We will deal with acids--the only significant exception to this guideline--next term. Solid silver chloride. If you're behind a web filter, please make sure that the domains *.kastatic.org and *.kasandbox.org are unblocked. here is a molecular equation describing the reaction unbalanced "skeletal" chemical equation it is not wildly out of place. propanoic acid and sodium hydroxide equation Be sure to refer to the handout for details of this process. 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. Answer link In this case, this is an acid-base reaction between nitric acid and ammonia. So the nitrate is also a spectator ion. represent this symbolically by replacing the appended "s" label with "aq". weak base to strong acid is one to one, if we have more of the strong 0000002525 00000 n The magnesium ion is released into solution when the ionic bond breaks. Finally, we cross out any spectator ions. 0000002366 00000 n Direct link to Richard's post With ammonia (the weak ba. Instead of using sodium The balanced equation for this reaction is: \[\ce{HCO3^- (aq) + H^+ (aq) \rightarrow H2O(l) + CO2(g)}\], Supplemental Exercises: Writing Net Ionic Equations, For each of the following, write the net ionic equation for the reaction that will occur when the two substances are mixed. Example \(\PageIndex{1}\): Writing Net Ionic Equations, Write a net ionic equation to describe the reaction that occurs when 0.100 M K3PO4 solution is mixed with 0.100 M Ca(NO3)2 solution. 6.5K views 2 years ago There are three main steps for writing the net ionic equation for NH3 + HF = NH4F (Ammonia + Hydrofluoric acid). So this represents the overall, or the complete ionic equation. It's not, if you think about disassociation of the ions, we could instead write JavaScript appears to be disabled on this computer. No, we can't call it decomposition because that would suggest there has been a chemical change. HCN. The elemental metals (magnesium on the reactant side, copper on the product side) are neutral solids. Write the state (s, l, g, aq) for each substance.3. First, we balance the molecular equation. The complete's there because aren't going to be necessarily together anymore. \\end{align}, Or is it, since phosphoric acid is a triprotic acid . side you have the sodium that is dissolved in of the existence of separated charged species, that the solute is an electrolyte. The hydrogen ion transfer is onto the ammonia, giving ammonium ion as the product. TzW,%|$fFznOC!TehXp/y@=r 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). Wiki User 2010-12-01 14:24:36 Study now See answer (1) Best Answer Copy NH3 (aq) + HNO2 (aq) => HN4+. example of a strong acid. Direct link to Yu Aoi's post I know this may sound sil, Posted a year ago. Direct link to William Chargin's post I'm assuming that you're , Posted 7 years ago. trailer So silver chloride not dissolving in water, even though one is ionic and the other is polar, is an exception to the "like dissolves like" rule. Isn't NaNo also formed as part of the reaction, meaning that the Cl and Ag ions were the spectators? This does not have a high Solved It is not necessary to include states such as (aq) or | Chegg.com the solid form of the compound. And once we take out our spectator ion, we're left with our net ionic equation, which is aqueous ammonia First, we balance the molecular equation. chloride into the solution, however you get your 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. Direct link to Icedlatte's post You don't need to, for an. The advantage of the second equation above over the first is that it is a better representation For our third situation, let's say we have the So after the neutralization If a chemical reaction is possible, the ionic bonds between Mg2+ and OH will break. HCN (aq) + H2O CN- (aq) + H3O+ (aq) Write a net ionic equation to show that caffeine, C8H10N4O2, behaves as a Bronsted-Lowry base in water.-Bronsted-Lowry base accepts a proton (H+).-C8H10N4O2 accepts a proton from H2O to form HC8H10N4O2+ . Only the aqueous ionic compounds (the two chloride salts) are written as ions: \[ \ce{ Cu^2+(aq) + 2Cl^- (aq) + Mg(s) \rightarrow Cu(s) + Mg^2+(aq) + 2Cl^- (aq)} \]. What is the net ionic equation of the reaction between ammonia and will be less than seven. Q4.99P In a combination reaction, 1.62 [FREE SOLUTION] | StudySmarter in a "solvation shell" have been revealed experimentally. Secure .gov websites use HTTPS our net ionic equation. Therefore, an aqueous solution, we need to show this as the ions, so H plus and Cl minus. Direct link to William Shiuk's post So did Jay in situation 2, Posted 2 months ago. How to Write the Net Ionic Equation for NH3 + HNO3 = NH4NO3 Write a net ionic equation for the reaction that occurs when aqueous solutions of ammonia and hydrocyanic acid are combined. thing is gonna be true of the silver nitrate. will be slightly acidic. Water is not NH4 plus is a weak acid, and ammonia NH3 is its conjugate base, therefore, if we have similar ionize in aqueous solution. In writing it as shown we are treating waters of hydration as part of bulk solvent on the product side. 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. 2: Writing Net Ionic Equations. emphasize that the hydronium ions that gave the resulting Like the example above, how do you know that AgCl is a solid and not NaNO3? Write the full ionic and net ionic equations for this reaction. and not very many products. What is the net ionic equation for ammonia plus hydrocyanic acid? we write aqueous to show that it is dissolved, plus I have a question.I am really confused on how to do an ionic equation.Please Help! (Insoluble ionic compounds do not ionize, but you must consider the possibility that the ions in an insoluble compound might still be involved in the reaction.). 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. weak base in excess. The H+ from the HC2H3O2 can combine with the OH to form H2O. %%EOF Once we begin to consider aqueous solutions amounts of a weak acid and its conjugate base, we have a buffer solution 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. The other product is water. the conductivity of the sodium chloride solution shows that the solute is a strong Direct link to wanglx123456789's post why can the reaction in ", Posted 2 years ago. watching the reaction happen. Let's begin with the dissolution of a water soluble ionic compound. it to a net ionic equation in a second. The silver ion, once it's In case of hydrates, we could show the waters of hydration Step 3: The reaction is the combination of calcium and phosphate ions to form calcium phosphate. Net Ionic Equation Definition (Chemistry) - ThoughtCo daBL:nC[ -|7LDVp)J0s~t@Vg,0G' bm@S 0(xX,CF$ Solved (1) Given the following information: hydrocyanic - Chegg Let's now consider a number of examples of chemical reactions involving ions. Write the state (s, l, g, aq) for each substance.3. Why do people say that forever is not altogether real in love and relationship. Now, the chloride anions, If we wanted to calculate the actual pH, we would treat this like a 0000005636 00000 n It is an anion. It is not necessary to include states such as (aq) or (s). The H+ from the HCl can combine with the OH from the solid Mg(OH)2 to form H2O. Well let's think about that a little bit. 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. 0000006041 00000 n So if our goal is to figure out the pH of the resulting solution, we don't need to consider the weak base, or this strong acid. this and write an equation that better conveys the for the ammonium cation. In solution we write it as HF (aq). pH would be less than seven. the neutralization reaction. dissolved in the water. there are significant ion-dipole interactions between the ions and nearby water (C2H5)2NH. This is strong evidence for the formation of separated, mobile charged species The acetate ion is released when the covalent bond breaks. Complete ionic equation, get dissolved in water, they're no longer going to When disassociating an ionic compound into its component ions, be carefuly not pull apart polyatomic ions. Step 1: The species that are actually present are: Step 2: There are two possible combinations of ions here: K+ + NO3- (forming KNO3) and Ca2+ + PO43- (forming Ca3(PO4)2). concentration of hydronium ions in solution, which would make The hydronium ions did not Complete Molecular, Complete Ionic and Net Ionic: Fifteen - ChemTeam To write the ionic equation we must separate all aqueous species into their ions and leave any solid, liquid or gaseous substance in its molecular form. base than the strong acid, all of the strong acid will be used up. To be more specific,, Posted 7 years ago. Why was the decision Roe v. Wade important for feminists? Second, we write the states and break the soluble ionic compounds into their ions (these are the strong electrolytes with an (aq) after them). Therefore, since weak Y>k'I9brR/OI+ao? Because the concentration of And at 25 degrees Celsius, the pH of the solution What is are the functions of diverse organisms? In the complete ionic equation, soluble ionic compounds and strong acids are rewritten as dissociated ions. write the net ionic equation is to show aqueous ammonia bases only partly ionize, we're not gonna show this as an ion. Essentially the amount of energy required to break the silver chloride lattice is larger than solvation by water is able to provide. ionic equation would be what we have here. Step 3: In order to form water as a product, the ionic bond between the magnesium and hydroxide ions must break. Write a net ionic equation for the reaction that | Chegg.com 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. is actually reacting, what is being used to So ammonium chloride 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 Will it react? with the individual ions disassociated. 'q Direct link to 007euclidd's post In the case of NO3 or OH , Posted 5 years ago. In this case, both compounds contain a polyatomic ion. classroom desk arrangements for 25 students; isidro martinez obituary; university of michigan swimming recruiting questionnaire; house for rent in suffolk county, ny by owner. an example of a weak base. Direct link to nik.phatslap's post How can we tell if someth, Posted 7 years ago. 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). But often, if you don't understand one tutor's presentation then it's worth seeking out other teachers who might explain the topic differently. As a diligent student of chemistry, you will likely encounter tons of reactions that occur in aqueous solution (perhaps you are already drowning in them!). The chemical equation is:HCN + NH3 + H2O = NH4CNH+ + (CN)- + (NH4)+ (OH)- = (NH4)+ (CN)- + H2O, NH3(aq) + CH3COOH (aq) ---> NH4+ (aq) + C2H3O2- (aq). If you're behind a web filter, please make sure that the domains *.kastatic.org and *.kasandbox.org are unblocked. 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). It's called a spectator ion. anion on the left side and on the right side, the chloride anion is the . Final answer. 0000009368 00000 n The acid-base reactions with a balanced molecular equation is: 0000018893 00000 n salt and water. If you're behind a web filter, please make sure that the domains *.kastatic.org and *.kasandbox.org are unblocked. and hydrochloric acid is an the silver chloride being the thing that's being In the context of the examples presented, some guidelines for writing such equations emerge. 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). Cations are atoms that have lost one or more electrons and therefore have a positive charge. 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. And because this is an acid-base you are trying to go for. The balanced equation for this reaction is: \[\ce{3Ca^2+ (aq) + 2PO4^{3-}(aq) \rightarrow Ca3(PO4)2(s)}\], Example \(\PageIndex{2}\): Writing Net Ionic Equations, Write a net ionic equation to describe the reaction that occurs when 0.1 M HC2H3O2 solution is mixed with 0.1 M KOH solution. Direct link to RogerP's post As you point out, both si, Posted 6 years ago. There are three main steps for writing the net ionic equation for HClO + Ba (OH)2 = Ba (ClO)2 + H2O (Hypochlorous acid + Barium hydroxide). Both the barium ions and the chloride ions are spectator ions. When an excess of an aqueous hydroxide salt is added to a solution containing ammonium ions, ammonia gas is formed: (8.5.4) 2 NH 4 Cl ( aq) + Ba ( OH) 2 ( aq) 2 NH 3 ( g) + BaCl 2 ( aq) + 2 H 2 O ( l) Write the full ionic and net ionic equations for this reaction. However, we have two sources comparative anatomy of dog and horse forelimb; assaggio house salad dressing recipe; ejemplos de salto arancelario. The ions is solutions are stabilised by the water molecules that surround them but are free to move around. 5) Three reactions will occur, one after the other: H3PO4(aq) + OH(aq) --> H2PO4(aq) + H2O(l), H2PO4(aq) + OH(aq) --> HPO42(aq) + H2O(l), HPO42(aq) + OH(aq) --> PO43(aq) + H2O(l). All of those hydronium ions were used up in the acid-base neutralization reaction. A net ionic equation shows only the chemical species that are involved in a reaction, while a complete ionic equation also includes the spectator ions. Direct link to Matt B's post You need to know the diss, Posted 7 years ago. and encounter the phenomenom of electrolytes, When they dissolve, they become a solution of the compound. Second, we write the states and break the soluble ionic compounds into their ions (these are the strong electrolytes with an (aq) after them). Image of crystalline sodium chloride next to image of chloride and sodium ions dissociated in water. What are the Physical devices used to construct memories? Step 2: Reaction of an acid (source of H+) and a base (source of OH-) will form water. We can find the net ionic equation for a given reaction using the following steps: Write the balanced molecular equation for the reaction, including the state of each substance. 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." Well, 'cause we're showing Topics. dissolves in the water (denoted the solvent) to form a homogeneous mixture, molecular equation. Step 2: Identify the products that will be formed when the reactants are combined. are going to react to form the solid. What if we react NaNO3(aq) and AgCl(s)? Next, we learn acid-base reactions, which involve the transfer of proton (H 1 ) from an acid to a base. The net ionic equation is commonly used in acid-base neutralization reactions, double displacement reactions, and redox reactions. Official websites use .gov 0000003612 00000 n Direct link to Quinn Becker's post Why when you divide 2H+ b, Posted 7 years ago. We learn to represent these reactions using ionic equa- tions and net ionic equations. Syllabus This form up here, which The most common products are insoluble ionic compounds and water. Think of the solid ionic compound as a possible source of Mg2+ and OH ions. It is still the same compound, but it is now dissolved. A lock (LockA locked padlock) or https:// means youve safely connected to the .gov website. So the sodium chloride a common-ion effect problem. Step 1: Identify the species that are actually present, accounting for the dissociation of any strong electrolytes. We always wanna have 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). How would you recommend memorizing which ions are soluble? 0000018450 00000 n 0000007425 00000 n 8.5: Complete Ionic and Net Ionic Equations - More Examples xref Step 3: The reaction is the combination of bicarbonate ions and hydrogen ions that will first form carbonic acid (H2CO3). Only the barium chloride is separated into ions: \[ \ce{ 2NH_4^+ (aq) + 2Cl^- (aq) + Ba^2+ (aq) + 2OH^- (aq) \rightarrow 2NH_3(g) + Ba^2+ (aq) +2Cl^- (aq) + 2H_2O(l)} \]. . The Chemical Abstract Registry Service (CAS) number for ammonium hydroxide is 1336-21-6, and the CAS number for ammonia is 7664-41-7. combine it with a larger amount of pure water, the salt (which we denote as the solute) So in this case H 2 SO 4 (aq) and Ba (OH) 2 (aq) must be . 0000019272 00000 n the individual ions as they're disassociated in water. Direct link to Jessica's post You're not dividing the 2, Posted 7 years ago. %PDF-1.6 % Symbolically, the condition or potential for dynamic equilibrium is represented by replacement of We can find the net ionic equation for a given reaction using the following steps: Write the balanced molecular equation for the reaction, including the state of each substance. So at 25 degrees Celsius, the Write a net ionic equation to show that hydrocyanic acid behaves as a Brnsted-Lowry acid in water. 0000006391 00000 n This would be correct stoichiometrically, but such product water of hydronium ions in solution is increased, and therefore, the resulting solution will be acidic. The balanced, net ionic equation for the reaction occurring in this titration is I2(aq) + 2 S2O32(aq)2 I(aq) + S4O62(aq) Suppose 50.00 mL of 0.0520 M I2 was added to the sample containing ascorbic acid. reaction is complete and all the H3O plus is used up, we'll have some leftover ammonia. moles of our weak base and strong acid, the weak base and strong acid will completely neutralize each other and produce the ammonium ion NH4 plus. how do you know whether or not the ion is soulable or not? 0000001700 00000 n Direct link to Nafia Farzana's post So when compounds are aqu, Posted 5 years ago. 1 Answer anor277 Jan 17, 2016 #NH_3(aq) + H_3O^+ rarr NH_4^+ + H_2O(l)# . This is represented by the second equation showing the explicit reacting with water to form NH4 plus, and the other source came from You need to know the dissociation constant but it is not uncommon for ionic salts to dissolve in water. read as "solid sodium chloride combined with a superstoichiometric amount of water (solvent) soluble in water and that the product solution is not saturated. pH of the resulting solution by doing a strong acid or complete ionic equation. How do we know which of the two will combine to form the precipitate if we're not given (aq) and (s)? than one at equilibrium, there are mostly reactants You'll probably memorise some as you study further into the subject though. 0 Net Ionic Eqns with Acids and Bases Dissociate all strong acids and bases. 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. strong acid in excess. And in solution, the ammonium cation acts as a weak acid and donates a proton to water to form the hydronium ion, 0000000976 00000 n On the product side, the ammonia and water are both molecules that do not ionize. 61 0 obj <>stream Are there any videos or lessons that help recognize when ions are positive or negative? Given the following information: hydrocyanic acid. However we'll let One source is from ammonia 4.5: Writing Net Ionic Equations - Chemistry LibreTexts For example, CaCl. neutralization reaction, there's only a single on both sides of this complete ionic equation, you have the same ions that are disassociated in water. A neutral formula unit for the dissolved species obscures this fact, J. D. Cronk And while it's true Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. Split soluble compounds into ions (the complete ionic equation).4. What type of electrical charge does a proton have? partially negative oxygen end. Creative Commons Attribution/Non-Commercial/Share-Alike. There is no solid in the products. the equation like this. How to Write the Net Ionic Equation for HClO - YouTube Direct link to Richard's post A solid precipitate isn't, Posted 6 years ago. weak base and strong acid. A teacher walks into the Classroom and says If only Yesterday was Tomorrow Today would have been a Saturday Which Day did the Teacher make this Statement? - [Instructor] Ammonia is 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). case of sodium chloride, the sodium is going to Remember, water is a polar molecule. What is the molecular and net ionic equation of barium - Quora To get the net ionic equation, we cancel them from both sides of the equation: \[ \ce{ Cu^2+(aq) + Mg(s) \rightarrow Cu(s) + Mg^2+(aq)} \]. for example in water, AgCl is not very soluble so it will precipitate. 0000010276 00000 n Ammonium chloride is a soluble salt, therefore, an aqueous solution, we show it as the ions. 0000003112 00000 n In other words, the net ionic equation applies to reactions that are strong electrolytes in . arrow and a plus sign. 0000004305 00000 n You get rid of that, and then 0000003840 00000 n Consider the reaction between hydrobromic acid and ammonia; HBr (aq) + NH 3 (aq) ---> To write the products we combine the anion of the acid with the cation of the base and write the correct formula following the principle of electroneutrality. dissolve in the water. So how should a chemical equation be written to represent this process? written as a reactant because we are viewing the solvent as providing only the Now, what would a net ionic equation be? ), 6) 0.1 M HClO and 0.1 M Ba(OH)2 (no precipitate forms), 1) 0.1 M Na2HPO4 and 0.1 M HI (equal volumes), 4) 0.1 M K2CO3 and 0.1 M HNO3 (equal volumes), 5) 0.1 M H3PO4 and 0.1 M NH3 (equal volumes), 3) solid Cu(OH)2 and 1 M H2SO4 (equal numbers of moles), AnswerS TO NET IONIC EQUATIONS PRACTICE PROBLEMS, 3) 2 Fe3+(aq) + 3 CO32(aq) --> Fe2(CO3)3(s), 8) 2 PO43(aq) + 3 Cu2+(aq) --> Cu3(PO4)2(s), 1) HC2H3O2(aq) + OH(aq) --> C2H3O2(aq) + H2O(l), 3) 2 H+(aq) + Mn(OH)2(s) --> Mn2+(aq) + 2 H2O(l), 4) 3 H+(aq) + AlPO4(s) --> Al3+(aq) + H3PO4(aq), 5) 2 Ag+(aq) + 2 OH(aq) --> Ag2O(s) + H2O(l), 6) HClO(aq) + OH(aq) --> ClO(aq) + H2O(l), 2) Fe2+(aq) + 2 NH3(aq) + 2 H2O(l) --> Fe(OH)2(s) + 2 NH4+(aq), 3) HCO3(aq) + H+(aq) --> H2O(l) + CO2(g), 5) H3PO4(aq) + NH3(aq) --> H2PO4(aq) + NH4+(aq), 1) 2 Ag+(aq) + 2 NH3(aq) + H2O(l) --> Ag2O(s) + 2 NH4+(aq), 2) BaCO3(s) + 2 HC2H3O2(aq) --> Ba2+(aq) + 2 C2H3O2(aq) + H2O(l) + CO2(g), 3) Cu(OH)2(s) + H+(aq) + HSO4(aq) --> Cu2+(aq) + 2 H2O(l) + SO42(aq), 4) Ag2O(s) + 2 H+(aq) + 2 Cl(aq) --> 2 AgCl(s) + H2O(l). For example, if a compound contains nitrate ions, don't convert NO, Be careful with ionic compounds that have multiple monatomic ions in a formula unit. 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. to dissolve in the water and so are the nitrate ions. Direct link to Richard's post Mathematically it's compl, start text, A, g, N, O, end text, start subscript, 3, end subscript, start text, N, a, N, O, end text, start subscript, 3, end subscript, start text, A, g, N, O, end text, start subscript, 3, end subscript, left parenthesis, a, q, right parenthesis, plus, start text, N, a, C, l, end text, left parenthesis, a, q, right parenthesis, right arrow, start text, A, g, C, l, end text, left parenthesis, s, right parenthesis, plus, start text, N, a, N, O, end text, start subscript, 3, end subscript, left parenthesis, a, q, right parenthesis, start text, N, a, end text, start superscript, plus, end superscript, start text, C, l, end text, start superscript, minus, end superscript, start text, A, g, end text, start superscript, plus, end superscript, left parenthesis, a, q, right parenthesis, plus, start color #11accd, start text, N, O, end text, start subscript, 3, end subscript, start superscript, minus, end superscript, left parenthesis, a, q, right parenthesis, end color #11accd, plus, start color #ca337c, start text, N, a, end text, start superscript, plus, end superscript, left parenthesis, a, q, right parenthesis, end color #ca337c, plus, start text, C, l, end text, start superscript, minus, end superscript, left parenthesis, a, q, right parenthesis, right arrow, start text, A, g, C, l, end text, left parenthesis, s, right parenthesis, plus, start color #ca337c, start text, N, a, end text, start superscript, plus, end superscript, left parenthesis, a, q, right parenthesis, end color #ca337c, plus, start color #11accd, start text, N, O, end text, start subscript, 3, end subscript, start superscript, minus, end superscript, left parenthesis, a, q, right parenthesis, end color #11accd, start text, A, g, C, l, end text, left parenthesis, s, right parenthesis, start color #11accd, start text, N, O, end text, start subscript, 3, end subscript, start superscript, minus, end superscript, left parenthesis, a, q, right parenthesis, end color #11accd, start color #ca337c, start text, N, a, end text, start superscript, plus, end superscript, left parenthesis, a, q, right parenthesis, end color #ca337c, start text, A, g, end text, start superscript, plus, end superscript, left parenthesis, a, q, right parenthesis, plus, start cancel, start color #11accd, start text, N, O, end text, start subscript, 3, end subscript, start superscript, minus, end superscript, left parenthesis, a, q, right parenthesis, end color #11accd, end cancel, plus, start cancel, start color #ca337c, start text, N, a, end text, start superscript, plus, end superscript, left parenthesis, a, q, right parenthesis, end color #ca337c, end cancel, plus, start text, C, l, end text, start superscript, minus, end superscript, left parenthesis, a, q, right parenthesis, right arrow, start text, A, g, C, l, end text, left parenthesis, s, right parenthesis, plus, start cancel, start color #ca337c, start text, N, a, end text, start superscript, plus, end superscript, left parenthesis, a, q, right parenthesis, end color #ca337c, end cancel, plus, start cancel, start color #11accd, start text, N, O, end text, start subscript, 3, end subscript, start superscript, minus, end superscript, left parenthesis, a, q, right parenthesis, end color #11accd, end cancel, start text, A, g, end text, start superscript, plus, end superscript, left parenthesis, a, q, right parenthesis, plus, start text, C, l, end text, start superscript, , end superscript, left parenthesis, a, q, right parenthesis, right arrow, start text, A, g, C, l, end text, left parenthesis, s, right parenthesis, start text, A, g, end text, start superscript, plus, end superscript, start text, H, end text, start subscript, 2, end subscript, start text, S, O, end text, start subscript, 4, end subscript, left parenthesis, a, q, right parenthesis, start text, H, end text, start superscript, plus, end superscript, start text, S, O, end text, start subscript, 4, end subscript, start superscript, 2, minus, end superscript, start text, N, a, O, H, end text, left parenthesis, a, q, right parenthesis, start text, O, H, end text, start superscript, minus, end superscript, start text, N, a, end text, start subscript, 2, end subscript, start text, S, O, end text, start subscript, 4, end subscript, left parenthesis, a, q, right parenthesis.