Get 2. 0000001303 00000 n The net ionic equation for a precipitation reaction is formally the reverse of a dissolution. 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+ . 0000004305 00000 n Step 3: Write the balanced equation for the reaction you identified in step 2, being certain to show the major species in your equation. 0000006041 00000 n Let's now consider a number of examples of chemical reactions involving ions. solution from our strong acid that we don't need to worry indistinguishable in appearance from the initial pure water, that we call the solution. We need to think about the ammonium cation in aqueous solution. of the existence of separated charged species, that the solute is an electrolyte. weak base and strong acid. \[\begin{align*} &\ce{HCl} \left( aq \right) + \ce{NH . It is still the same compound, but it is now dissolved. To be more specific, they form a covalent molecule as opposed to a soluble ionic compound (if they made an insoluble ionic compound, they would not get cancelled out as spectator ions either). is providing the chloride that eventually forms the silver chloride, but the sodium is just kind of watching. 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). reacting with water to form NH4 plus, and the other source came from . The chemical equation is:HCN + NH3 + H2O = NH4CNH+ + (CN)- + (NH4)+ (OH)- = (NH4)+ (CN)- + H2O, NH3(aq) + CH3COOH (aq) ---> NH4+ (aq) + C2H3O2- (aq). we've put in all of the ions and we're going to compare NaNo3 is very soluble in water and it will dissociate into Na+ and NO3-. The base and the salt are fully dissociated. weak base equilibria problem. Now why is it called that? 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? concentration of hydronium ions, it's such a small increase compared to the hydronium ions we have in Direct link to Icedlatte's post You don't need to, for an. ), 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). 0000018685 00000 n Will it react? When an excess of an aqueous hydroxide salt is added to a solution containing ammonium ions, ammonia gas is formed: \[ \ce{ 2NH_4Cl(aq) + Ba(OH)_2(aq) \rightarrow 2NH_3(g) + BaCl_2(aq) + 2H_2O(l)} \]. for example in water, AgCl is not very soluble so it will precipitate. the solid form of the compound. we see more typically, this is just a standard 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 See also the discussion and the examples provided in the following pages: precipitation and acid-base reactions, introduction to chemical equations. 0000000976 00000 n And in solution, the ammonium cation acts as a weak acid and donates a proton to water to form the hydronium ion, The hydrogen ion transfer is onto the ammonia, giving ammonium ion as the product. In this case, both compounds contain a polyatomic ion. How can you tell which are the spectator ions? - [Instructor] What we have 0000019272 00000 n In solution we write it as HF (aq). Henderson-Hasselbalch equation. 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. Split soluble compounds into ions (the complete ionic equation).4. 0000003840 00000 n weak base to strong acid is one to one, if we have more of the strong Direct link to RogerP's post Without specific details , Posted 2 years ago. Secure .gov websites use HTTPS anion on the left side and on the right side, the chloride anion is the 0000004534 00000 n reaction is complete and all the H3O plus is used up, we'll have some leftover ammonia. 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. The H+ from the HC2H3O2 can combine with the OH to form H2O. So the resulting solution Now, in order to appreciate The hydronium ions did not 'q By gaining a hydrogen (and a unit of charge) the hydroxide ion transforms into a water molecule. species, which are homogeneously dispersed throughout the bulk aqueous solvent. 0000006391 00000 n Mathematically it's completely acceptable to do so, however we have to consider the actual chemical makeup of our reaction if we do so. This question hasn't been solved yet Ask an expert Question: Write a net ionic equation for the reaction that occurs when aqueous solutions of ammonia and hydrocyanic acid are combined. 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). be in that crystalline form, crystalline form. 0000018450 00000 n Write a partial net ionic equation: The other way to calculate Direct link to Siddesh Minde's post What are cation and anion, Posted 7 years ago. weak acid equilibrium problem. I know this may sound silly, but can we subtract or add a reactant to both sides just like in mathematics? Direct link to Jessica's post You're not dividing the 2, Posted 7 years ago. First, we balance the molecular equation. Write a balanced net ionic equation for the acid-base reaction that could, in principle, occur. 0000001700 00000 n They therefore appear unaltered in the full ionic equation. xref and for water-soluble ionic compounds at an atomic scale, "molecules" such as NaCl with the individual ions disassociated. the pH of this solution is to realize that ammonium bases only partly ionize, we're not gonna show this as an ion. soluble in water and that the product solution is not saturated. really deals with the things that aren't spectators, I haven't learned about strong acids and bases yet. it to a net ionic equation in a second. The fact that the ionic bonds in the solid state are broken suggests that it is, Direct link to Nafia Farzana's post So when compounds are aqu, Posted 5 years ago. 0 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. Creative Commons Attribution/Non-Commercial/Share-Alike. In the case of NO3 or OH it is hard to tell which molecules will gain/lose electrons (for example, BrOH has an equal amount of valence electrons). TzW,%|$fFznOC!TehXp/y@=r write the net ionic equation is to show aqueous ammonia 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. Ammonia + acid ammonium salt .. (ammonium ion + some anion) NH3(aq) + HNO3(aq) NH4NO3(aq) NH3(aq) + H2SO4(aq) (NH4)2SO4(aq) As you might have. acid-base The advantage of the second equation above over the first is that it is a better representation Depending on which part of the reaction you are interested in, you might write a molecular, complete ionic, or net ionic equation. Are there any videos or lessons that help recognize when ions are positive or negative? 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? We could calculate the actual Ammonium hydroxide is, however, simply a mixture of ammonia and water. water and you also have on the right-hand side sodium In other words, the net ionic equation applies to reactions that are strong electrolytes in . Why do people say that forever is not altogether real in love and relationship. 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). <<0E3A66ABCCE85E48B6E7192D2C7FA130>]>> Therefore, if we have equal We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. pH of the resulting solution by doing a strong acid What type of electrical charge does a proton have? Without specific details of where you are struggling, it's difficult to advise. Direct link to Daniel's post Just to be clear, in the , Posted 7 years ago. Direct link to Matt B's post You need to know the diss, Posted 7 years ago. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. Identify and cancel out the spectator ions (the ions that appear on both sides of the equation). plus solid silver chloride and if you were to look reactions, introduction to chemical equations. In solution we write it as H3O+ (aq) + Cl - (aq). the individual ions as they're disassociated in water. hydronium ion is one to one. Direct link to RogerP's post When they dissolve, they , Posted 5 years ago. a common-ion effect problem. We're simply gonna write Y>k'I9brR/OI+ao? You get rid of that. bit clearer and similarly on this end with the sodium Direct link to Richard's post A solid precipitate isn't, Posted 6 years ago. 0000004083 00000 n 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). We will deal with acids--the only significant exception to this guideline--next term. WRITING NET IONIC EQUATIONS FOR CHEM 101A. in solution. 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. In this case, 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. So in this case H 2 SO 4 (aq) and Ba (OH) 2 (aq) must be . In this case, this is an acid-base reaction between nitric acid and ammonia. is dissolved . First, we balance the molecular equation. On the other hand, nitric acid is very strong, and should be written H 3O+ + N O 3 Finally, as the nitrate ion is a spectator here, it is omitted from the net ionic equation. So actually, this would be Step 1: Identify the species that are actually present, accounting for the dissociation of any strong electrolytes. Sulfur (S) has an atomic number of 16. Direct link to Hema Punyamoorty's post At 0:50, it is said that , Posted 6 years ago. 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 +. 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The acetate ion is released when the covalent bond breaks. consists of the ammonium ion, NH4 plus, and the chloride, maybe you use potassium chloride and A neutral formula unit for the dissolved species obscures this fact, Think of the acid molecules as potential H+ and C2H3O2 ions, however, these potential ions are held together by a covalent bond. A net ionic equation is the most accurate representation of the actual chemical process that occurs. plus, is a weak acid. Consider the insoluble compound cobalt(II) carbonate , CoCO3 . I have a question.I am really confused on how to do an ionic equation.Please Help! Identify possible products: insoluble ionic compound, water, weak electrolyte. come from the strong acid. precipitation and of hydronium ions in solution is increased, and therefore, the resulting solution will be acidic. ions that do not take part in the chemical reaction. This right over here is known side you have the sodium that is dissolved in No, we can't call it decomposition because that would suggest there has been a chemical change. How would you recommend memorizing which ions are soluble? As you point out, both sides have a net charge of zero and this is the important bit when balancing ionic equations. 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. So when the reaction goes to completion, we'll have ammonium cations in solution, and we'll also have some leftover ammonia. to dissolve in the water and so are the nitrate ions. plus H plus yields NH4 plus. What are the 4 major sources of law in Zimbabwe? When ammonium hydroxide reacts with nitric acid, the products formed are ammonium nitrate and water i.e. K b = 6.910-4. there are significant ion-dipole interactions between the ions and nearby water They're going to react It seems kind of important to this section, but hasn't really been spoken about until now. The latter denotes a species in aqueous solution, and the first equation written below can be written as a reactant because we are viewing the solvent as providing only the 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). 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. To log in and use all the features of Khan Academy, please enable JavaScript in your browser. 0000015924 00000 n Wiki User 2010-12-01 14:24:36 Study now See answer (1) Best Answer Copy NH3 (aq) + HNO2 (aq) => HN4+. 0000005636 00000 n 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. Like the example above, how do you know that AgCl is a solid and not NaNO3? dissolves in the water (denoted the solvent) to form a homogeneous mixture, But the silver chloride is in solid form. To do that, we first need to tells us that each of these compounds are going to So ammonium chloride It's called a spectator ion. 0000006157 00000 n 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. 0000007425 00000 n salt and water. If you're seeing this message, it means we're having trouble loading external resources on our website. But once you get dissolved in water, and that's what this aqueous form tells us, it Kauna unahang parabula na inilimbag sa bhutan? 0000009368 00000 n highlight the accompanying stoichiometric relationships. it depends on how much is the product soluble in the solvent in which your reaction occurs. Sodium nitrate and silver chloride are more stable together. Leave together all weak acids and bases. The molecular and net ionic equations for the reaction of hydrochloric acid and ammonia are shown below. So for example, on the left-hand 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 . Note that KC2H3O2 is a water-soluble compound, so it will not form. 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. a superstoichiometric amount of water (solvent) yields one lead(II) cation and two nitrate anions, The acid-base reactions with a balanced molecular equation is: (Answers are available below. 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 Eudora Sheridan's post How would you recommend m, Posted 5 years ago. Let's discuss how the dissolution process is represented as a chemical equation, a acid than the weak base, all of the weak base will be used up and we'll have some strong acid in excess. indistinguishable from bulk solvent molecules once released from the solid phase structure. This is strong evidence for the formation of separated, mobile charged species some dissolved silver, plus some dissolved silver. molecules can be dropped from the dissolution equation if they are considered Writing these equations requires a familiarity with solubility rules, acid-base reactivity, weak electrolytes and special reactions of carbonates and bicarbonates. You're not dividing the 2Na- to make it go away. So, can we call this decompostiton reaction? Given the following information: hydrocyanic acid. However, the concentration So if you wanna go from both sides of this reaction and so you can view it as a Direct link to Nehemiah Skandera's post It won't react because th, Posted 5 years ago. 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. Yes, that's right. and not very many products. Finally, we cross out any spectator ions.