barium nitrate and sodium hydroxide ionic equation

PDF Worksheet Molecular and Net Key - Cerritos College A suspension of magnesium hydroxide in water . Include phases. Net Ionic Equation for HNO3 + NaOH (Strong Base and Strong ... Write a net ionic equation for the reaction that occurs when potassium sulfite (aq) and excess hydrobromic acid (aq) are combined. Determinations of the solubility of a salt may be made by reference to SOLUBILITIES OF IONIC COMPOUNDS. CHEM 101 - Ionic and net ionic equations (a) Write a balanced molecular equation for the reaction between aqueous solutions of acetic acid (CH 3 COOH) and barium hydroxide, Ba(OH) 2. Hydrofluoric acid, HF, a weak acid, will react with sodium hydroxide, NaOH, a strong base, to produce aqueous sodium fluoride, NaF, and water. These unreacted ions (spectator ions) can be left out of the total ionic equation to yield the net ionic equation. solution of calcium chloride. barium nitrate and sodium sulfate ionic equation A suspension of magnesium hydroxide in water . Hence, it is written in molecular form. Solved Write the molecular, ionic, and net ionic equations ... Net ionic: S 2- (aq) + Pb 2+ (aq) à PbS (s) 4. copper (II) sulfate + barium chloride. Barium chloride reacts with aluminum sulfate. Top of Page. PDF Q1. - irp-cdn.multiscreensite.com Answers: 3 Ag+(aq) + PO 4 3-(aq) → Ag 3 PO 4 (s) 4. When ammonium chloride (NH 4 Cl) is heated with barium hydroxide ( Ba(OH) 2), ammonia gas is released and colorless solution is given as another product.NH 4 Cl is a weak acid and barium hydroxde is a strong base. Write the molecular, ionic, and net ionic equations for the following: 1. aluminum sulfate + lead(II) nitrate 2. aluminum sulfate + sodium phosphate 3. aluminum sulfate + copper(II) nitrate 4. aluminum sulfate + barium chloride 5. potassium hydroxide + lead(II) nitrate 6. potassium hydroxide + sodium phosphate 7. potassium hydroxide + barium chloride 8. potassium hydroxide + aluminum sulfate . This means that we will split them apart in the net ionic equation. Barium nitrate solution can be used instead of barium chloride solution. Barium sulphate is one of the most insoluble compounds known. **3rd is the Ionic Equation **4th is the Net Ionic Equation . Total Ionic Equation: Na+ (aq) + Cl - (aq) + Ag + (aq) + NO 3 - (aq) → Na + (aq) + NO 3 - (aq) + AgCl (s) Note that during the course of reaction, there has been no change in the Na+and NO 3 -ions. A few drops of dilute sodium hydroxide solution react to form a white precipitate with aluminium ions, calcium ions and magnesium ions. PDF Group 2: The Alkaline Earth Metals - chemrevise Enter an equation of a chemical reaction and click 'Balance'. H 2 O is a molecular compound. The reaction of Nitric acid and Sodium hydroxide represents a net ionic equation involving a strong acid and strong base. Molecular: Fe(NO) 3 (aq) + 3Na(OH) (aq) à Fe(OH) 3 (s) + 3Na(NO 3) (aq) Net ionic: Fe 3+ (aq) + 3OH-(aq) à . However, when additional aqueous . Write the formula for each compound below: a. magnesium iodide MgI2. If you are given just the names of the reactants. Um they're asking us to write based on what we're given complete and net ionic equations for each example. What is the total iconic equation and net ionic equation ... Write a net ionic equation to show why solid sodium hydroxide, NaOH (s), forms a basic solution when it dissolves in water. ∙ 2009-07-27 09:48:46. Copy. What is the net ionic equation for the reaction between silver nitrate and sodium hydroxide? It is a molecule so it cannot form ionic ties. chemistry. [Algorithmic] If all of the chloride in a 5.000-g sample of an unknown metal chloride is. this question addresses ionic equations. The balanced chemical equation for this reaction would look like this 2NaOH(aq] + Cu(NO3)2 (aq] → Cu(OH)2 (s] ⏐ ↓ +2NaNO3 (aq] Theoretically, when an aqueous solution of 0.1 M sodium hydroxide reacts with an aqueous solution of 0.1 M barium nitrate, there should be no visible change as colourless aqueous solutions of sodium nitrate and barium hydroxide are produced. Ba(OH)2 (S) + aq Ba2+ (aq) + 2OH-(aq) Magnesium hydroxide is classed as insoluble in water. bases are sodium hydroxide, NaOH, potassium hydroxide, KOH, calcium hydroxide, Ca(OH) 2, and barium hydroxide, Ba(OH) 2. (b) What is the net ionic equation? It has a role as a fertilizer. Learn how to use the molecular equation to write the complete ionic and net ionic equations for a reaction occurring in aqueous solution. These are not reacting, and are therefore spectator ions, and cancel out: Ba2+(aq) + SO42−(aq) → BaSO4(s) What is left over becomes the net ionic equation for the precipitation reaction. Then we have our net ionic species which is essentially a condensed version of our total Ionic equation. The majority of time, a faint white precipitate of barium hydroxide is formed. barium nitrate + sodium hydroxide barium hydroxide + sodium nitrate . Post any follow up questions here to help if you don't understand what I did above. How to Identify Chemicals in Solution: Test Methods & Materials. If you are given just the names of the reactants. Write the balanced chemical equation for each of these reactions. Wiki User. E-mail instructor: Eden Francis HF(aq) + NaOH(aq) → NaF(aq) +H2O(l) Now, the important thing to remember here is that hydrofluoric acid is a weak acid, which implies that it does not dissociate completely in aqueous solution to form . Ionic Equation Worksheet Write balanced molecular, total ionic, and net ionic equations for each of the following. Write the balanced chemical equation for each of these reactions. Write the net ionic equation for the precipitation reaction that occurs when aqueous solutions of silver nitrate and potassium phosphate are mixed. The hydrochloric acid is added first to remove any carbonate ions that might be present - they would also produce a white precipitate, giving a false positive result. Net Ionic Equation Worksheet READ THIS: When two solutions of ionic compounds are mixed, a solid may form. Check 35+ pages net ionic equation of sodium sulfate and barium hydroxide explanation in Google Sheet format. Second, we write the states and break the soluble ionic compounds into their ions (these are the . In brief Theoretically, when an aqueous solution of 0.1 M sodium hydroxide reacts with an aqueous solution of 0.1 M barium nitrate, there should be no visible change as colourless aqueous solutions of sodium nitrate and barium hydroxide are produced. BaCl2 + Na2SO4 ==> BaSO4 (s) + 2Na+ + 2Cl- So the net ionic equation is 2Na+ + 2Cl-. Include phases. The hydrated form is freely soluble in water, ethanol, and acetone Barium chloride R BaCl 2,2H 2 O (SRIP, 1963, p. 45). Strong acids and strong bases are considered strong electrolytes and will dissociate completely. Total Ionic Equation: Mg 2+ (aq) + 2 NO 3- (aq) + Ca 2+ (aq) + 2 Cl- (aq)--> Ca 2+ (aq) + 2 NO 3- (aq) + Mg 2+ (aq) + 2 Cl- (aq) Net Ionic Equation: No Reaction : 5. potassium sulfate and barium chloride . Aqueous sodium hydroxide reacts with aqueous copper(II) sulfate to precipitate copper(II) hydroxide. Net ionic: S 2-(aq) + Pb 2+ (aq) à PbS(s) 4. copper(II) sulfate + barium chloride. The preparation of Ba(NO3)2 by double conversion of barium chloride and sodium nitrate or calcium nitrate is described in the Eastern European patent literature. 26The net ionic equation for the combination of aqueous sodium sulfate and aqueous barium hydroxide is the same as the net ionic equation for any combination of a soluble sulfate . Ionic equation: Ag++ OH- → AgOH The reaction between sodium hydroxide and silver nitrate will form a precipitate called silver hydroxide which follows the solubility rule that most hydroxides are insoluble. 2 Strontium hydroxide Sr+2(aq) + 2 OH-(aq) Ba(OH) 2 Barium hydroxide Ba+2(aq) + 2 OH-(aq) (c) Soluble salts. Soluble salts are written as their aqueous ions: NaCl(aq) Sodium chloride Na+-(aq) + Cl (aq) K 24 SO (aq) Potassium sulfate 2 K+-(aq . net ionic equation: 2H +(aq) + SO 42-(aq) + Ba 2+(aq) + 2OH -(aq) ---> BaSO 4 (s) + 2H 2 O (l) So the net ionic equation and the ionic equaton are the same. 2. An aqueous solution of barium nitrate and an aqueous solution of sodium sulfate are mixed together. Problem #31: Write the net ionic equation for: AsCl 3 + 3H 2 O(ℓ) ---> 3HCl(aq) + As(OH) 3 (aq). b) 10.10%. ions appear in the same form and number on both sides of the equation. chloride. Solution: 2CH 3 COONa(aq) + Ba(NO 3) 2 (aq) ---> Ba(CH 3 COO) 2 (aq) + 2NaNO 3 (aq) All four substances are soluble and all ionize 100% in solution. b. aluminum oxide Al2O3. of chemical interest! Pb²⁺ (aq) + 2 OH⁻ (aq) → Pb(OH)₂ (s) Write a net ionic equation for the following situation. Magnesium chloride and sodium hydroxide; Mg2+(aq) + 2OH-(aq) --> Mg(OH)2(s) Ammonium sulfate and barium nitrate; No reaction occurs. Ba (NO3)2 + 2NaOH â†' Ba (OH)2 + 2NaNO3. So for the first example, we were given that we have potassium sulfate reacting with calcium iodine to produce a solid calcium sulfate and Equus potassium iodine. Acid-Base Neutralization Reactions In an acid-base neutralization reaction, (another type of double-replacement reaction), an acid can react with a metal hydroxide base to produce water and a salt: HCl(aq) + NaOH(aq) H 2 It is a double displacement reaction. Problem #44: (a) What is the balanced equation of sodium acetate and barium nitrate? Now cancel the ions common to each side. 1. Ch 7 Notes (Part 2). Simplest Ionic Equation for formation of Mg(OH)2 (s) Mg2+ (aq) + 2OH-(aq) Mg(OH) 2 (s). a. sodium sulfate and potassium chloride b. potassium sulfide and calcium nitrate c. sodium hydroxide and silver nitrate d. … Solutions of 0.1 M solutions of lead(II) nitrate and sodium iodide are mixed. the reaction of the alkali sodium hydroxide with ammonium salts . Barium hydroxide react with nitric acid Ba (OH) 2 + 2HNO 3 → Ba (NO 3) 2 + 2H 2 O [ Check the balance ] Barium hydroxide react with nitric acid to produce barium nitrate and water. 1. For the reaction between sodium hydroxide and acetic mountain in aqueous solution, we're asked come write: the balanced formula equation, the finish ionic equation, and also the network ionic equation. Sodium nitrate appears as a white crystalline solid. So the little acquis subscript always represents the fact that that means we have . Barium chloride and sulfuric acid Iron(II) chloride and sodium hydroxide Copper sulfate and potassium hydroxide Lead nitrate and sodium chloride Calcium chloride and sodium carbonate Aluminium nitrate and sodium hydroxide Sodium sulfate and barium nitrate SciPadpg44 Ca2+ + SO 4 2‐ CaSO 4 Ba2+ + SO 4 2‐ BaSO 4 Similarly, among the products, NaCl exist as Na+ and Cl- ions. a. HCl is a strong acid which completely dissociates in water. BaCl2 + Na2SO4 ==> BaSO4 (s) + 2Na+ + 2Cl- So the net ionic equation is 2Na+ + 2Cl-. chemistry. So for example, the dissociation equations for the soluble ionic compounds ammonium sulfate and sodium nitrate are (NH 4) 2 SO 4 (s) → 2 NH 4 + (aq) + SO 4 2− (aq) Hence, it is written in molecular form. Next, we have sodium hydroxide reacting with silver nitrate. Conclusion: NR (no reaction) Notice how the question asks you what the net . equation: (next page) However, if excess sodium hydroxide solution is added: the . For example, a molecule of PbI 2 splits into the ions Pb 2+, I-, and a second I-. a. ammonium sulfate and barium nitrate b. lead(II) nitrate and sodium chloride c. sodium phosphate and potassium nitrate d. sodium bromide and rubidium chloride e. copper(II) chloride and sodium hydroxide The ionic equations for the reaction are; Fe(NO 3) 3 ----- > Fe +3 + 3NO 3-1 NaOH ----- > Na +1 . 2NH4^+ is on both sides so cancel. Barium nitrate + sodium hydroxide â†' barium hydroxide + sodium nitrate. How to Identify Chemicals in Solution: Test Methods & Materials. When aqueous sodium hydroxide is added to a solution containing lead(II) nitrate, a solid precipitate forms. 3. 6 For the reaction between sodium carbonate (Na2CO3) and silver nitrate (AgNO3) Molecular equation: 2AgNO3 (l) + Na2CO3 (l) → Ag2CO3(s . Sodium has a plus. Ba^2+ (aq) + C2O4^2- (aq) ==> BaC2O4 (s) You do the others. Sodium nitrate is the inorganic nitrate salt of sodium. 100.0 mL of 1.0 M iron (III) nitrate is mixed with 100.0 mL of 1.0 M sodium hydroxide. AgNO 3 + KCl AgCl(ppt) + KNO 3. silver nitrate + potassium chloride silver chloride + potassium nitrate . When aqueous sodium hydroxide is added to a solution containing lead(II) nitrate, a solid precipitate forms. Ionic equation for barium chloride and sulphuric acid? sodium chloride + water + carbon dioxide, NaHCO3(s) + HCl(aq) Does a reaction occur when aqueous solutions of cobalt(II) nitrate and ammonium sulfate are combined? The answer will appear below; Always use the upper case for the first character in the element name and the lower case for the second character. Inter state form of sales tax income tax? The formula of the oxide is, therefore, Cr. 2 Strontium hydroxide Sr+2(aq) + 2 OH-(aq) Ba(OH) 2 Barium hydroxide Ba+2(aq) + 2 OH-(aq) (c) Soluble salts. check_circle. #1 is fine. However, when additional aqueous . One calcium two plus combines with one sulfide to minus to produce calcium sulfide. The reaction of Sodium hydroxide and Acetic acid (also called Ethanoic acid) represents a net ionic equation involving a strong base and a weak acid. Total-ionic - 3) Sodium ana nitrate. First, we balance the molecular equation. Supplied sulfuric acid is 2-acid hydrochloric. We deal with the problem in 4 steps: Step 1: compose the formula equation. This is the net ionic equation, showing only the ions involved in the reaction. BaCl2 + Na2SO4 ==> BaSO4 (s) + 2Na+ + 2Cl- So the net ionic equation is 2Na+ + 2Cl-. Ammonium chloride + sodium hydroxide 8. Barium and sulfate ions react to form barium sulfate precipitate, and the sodium and nitrate ions are unchanged - they are spectator ions. Barium hydroxide would easily dissolve in water. Strong acids and strong bases are considered strong electrolytes and will dissociate completely. Ba OH2 Barium hydroxide is an ionic bond What is chemical bond ionic bond covalent bond. The hydroxide ions present would make the solution strongly alkaline. Ammonium nitrate dissociates into ammonium ions and bromide ions. This means that we will split them apart in the net ionic equation. Part I: Identify the type of reaction and write a balanced chemical equation for each of the following reactions. Strong bases are considered strong electrolytes and will dissociate completely. A precipitate forms. d. aluminum hydroxide Al(OH)3. e. rubidium phosphide Rb3P. What is the net ionic equation for the acid base reaction of hydrobromic acid with sodium hydroxide? Best Answer. c. sodium sulfate Na2SO4. Net Ionic Equation Worksheet READ THIS: When two solutions of ionic compounds are mixed, a solid may form. Hydrobromic acid, #"HBr"#, is a strong acid and sodium hydroxide, #"NaOH"#, is a strong base . An aqueous solution of barium nitrate and an aqueous solution of sodium sulfate are mixed together. Balanced barium hydroxide and sodium sulfate? Identify the other sodium halide that must be present in this mixture of two sodium halides. equatbn: equatõn: 4) aM potassium Molecular H u H Total-ionic equatbn: H 6 Net-ionic equation: 5) arrvmniurn Molecular equation Ba (9) + (9 Total-ionic Net-Onic equation: 6) Potassium hydroxide and copper(ll) nitrate. Honors Chemistry Name_____ Period_____ Net Ionic Equation Worksheet READ THIS: When two solutions of ionic compounds are mixed, a solid may form. 2NO3^- is on both sides so cancel. Barium Nitrate + Potassium Carbonate . Any ammonium salt on reaction with an alkali would liberate ammonia gas. A solution of sodium hydroxide is added to a solution of lead (II) nitrate. According to our If precipitation is expected, write a balanced net ionic equation for the reaction. can u plz help me in this Select "True" or "False" to indicate whether or not the stated reaction (or "no reaction") correctly corresponds to the expected observation in each case. f. barium nitrate Ba(NO3)2. g. nickel (III) hydroxide Ni(OH)3. h. lead(IV . When sodium hydroxide was added to barium nitrate we expected a clear solution as the WACE chemistry data sheets and our MSDS for barium hydroxide indicate that it is soluble, as are all nitrates. A) NaOH(aq) + HBr(aq) → H2O(l) + NaBr(aq) B) Is sodium nitrate a solid? acetic acid + sodium hydroxide . Ammonium Chloride and Barium Hydroxide Reaction | NH 4 Cl + Ba(OH) 2. _____ _____ _____ (3) (ii) Give one reason why the silver nitrate solution was acidified before it was used in this test. precipitated as AgCl with 70.90 mL of 0.2010 M AgNO3 , what is the percentage of chloride in the sample? Barium and sulfate ions react to form barium sulfate precipitate, and the sodium and nitrate ions are unchanged - they are spectator ions. The net ionic equation for this reaction is: What you have now is the total ioinic equation. This type of reaction is called a precipitation reaction , and the solid produced in the reaction is known as the precipitate . This type of reaction is called a precipitation reaction , and the solid produced in the reaction is known as the precipitate . By convention the cation is usually written first. Barium and sulfate ions react to form barium sulfate precipitate, and the sodium and nitrate ions are unchanged - they are spectator ions. . And what is left is the Net Ionic equation. Determinations of the solubility of a salt may be made by reference to SOLUBILITIES OF IONIC COMPOUNDS. Iron (III) hydroxide Fe(OH)3 barium phosphide Ba3P2 IONIC FORMULAS PRACTICE PROBLEMS. Ba 2+ + SO 4 2− → BaSO 4. Sodium hydroxide - concentrated solution. Barium nitrate and sodium sulphate react together to form one soluble salt, sodium nitrate, and an insoluble salt, barium sulphate. 2) Barium chloride and sodium sulfate. 274. Write the simplest ionic equation for the formation of this precipitate from silver ions and the correct halide ion. **3rd is the Ionic Equation **4th is the Net Ionic Equation . Simplest Ionic Equation for formation of Mg(OH)2 (s) Mg2+ (aq) + 2OH-(aq) Mg(OH) 2 (s). The hydroxide ions present would make the solution strongly alkaline. Examples: Fe, Au, Co, Br, C, O, N, F. Compare: Co - cobalt and CO - carbon monoxide; To enter an electron into a chemical equation use {-} or e Of course, just like any other chemical equation, it must be balanced: the number of atoms of each type and the net charge on each side of the equation must be the same. The reaction will produce copper (II) hydroxide, Cu(OH)2, an insoluble ionic compound that precipitates out of solution, and aqueous sodium nitrate, NaNO3, another soluble ionic compound. Write the molecular equation, ionic equation and net ionic equation for this reaction. (ii) Sodium hydroxide solution (in water) reacts with hydrochloric acid solution (in water) to produce sodium chloride solution and water. Back to Couse Homepage. Molecular: BaCl 2 (aq) CuSO 4 (aq) à BaSO 4 (s) + CuCl 2 (aq) Net ionic: Ba 2+ (aq) + SO 4 2-(aq) à BaSO 4 (s) 5. sodium hydroxide + iron(III) nitrate. Answer (1 of 1): Chemical formulas for barium nitrate and ammonium carbonate are BA (NO3) 2 and (NH4) 2CO3. Barium stimulates striated, cardiac, and smooth muscle, regardless of . 1. Sodium carbonate + hydrochloric acid 6. hydrochloric acid + sodium CuSO4 (aq)+ 2NaOH (aq) -> Cu (OH)2 (s) + Na2SO4 (aq) Now you have to write an ionic equation which involves splitting up each compound, that is in aqueous form, into it's parts and writing the. 46. Al 2 (SO 4) 3 + 3Ba (NO 3) 2 → 3BaSO 4 + 2Al (NO 3) 3 [ Check the balance ] Aluminium sulfate react with barium nitrate to produce barium sulfate and aluminum nitrate. Barium hydroxide would easily dissolve in water. Experiment 3 Part 1 Answers: Reaction: Net Ionic Equation a) Sodium chloride and ammonium nitrate: No RXN b) Sodium chloride and silver nitrate: Ag (aq) Cl (aq) AgCl(s)+−+→ c) Sodium chloride and barium nitrate: No RXN HNO 3 + NaOH = NaNO 3 + H 2 O is a neutralization reaction . After carefully removing any sulfur formed and the heavy metals, the barium nitrate is crystallized at low temperatures. Solution: 1) Comments on each compound: AsCl 3 is a molecular compound. Sodium hydroxide is a good example of a compound with both ionic and molecular bonds because the bond between the sodium ion and hydroxide ion is ionic but the bond between the oxygen atom and. #2 you are showing the reaction between aluminum sulfate and sodium hydroxide; not aluminum bromide. (Na)2 O + H2O--> 2NaOH. #3 carbonic acid is unstable and breaks up into CO2 and H2O (H2CO3 --> H2O + CO2) #4 looks good, but Ba (Br)2 should be written as BaBr2 and you can divide your net ionic . A highly bioavailable pure liquid form of magnesium. However a white precipitate formed….Additional Information. Consider the reaction when aqueous solutions of potassium nitrate and barium hydroxide are combined. 0. There are three main steps for writing the net ionic equation for BaCl2 + NaOH = Ba (OH)2 + NaCl (Barium chloride + Sodium hydroxide). acetic acid + sodium hydroxide . This answer is . The net ionic equation for this reaction is: Consider the reaction when aqueous solutions of aluminum bromide and potassium hydroxide are . This is the complete ionic equation. 1. Aqueous potassium carbonate reacts with aqueous silver nitrate to precipitate silver carbonate. HClO 4 + KOH → KClO 4 + H 2 O Perchloric acid react with potassium hydroxide to produce potassium perchlorate and water. If we remove the unchanged ions from each side of the equation: Ba 2+ + 2 NO 3-+ 2 Na + + SO 4 2-→ BaSO 4 (s) . [Algorithmic] You mix 60.0 mL of 1.0 M silver nitrate with 25.0 mL of 0.80 M sodium. Weak acids only dissociate partially and are not . You are watching: Acetic acid and naoh net ionic equation. How long does it take to cook a 23 pound turkey in an oven? Looking at the list of acids and bases at the top of the page you can imagine ALL the possibilities. These are called net ionic equations. This is the complete ionic equation. 2 NaOH + Ba (NO 3) 2 → 2NaNO 3 + Ba (OH) 2 a) Ag⁺ (aq) 44. A white precipitate of barium sulfate forms if sulfate ions are present. What's left is the net ionic equation. Soluble salts are written as their aqueous ions: NaCl(aq) Sodium chloride Na+-(aq) + Cl (aq) K 24 SO (aq) Potassium sulfate 2 K+-(aq . Al 2 (SO 4) 3 + 3Ba (NO 3) 2 → 3BaSO 4 + 2Al (NO 3) 3 [ Check the balance ] Aluminium sulfate react with barium nitrate to produce barium sulfate and aluminum nitrate. Al2SO4 is the wrong formula for aluminum sulfate. The conventional equation for the reaction is: NH4NO3 + NaOH = NaNO3 + NH3 + H2O Here, both the reactants (NH4NO3 and NaOH) are ionic compounds, and they always exist as NH4+, NO3- ions and Na+ and OH- ions respectively in aqueous solution. . This type of reaction is called a precipitation reaction, and the solid produced in the reaction is known as the precipitate.You can predict whether a precipitate will form using a list of solubility rules such as those found in the table below. Hopefully, you can see then that potassium and nitrate are our spectator ions, which cancel from both sides of the complete Ionic equation. Ba(OH)2 (S) + aq Ba2+ (aq) + 2OH-(aq) Magnesium hydroxide is classed as insoluble in water. Step 2: Predict whether either of the possible products is water insoluble. AgNO 3 + NaOH AgOH(ppt) + NaNO 3. silver nitrate + sodium hydroxide silver hydroxide + sodium nitrate . Barium Nitrate + Potassium Carbonate . How to Write the Net Ionic Equation for BaCl2 + NaOH = Ba (OH)2 + NaCl. Write the molecular equation, ionic equation, and net ionic equation for. Balanced molecular equation (leave ionic species as molecules) Fe(NO 3) 3(aq) + 3NaOH(aq) Æ Fe(OH) 3(s) + 3NaNO 3(aq) b. A neutralization reaction, if excess sodium hydroxide the possible products is water insoluble calcium two plus with. 3. h. lead ( IV → Ag 3 PO 4 3- ( aq ) Ag... 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