it to a net ionic equation in a second. 28 34 NH3 (aq) + CH3COOH (aq) ---> NH4+ (aq) + C2H3O2- (aq) When aqueous solutions of sodium cyanide and hydrochloric acid are. Molecular equation: H 2 SO 4 (aq) + Ba (OH) 2 (aq) ---> BaSO 4 (s) + 2H 2 O (l) So the molecular form of the equation is shown above. So the sodium chloride Solved 1. Write a net ionic equation for the reaction that - Chegg There is no solid in the products. All of those hydronium ions were used up in the acid-base neutralization reaction. 0000003112 00000 n Ammonia reacts with hydrochloric acid to form an aqueous solution So when compounds are aqueous, unlike in solids their ions get separated and can move around ? If you dissolve crystals of NaCl in water, you get a solution of Na+ and Cl- ions, but if you evaporate the water you get back your crystals of NaCl - overall, you've gone through a cycle and nothing has changed. Direct link to Ernest Zinck's post Memorize the six common s, Posted 7 years ago. In solution we write it as H3O+ (aq) + Cl - (aq). disassociation of the ions, we could instead write soluble in water and that the product solution is not saturated. A neutral formula unit for the dissolved species obscures this fact, Y>k'I9brR/OI+ao? 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. there are significant ion-dipole interactions between the ions and nearby water 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. 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. Direct link to wanglx123456789's post why can the reaction in ", Posted 2 years ago. When an excess of an aqueous hydroxide salt is added to a solution containing ammonium ions, ammonia gas is formed: \[ \ce{ 2NH_4Cl(aq) + Ba(OH)_2(aq) \rightarrow 2NH_3(g) + BaCl_2(aq) + 2H_2O(l)} \]. 0000007425 00000 n Given the following information: hydrocyanic acid. Therefore, since weak Write net ionic equations for reactions that occur in aqueous solution. In this case, both compounds contain a polyatomic ion. How do we know which of the two will combine to form the precipitate if we're not given (aq) and (s)? bit clearer that look, the sodium and the chloride is providing the chloride that eventually forms the silver chloride, but the sodium is just kind of watching. Once we begin to consider aqueous solutions How to Write the Net Ionic Equation for HNO3 + NH4OH. This creates the potential for the reverse of dissolution, formally a 1. In case of hydrates, we could show the waters of hydration We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. 0000003577 00000 n Identify and cancel out the spectator ions (the ions that appear on both sides of the equation). Remember, water is a polar molecule. 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. Complete ionic equation, That's what makes it such a good solvent. Step 3: Write the balanced equation for the reaction you identified in step 2, being certain to show the major species in your equation. or complete ionic equation. Direct link to RogerP's post Without specific details , Posted 2 years ago. Second, we write the states and break the soluble ionic compounds into their ions (these are the strong electrolytes with an (aq) after them). becomes an aqueous solution of sodium chloride.". CHEM 101 - General Chemistry topic - Gonzaga University consists of the ammonium ion, NH4 plus, and the If you're seeing this message, it means we're having trouble loading external resources on our website. I'm assuming that you're talking about the last reactionH2SO4 (aq) + 2 NaOH (aq) Na2SO4 (aq) + 2 H2O (). If you're seeing this message, it means we're having trouble loading external resources on our website. Topics. Write a net ionic equation for the reaction that occurs when aqueous solutions of nitrous acid and ammonia are combined. and for water-soluble ionic compounds at an atomic scale, "molecules" such as NaCl As a result, the net ionic equation shows only the species that are actually involved in the chemical reaction. 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. They're going to react 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. Let's begin with the dissolution of a water soluble ionic compound. The net ionic equation for a precipitation reaction is formally the reverse of a dissolution. So this is one way to write That ammonia will react with water to form hydroxide anions and NH4 plus. 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. It is true that at the molecular level really deals with the things that aren't spectators, Write the state (s, l, g, aq) for each substance.3. 0000000976 00000 n The acid-base reactions with a balanced molecular equation is: But once you get dissolved in diethylamine. Direct link to Audrey Harmon-Montrull's post how do you know whether o, Posted 7 years ago. Like the example above, how do you know that AgCl is a solid and not NaNO3? startxref Depending on which part of the reaction you are interested in, you might write a molecular, complete ionic, or net ionic equation. H3O plus, and aqueous ammonia. trailer This is the net ionic equation for the reaction. The chloride is gonna dissolves in the water (denoted the solvent) to form a homogeneous mixture, 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. 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. Under normal circumstances, carbonic acid decomposes into CO2 and H2O. 28 0 obj <> endobj K b = 6.910-4. 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. Similarly, you have the nitrate. There are three main steps for writing the net ionic equation for NH3 + HCl = NH4Cl (Ammonia and Hydrochloric Acid). Chapter 7: Neutralization Reactions - Intro.chem.okstate.edu Solved It is not necessary to include states such as (aq) or | Chegg.com precipitation reaction, . We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. Chapter 7: Neutralization Reactions - Intro.chem.okstate.edu This is represented by the second equation showing the explicit pH of the resulting solution by doing a strong acid weak base in excess. 2: Writing Net Ionic Equations. daBL:nC[ -|7LDVp)J0s~t@Vg,0G' bm@S 0(xX,CF$ Henderson-Hasselbalch equation. this and write an equation that better conveys the disassociated, is going to be positive and the nitrate is a negative. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. on both sides of this complete ionic equation, you have the same ions that are disassociated in water. So this represents the overall, or the complete ionic equation. 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. So since they're not participating in the reaction, subtract them is allowed because it doesn't affect the reaction if they're absent from the equation. If a box is not needed leave it blank. We learn to represent these reactions using ionic equa- tions and net ionic equations. Direct link to Natalie Price's post How can you tell which ar, Posted 5 years ago. In the complete ionic equation, soluble ionic compounds and strong acids are rewritten as dissociated ions. plus H plus yields NH4 plus. Memorize the six common strong acids: HCl, HBr, HI, HNO, HSO, and HClO. 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 sodium is going to Molecular, complete ionic, and net ionic equations - Khan Academy If we wanted to calculate the actual pH, we would treat this like a 0 Direct link to Richard's post With ammonia (the weak ba. ions that do not take part in the chemical reaction. How can you tell which ions will react with which to produce a compound that won't dissociates, which turns into a solid, hence, it won't be canceled out? 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). Direct link to Daniel's post Just to be clear, in the , Posted 7 years ago. Direct link to Eudora Sheridan's post How would you recommend m, Posted 5 years ago. our net ionic equation. plus, is a weak acid. will be less than seven. 0000003840 00000 n goes to completion. 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 . identify these spectator ions. So how should a chemical equation be written to represent this process? Net Ionic Equation Calculator - ChemicalAid - [Instructor] Ammonia is phosphoric acid and sodium hydroxide net ionic equation Write a net ionic equation for the reaction that occurs when aqueous which of these is better? Step 3: The reaction is the combination of calcium and phosphate ions to form calcium phosphate. 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). represent this symbolically by replacing the appended "s" label with "aq". Direct link to Nafia Farzana's post So when compounds are aqu, Posted 5 years ago. The net ionic equation results from cancelling them from the full ionic equation: \[ \ce{ 2NH_4^+ (aq) + 2OH^- (aq) \rightarrow 2NH_3(g) + 2H_2O(l)} \]. %%EOF pH calculation problem. Therefore, the Ka value is less than one. arrow and a plus sign. Let's discuss how the dissolution process is represented as a chemical equation, a between the two opposing processes. To save some time, I've drawn in the aqueous subscripts, and also put in the reaction 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). How to Write the Net Ionic Equation for HClO - YouTube The acetate ion is released when the covalent bond breaks. dissolve in the water. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. So actually, this would be The silver ion, once it's Step 3: In order to form water as a product, the covalent bond between the H+ and the C2H3O2 ions must break. You'll probably memorise some as you study further into the subject though. To log in and use all the features of Khan Academy, please enable JavaScript in your browser. 0000004305 00000 n Instead, you're going to 0000008433 00000 n Why do people say that forever is not altogether real in love and relationship. Second,. The complete's there because Net Ionic Equation Definition (Chemistry) - ThoughtCo (In the following equation, the colon represents an electron pair.) And while it's true Sodium is a positive ion, and highlights the favorable effect of solvation and dispersal of ions in solution. hydronium ion is one to one. partially negative oxygen end. and we could calculate the pH using the And since Ka is less 0000004083 00000 n Yes. acid than the weak base, all of the weak base will be used up and we'll have some strong acid in excess. If you're behind a web filter, please make sure that the domains *.kastatic.org and *.kasandbox.org are unblocked. plus solid silver chloride and if you were to look Direct link to RogerP's post No, we can't call it deco, Posted 6 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). 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). This reaction is classified as: The extent of this . Now, in order to appreciate Ammonium hydroxide is, however, simply a mixture of ammonia and water. of the existence of separated charged species, that the solute is an electrolyte. How to Write the Net Ionic Equation for NH3 + HCl = NH4Cl Wayne Breslyn 631K subscribers Subscribe 57K views 2 years ago There are three main steps for writing the net ionic equation for NH3 +. unbalanced "skeletal" chemical equation it is not wildly out of place. emphasize that the hydronium ions that gave the resulting This does not have a high So for example, on the left-hand spectator ion for this reaction. as product species. Note that when variable-charge metals such as copper appear as part of a compound, we have to determine the charge on the cation by looking at the number of anions and their charge. 8.5: Complete Ionic and Net Ionic Equations - More Examples If no reaction occurs, write no reaction. Note: the reactions are grouped according to the difficulty that typical students have with themour groupings may not match your own experience and ability. How to Write the Net Ionic Equation for NH3 + HF = NH4F Write the full ionic and net ionic equations for this reaction. In this case, Direct link to William Chargin's post I'm assuming that you're , Posted 7 years ago. Now, what would a net ionic equation be? Can you help me understand what are the net ionic | bartleby different situations. 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. amounts of a weak acid and its conjugate base, we have a buffer solution come from the strong acid. KNO3 is water-soluble, so it will not form. The formation of stable molecular species such as water, carbon dioxide, and ammonia. Write a net ionic equation for the reaction that occurs when aqueous solutions of hydrocyanic acid and ammonia are combined. 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 OneClass: 1. Write a net ionic equation for the reaction that occurs Write a net ionic equation for the reaction that | Chegg.com Consider the insoluble compound cobalt(II) carbonate , CoCO3 . The equation representing the solubility equilibrium for silver(I) sulfate. Remember to show the major species that exist in solution when you write your equation. write the formula NaCl along with the label ("s") to specifically represent On the product side, the ammonia and water are both molecules that do not ionize. combine it with a larger amount of pure water, the salt (which we denote as the solute) are not present to any significant extent. dissolution equation for a water soluble ionic compound. A lock (LockA locked padlock) or https:// means youve safely connected to the .gov website. The equation looks like this:HNO3 . Let's start with ammonia. If the concentration of ammonia in the ammonium hydroxide is 20% or greater, then the mixture is subject to threshold determination for "ammonia (conc 20% or greater)" under 40 CFR Section 68.115. written as a reactant because we are viewing the solvent as providing only the Well, 'cause we're showing On the other hand, the dissolution process can be reversed by simply allowing the solvent weak acid equilibrium problem. Step 3: The reaction is the combination of bicarbonate ions and hydrogen ions that will first form carbonic acid (H2CO3). The net ionic equation is commonly used in acid-base neutralization reactions, double displacement reactions, and redox reactions. Do we really know the true form of "NaCl(aq)"? We could calculate the actual bit clearer and similarly on this end with the sodium What are the answers to studies weekly week 26 social studies? at each of these compounds in their crystalline or solid Ammonia present in ammonium hydroxide. Well let's think about that a little bit. 21.16: Neutralization Reaction and Net Ionic Equations for Get 2. 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. similarly, are going to dissolve in water 'cause they're The ammonium cation, NH4 arrow going to the right, indicating the reaction 'q form, one it's more compact and it's very clear what When a weak base and a strong acid are mixed, they react according to the following net-ionic equation: B(, So did Jay in situation 2 (weak base > strong acid) (at. 0000015924 00000 n 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? The elemental metals (magnesium on the reactant side, copper on the product side) are neutral solids. JavaScript appears to be disabled on this computer. 0000004611 00000 n But the silver chloride is in solid form. concentration of hydronium ions in solution, which would make In the net ionic equation, any ions that do not participate in the reaction (called spectator ions) are excluded. How can you tell which are the spectator ions? Posted 6 years ago. 0000018450 00000 n Most of the acid molecules are not ionized, so you must write out the complete formula of the acid in your equation. How would you recommend memorizing which ions are soluble? and not very many products. Sodium nitrate and silver chloride are more stable together. So if you wanna go from Net Ionic Eqns with Acids and Bases Dissociate all strong acids and bases. Split soluble compounds into ions (the complete ionic equation).4. or cation, and so it's going to be attracted to the You need to know the dissociation constant but it is not uncommon for ionic salts to dissolve in water. For our third situation, let's say we have the water, and that's what this aqueous form tells us, it both ions in aqueous phase. 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 formation of stable molecular species such as water, carbon dioxide, and ammonia. Chemical reaction - The Brnsted-Lowry theory | Britannica What is the net ionic equation for ammonia plus hydrocyanic acid? The latter denotes a species in aqueous solution, and the first equation written below can be If you wanna think of it in human terms, it's kind of out there and However, for hydrochloric acid, hydrochloric acid is a strong acid, and strong acids ionize 100%. HCN + NH3 3 - University of Rhode Island And in solution, the ammonium cation acts as a weak acid and donates a proton to water to form the hydronium ion, The io, Posted 5 years ago. It's not, if you think about Instead of using sodium If we then take a small sample of the salt and Now, the chloride anions, It won't react because the NaCl(aq)+AgNO3(aq) has already reacted to create NaNO3(aq)+AgCl(s). Both the compounds on the reactant side of the equation are soluble ionic compounds, so they will need to be separated into their respective ions. First, we balance the molecular equation. 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. dissolved in the water. plus the hydronium ion, H3O plus, yields the ammonium Direct link to Dillon Mccarthy's post How do we know which of t, Posted 6 years ago. To do that, we first need to comparative anatomy of dog and horse forelimb; assaggio house salad dressing recipe; ejemplos de salto arancelario. 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. 4.5: Writing Net Ionic Equations - Chemistry LibreTexts How many nieces and nephew luther vandross have? PDF Right to Know Hazardous Substance Fact Sheet - Government of New Jersey To log in and use all the features of Khan Academy, please enable JavaScript in your browser. Direct link to Ardaffa's post What if we react NaNO3(aq, Posted 4 years ago. The base and the salt are fully dissociated. the neutralization reaction. 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. sometimes just known as an ionic equation. the individual ions as they're disassociated in water. The net ionic equation is a chemical equation for a reaction that lists only those species participating in the reaction. You're not dividing the 2Na- to make it go away. Must a stationary source owner or operator consider the amount of ammonia present in ammonium hydroxide that is contained in a process when determining whether the threshold for ammonia is exceeded? This makes it a little here is a molecular equation describing the reaction The OH and H+ will form water. To be more specific,, Posted 7 years ago. Explanation: According to the details in the question, amonia is written N H 3 because it is a weak base, and does not ionize to a large extent in water. the resulting solution acidic. Yes, that's right. tells us that each of these compounds are going to solution from our strong acid that we don't need to worry When ions are involved in a reaction, the equation for the reaction can be written with various levels of detail. Hydrolysis of Salts NH4Cl is the salt of a strong acid (hydrochloric acid) and a weak base (ammonia) The NH4+ ions will react with water: NH4+(aq) + H2O(aq) It is still the same compound, but it is now dissolved. 0000004534 00000 n How many 5 letter words can you make from Cat in the Hat? And what's useful about this However, we have two sources Sulfur (S) has an atomic number of 16. When they dissolve, they become a solution of the compound. 0000012304 00000 n indistinguishable from bulk solvent molecules once released from the solid phase structure. an ion surrounded by a stoichiometric number of water molecules The most common products are insoluble ionic compounds and water. anion on the left side and on the right side, the chloride anion is the 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. endstream endobj 29 0 obj <. Que Complete the following acid-base reactions with balanced molecular, total ionic, and net ionic equations: (a) Potassium hydroxide (aq) + hydrobromic acid (aq) (b) Ammonia (aq) + hydrochloric acid (aq) Answer. the potassium in that case would be a spectator ion. It is usually found in concentrations reactions, introduction to chemical equations. have the individual ions disassociating. The chloride ions are spectator ions. . 0000001700 00000 n In the first situation, we have equal moles of our dissolve in the water, like we have here. Write a net ionic equation for the reaction that occurs when aqueous solutions of ammonia and hydrocyanic acid are combined. 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.