h2so3 dissociation equation

The acid dissociation constant is the equilibrium constant of the dissociation reaction of an acid and is denoted by K a. Some measured values of the pH during the titration are given This compound liberates corrosive, toxic and irritating gases. -3 solution? below. Created by Yuki Jung. Equiv Pt The equilibrium constant is a way to measure what percentage of each acid is in the dissociated state (products) versus the. NaOH. Used in the manufacturing of paper products. Am. The equilibrium constant for this dissociation is as follows: \[K=\dfrac{[H_3O^+][A^]}{[H_2O][HA]} \label{16.5.2} \]. Log in here. Sulphuric acid can affect you by breathing in and moving through your skin. Already a member? Measurements of the conductivity of 0.1 M solutions of both HI and \(HNO_3\) in acetic acid show that HI is completely dissociated, but \(HNO_3\) is only partially dissociated and behaves like a weak acid in this solvent. 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. Article Google Scholar. The relative strengths of some common acids and their conjugate bases are shown graphically in Figure \(\PageIndex{1}\). Like all equilibrium constants, acidbase ionization constants are actually measured in terms of the activities of \(H^+\) or \(OH^\), thus making them unitless. * 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). Sulfurous acid is not a monoprotic acid. 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 \(pK_b\). SIDE NOTE Sulfurous acid molecules are actually represented as sulfur dioxide and water. Since we have a two substances combining, SO2 + H2O = H2SO3 is a Synthesis Reaction (also called a Combination Reaction" reaction). Chem. Balanced equation of zinc carbonate + nitric acid = zinc nitrate + carbon dioxide + water. The [H+] = 0.0042M in a 0.10 M solution of formic acid (HCOOH - one ionizable hydrogen.) There are 100 M of 0.765 M sulfuric acid (H2SO4) that reacts with 23.9 grams of barium chloride (BaCl2). The larger the \(K_a\), the stronger the acid and the higher the \(H^+\) concentration at equilibrium. My code is GPL licensed, can I issue a license to have my code be distributed in a specific MIT licensed project? Soc.96, 57015707. How does dimethyl sulfate react with water to produce methanol? Environ.18, 26712684. {/eq}? Write the reaction between formic acid and water. Stack Exchange network consists of 181 Q&A communities including Stack Overflow, the largest, most trusted online community for developers to learn, share their knowledge, and build their careers. It is important to be able to write dissociation equations. 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 \(NO_3^\). in NaCl solutions. The extrapolated values in water were found to be in good agreement with literature data. 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. How to match a specific column position till the end of line? The experimental results have been used to determine the Pitzer interaction parameters for SO2, HSO It is a sulphur oxoacid, tautomer of a sulfonic acid, and conjugate acid of a hydrogensulfite. Acta52, 20472051. Connect and share knowledge within a single location that is structured and easy to search. Calculate \(K_b\) and \(pK_b\) of the butyrate ion (\(CH_3CH_2CH_2CO_2^\)). Also, related results for the photolysis of nitric acid, to quote: Here we present both field and laboratory results to demonstrate that HNO3 deposited on ground and vegetation surfaces may undergo effective photolysis to form HONO and NOx, 12 orders of magnitude faster than in the gas phase and aqueous phase. Select the correct answer and click on the Finish buttonCheck your score and answers at the end of the quiz, Visit BYJUS for all Chemistry related queries and study materials, Your Mobile number and Email id will not be published. S + HNO3 --%3E H2SO4 + NO2 + H2O. 11.2 Pitzer, K. S. and Kim, J. J., 1974, Thermodynamics of electrolytes. In order to balance H2SO3 = H2O + SO2 you'll need to watch out for two things. There is a simple relationship between the magnitude of \(K_a\) for an acid and \(K_b\) for its conjugate base. How does NH_4 react with water to form an acidic 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. 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. 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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When the equation below is balanced and all coefficients are reduced to the lowest whole number, what is the sum of all coefficients? Anyone you share the following link with will be able to read this content: Sorry, a shareable link is not currently available for this article. What volume of an 18.0 M H2SO4 solution contains 0.85 moles of H2SO4? Use H3O+ instead of H+. Solution Chem.15, 9891002. It is corrosive to tissue and metals. Phosphoric acid is not a particularly strong acid as indicated by its first dissociation constant. 7.1, 7.6, 10.1, Because of the use of negative logarithms, smaller values of \(pK_a\) correspond to larger acid ionization constants and hence stronger acids. How many ml of 0.335 M NaOH must be added to react completely with sulfuric aci, What is sulfur's oxidation number in the following reaction? The fully protonated species is always the strongest acid because it is easier to remove a proton from a neutral molecule than from a negatively charged ion. Required fields are marked *. Learn more about the Structure, physical and chemical properties of H2SO3 from the experts at BYJUS. Our summaries and analyses are written by experts, and your questions are answered by real teachers. 2-4 0.250 L of 0.430 M H2SO4 is mixed with 0.200 L of 0.200 M KOH. Chem.49, 2934. HI + KMnO4 + H2SO4 arrow I2 + MnSO4 + K2SO4 + H2O. * in artificial seawater were found to be in good agreement with the calculated values using the derived Pitzer parameters. 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 larger the \(K_b\), the stronger the base and the higher the \(OH^\) concentration at equilibrium. 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 . Like any other conjugate acidbase pair, the strengths of the conjugate acids and bases are related by \(pK_a\) + \(pK_b\) = pKw. Activity and osmotic coefficients for mixed electrolytes, J. Some measured values of the pH during the titration are given 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. and SO Educators go through a rigorous application process, and every answer they submit is reviewed by our in-house editorial team. 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 concentration of the LiOH solution? What is the. a- degree of dissociation. below. It is a diprotic acid, meaning that it yields two protons (H+) per molecule. What is the molarity of the H2SO3 Eng. Two species that differ by only a proton constitute a conjugate acidbase pair. Goldberg, R. N. and Parker, V. B., 1985, Thermodynamics of solution of SO2 (g) in water and of aqueous sulfur dioxide solutions, J. Res. Site design / logo 2023 Stack Exchange Inc; user contributions licensed under CC BY-SA. The conjugate acidbase pairs are listed in order (from top to bottom) of increasing acid strength, which corresponds to decreasing values of \(pK_a\). b) How many electrons are transferred in the reaction? 2023 eNotes.com, Inc. All Rights Reserved, https://www.scribd.com/doc/3274102/table-Ka-pKa. From Table \(\PageIndex{1}\), we see that the \(pK_a\) of \(HSO_4^\) is 1.99. Learn more about Institutional subscriptions. Write a net ionic equation for the reaction that occurs, when aqueous solutions of hypochlorous acid and barium hydroxide are combined. a) CaOH and H2SO3 b) CaOH and H2SO4 c) Ca(OH)2 and H2SO3 d) Ca(OH)2 and H2SO4, a. Write molar and ionic equations of hydrolysis for FeCl3. 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. Sulfurous acid, H2SO3, is a weak diprotic acid with acid-dissociation constants: Ka 1 =1.210-2 Ka 2 =6.210-8. Smaller values of \(pK_a\) correspond to larger acid ionization constants and hence stronger acids. Chem.77, 23002308. Dissociation is the separation of ions that occurs when a solid ionic compound dissolves. We could also have converted \(K_b\) to \(pK_b\) to obtain the same answer: \[pK_b=\log(5.4 \times 10^{4})=3.27 \nonumber \], \[K_a=10^{pK_a}=10^{10.73}=1.9 \times 10^{11} \nonumber \]. Hence the \(pK_b\) of \(SO_4^{2}\) is 14.00 1.99 = 12.01. What volume of 0.500 M H2SO4 is needed to react completely with 20.0 mL of 0.458 M LiOH? 2003-2023 Chegg Inc. All rights reserved. Millero, F. J., 1982, Use of models to determine ionic interactions in natural waters, Thalassia Jugoslavica18, 253291. Accessed 4 Mar. sulfur dioxide (g) + water (l) sulfurous acid (H2SO3) (g) a. Rosenstiel School of Marine and Atmospheric Science, University of Miami, 4600 Rickenbacker Causeway, 33149, Miami, FL, U.S.A. Frank J. Millero,J. Peter Hershey,George Johnson&Jia-Zhong Zhang, You can also search for this author in For a polyprotic acid, acid strength decreases and the \(pK_a\) increases with the sequential loss of each proton. ?. Disconnect between goals and daily tasksIs it me, or the industry? The equilibrium constant for this reaction is the base ionization constant (Kb), also called the base dissociation constant: \[K_b= \frac{[BH^+][OH^]}{[B]} \label{16.5.5} \]. The equilibrium will therefore lie to the right, favoring the formation of the weaker acidbase pair: \[ \underset{\text{stronger acid}}{CH_3CH_2CO_2H_{(aq)}} + \underset{\text{stronger base}}{CN^-_{(aq)}} \ce{<=>>} \underset{\text{weaker base}}{CH_3CH_2CO^-_{2(aq)}} +\underset{\text{weaker acid}} {HCN_{(aq)}} \nonumber \], A Video Discussing Polyprotic Acids: Polyprotic Acids [youtu.be]. Consider, for example, the \(HSO_4^/ SO_4^{2}\) conjugate acidbase pair. 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). How many moles are there in 7.52*10^24 formula units of H2SO4? Sulfuric acid is a strong acid and completely dissolves in water. Part AGiven that sulfurous acid dissociates in water in two stepsAccording to given data First equivalence point is at 100mL and Half equivalence for. Chem.79, 20962098. The \(pK_a\) of butyric acid at 25C is 4.83. HSO3- + H2O <---> H3O+ + SO3^2- ; Ka2 = Chemistry questions and answers. -3 - 85.214.46.134. * for the dissociation of H2S in various media, Geochim. Solution Chem.3, 539546. 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: \[\text{stronger acid + stronger base} \ce{ <=>>} \text{weaker acid + weaker base} \nonumber \]. K a is commonly expressed in units of mol/L. B.) Also, related results for the photolysis of nitric acid, to quote: b) 250 mL of a 0.67 M solution of sulfurous acid is titrated with a solution of 0.1 M NaOH. Sulfurous Acid (H2SO3) - Sulfurous Acid is the chemical name of H2SO3. Sulfur dioxide (SO2) is produced during the combustion of fossil fuels containing sulfur. 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. What am I doing wrong here in the PlotLegends specification? What is the mass of oxygen in 250 g of sulfuric acid, H2SO4? Sulfurous acid, H 2 SO 3, is a diprotic acid K a1 = 1.3 10-2 and K a2 = 6.3 10-8.The acid forms when sulfur dioxide (a gas with a suffocating odor) dissolves in water. b. Which acid and base react to form water and sodium sulfate? 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: \[ \ce{ CH_3CO_2H_{(aq)} + H_2O_{(l)} <<=> H_3O^+_{(aq)} + CH_3CO_{2(aq)}^- } \nonumber \]. Other examples that you may encounter are potassium hydride (\(KH\)) and organometallic compounds such as methyl lithium (\(CH_3Li\)). Consider \(H_2SO_4\), for example: \[HSO^_{4 (aq)} \ce{ <=>>} SO^{2}_{4(aq)}+H^+_{(aq)} \;\;\; pK_a=-2 \nonumber \]. Your Mobile number and Email id will not be published. This order corresponds to decreasing strength of the conjugate base or increasing values of \(pK_b\). 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. It is soluble in water with the release of heat. Predict whether the equilibrium for each reaction lies to the left or the right as written. With our Essay Lab, you can create a customized outline within seconds to get started on your essay right away. Latest answer posted July 17, 2012 at 2:55:17 PM. 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. Because \(pK_b = \log K_b\), \(K_b\) is \(10^{9.17} = 6.8 \times 10^{10}\). "Use chemical equations to prove that H2SO3 is stronger than H2S." 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? pH------ 1.4, 1.8, 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. The equilibrium will therefore lie to the right, favoring the formation of the weaker acidbase pair: \[ \underset{\text{stronger acid}}{NH^+_{4(aq)}} + \underset{\text{stronger base}}{PO^{3-}_{4(aq)}} \ce{<=>>} \underset{\text{weaker base}}{NH_{3(aq)}} +\underset{\text{weaker acid}} {HPO^{2-}_{4(aq)}} \nonumber \]. Acidbase reactions always contain two conjugate acidbase pairs. Difficulties with estimation of epsilon-delta limit proof. What is the theoretical yield of sodium sulfate formed from the reaction of 42.2 g of sulfu. volume8,pages 377389 (1989)Cite this article. This problem has been solved! copyright 2003-2023 Homework.Study.com. The solubility of SO2 and the dissociation of H2SO3 in NaCl solutions. 2023 Springer Nature Switzerland AG. Calculate Ka1 and Ka2 Atmos.8, 761776. What is acid dissociation reaction for CH_3CO_2H? A conjugate acid is formed when a proton is added to a base, and a conjugate base is formed when a proton is removed from an acid. 1st Equiv Point (pH= 7.1; mL NaOH= 100). 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 \(H_2O\). 2 What is the formula mass of sulfuric acid? Write balanced chemical equations for the sequence of reactions that sulfurous acid can undergo when it's dissolved in water. with possible eye damage. We are given the \(pK_a\) for butyric acid and asked to calculate the \(K_b\) and the \(pK_b\) for its conjugate base, the butyrate ion. The equilibrium in the first reaction lies far to the right, consistent with \(H_2SO_4\) being a strong acid. Thanks for contributing an answer to Chemistry Stack Exchange! 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). Res.88, 10,72110,732. Some measured values of the pH during the titration are given below. https://doi.org/10.1007/BF00052711. Thanks for bringing up this topic, and I would have appreciated it a few years earlier, however! If the temperature of the solution rises by 13.2^oC, what is the heat of neutralization for sulfuric acid, in kJ/mo. Millero, F. J. and Thurmond, V., 1983, The ionization of carbonic acid in NaMgCl solutions at 25 C, J. In its molten form, it can cause severe burns to the eyes and skin. Sulfurous acid is a corrosive chemical and What is the formula for salt produced from the neutralization reaction between sulfuric acid and sodium hydroxide? Data18, 241242. The conjugate acidbase pairs are \(CH_3CH_2CO_2H/CH_3CH_2CO_2^\) and \(HCN/CN^\). b. In particular, we would expect the \(pK_a\) of propionic acid to be similar in magnitude to the \(pK_a\) of acetic acid. This is a preview of subscription content, access via your institution. 26) WRITE A BALANCED EQUATION FOR THE DISSOCIATION OF THE FOLLOWING ELECTROLYTES: a) H2SO3, strong e) HC2H3O2, weak c) C12H22O11 (sugar) , non-electrolyte . Sulphurous Acid is used as an intermediate in industries. J Atmos Chem 8, 377389 (1989). The \(pK_a\) and \(pK_b\) for an acid and its conjugate base are related as shown in Equations \(\ref{16.5.15}\) and \(\ref{16.5.16}\). A. and Riley, J. P., 1979, Solubility of sulfur dioxide in distilled water and decarbonated sea water, J. Chem. Each acid and each base has an associated ionization constant that corresponds to its acid or base strength. Hence the ionization equilibrium lies virtually all the way to the right, as represented by a single arrow: \[HCl_{(aq)} + H_2O_{(l)} \rightarrow H_3O^+_{(aq)}+Cl^_{(aq)} \label{16.5.17} \]. How can this new ban on drag possibly be considered constitutional? Which of the salts hydrolyze in aqueous solution: CaSO4, (NH4)2CO3, or Al2S3? 4 2 is an extremely weak acid. Substituting the \(pK_a\) and solving for the \(pK_b\). Done on a Microsoft Surface Pro 3. 7, CRC Press, Boca Raton, Florida, pp. Eng. Its \(pK_a\) is 3.86 at 25C. Write a net ionic equation for the reaction that occurs when aqueous solutions of perchloric acid and ammonia are combined. Chem1 Virtual Textbook. Consider the reaction of sulfuric acid, H2SO4, with sodium hydroxide, NaOH. All rights reserved. H2SO4 + H2O = HSO4 (-)+ H3O (+) Here, the HSO4 (-) ion, with a unit negative charge, is the conjugate base of H2SO4. IV. 1 If you preorder a special airline meal (e.g. Each successive dissociation step occurs with decreasing ease. Then refer to Tables \(\PageIndex{1}\)and\(\PageIndex{2}\) and Figure \(\PageIndex{2}\) to determine which is the stronger acid and base. What is the concentration of sulfite ion, SO 3 2-, in the solution?Note that K a1 is relatively latge. 1st Equiv Pt. Supporting source: See Page S6,Table S2, Eq (1), Eq (2), Eq (5) and Eq (12) in this available supplement. What is the name of the acid formed when H2S gas is dissolved in water? H2SO4 (aq) + 2NaOH (aq) 2H2O (l) + Na2SO4 (aq) Suppose a beaker contains 34.9 mL of 0.164 M H2SO4. Solution Chem.12, 401412. How many mL of NaOH must be added to reach the first equivalence point? For an aqueous solution of a weak acid, the dissociation constant is called the acid ionization constant (\(K_a\)). Thus, the ion H. 2. Give the balanced chemical reaction, ICE table, and show your calculation. What is the pH of a 0.05 M solution of formic acid? Thus acid strength decreases with the loss of subsequent protons, and, correspondingly, the \(pK_a\) increases. 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? B.) Hoffmann, M. R. and Edwards, J. O., 1975, Kinetics of the oxidation of sulfite by hydrogen peroxide in acid solution, J. Phys. The constants \(K_a\) and \(K_b\) are related as shown in Equation \(\ref{16.5.10}\). The magnitude of the equilibrium constant for an ionization reaction can be used to determine the relative strengths of acids and bases. 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) \\ Conversely, the sulfate ion (\(SO_4^{2}\)) is a polyprotic base that is capable of accepting two protons in a stepwise manner: \[SO^{2}_{4 (aq)} + H_2O_{(aq)} \ce{ <=>>} HSO^{}_{4(aq)}+OH_{(aq)}^- \nonumber \], \[HSO^{}_{4 (aq)} + H_2O_{(aq)} \ce{ <=>>} H_2SO_{4(aq)}+OH_{(aq)}^- \label{16.6} \]. 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: \[B_{(aq)}+H_2O_{(l)} \rightleftharpoons BH^+_{(aq)}+OH^_{(aq)} \label{16.5.4} \]. Write the net ionic equation for the reaction between hypochlorous acid and sodium hydroxide? two steps: Learn more about Stack Overflow the company, and our products. What type of reaction is a neutralization reaction? Once again, the activity of water has a value of 1, so water does not appear in the equilibrium constant expression. Screen capture done with Camtasia Studio 4.0. [H3O+][SO3^2-] / [HSO3-]. ), Activity Coefficients in Electrolyte Solutions, Vol. 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}. Conversely, smaller values of \(pK_b\) correspond to larger base ionization constants and hence stronger bases. What is the pH of a 0.25 M solution of sulfurous acid? Latest answer posted December 07, 2018 at 12:04:01 PM. Let us know your assignment type and we'll make sure to get you exactly the kind of answer you need. 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: \[K_2O_{(s)}+H_2O_{(l)} \rightarrow 2OH^_{(aq)}+2K^+_{(aq)} \label{16.5.18} \], \[NaOCH_{3(s)}+H_2O_{(l)} \rightarrow OH^_{(aq)}+Na^+_{(aq)}+CH_3OH_{(aq)} \label{16.5.19} \], \[NaNH_{2(s)}+H_2O_{(l)} \rightarrow OH^_{(aq)}+Na^+_{(aq)}+NH_{3(aq)} \label{16.5.20} \]. Unfortunately, however, the formulas of oxoacids are almost always written with hydrogen on the left and oxygen on the right, giving \(HNO_3\) instead. This is called a neutralization reaction and will produce water and potassium sulfate. Since there are two steps in this reaction, we can write two equilibrium constant expressions. Millero, F. J., 1983, The estimation of the pK