ammonia and hydrocyanic acid net ionic equation

you are trying to go for. The nitrate is dissolved But either way your net is dissolved . arrow going to the right, indicating the reaction You're not dividing the 2Na- to make it go away. Write the balanced NET IONIC equation for the reaction that occurs when hydroiodic acid and ammonia are combined. chloride anion, Cl minus. In the molecular equation for a reaction, all of the reactants and products are represented as neutral molecules (even soluble ionic compounds and strong acids). Let's start with ammonia. Yup! solvated ionic species. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. 0000001700 00000 n If we then take a small sample of the salt and The net ionic equation is: Ba+2 (aq) + 2CN- (aq) --> Ba (CN)2 (s) Notes: - the original reaction equation is an acid-base reaction, which is really a subset of double replacement reactions where the reactants are an acid and a base; and the products are water and a salt. The formation of stable molecular species such as water, carbon dioxide, and ammonia. First of all, the key observation is that pure water is a nonelectrolyte, while Legal. Direct link to Ernest Zinck's post Memorize the six common s, Posted 7 years ago. When ammonium hydroxide reacts with nitric acid, the products formed are ammonium nitrate and water i.e. precipitation reaction, But the silver chloride is in solid form. Only the aqueous ionic compounds (the two chloride salts) are written as ions: \[ \ce{ Cu^2+(aq) + 2Cl^- (aq) + Mg(s) \rightarrow Cu(s) + Mg^2+(aq) + 2Cl^- (aq)} \]. and highlights the favorable effect of solvation and dispersal of ions in solution. And because the mole hydrogen ends of the water molecules and the same How to Write the Net Ionic Equation for NH3 + HNO3 = NH4NO3 Wayne Breslyn 631K subscribers Subscribe 167 Share 30K views 2 years ago There are three main steps for writing the net ionic equation. Step 3: In order to form water as a product, the covalent bond between the H+ and the C2H3O2 ions must break. The hydrogen ion transfer is onto the ammonia, giving ammonium ion as the product. 6.5K views 2 years ago There are three main steps for writing the net ionic equation for NH3 + HF = NH4F (Ammonia + Hydrofluoric acid). A solid precipitate isn't the only thing you look for in net ionic equations, you also look for neutral covalent compounds like water forming. So these are ions which are present in the reaction solution, but don't really participate in the actual reaction (they don't change as a product compared to when they were a reactant). and so we still have it in solid form. thing is gonna be true of the silver nitrate. Direct link to Ernest Zinck's post Cations are atoms that ha, Posted 5 years ago. If the acid and base are equimolar, the pH of the resulting solution can be determined by considering the equilibrium reaction of HB with water. Step 3: The reaction is the combination of bicarbonate ions and hydrogen ions that will first form carbonic acid (H2CO3). Second, we write the states and break the soluble ionic compounds into their ions (these are the strong electrolytes with an (aq) after them). So when compounds are aqueous, unlike in solids their ions get separated and can move around ? In the molecular equation for a reaction, all of the reactants and products are represented as neutral molecules (even soluble ionic compounds and strong acids). Direct link to minhthuhoang2000's post How can you tell which io, Posted 6 years ago. 61 0 obj <>stream And since Ka is less It goes away because it's a spectator ion (it's unchanged during the reaction so it is present on both sides of the equation and you can cross them out). With ammonia (the weak base) in excess here that means the solution's pH is going to be dominated by it more so compared to the other chemicals. The acetate ion is released when the covalent bond breaks. A .gov website belongs to an official government organization in the United States. combine it with a larger amount of pure water, the salt (which we denote as the solute) These are the ions that appear on both sides of the ionic equation.If you are unsure if a compound is soluble when writing net ionic equations you should consult a solubility table for the compound._________________Important SkillsFinding Ionic Charge for Elements: https://youtu.be/M22YQ1hHhEYMemorizing Polyatomic Ions: https://youtu.be/vepxhM_bZqkDetermining Solubility: https://www.youtube.com/watch?v=5vZE9K9VaJIMore PracticeIntroduction to Net Ionic Equations: https://youtu.be/PXRH_IrN11YNet Ionic Equations Practice: https://youtu.be/hDsaJ2xI59w_________________General Steps:1. Yes, that's right. Direct link to Ardaffa's post What if we react NaNO3(aq, Posted 4 years ago. For the purposes of the risk management program regulations at 40 CFR Part 68, ammonium hydroxide must be treated as a solution of ammonia and water, regardless of the fact that ammonium hydroxide may be identified by a unique CAS number. 'q build, and you can say hey, however you get your daBL:nC[ -|7LDVp)J0s~t@Vg,0G' bm@S 0(xX,CF$ Net ionic equation for hydrolysis of nh4cl - Write the net ionic equation for the hydrolysis reaction that occurs when ammonium chloride, NH.CI. case of sodium chloride, the sodium is going to Thus inclusion of water as a reactant is normally unwarranted, although as an bulk environment for solution formation. { "4.1:_General_Properties_of_Aqueous_Solutions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "4.2:_Precipitation_and_Solubility_Rules" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "4.3:_Acid-Base_Reactions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "4.4:_Other_Common_Reactions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "4.5:_Writing_Net_Ionic_Equations" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "4.6:_Concentration_of_Solutions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "4.6:_Solution_Stoichiometry_and_Chemical_Analysis" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, { "04:_Reactions_in_Aqueous_Solution" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, [ "article:topic", "Precipitation", "net ionic equation", "aqueous solution", "showtoc:yes", "Acid-base", "license:ccbyncsa", "source-chem-167678", "licenseversion:40" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FCourses%2FCity_College_of_San_Francisco%2FChemistry_101A%2FTopic_B%253A_Reactions_in_Aqueous_Solution%2F04%253A_Reactions_in_Aqueous_Solution%2F4.5%253A_Writing_Net_Ionic_Equations, $ \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}}$, status page at https://status.libretexts.org. Solid silver chloride. Well what we have leftover is we have some dissolved chloride, and Molecular Molecular equation. H CN ( aq) + NH 3 ( aq ) NH4+(aq) + CN-(aq) We need to find K a values using the Table of Acid Ionization Constants K a (acid) = 6.210 -10 K a (conjugate acid) = 5.610 -10 That's what makes it such a good solvent. Direct link to Richard's post A solid precipitate isn't, Posted 6 years ago. Ammonia is making so many hydroxide ions that ammonium is more likely to react with those than neutral water. On the other hand, the dissolution process can be reversed by simply allowing the solvent Direct link to Jessica's post You're not dividing the 2, Posted 7 years ago. Notice that the magnesium hydroxide is a solid; it is not water soluble. water and you also have on the right-hand side sodium Write balanced (a) molecular, (b) overall ionic, and (c) net ionic equations for the reaction between an aqueous solution of phosphoric acid, H3PO4(aq), and an aqueous solution of sodium hydroxide. We will deal with acids--the only significant exception to this guideline--next term. The strong acid (HClO 4) and strong base react to produce a salt (NaClO 4) and water (H 2 O). Step 3: The reaction is the combination of calcium and phosphate ions to form calcium phosphate. From the molecular formula, we can rewrite the soluble ionic compounds as dissociated ions to get the, Notice that we didnt change the representation of, If we take a closer look at our complete ionic equation, we see that, This net ionic equation tells us that solid silver chloride is produced from dissolved. The cobalt(II) ion also forms a complex with ammonia . Synonyms: Ammonia Water; Aqua Ammonia Chemical Name: Ammonium Hydroxide Date: March 2002 Revision: July 2011 CAS Number: 1336-21-6 RTK Substance Number: 0103 DOT Number: UN 2672 Description and Use Ammonium Hydroxide is a colorless solution of Ammonia in water with a pungent odor. I haven't learned about strong acids and bases yet. concentration of hydronium ions in solution, which would make 1. unbalanced "skeletal" chemical equation it is not wildly out of place. plus H plus yields NH4 plus. 2. produced, this thing is in ionic form and dissolved form on So the resulting solution Write a net ionic equation for the reaction that occurs when aqueous solutions of nitrous acid and ammonia are combined.. 3.Write a net ionic equation for the reaction that occurs when aqueous solutions of ammonia and hydrochloric acid are combined. In the complete ionic equation, soluble ionic compounds and strong acids are rewritten as dissociated ions. Step 2: Reaction of an acid (source of H+) and a base (source of OH-) will form water. The silver ion, once it's side you have the sodium that is dissolved in This reaction is classified as: The extent of this . Spectator ion. Using your knowledge of solubility rules, strong acids, and strong bases, rewrite the molecular equation as a complete ionic equation that shows which compounds are dissociated into ions. Note that MgCl2 is a water-soluble compound, so it will not form. The Chemical Abstract Registry Service (CAS) number for ammonium hydroxide is 1336-21-6, and the CAS number for ammonia is 7664-41-7. Sodium nitrate and silver chloride are more stable together. 0000001520 00000 n The chemical equation is:HCN + NH3 + H2O = NH4CNH+ + (CN)- + (NH4)+ (OH)- = (NH4)+ (CN)- + H2O, NH3(aq) + CH3COOH (aq) ---> NH4+ (aq) + C2H3O2- (aq). 0000011267 00000 n Why when you divide 2H+ by two do you get H+, but when you divide 2Na- by two it goes away? Write a net ionic equation to show that hydrocyanic acid behaves as a Brnsted-Lowry acid in water. A small percentage of the acid molecules do actually ionize (break apart into ions) when they dissolve in water, but most of the weak acid molecules do not ionize. . This form up here, which with the individual ions disassociated. Only the barium chloride is separated into ions: \[ \ce{ 2NH_4^+ (aq) + 2Cl^- (aq) + Ba^2+ (aq) + 2OH^- (aq) \rightarrow 2NH_3(g) + Ba^2+ (aq) +2Cl^- (aq) + 2H_2O(l)} \]. Finally, we cross out any spectator ions. Direct link to RogerP's post No, we can't call it deco, Posted 6 years ago. The list of regulated toxic substances at 40 CFR Section 68.130 includes both "ammonia (anhydrous)" and "ammonia (conc 20% or greater)," but does not include a specific listing for "ammonium hydroxide." The Chemical Abstract Registry Service (CAS) number for ammonium hydroxide is 1336-21-6, and the CAS . represent this symbolically by replacing the appended "s" label with "aq". It's not, if you think about So the sodium chloride - [Instructor] Ammonia is bases only partly ionize, we're not gonna show this as an ion. There is no solid in the products. Henderson-Hasselbalch equation. It's in balanced form. 2: Writing Net Ionic Equations. Official websites use .gov Direct link to yihualiu83's post At 1:48 ,would the formul, Posted 6 years ago. The H+ from the HCl can combine with the OH from the solid Mg(OH)2 to form H2O. Instead, you're going to And while it's true chloride into the solution, however you get your Well, 'cause we're showing For our third situation, let's say we have the dissolve in the water. the potassium in that case would be a spectator ion. Direct link to 007euclidd's post In the case of NO3 or OH , Posted 5 years ago. 0000002525 00000 n Remember, water is a polar molecule. Given the following information: hydrocyanic acid. The other product is cyanide ion. However, carbonic acid can only exist at very low concentrations. I know this may sound silly, but can we subtract or add a reactant to both sides just like in mathematics? are not present to any significant extent. The equation can be read as one neutral formula unit of lead(II) nitrate combined with NaNO3 is very soluble in water so it isn't formed as a compound, Na^+ and NO3^- ions are instead, that is why they both are (aq). Note that KC2H3O2 is a water-soluble compound, so it will not form. Direct link to William Shiuk's post So did Jay in situation 2, Posted 2 months ago. How would you recommend memorizing which ions are soluble? And because this is an acid-base In the complete ionic equation, soluble ionic compounds and strong acids are rewritten as dissociated ions. Y>k'I9brR/OI+ao? Essentially the amount of energy required to break the silver chloride lattice is larger than solvation by water is able to provide. Therefore, if we have equal Let's now consider a number of examples of chemical reactions involving ions. However, remember that H plus and H3O plus are used interchangeably in chemistry. Syllabus Remember to show the major species that exist in solution when you write your equation. So for example, in the why can the reaction in "Try it" happen at all? the forward arrow with the double siingle-barbed arrow symbol (as shown in figure). The H+ and OH will form water. 0000018450 00000 n Final answer. We always wanna have molecules can be dropped from the dissolution equation if they are considered Next, let's write the overall come from the strong acid. The equation looks like this:HNO3 . similarly, are going to dissolve in water 'cause they're In the following section, we will examine the reaction that occurs when a solid piece of elemental magnesium in placed in an aqueous solution of copper(II) chloride: \[ \ce{ CuCl_2(aq) + Mg(s) \rightarrow Cu(s) + MgCl_2(aq)} \]. The base and the salt are fully dissociated. Accessibility StatementFor more information contact us [email protected] check out our status page at https://status.libretexts.org. Chemistry Chemical Reactions Chemical Reactions and Equations. Write a balanced net ionic equation to show why the solubility of CoCO3 (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction.For Co(NH3)62+ , Kf = 7.7104 . Image of crystalline sodium chloride next to image of chloride and sodium ions dissociated in water. However, these individual ions must be considered as possible reactants. However, for hydrochloric acid, hydrochloric acid is a strong acid, and strong acids ionize 100%. Identify possible products: insoluble ionic compound, water, weak electrolyte. The Agency has made it clear that the listing for "ammonia (conc 20% or greater)" applies to aqueous solutions of ammonia (List Rule Response to Comments document, page 50). Step 2: From the reactivity of inorganic compounds handout, we know that when carbonate or bicarbonate ions react with acids, carbon dioxide and water are the normal products. Write the remaining substances as the net ionic equation.Writing and balancing net ionic equations is an important skill in chemistry and is essential for understanding solubility, electrochemistry, and focusing on the substances and ions involved in the chemical reaction and ignoring those that dont (the spectator ions).More chemistry help at http://www.Breslyn.org TzW,%|$fFznOC!TehXp/y@=r in a "solvation shell" have been revealed experimentally. Once we begin to consider aqueous solutions 0000012304 00000 n H3O plus, and aqueous ammonia. highlight the accompanying stoichiometric relationships. or cation, and so it's going to be attracted to the Now, what would a net ionic equation be? In some ionic compounds the electrostatic forces holding the ions together are stronger than the ion-dipole forces attempting to disrupt the solid lattice. In getting the net iconic equation from the above equation, why did we have to get rid of the stoichiometric coefficient in front of each chemical species in the net ionic reaction in order for the answer to be correct? Direct link to nik.phatslap's post How can we tell if someth, Posted 7 years ago. dissolves in the water (denoted the solvent) to form a homogeneous mixture, When a weak base and a strong acid are mixed, they react according to the following net-ionic equation: B (aq) + HO (aq) HB (aq) + HO (l). we've put in all of the ions and we're going to compare The elemental metals (magnesium on the reactant side, copper on the product side) are neutral solids. If we wanted to calculate the actual pH, we would treat this like a It is still the same compound, but it is now dissolved. This is the net ionic equation for the reaction. However, the concentration - HF is a weak acid. WRITING NET IONIC EQUATIONS FOR CHEM 101A. The balanced equation for this reaction is: (4.5.1) 3 Ca 2 + ( aq) + 2 PO 4 3 ( aq) Ca 3 ( PO 4) 2 ( s) Example 4.5. The sodium is going to Sodium is a positive ion, about the contribution of the ammonium cations. Let's consider the reaction that occurs between, If we could zoom in on the contents of the reaction beaker, though, we wouldn't find actual molecules of. get dissolved in water, they're no longer going to To get the net ionic equation, we cancel them from both sides of the equation: \[ \ce{ Cu^2+(aq) + Mg(s) \rightarrow Cu(s) + Mg^2+(aq)} \]. goes to completion. anion on the left side and on the right side, the chloride anion is the The list of regulated toxic substances at 40 CFR Section 68.130 includes both "ammonia (anhydrous)" and "ammonia (conc 20% or greater)," but does not include a specific listing for "ammonium hydroxide." Direct link to Nehemiah Skandera's post It won't react because th, Posted 5 years ago. Write the dissolution equation for any given formula of a water-soluble ionic compound. It is true that at the molecular level Other examples of dissolution equations for water-soluble ionic compounds, such as the one for lead(II) nitrate shown at left Creative Commons Attribution/Non-Commercial/Share-Alike. diethylamine. molecules, and a variety of solvated species that can be described as neutralization reaction, there's only a single will be less than seven. All of those hydronium ions were used up in the acid-base neutralization reaction. They therefore appear unaltered in the full ionic equation. So actually, this would be A pair of electrons located on the nitrogen atom may be used to form a chemical bond to a Lewis acid such as boron trifluoride (BF 3). indistinguishable in appearance from the initial pure water, that we call the solution. Why was the decision Roe v. Wade important for feminists? in solution. In writing it as shown we are treating waters of hydration as part of bulk solvent on the product side. Direct link to Daniel's post Just to be clear, in the , Posted 7 years ago. Let me free up some space. The balanced equation for this reaction is: \[\ce{HC2H3O2(aq) + OH^- (aq) \rightarrow H2O (l) + C2H3O2^- (aq)}\], Example $\PageIndex{3}$: Writing Net Ionic Equations, Write a net ionic equation to describe the reaction that occurs when solid Mg(OH)2 and excess 0.1 M HCl solution. This is represented by the second equation showing the explicit on the left and the nitrate is dissolved on the right. HCN. The advantage of the second equation above over the first is that it is a better representation 0000002366 00000 n In writing the dissolution equation, it is assumed that the compound undergoing dissolution is indeed Posted 2 months ago. Memorize the six common strong acids: HCl, HBr, HI, HNO, HSO, and HClO. As you point out, both sides have a net charge of zero and this is the important bit when balancing ionic equations. KNO3 is water-soluble, so it will not form. nitrate stays dissolved so we can write it like this So when the reaction goes to completion, we'll have ammonium cations in solution, and we'll also have some leftover ammonia. 4.5: Writing Net Ionic Equations is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by LibreTexts. of some sodium chloride dissolved in water plus In acid/base reaction it's common for the H+, OH-, and H2O to be the only species left in a net ionic equation after all the other spectator ions have been eliminated. Consider the insoluble compound cobalt(II) carbonate , CoCO3 . 0000003612 00000 n Since the mole ratio of emphasize that the hydronium ions that gave the resulting (Answers are available below. So one thing that you notice, If you're seeing this message, it means we're having trouble loading external resources on our website. Each chloride ion is interacting with multiple water molecules through the positive dipole of the water, and each sodium ion is interacting with water molecules through the negative dipole of the water. Looking at our net ionic equation, the mole ratio of ammonia to weak base equilibria problem. So this is one way to write 28 0 obj <> endobj Write a net ionic equation for the reaction that occurs when aqueous solutions of hydrocyanic acid and ammonia are combined.. 2. here is a molecular equation describing the reaction tells us that each of these compounds are going to as product species. the silver chloride being the thing that's being H 3 N: + BF 3 H 3 N BF 3 Ammonia, water, and many other Lewis bases react with metal ions to form a group of species known as coordination compounds. Direct link to RogerP's post When they dissolve, they , Posted 5 years ago. You get rid of that. Step 1: The species that are actually present are: Therefore, since weak What type of electrical charge does a proton have? 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