which corresponds to decreasing values of $pK_a$. Hence the $pK_b$ of $SO_4^{2}$ is 14.00 1.99 = 12.01. The [H+] = 0.0042M in a 0.10 M solution of formic acid (HCOOH - one ionizable hydrogen.) Equilibrium always favors the formation of the weaker acidbase pair. What is the cation reaction with water, cation K_a, anion reaction with water, anion K_b, acidic base prediction, and pH of solution of sodium sulfate? Write a net ionic equation for the reaction that occurs when aqueous solutions of perchloric acid and ammonia are combined. 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: \[K_2O_{(s)}+H_2O_{(l)} \rightarrow 2OH^_{(aq)}+2K^+_{(aq)} \label{16.5.18} \], \[NaOCH_{3(s)}+H_2O_{(l)} \rightarrow OH^_{(aq)}+Na^+_{(aq)}+CH_3OH_{(aq)} \label{16.5.19} \], \[NaNH_{2(s)}+H_2O_{(l)} \rightarrow OH^_{(aq)}+Na^+_{(aq)}+NH_{3(aq)} \label{16.5.20} \]. c. What is the % dissociation for formic acid? 7, CRC Press, Boca Raton, Florida, pp. Write a net ionic equation for the reaction that occurs, when aqueous solutions of hypochlorous acid and barium hydroxide are combined. Why does sodium react with water to produce a hydroxide, while zinc produces an oxide? To learn more, see our tips on writing great answers. What is the result of dissociation of water? Simply undo the crisscross method that you learned when writing chemical formulas of ionic compounds. Cattell, F. C. R., Scott, W. D., and Du, Cross, D., 1977, Chemical composition of aerosol particles greater than 1 m diameter in the vicinity of Tasmania, J. Geophys. - 85.214.46.134. Polyprotic acids (and bases) lose (and gain) protons in a stepwise manner, with the fully protonated species being the strongest acid and the fully deprotonated species the strongest base. N a H C O X 3 + H X 2 O N a X + + O H X + H X 2 O + C O X 2, but that has water on both sides of the equation. Some measured values of the pH during the titration are given N a H C O X 3 + H X 2 O N a X + + O H X + H X 2 C O X 3, but doesn't H X 2 C O X 3 decompose into H X 2 O + C O X 2? What is the number of moles of acid and how many alkali present in the following chemical reaction: 2KOH + H2SO4 to form K2SO4 + 2H20. Provided by the Springer Nature SharedIt content-sharing initiative, Over 10 million scientific documents at your fingertips, Not logged in A New Mechanism of Acid Rain Generation from HOSO at the AirWater Interface, We've added a "Necessary cookies only" option to the cookie consent popup. H2SO4(aq)+2NaOH(aq)=2H2O(l)+Na2SO4(aq) Suppose a beaker contains 34.9mL of 0.164M H2SO4. 1, Chap. b. Because the stronger acid forms the weaker conjugate base, we predict that cyanide will be a stronger base than propionate. IV. 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. Write a net ionic equation for the reaction that occurs, when ammonium carbonate (aq) and excess hydroiodic acid are combined. Sulfurous acid is an intermediate species in the formation of acid rain from sulfur dioxide.[2]. HBr + Al (OH)3 = H2O + AlBr3 Al (C2H3O2)3 + MgSO4 = Al2 (SO4)3 + Mg (C2H3O2)2 KI + CuSO4 = CuI + I2 + K2SO4 CsCl + Al (OH)3 = CsOH + AlCl3 MgI2 + Ag2SO4 = AgI + MgSO4 Mn + CuSO4 = MnSO4 + Cu BaS + NH4Cl = (NH4)2S + BaCl2 Ca (NO3)2 + K3PO4 = KNO3 + Ca3 (PO4)2 KF + H2SO4 = HF + K2SO4 FeCl2 + K3PO4 = Fe3 (PO4)2 + KCl Zn + CoCl2 = Co + ZnCl2 Since we have a two substances combining, SO2 + H2O = H2SO3 is a Synthesis Reaction (also called a Combination Reaction" reaction). Sulfurous acid, H2SO3, has two dissociation constants, Ki = 1.7 X 10-2, and Kz = 6.0 x 10 8. The corresponding expression for the reaction of cyanide with water is as follows: \[K_b=\dfrac{[OH^][HCN]}{[CN^]} \label{16.5.9} \]. There is a simple relationship between the magnitude of $K_a$ for an acid and $K_b$ for its conjugate base. 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: \[\text{stronger acid + stronger base} \ce{ <=>>} \text{weaker acid + weaker base} \nonumber \]. The equilibrium constant for this dissociation is as follows: \[K=\dfrac{[H_3O^+][A^]}{[H_2O][HA]} \label{16.5.2} \]. 2NaOH + H2SO4 rightarrow Na2SO4 + 2H2O. Goldberg, R. N. and Parker, V. B., 1985, Thermodynamics of solution of SO2 (g) in water and of aqueous sulfur dioxide solutions, J. Res. Acta52, 20472051. Cosmochim. Consider the following unbalanced equation for a chemical reaction: S + NO3^- + H^+ = SO2 + NO + H2O. Chem. The hydrogen sulfate ion ($HSO_4^$) is both the conjugate base of $H_2SO_4$ and the conjugate acid of $SO_4^{2}$. H two will form, it is an irreversible reaction . and SO Calculate Ka1 and Ka2 According to Raman spectra of SO 2 solutions shows that the intensities of the signals are consistent with the equilibrium as follows: SO 2 + H 2 O HSO 3 + H + where, Ka = 1.5410 2 and p Ka = 1.81. Some measured values of the pH during the titration are given The resultant parameters . Conversely, the conjugate bases of these strong acids are weaker bases than water. When the equation below is balanced and all coefficients are reduced to the lowest whole number, what is the sum of all coefficients? (Factorization), Identify those arcade games from a 1983 Brazilian music video. Hydrolysis of one mole of peroxydisulphuric acid with one mol. 1st Equiv Point (pH= 7.1; mL NaOH= 100). It is a stronger acid than acetic acid, but weaker than sulfuric acid and hydrochloric acid. It is soluble in water with the release of heat. What volume of an 18.0 M H2SO4 solution contains 0.85 moles of H2SO4? Let us know your assignment type and we'll make sure to get you exactly the kind of answer you need. A 150mL sample of H2SO3 was titrated with 0.10M The equilibrium constant expression for the ionization of HCN is as follows: \[K_a=\dfrac{[H^+][CN^]}{[HCN]} \label{16.5.8} \]. {/eq}? As you can see, the bisulfite anion can reform the sulfurous acid by accepting a proton. Part two of the question asked whether the solution would be acidic, basic, or neutral. Consider, for example, the ionization of hydrocyanic acid ($HCN$) in water to produce an acidic solution, and the reaction of $CN^$ with water to produce a basic solution: \[HCN_{(aq)} \rightleftharpoons H^+_{(aq)}+CN^_{(aq)} \label{16.5.6} \], \[CN^_{(aq)}+H_2O_{(l)} \rightleftharpoons OH^_{(aq)}+HCN_{(aq)} \label{16.5.7} \].