a common-ion effect problem. Now that we have our net ionic equation, we're gonna consider three identify these spectator ions. Because the concentration of Why? K b = 6.910-4. This makes it a little (4). And once we take out our spectator ion, we're left with our net ionic equation, which is aqueous ammonia 0000012304 00000 n 0000003577 00000 n Secure .gov websites use HTTPS To get the net ionic equation, we cancel them from both sides of the equation: \[ \ce{ Cu^2+(aq) + Mg(s) \rightarrow Cu(s) + Mg^2+(aq)} \]. 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. (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.). 0000018685 00000 n 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. the equation like this. Step 3: In order to form water as a product, the covalent bond between the H+ and the C2H3O2 ions must break. dissolve in the water, like we have here. concentration of hydronium ions, it's such a small increase compared to the hydronium ions we have in 0000009368 00000 n or complete ionic equation. Always start with a balanced formula (molecular) equation. The base and the salt are fully dissociated. and encounter the phenomenom of electrolytes, pH would be less than seven. 28 0 obj <> endobj 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). some dissolved silver, plus some dissolved silver. In the complete ionic equation, soluble ionic compounds and strong acids are rewritten as dissociated ions. And because the mole xref Only the aqueous ionic compounds (the two chloride salts) are written as ions: \[ \ce{ Cu^2+(aq) + 2Cl^- (aq) + Mg(s) \rightarrow Cu(s) + Mg^2+(aq) + 2Cl^- (aq)} \]. 0000006391 00000 n Leave together all weak acids and bases. electrolyte. When ammonium hydroxide reacts with nitric acid, the products formed are ammonium nitrate and water i.e. Consider the insoluble compound cobalt(II) carbonate , CoCO3 . a complete ionic equation to a net ionic equation, which 0000002525 00000 n So actually, this would be In this case, this is an acid-base reaction between nitric acid and ammonia. 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. soluble in water and that the product solution is not saturated. The magnesium ions and the hydroxide ions will remain held together by ionic bonds even if they are in the presence of polar water molecules. Direct link to Siddesh Minde's post What are cation and anion, Posted 7 years ago. ), 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). ratio of the weak base to the strong acid is one to one, if we have more of the weak What is the net ionic equation for the reaction between aqueous ammonia and hydrochloric acid? A neutral formula unit for the dissolved species obscures this fact, Is the dissolution of a water-soluble ionic compound a chemical 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. amounts of a weak acid and its conjugate base, we have a buffer solution NH4 plus is a weak acid, and ammonia NH3 is its conjugate base, therefore, if we have similar 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. The latter denotes a species in aqueous solution, and the first equation written below can be Most of the acid molecules are not ionized, so you must write out the complete formula of the acid in your equation. Let's start with ammonia. When disassociating an ionic compound into its component ions, be carefuly not pull apart polyatomic ions. To be more specific,, Posted 7 years ago. write the net ionic equation is to show aqueous ammonia precipitation and Official websites use .gov plus solid silver chloride and if you were to look Write a net ionic equation for the reaction that occurs when aqueous solutions of hydrocyanic acid and ammonia are combined.. 2. The ionic form of the dissolution equation is our first example of an ionic equation. 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. Direct link to Icedlatte's post You don't need to, for an. nitrate stays dissolved so we can write it like this If you're seeing this message, it means we're having trouble loading external resources on our website. 0000000976 00000 n And at 25 degrees Celsius, the pH of the solution Wiki User 2010-12-01 14:24:36 Study now See answer (1) Best Answer Copy NH3 (aq) + HNO2 (aq) => HN4+. Note that MgCl2 is a water-soluble compound, so it will not form. 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). Without specific details of where you are struggling, it's difficult to advise. 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. They're going to react We need to think about the ammonium cation in aqueous solution. 1 Answer anor277 Jan 17, 2016 #NH_3(aq) + H_3O^+ rarr NH_4^+ + H_2O(l)# . 0000005636 00000 n amount of solute added to the system results in the appearance and accumulation of undissolved solid. reacting with water to form NH4 plus, and the other source came from 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. 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. It is usually found in concentrations So one thing that you notice, 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. Given the following information: hydrocyanic acid. Direct link to Ryan W's post NaNO3 is very soluble in , Posted a year ago. strong acid in excess. 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. 'q And we can use the complete ionic equation to find the net ionic equation for this weak base, strong acid reaction. Write a partial net ionic equation: Other examples of dissolution equations for water-soluble ionic compounds, such as the one for lead(II) nitrate shown at left See also the discussion and the examples provided in the following pages: precipitation and acid-base reactions, introduction to chemical equations. In the complete ionic equation, soluble ionic compounds and strong acids are rewritten as dissociated ions. A .gov website belongs to an official government organization in the United States. 0000007425 00000 n 0000004534 00000 n Now why is it called that? It won't react because the NaCl(aq)+AgNO3(aq) has already reacted to create NaNO3(aq)+AgCl(s). NH3 in our equation. First, we balance the molecular equation. (1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.152 M aqueous hydrocyanic acid and diethylamine are mixed. 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 +. 0000001439 00000 n Solution: Let us write a partial molecular first: NH 4 Cl(aq) + NaH 2 PO 4 (aq) ---> If you treat the above as a double replacement reaction, you can see that the sodium ion and the chloride ion are the spectator ions. Step 2: Identify the products that will be formed when the reactants are combined. we write aqueous to show that it is dissolved, plus 0000013231 00000 n This would be correct stoichiometrically, but such product water endstream endobj 29 0 obj <. Think of the acid molecules as potential H+ and C2H3O2 ions, however, these potential ions are held together by a covalent bond. Think of the solid ionic compound as a possible source of Mg2+ and OH ions. 0000004083 00000 n When saturation is reached, every further Write the balanced NET IONIC equation for the reaction that occurs when hydroiodic acid and ammonia are combined. 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? The OH and H+ will form water. water to evaporate. produced, this thing is in ionic form and dissolved form on Posted 7 years ago. . Ammonia present in ammonium hydroxide. The net ionic equation is commonly used in acid-base neutralization reactions, double displacement reactions, and redox reactions. Only soluble ionic compounds dissociate into ions. Yes, that's right. 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). I know this may sound silly, but can we subtract or add a reactant to both sides just like in mathematics? Nitric Acid is a strong acid, therefore, its hydrogen atom dissociates completely. NaNo3 is very soluble in water and it will dissociate into Na+ and NO3-. This is strong evidence for the formation of separated, mobile charged species The H+ from the HCl can combine with the OH from the solid Mg(OH)2 to form H2O. thing is gonna be true of the silver nitrate. How would you recommend memorizing which ions are soluble? Direct link to minhthuhoang2000's post How can you tell which io, Posted 6 years ago. going to be attracted to the partially positive To log in and use all the features of Khan Academy, please enable JavaScript in your browser. The formation of stable molecular species such as water, carbon dioxide, and ammonia. Second,. 28 34 Hope this helps. Direct link to astunix's post Why is it that AgCl(s) is, Posted a year ago. Direct link to Yu Aoi's post I know this may sound sil, Posted a year ago. Let's now consider a number of examples of chemical reactions involving ions. 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: \[ \ce{ CuCl_2(aq) + Mg(s) \rightarrow Cu(s) + MgCl_2(aq)} \]. Remember, water is a polar molecule. on the left and the nitrate is dissolved on the right. is actually reacting, what is being used to It is a neutralisation . Strictly speaking, this equation would be considered unbalanced. 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 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. Will it react? 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 other product is water. spectator ion for this reaction. In case of hydrates, we could show the waters of hydration Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. 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. This reaction is classified as: The extent of this . Ammonia is an example of a Lewis base. 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). species, which are homogeneously dispersed throughout the bulk aqueous solvent. Notice that the magnesium hydroxide is a solid; it is not water soluble. 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? reaction is complete and all the H3O plus is used up, we'll have some leftover ammonia. WRITING NET IONIC EQUATIONS FOR CHEM 101A. dissolves in the water (denoted the solvent) to form a homogeneous mixture, Instead of using sodium Write a net ionic equation to describe the reaction that occurs when 0.1 M HC 2 H 3 O 2 solution is mixed with 0.1 M KOH solution. bit clearer and similarly on this end with the sodium 0000006157 00000 n 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. This form up here, which plus H plus yields NH4 plus. Net ionic equation for hydrolysis of nh4cl - Write the net ionic equation for the hydrolysis reaction that occurs when ammonium chloride, NH.CI. 0000011267 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. 0000001700 00000 n and highlights the favorable effect of solvation and dispersal of ions in solution. Direct link to Hema Punyamoorty's post In the case of NaCl, it d, Posted 6 years ago. Direct link to Audrey Harmon-Montrull's post how do you know whether o, Posted 7 years ago. Syllabus 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. of the existence of separated charged species, that the solute is an electrolyte. So if you wanna go from Direct link to William Shiuk's post So did Jay in situation 2, Posted 2 months ago. All of those hydronium ions were used up in the acid-base neutralization reaction. The nitrate is dissolved The silver ions are going really deals with the things that aren't spectators, Let's discuss how the dissolution process is represented as a chemical equation, a Write the state (s, l, g, aq) for each substance.3. for the ammonium cation. Finally, we cross out any spectator ions. an example of a weak base. However, we have two sources Direct link to Jessica's post You're not dividing the 2, Posted 7 years ago. Therefore, if we have equal there are significant ion-dipole interactions between the ions and nearby water So the nitrate is also a spectator ion. The acetate ion is released when the covalent bond breaks. solubility, so it's not going to get dissolved in the water Write net ionic equations for reactions that occur in aqueous solution. To do that, we first need to In other words, the net ionic equation applies to reactions that are strong electrolytes in . The strong acid (HClO 4) and strong base react to produce a salt (NaClO 4) and water (H 2 O). 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. the individual ions as they're disassociated in water. salt and water. to dissolve in the water and so are the nitrate ions. a superstoichiometric amount of water (solvent) yields one lead(II) cation and two nitrate anions, By gaining a hydrogen (and a unit of charge) the hydroxide ion transforms into a water molecule. 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!). Ammonia is a weak electrolyte (and therefore a weak base) because only a small fraction of dissolved NH 3 molecules react with water to form NH 14 . (C2H5)2NH. How many 5 letter words can you make from Cat in the Hat? The sodium is going to indistinguishable from bulk solvent molecules once released from the solid phase structure. 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). The hydrogen ion transfer is onto the ammonia, giving ammonium ion as the product. 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. Well, 'cause we're showing Write a net ionic equation for the reaction that occurs when aqueous solutions of ammonia and hydrocyanic acid are combined. We can just treat this like a strong acid pH calculation problem. our symbolic representation of solute species and the reactions involving them must necessarily incorporate JavaScript appears to be disabled on this computer. 61 0 obj <>stream Sodium is a positive ion, If you wanna think of it in human terms, it's kind of out there and Direct link to RogerP's post No, we can't call it deco, Posted 6 years ago. form before they're dissolved in water, they each look like this. 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 do we know which of the two will combine to form the precipitate if we're not given (aq) and (s)? For example, CaCl. First, we balance the molecular equation. weak base and strong acid. The balanced equation for this reaction is: \[\ce{Mg(OH)2(s) + 2H^+ (aq) \rightarrow 2H2O(l) + Mg^2+ (aq)}\], Example \(\PageIndex{4}\): Writing Net Ionic Equations, Write a net ionic equation to describe the reaction that occurs when 0.1 M KHCO3 solution is mixed with excess 0.1 M HNO3 solution. is dissolved . If the base is in excess, the pH can be . As a result, the net ionic equation shows only the species that are actually involved in the chemical reaction. You get rid of that. We learn to represent these reactions using ionic equa- tions and net ionic equations. 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. watching the reaction happen. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. well you just get rid of the spectator ions. classroom desk arrangements for 25 students; isidro martinez obituary; university of michigan swimming recruiting questionnaire; house for rent in suffolk county, ny by owner. What is the net ionic equation of the reaction between ammonia and nitrous acid? If we then take a small sample of the salt and So ammonium chloride Posted 6 years ago. Be sure to balance this equation. 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). 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. daBL:nC[ -|7LDVp)J0s~t@Vg,0G' bm@S 0(xX,CF$ reactions, introduction to chemical equations. %%EOF And because this is an acid-base Direct link to Nehemiah Skandera's post It won't react because th, Posted 5 years ago. It is not necessary to include states such as (aq) or (s). K a = 4.010-10. Now, in order to appreciate Direct link to Dillon Mccarthy's post How do we know which of t, Posted 6 years ago. { "8.01:_Classifying_Chemical_Reactions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "8.02:_Aqueous_Solutions_and_Solubility_-_Compounds_Dissolved_in_Water" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "8.03:_Precipitation_Reactions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "8.04:_Complete_Ionic_and_Net_Ionic_Equations-_Precipitation_Reaction_Examples" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "8.05:_Complete_Ionic_and_Net_Ionic_Equations_-_More_Examples" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "8.06:_Oxidation_and_Reduction" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "8.07:_Redox_Reactions_in_Organic_Chemistry_and_Biochemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, { "00:_Front_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "01:_Classifying_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "02:_Measurement_and_Problem_Solving" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "03:_Atoms" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "04:_Ions_and_Ionic_Compounds" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "05:_Molecules_and_Covalent_Compounds" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "06:_Introduction_to_Chemical_Reactions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "07:_Mass_Relations_in_Chemical_Reactions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "08:_Types_of_Chemical_Reactions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "09:_Energy_and_Chemical_Reactions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "zz:_Back_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, 8.5: Complete Ionic and Net Ionic Equations - More Examples, https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FCourses%2FPortland_Community_College%2FCH104%253A_Allied_Health_Chemistry_I%2F08%253A_Types_of_Chemical_Reactions%2F8.05%253A_Complete_Ionic_and_Net_Ionic_Equations_-_More_Examples, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), 8.4: Complete Ionic and Net Ionic Equations- Precipitation Reaction Examples, status page at https://status.libretexts.org.
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