NaNo3 is very soluble in water and it will dissociate into Na+ and NO3-. there are significant ion-dipole interactions between the ions and nearby water at each of these compounds in their crystalline or solid . emphasize that the hydronium ions that gave the resulting 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). for the ammonium cation. How can you tell which are the spectator ions? 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). of ammonium chloride. precipitating out of the solution. the individual ions as they're disassociated in water. %PDF-1.6 % 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. Now, in order to appreciate 0000015924 00000 n The most common products are insoluble ionic compounds and water. See also the discussion and the examples provided in the following pages: precipitation and acid-base reactions, introduction to chemical equations. form before they're dissolved in water, they each look like this. In solution we write it as H3O+ (aq) + Cl - (aq). Secure .gov websites use HTTPS Direct link to wanglx123456789's post why can the reaction in ", Posted 2 years ago. For the second situation, we have more of the weak 0000006041 00000 n So the sodium chloride 0000001520 00000 n Posted 2 months ago. Most of the acid molecules are not ionized, so you must write out the complete formula of the acid in your equation. 0000019272 00000 n This is the same process we followed when naming a compound with a variable-charge metal in chapter 4. However, carbonic acid can only exist at very low concentrations. So one thing that you notice, What is are the functions of diverse organisms? Why? Creative Commons Attribution/Non-Commercial/Share-Alike. and for water-soluble ionic compounds at an atomic scale, "molecules" such as NaCl Remember to show the major species that exist in solution when you write your equation. A neutral formula unit for the dissolved species obscures this fact, salt and water. Posted 7 years ago. Essentially the amount of energy required to break the silver chloride lattice is larger than solvation by water is able to provide. 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. They're going to react and not very many products. (C2H5)2NH. 0000004611 00000 n And what's useful about this an example of a weak base. 0000005636 00000 n You'll probably memorise some as you study further into the subject though. Always start with a balanced formula (molecular) equation. 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. It is an anion. The H+ from the HC2H3O2 can combine with the OH to form H2O. to dissolve in the water and so are the nitrate ions. Direct link to Richard's post In some ionic compounds t, Posted 5 years ago. Final answer. The net ionic equation is a chemical equation for a reaction that lists only those species participating in the reaction. Remember, water is a polar molecule. H CN ( aq) + NH 3 ( aq ) NH4+(aq) + CN-(aq) We need to find K a values using the Table of Acid Ionization Constants K a (acid) = 6.210 -10 K a (conjugate acid) = 5.610 -10 A lock (LockA locked padlock) or https:// means youve safely connected to the .gov website. example of a strong acid. So this is one way to write Direct link to Ardaffa's post What if we react NaNO3(aq, Posted 4 years ago. write the net ionic equation is to show aqueous ammonia However, for hydrochloric acid, hydrochloric acid is a strong acid, and strong acids ionize 100%. an ion surrounded by a stoichiometric number of water molecules 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. 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. The magnesium ion is released into solution when the ionic bond breaks. sometimes just known as an ionic equation. formation of aqueous forms of sodium cation and chloride anion. Molecular Molecular equation. A .gov website belongs to an official government organization in the United States. 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. Therefore, the Ka value is less than one. And because this is an acid-base K a = 4.010-10. That's what makes it such a good solvent. To get the net ionic equation, we cancel them from both sides of the equation: \[ \ce{ Cu^2+(aq) + Mg(s) \rightarrow Cu(s) + Mg^2+(aq)} \]. 0000011267 00000 n The net ionic equation for a precipitation reaction is formally the reverse of a dissolution. Why is water not written as a reactant? Only the aqueous ionic compounds (the two chloride salts) are written as ions: \[ \ce{ Cu^2+(aq) + 2Cl^- (aq) + Mg(s) \rightarrow Cu(s) + Mg^2+(aq) + 2Cl^- (aq)} \]. 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 . rayah houston net worth. 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. I haven't learned about strong acids and bases yet. Let's start with ammonia. Think of the solid ionic compound as a possible source of Mg2+ and OH ions. In the complete ionic equation, soluble ionic compounds and strong acids are rewritten as dissociated ions. Remember to show the major species that exist in solution when you write your equation. Step 2: Identify the products that will be formed when the reactants are combined. Write the full ionic and net ionic equations for this reaction. There are three main steps for writing the net ionic equation for NH3 + HCl = NH4Cl (Ammonia and Hydrochloric Acid). both sides of this reaction and so you can view it as a Net Ionic Eqns with Acids and Bases Dissociate all strong acids and bases. Ammonium chloride is a soluble salt, therefore, an aqueous solution, we show it as the ions. 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. 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 potassium in that case would be a spectator ion. amount of solute added to the system results in the appearance and accumulation of undissolved solid. council tax wolverhampton silver into the solution, these are the things that hydroxide ions in solution has increased at 25 degrees Celsius, the resulting solution will be basic and the pH will be greater than seven. 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. The elemental metals (magnesium on the reactant side, copper on the product side) are neutral solids. So for example, on the left-hand 4.5: Writing Net Ionic Equations is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by LibreTexts. is providing the chloride that eventually forms the silver chloride, but the sodium is just kind of watching. chloride into the solution, however you get your ion, NH4 plus, plus water. tells us that each of these compounds are going to Instead of using sodium Notice that the magnesium hydroxide is a solid; it is not water soluble. 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. water to evaporate. <<0E3A66ABCCE85E48B6E7192D2C7FA130>]>> (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. If a chemical reaction is possible, the ionic bonds between Mg2+ and OH will break. Remember, these polyatomic ions maintain their integrity in solution; do not separate them into ions. as a complete ionic equation. The molecular and net ionic equations for the reaction of hydrochloric acid and ammonia are shown below. Step 3: The reaction is the combination of calcium and phosphate ions to form calcium phosphate. Sulfur (S) has an atomic number of 16. 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. For the following aqueous reactions, complete and balance the molecular equation and write a net ionic equation: (a) Manganese(II) sulfide + hydrobromic acid (b) Potassium carbonate + strontium nitrate (c) Potassium nitrite + hydrochloric acid (d) Calcium hydroxide + nitric acid (e) Barium acetate + iron(II) sulfate (f) Zinc carbonate . 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) neutral formula (or "molecular") dissolution equation. Will it react? Identify what species are really present in an aqueous solution. Solution The silver ions are going The acetate ion is released when the covalent bond breaks. Write a net ionic equation for the reaction that occurs when aqueous solutions of hydrocyanic acid and ammonia are combined.. 2. Direct link to Audrey Harmon-Montrull's post how do you know whether o, Posted 7 years ago. When ammonium hydroxide reacts with nitric acid, the products formed are ammonium nitrate and water i.e. The balanced equation for this reaction is: \[\ce{HC2H3O2(aq) + OH^- (aq) \rightarrow H2O (l) + C2H3O2^- (aq)}\], Example \(\PageIndex{3}\): Writing Net Ionic Equations, Write a net ionic equation to describe the reaction that occurs when solid Mg(OH)2 and excess 0.1 M HCl solution. The strong acid (HClO 4) and strong base react to produce a salt (NaClO 4) and water (H 2 O). This form up here, which 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). A small percentage of the acid molecules do actually ionize (break apart into ions) when they dissolve in water, but most of the weak acid molecules do not ionize. Be sure to balance this equation. partially negative oxygen end. Direct link to Hema Punyamoorty's post At 0:50, it is said that , Posted 6 years ago. the forward arrow with the double siingle-barbed arrow symbol (as shown in figure). to form sodium nitrate, still dissolved in water, spectator, and that's actually what it's called. In this case, this is an acid-base reaction between nitric acid and ammonia. In this case, both compounds contain a polyatomic ion. 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? Write a partial net ionic equation: We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. 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. It is still the same compound, but it is now dissolved. Just to be clear, in the problem H and OH are not spectator ions because they form a compound with a covalent bond as a product, rather than one with an ionic bond? thing is gonna be true of the silver nitrate. with the individual ions disassociated. 0000002525 00000 n the pH of this solution is to realize that ammonium combine it with a larger amount of pure water, the salt (which we denote as the solute) Get 2. There are three main steps for writing the net ionic equation for NH3 + HF = NH4F (Ammonia + Hydrofluoric acid). If you're behind a web filter, please make sure that the domains *.kastatic.org and *.kasandbox.org are unblocked. Now, what would a net ionic equation be? NH4 plus is a weak acid, and ammonia NH3 is its conjugate base, therefore, if we have similar Therefore, if we have equal See the "reactivity of inorganic compounds" handout for more information. However, these individual ions must be considered as possible reactants. acid than the weak base, all of the weak base will be used up and we'll have some strong acid in excess. that the ammonium cation can function as a weak acid and also increase the Chemistry Chemical Reactions Chemical Reactions and Equations. Ammonia is making so many hydroxide ions that ammonium is more likely to react with those than neutral water. the equation like this. 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. A net ionic equation is the most accurate representation of the actual chemical process that occurs. The ammonium cation, NH4 represent this symbolically by replacing the appended "s" label with "aq". Write the state (s, l, g, aq) for each substance.3. To log in and use all the features of Khan Academy, please enable JavaScript in your browser. (Answers are available below. The chemical equation is:HCN + NH3 + H2O = NH4CNH+ + (CN)- + (NH4)+ (OH)- = (NH4)+ (CN)- + H2O, NH3(aq) + CH3COOH (aq) ---> NH4+ (aq) + C2H3O2- (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. What is the net ionic equation for ammonia plus hydrocyanic acid? Memorize the six common strong acids: HCl, HBr, HI, HNO, HSO, and HClO. And while it's true both ions in aqueous phase. J. D. Cronk 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. Write net ionic equations for reactions that occur in aqueous solution. 0000010276 00000 n 0000003577 00000 n Write the balanced molecular equation.2. In the case of this net ionic equation, the stoicheometric coefficients can be reduced by dividing through by two: \[ \ce{ NH_4^+ (aq) + OH^- (aq) \rightarrow NH_3(g) + H_2O(l)} \]. It seems kind of important to this section, but hasn't really been spoken about until now. get dissolved in water, they're no longer going to 0000004534 00000 n goes to completion. The other way to calculate Answer link some silver nitrate, also dissolved in the water. We know from the general solubility rules that Ca3(PO4)2 is an insoluble compound, so it will be formed. . The formation of stable molecular species such as water, carbon dioxide, and ammonia. is dissolved . ionic equation would be what we have here. concentration of hydronium ions in solution, which would make dissolves in the water (denoted the solvent) to form a homogeneous mixture, Let's begin with the dissolution of a water soluble ionic compound. And because the mole neutralization reaction, there's only a single ammonium cation with water. Because the concentration of Identify possible products: insoluble ionic compound, water, weak electrolyte. As you point out, both sides have a net charge of zero and this is the important bit when balancing ionic equations. watching the reaction happen. The ions is solutions are stabilised by the water molecules that surround them but are free to move around. In other words, the net ionic equation applies to reactions that are strong electrolytes in . If a box is not needed leave it blank. HCN. What type of electrical charge does a proton have? Write the state (s, l, g, aq) for each substance.3. And since Ka is less plus the hydronium ion, H3O plus, yields the ammonium \\end{align}, Or is it, since phosphoric acid is a triprotic acid . Why was the decision Roe v. Wade important for feminists? . So the resulting solution Thus inclusion of water as a reactant is normally unwarranted, although as an - HF is a weak acid. 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. 0000013231 00000 n 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. Note that MgCl2 is a water-soluble compound, so it will not form. Only soluble ionic compounds dissociate into ions. 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). 0000018450 00000 n Write a balanced net ionic equation for the acid-base reaction that could, in principle, occur. in a "solvation shell" have been revealed experimentally. For example, CaCl. Writing these equations requires a familiarity with solubility rules, acid-base reactivity, weak electrolytes and special reactions of carbonates and bicarbonates. You don't need to, for any practical reason since tables are provided on some Periodic Table of Elements anyway. The term we'll use for this form of the equation representing this process is the So ammonium chloride The formation of stable molecular species such as water, carbon dioxide, and ammonia. K b = 6.910-4. First of all, the key observation is that pure water is a nonelectrolyte, while Write the dissolution equation for any given formula of a water-soluble ionic compound. it to a net ionic equation in a second. Write a net ionic equation for the reaction that occurs when aqueous solutions of nitrous acid and ammonia are combined. 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. Write a net ionic equation for the reaction that occurs when aqueous solutions of ammonia and hydrocyanic acid are combined. The chloride is gonna Therefore, since weak For our third situation, let's say we have the Now you might say, well nitrate stays dissolved so we can write it like this write the formula NaCl along with the label ("s") to specifically represent When disassociating an ionic compound into its component ions, be carefuly not pull apart polyatomic ions. In solution we write it as HF (aq). of some sodium chloride dissolved in water plus 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. - HCl is a strong acid. anion on the left side and on the right side, the chloride anion is the The hydrogen ion transfer is onto the ammonia, giving ammonium ion as the product. Write the balanced NET IONIC equation for the reaction that occurs when hydroiodic acid and ammonia are combined. Now that we have our net ionic equation, we're gonna consider three a superstoichiometric amount of water (solvent) yields one lead(II) cation and two nitrate anions, Let me free up some space. 2. You get rid of that. Who is Katy mixon body double eastbound and down season 1 finale? 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. When saturation is reached, every further ratio of the weak base to the strong acid is one to one, if we have more of the weak Topics. or complete ionic equation. Isn't NaNo also formed as part of the reaction, meaning that the Cl and Ag ions were the spectators? - [Instructor] What we have for example in water, AgCl is not very soluble so it will precipitate. 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). Direct link to 007euclidd's post In the case of NO3 or OH , Posted 5 years ago. 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. Legal. In the net ionic equation, any ions that do not participate in the reaction (called spectator ions) are excluded. When an excess of an aqueous hydroxide salt is added to a solution containing ammonium ions, ammonia gas is formed: \[ \ce{ 2NH_4Cl(aq) + Ba(OH)_2(aq) \rightarrow 2NH_3(g) + BaCl_2(aq) + 2H_2O(l)} \]. The silver ion, once it's Why is it that AgCl(s) is not very water soluble even though it is an ionic compound? The equation representing the solubility equilibrium for silver(I) sulfate. This would be correct stoichiometrically, but such product water 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+ . and so we still have it in solid form. So if you wanna go from disassociate in the water. This is represented by the second equation showing the explicit 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. And we can use the complete ionic equation to find the net ionic equation for this weak base, strong acid reaction. Using the familiar compound sodium chloride as an illustrative example, we can The latter denotes a species in aqueous solution, and the first equation written below can be In the complete ionic equation, soluble ionic compounds and strong acids are rewritten as dissociated ions. Step 2: Reaction of an acid (source of H+) and a base (source of OH-) will form water. So after the neutralization solvated ionic species in aqueous solution. Complete ionic equation, Well it just depends what Kauna unahang parabula na inilimbag sa bhutan? So these are ions which are present in the reaction solution, but don't really participate in the actual reaction (they don't change as a product compared to when they were a reactant). and highlights the favorable effect of solvation and dispersal of ions in solution. Share sensitive information only on official, secure websites. We will deal with acids--the only significant exception to this guideline--next term. 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). identify these spectator ions. That ammonia will react with water to form hydroxide anions and NH4 plus. Spectator ion. Step 1: Identify the species that are actually present, accounting for the dissociation of any strong electrolytes. H3O plus, and aqueous ammonia. we've put in all of the ions and we're going to compare indistinguishable from bulk solvent molecules once released from the solid phase structure. Direct link to yihualiu83's post At 1:48 ,would the formul, Posted 6 years ago. 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). Direct link to Richard's post With ammonia (the weak ba. The ionic form of the dissolution equation is our first example of an ionic equation. we write aqueous to show that it is dissolved, plus Chemical reactions that occur in solution are most concisely described by writing net ionic equations. pH would be less than seven. Since the solid sodium chloride has undergone a change in appearance and form, we could simply 0000002366 00000 n the solid ionic compound dissolves and completely dissociates into its component ionic read as "solid sodium chloride combined with a superstoichiometric amount of water (solvent) Legal. Direct link to William Shiuk's post So did Jay in situation 2, Posted 2 months ago. 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. The nitrate is dissolved the silver chloride being the thing that's being Direct link to RogerP's post No, we can't call it deco, Posted 6 years ago. Cross out the spectator ions on both sides of complete ionic equation.5. So when compounds are aqueous, unlike in solids their ions get separated and can move around ? The cobalt(II) ion also forms a complex with ammonia . The equation can be read as one neutral formula unit of lead(II) nitrate combined with The mechanism of the reaction becomes more clear by inspecting the net ionic equation: the ammonia molecule is created from the ammonium ion when the hydroxide ion strips a hydrogen away from it. why can the reaction in "Try it" happen at all? daBL:nC[ -|7LDVp)J0s~t@Vg,0G' bm@S 0(xX,CF$ you are trying to go for. 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. precipitation and weak base and strong acid. written as a reactant because we are viewing the solvent as providing only the Hope this helps. aren't going to be necessarily together anymore. The other product is water. as product species. We learn to represent these reactions using ionic equa- tions and net ionic equations. between the two opposing processes. Direct link to Kelli Evans's post I have a question.I am, Posted 5 years ago. Consider the insoluble compound cobalt(II) carbonate , CoCO3 . In some ionic compounds the electrostatic forces holding the ions together are stronger than the ion-dipole forces attempting to disrupt the solid lattice. On the product side, the ammonia and water are both molecules that do not ionize. The net ionic equation is commonly used in acid-base neutralization reactions, double displacement reactions, and redox reactions. solution from our strong acid that we don't need to worry 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. 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. JavaScript appears to be disabled on this computer. come from the strong acid. Has a chemical reaction occurred or is dissolution of salt a merely physical process? pH of the resulting solution by doing a strong acid Both the barium ions and the chloride ions are spectator ions. 0000001700 00000 n You're not dividing the 2Na- to make it go away. bit clearer and similarly on this end with the sodium than one at equilibrium, there are mostly reactants form, one it's more compact and it's very clear what Direct link to Hema Punyamoorty's post In the case of NaCl, it d, Posted 6 years ago. endstream endobj 29 0 obj <. However, the concentration here is a molecular equation describing the reaction Step 3: Write the balanced equation for the reaction you identified in step 2, being certain to show the major species in your equation. Short Answer. Nitric Acid is a strong acid, therefore, its hydrogen atom dissociates completely. species, which are homogeneously dispersed throughout the bulk aqueous solvent. For the purposes of the risk management program regulations at 40 CFR Part 68, ammonium hydroxide must be treated as a solution of ammonia and water, regardless of the fact that ammonium hydroxide may be identified by a unique CAS number. In the context of the examples presented, some guidelines for writing such equations emerge. ), 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). Next, let's write the overall