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Write the balanced molecular equation, complete ionic equation, and net ionic equation for the reaction that occurs between magnesium nitrate and lithium sulfate. Write the molecular equation, complete ionic equation, and net ionic equation for the reaction between sliver nitrate and mercury (II) chloride. D) gain of oxygen, loss of mass Consider the reaction between sodium chloride (NaCl) and copper sulfate (CuSO4) in aqueous solution. Determine precipitate solubility according to solubility rules. Evaluate the axon length, myelination (or lack thereof), and the neurotransmitter used. Write a balanced chemical equation for the following reaction: Magnesium metal reacts with copper(l)chloride to give copper metal and magnesium chloride. C) potassium hypochlorite A balloon is placed over the mouth of the flask to collect the hydrogen gas that is generated. . Write the complete ionic equation, which includes all of the ions. C) MgO (s) + H2O (l) Mg(OH)2 (s) Write a balanced formula equation, complete ionic equation, and net ionic equation for the reaction that occurs between ammonium chloride and silver nitrate. >> Write the formula equation for Magnesium nitrate and sodium carbonate. Write the balanced equation for the reaction between potassium phosphate and barium chloride which forms barium phosphate and potassium chloride. /Catalog A link to the app was sent to your phone. E) 0.145 and 0.0483, A one-hundred fold dilution of an enzymatic buffer solution can be obtained by using ________. Write the balanced equation for Magnesium nitride reacting with water. A) equivalence point Write the balanced molecular equation, complete ionic equation, and net ionic equation for the reaction between aqueous solutions of iron(III) sulfate and sodium hydroxide. Sr(NO3)2(aq) + K2SO4(aq)KNO3(aq) + SrSO4(s). << R Provide the molecular equation and the net ionic equation for silver nitrate and sodium chloride. Addition of sulfurous acid (a weak acid) to barium hydroxide (a strong base) results in the formation of a precipitate. This equation represents the reaction that takes place when sodium metal is placed in water. Write the net ionic. If no reaction is expected to take place, explain why not. %PDF-1.4 What is the difference between these types of equations? Write the balanced chemical equation, write the overall ionic equation, identify the spectator ions and possible precipitates, and write the net ionic equation for: Mercury(II)chloride(aq) + Potassium sulfide(aq) ---> ____. D) potassium iodide Write the net ionic equation for the following reaction. Chemistry: Chapter 4 Quiz Flashcards | Quizlet 4 E) 2.7 10-2, How many moles of K+ are present in 343 mL of a 1.27 M solution of K3PO4? Write the balanced molecular equation, complete ionic equation, and net ionic equation for the reaction that occurs between aqueous solutions of cobalt(II) sulfate and sodium carbonate. Write the balanced molecular equation, total ionic equation, and net ionic equation for the reaction that occurs between potassium phosphate and strontium chloride. R Write the balanced molecular equation, total ionic equation, and net ionic equation for the reaction that occurs between potassium phosphate and strontium chloride. stream 0 [ This compound is ________. Water vapor reacts with sodium metal to produce solid sodium hydroxide and hydrogen gas. 0 Enter no reaction if no precipitate is formed. Write a balanced equation for the synthesis of strontium iodate monohydrate from strontium nitrate, potassium iodate, and water. obj Write the formula equation for Magnesium nitrate and lithium sulfate. 405 Write separate equations for the reactions of the solid metals magnesium, aluminum, and iron with diatomic oxygen gas to yield the corresponding metal oxides. endobj 3 A) crystallization Write the total ionic equation for Magnesium nitrate and strontium chloride. Colorful fireworks often involve the decomposition of barium nitrate and potassium chlorate and the reaction of the metals magnesium, aluminum, and iron with oxygen. What is the balanced chemical equation for the reaction of magnesium metal and silver nitrate using compound formulas? 8 B) SnCl2 (aq) + Cu (s) Sn (s) + CuCl2 (aq) /Pages /Resources The equation for this formation of ions is shown below. Write a balanced net ionic equation for the reactions that occur when the following aqueous solutions are mixed. Write the net ionic equation with correct balancing and identify the precipitate. A) a molecular compound and a weak electrolyte. 5 The chemical formula of magnesium nitrate, strontium chloride, magnesium chloride, and strontium nitrate are {eq}Mg(NO_3)_2, SrCl_2, MgCl_2, You can find out more about our use, change your default settings, and withdraw your consent at any time with effect for the future by visiting Cookies Settings, which can also be found in the footer of the site. Write the balanced molecular equation, complete ionic equation, and net ionic equation for the reaction that occurs between aqueous solutions of cobalt(II) sulfate and barium chloride. Of the species below, only ________ is not an electrolyte. C) 0.145 9 2 NaCl (aq) + CuSO4 (aq) 2 Na+ (aq) + SO42- (aq) + CuCl2 (s), The ionic form of this reaction is: 2 Na+ (aq) + 2 Cl- (aq) + Cu2+ (aq) + SO42- (aq) 2 Na+ (aq) + SO42- (aq) + CuCl2 (s). Write the molecular equation, the ionic equation, and the net ionic equation for the reaction between potassium chloride and sodium nitrate. Remove the spectator ions to produce the net ionic equation. Write the balanced molecular equation, total ionic equation, and net ionic equation for the reaction that occurs between sodium carbonate and strontium chloride. A) 125 E) 0.634, Bruce Edward Bursten, Catherine J. Murphy, H. Eugene Lemay, Matthew E. Stoltzfus, Patrick Woodward, Theodore E. Brown, Research Final Exam Presentation Questions. Write the total and net ionic equations for the reaction that occurs between aqueous solutions of silver(I) nitrate and magnesium chloride. Solid calcium carbonate is heated and decomposes to solid calcium oxide and carbon dioxide gas. Write the balanced molecular equation, total ionic equation, and net ionic equation for the reaction that occurs between sodium hydroxide and strontium chloride. (Assume the iron oxide contains Fe. D) 50.0 mL of 0.150 M solution of HCl ThoughtCo, Apr. An aqueous solution of magnesium nitrate and sodium phosphate and mixed together forming solid magnesium phosphate and aqueous sodium nitrate. D) 16.4 She has taught science courses at the high school, college, and graduate levels. When a buret is rinsed before a titration, which of the techniques below is the best procedure? Write the molecular equation, the ionic equation, and the net ionic equation for the reaction between nickel(II) chloride and silver(I) nitrate. /JavaScript >> Write the molecular equation, balanced equation, total ionic equation, and net ionic equation for the following: Sodium chloride and silver nitrate. If hydrogen ions are produced, the substance is called an acid. What is the balanced chemical equation for this reaction? Spectator ions may be either cations (positively-charged ions) or anions (negatively-charged ions). Write the balanced molecular equation for the reaction that occurs between magnesium nitrate and potassium chromate. Equal volumes of 0.2M solutions of lead(II) nitrate and potassium bromide are combined to form lead(II) bromide as a yellow precipitate. M. 1. 0 Which of the following represents the net ionic equation for the reaction? (Express your answer as a chemical equation. A) 1 part sample and 100 parts diluent Aqueous iron(III) sulfate is added to aqueous potassium chromate. Write the balanced chemical equation for silver nitrate reacting with potassium sulfate in a double replacement reaction. Which of the following represents a process in which a species is reduced? All other trademarks and copyrights are the property of their respective owners. Write the balanced molecular equation and net ionic equation for the reaction that occurs when aqueous solutions of Pb(NO3)2 and NH4Cl are mixed. Solved 07 Multiple Choice 07 The reaction between aqueous - Chegg Write the complete ionic equation to show the reaction of aqueous lead(lI) nitrate with aqueous potassium sulfate to form solid lead(I) sulfate and aqueous potassium nitrate B. 10. This highly water-soluble compound produced the foul-smelling gas H2S when the solution was acidified. Sodium carbonate + sodium hydroxide. We can tell from the formula of a salt how it can be produced. After all of the Li(s) has reacted with H2O(l), the solution in the flask is added to a clean, dry buret and used to titrate an aqueous solution of a monoprotic acid. When aqueous solutions of CaCl2 and AgNO3 are mixed, a reaction takes place producing aqueous Ca(NO3)2 and solid AgCl: [latex]{\text{CaCl}}_{2}\text{(}aq\text{)}+2{\text{AgNO}}_{3}\text{(}aq\text{)}\rightarrow\text{Ca}{\text{(}{\text{NO}}_{3}\text{)}}_{2}\text{(}aq\text{)}+2\text{AgCl(}s\text{)}[/latex]. D) 2SO2 (g) + O2 (g) 2SO3 (g) 0 H+(aq) + Cl-(aq) + K+(aq) + OH-(aq)H2O (l) + K+(aq) + Cl-(aq). Which of the following represents the net lonic equation for the reaction? Write a balanced equation for the reaction between strontium metal and water. Express your answ. b. A) atoms E) 0.215, The point in a titration at which the indicator changes is called the ________. B) KOH (aq) + HC2H3O2 (aq) H2O (l) + KC2H3O2 (aq) Molecular, complete ionic, and net ionic equations - Khan Academy /Page [ Magnesium nitrate is an ionic compound composed of magnesium ion and nitrate ion and strontium chloride is also an ionic compound composed of strontium ion and chloride ion. D) KOH (aq) + HC2H3O2 (aq) KC2H3O3 (aq) + H2 (g) Write a balanced chemical equation between magnesium chloride and sodium phosphate. 16. The net ionic equation for formation of an aqueous solution of Al(NO3)3 via mixing solid Al(OH)3 and aqueous nitric acid is ________. Write the balanced molecular equation, complete ionic equation, and net ionic equation for the reaction between aqueous solutions of sodium carbonate and barium chloride. The ionic form of this reaction is: 2 Na + (aq) + 2 Cl - (aq) + Cu 2+ (aq) + SO 42- (aq) 2 Na + (aq) + SO 42- (aq) + CuCl 2 (s) The sodium ions and sulfate ion are the spectator ions in this reaction. B) 8.60 Write the formula equation for Magnesium nitrate and strontium chloride Na2S (aq) + 2HCl (aq)2NaCl (aq) + H2S (g). Which of the following represents the net ionic equation for the reaction? What name is given to a solid that forms when two aqueous solutions are mixed? Write balanced molecular, complete ionic, and net ionic equations for this process. Write the complete ionic equation to show the reaction of aqueous lead(lI) nitrate with aqueous potassium sulfate to form solid lead(I) sulfate and aqueous potassium nitrate B. A) KOH (aq) + HC2H3O2 (aq) OH- (l) + HC2H3O2+ (aq) + K (s) /S Write the net ionic equation for the reaction of aqueous sodium chloride with aqueous silver nitrate. If no reaction occurs, write NO REACTION. D) H+ and OH- Write a balanced equation for the reaction that occurs when an aqueous solution of iron (II) chloride is mixed with an aqueous solution of potassium hydroxide. These ions exist in the same form on both sides of a chemical reaction. (E) PtCl4(s) + 2 Cl-(aq) PtCl62-(aq) Solutions - Conceptual | Chemistry Quiz - Quizizz /Type Write the balanced molecular equation and net ionic equation for the reaction between silver(I) nitrate and potassium cyanide. These notations are illustrated in the example equation here: [latex]2\text{Na(}s\text{)}+2{\text{H}}_{2}\text{O(}l\text{)}\rightarrow 2\text{NaOH(}aq\text{)}+{\text{H}}_{2}\text{(}g\text{)}[/latex]. Write a balanced equation for the precipitation reaction that occurs when aqueous solutions of potassium carbonate and chromium(II) chloride are combined. Write the net ionic equation for the reaction that occurs when aqueous nitric acid and aqueous strontium sulfide are mixed. Write the molecular equation and the net ionic equation for each of the following aqueous reactions. This net ionic equation indicates that solid silver chloride may be produced from dissolved chloride and silver(I) ions, regardless of the source of these ions. Write an overall balanced equation for the reaction that occurs when aqueous solutions of nickel(ii) chloride and potassium carbonate are combined. E) KOH (aq) + HC2H3O2 (aq) H2KC2H3O (aq) + O2 (g), B) KOH (aq) + HC2H3O2 (aq) H2O (l) + KC2H3O2 (aq), In which reaction does the oxidation number of oxygen increase? Write the molecular equation, complete ionic equation and the net equation for a reaction between silver nitrate and barium chloride solutions. Copper metal reacting with silver nitrate solution to make silver metal and copper(II) nitrate. Write the complete ionic equation for the following reaction: lithium sulfate and strontium chloride. Write the balanced equation for the reaction that occurs when an aqueous solution of iron(II) chloride is mixed with an aqueous solution of potassium hydroxide. D) Al(OH)3 (s) + 3H+ (aq) 3H2O (l) + Al3+ (aq). C) 16400 obj What is the balanced equation for magnesium chlorate = magnesium chloride + oxygen? Write the balanced molecular equation for the reaction that occurs between iron(III) chloride and silver nitrate. Our experts can answer your tough homework and study questions. Anaqueous solutionis a solution in which the solvent is water. 0 If no reaction will happen, write NR (no reaction). A) Zn (s) + 2Br- (aq) ZnBr2 (aq) () 201(aq) 2K (0) Cl(aq) +K (9) - KCI (aq). Which of the following represents the net ionic equation for the reaction? << Write the balanced molecular equation for the reaction that occurs between magnesium nitrate and potassium chromate. C) it reacts with water with great difficulty The net ionic equation for the reaction between aqueous sulfuric acid and aqueous sodium hydroxide is ________. Write the balanced molecular equation, complete ionic equation, and net ionic equation for the reaction that occurs between magnesium nitrate and lithium sulfate. Write a balanced equation for the reaction: Copper (II) Nitrate + Barium Chloride. The remaining ions are eliminated as spectator ions. (B) S8(s) + 8 O2(g) 8 SO2(g) Write a balanced chemical equation that shows the reaction that occurs when an aqueous solution of BaCl2 reacts with an aqueous solution of Na2SO4 to form aqueous sodium chloride and solid BaSO4. 1. A) 14.1 The two dissolved ionic compounds, NaOH and Na2CO3, can be represented as dissociated ions to yield the complete ionic equation: [latex]{\text{CO}}_{2}\text{(}aq\text{)}+2{\text{Na}}^{\text{+}}\text{(}aq\text{)}+2{\text{OH}}^{\text{-}}\text{(}aq\text{)}\rightarrow 2{\text{Na}}^{\text{+}}\text{(}aq\text{)}+{\text{CO}}_{3}{}^{\text{2-}}\text{(}aq\text{)}+{\text{H}}_{2}\text{O(}l\text{)}[/latex]. Write an equation for the reaction of solid silicon dioxide with hydrofluoric acid to yield gaseous silicon tetrafluoride and liquid water. E) 0.159, What volume (L) of 0.250 M HNO3 is required to neutralize a solution prepared by dissolving 17.5 g of NaOH in 350 mL of water? Write the net ionic equation for the reaction that occurs between magnesium nitrate and potassium chromate. E) mol solute/L solution. Write a balanced equation for the following: aqueous barium chloride reacts with aqueous sodium chromate to form aqueous sodium chloride and solid barium chromate. When aqueous solutions that contain ions are mixed, the ions may react in a double-replacement reaction. D) Ba(C2H3O2)2 (aq) + Na2SO4 (aq) BaSO4 (s) + 2NaC2H3O2(aq) B) dissolving 46.7 g of K2SO4 in water and diluting to a total volume of 250.0 mL Following the convention of using the smallest possible integers as coefficients, this equation is then written: [latex]{\text{Cl}}^{\text{-}}\text{(}aq\text{)}+{\text{Ag}}^{+}\text{(}aq\text{)}\rightarrow\text{AgCl(}s\text{)}[/latex]. Write a condensed equation as well as a net ionic equation for the reaction of aqueous silver nitrate with aqueous potassium chromate. C) iron No packages or subscriptions, pay only for the time you need. Write the net ionic, Write a balanced chemical equation for the following reaction. \ce {H2SO4} (aq) + \ce {2NaOH} (aq) \rightarrow \ce {2H2O} (l) + \ce {Na2SO4} (aq) HX 2SOX 4(aq) + 2NaOH(aq) 2HX 2O(l) + NaX 2SOX 4(aq) Write a balanced equation for the formation of magnesium nitride from its elements. E) Zn (s) + 2HI (aq) ZnI2(aq) + H2 (g), A) Cu (s) + 2HCl (aq) CuCl2 (aq) + H2 (g), Based on the activity series, which one of the reactions below will occur? D) Pb(NO3)2 (aq) + 2NaCl (aq) PbCl2 (s) + 2NaNO3 (aq) Hydrogen sulfide gas is produced, along with an aqueous solution of sodium chloride. B) H+, OH-, Cl-, and Ca2+ 2005 - 2023 Wyzant, Inc, a division of IXL Learning - All Rights Reserved, Drawing Cyclohexane Rings Organic Chemistry. b) Strontium nitrate and sodium sulfate. Solid aluminum metal reacts with solid diatomic iodine to form solid Al. Write a balanced chemical equation to demonstrate the reaction between an aqueous solution of silver nitrate (AgNO_3) and an aqueous solution of magnesium chloride (MgCl_2). R /Length Ionic compounds dissolved in water are, therefore, more realistically represented as dissociated ions, in this case: [latex]\begin{array}{l}{\text{CaCl}}_{2}\text{(}aq\text{)}\rightarrow{\text{Ca}}^{\text{2+}}\text{(}aq\text{)}+2{\text{Cl}}^{-}\text{(}aq\text{)}\\ 2{\text{AgNO}}_{3}\text{(}aq\text{)}\rightarrow 2{\text{Ag}}^{\text{+}}\text{(}aq\text{)}+2{\text{NO}}_{3}{}^{-}\text{(}aq\text{)}\\ \text{Ca}{\text{(}{\text{NO}}_{3}\text{)}}_{2}\text{(}aq\text{)}\rightarrow{\text{Ca}}^{\text{2+}}\text{(}aq\text{)}+2{\text{NO}}_{3}{}^{-}\text{(}aq\text{)}\end{array}[/latex]. B) 0.00155 When ionic compounds dissolve in water, they may dissociate into their constituent ions, which are subsequently dispersed homogenously throughout the resulting solution (a thorough discussion of this important process is provided in the chapter on solutions). A spectator ion is one that exists in the same form on both the reactant and product sides of a chemical reaction. Write balanced chemical, complete ionic, and net ionic equations for each of the following reactions. 0 Common abbreviations include s for solids, l for liquids, g for gases, and aq for substances dissolved in water (aqueous solutions, as introduced in the preceding chapter). Write the balanced chemical equation for the reaction that occurs between silver nitrate and barium chloride. These spectator ionsions whose presence is required to maintain charge neutralityare neither chemically nor physically changed by the process, and so they may be eliminated from the equation to yield a more succinct representation called a net ionic equation: [latex]\begin{array}{c}\cancel{{\text{Ca}}^{\text{2+}}\text{(}aq\text{)}}+2{\text{Cl}}^{-}\text{(}aq\text{)}+2{\text{Ag}}^{\text{+}}\text{(}aq\text{)}+\cancel{2{\text{NO}}_{3}{}^{\text{-}}\text{(}aq\text{)}}\rightarrow\cancel{{\text{Ca}}^{\text{2+}}\text{(}aq\text{)}}+\cancel{2{\text{NO}}_{3}{}^{-}\text{(}aq\text{)}}+2\text{AgCl(}s\text{)}\\ 2{\text{Cl}}^{-}\text{(}aq\text{)}+2{\text{Ag}}^{\text{+}}\text{(}aq\text{)}\rightarrow 2\text{AgCl(}s\text{)}\end{array}[/latex]. Does a precipitate form, and if so, what is it? Be sure to include the water in the formula for strontium iodate monohydrate. Write a molecular equation for the precipitation reaction that occurs (if any) when the following solutions are mixed. The solid magnesium hydroxide is added to a hydrochloric acid solution, producing dissolved magnesium chloride and liquid water. C) 1.75 35,000 worksheets, games, and lesson plans, Marketplace for millions of educator-created resources, Spanish-English dictionary, translator, and learning, Diccionario ingls-espaol, traductor y sitio de aprendizaje, a Question E) 375, A weak electrolyte exists predominantly as ________ in solution. In the laboratory you dissolve 21.4 g of potassium fluoride in a volumetric flask and add water to a total volume of 500. be What is the molarity of the solution? << /Names Write a balanced chemical equation for each step of the process. D) 3Hg (l) + 2Cr(NO3)3 (aq) 3Hg(NO3)2 + 2Cr (s) C) KOH (aq) + HC2H3O2 (aq) H2C2H3O3 (aq) + K (s) Write the net ionic equation for Sodium phosphate and Strontium Nitrate. [latex]{\text{CaCO}}_{3}\text{(}s\text{)}\stackrel{\Delta}{\rightarrow}\text{CaO(}s\text{)}+{\text{CO}}_{2}\text{(}g\text{)}[/latex]. Write complete ionic equation to show the reaction of aqueous Hg_2(NO_3)_2 with aqueous sodium chloride to form solid Hg_2Cl_2 and aqueous sodium nitrate. obj Sr2+(aq)+SO42(aq)SrSO4(s) Students also viewed AP Chem Units 3-4 18 termsImages TARYN_WRIGHT Also write the ionic equation and the net ionic equation. - Definition & Examples. 5, 2023, thoughtco.com/definition-of-spectator-ion-and-examples-605675. Write the balanced equation for the reaction that occurs when aqueous hydrobromic acid is added to a solution of ammonium sulfide. For example, the gaseous molecular compound hydrogen chloride (HCl) forms H and Cl ions in aqueous solution, which is called hydrochloric acid. The balanced reaction between aqueous potassium hydroxide and aqueous acetic acid is ________. Write the molecular, complete ionic, and net ionic equations for the reaction that occurs between magnesium nitrate and calcium chloride. The given reaction is an example of a double-replacement reaction in which strontium sulfide {eq}\rm (SrS) Which of the following represents the net lonic equation for the reaction? Dr. Helmenstine holds a Ph.D. in biomedical sciences and is a science writer, educator, and consultant. 2 B) loss of oxygen, gain of electrons /Parent D) 0.207 They appear unchanged in both the product and reactant side of the equation. Label the oxidation number for each atom in the balanced chemical equation. All of the following are true concerning 2.00 L of 0.100 M solution of Ca3(PO4)2 except for ________. D) mol solute/kg solvent D) 0.070 Write balanced molecular, complete ionic, and net ionic equations for this process. Solid sodium fluoride is added to an aqueous solution of ammonium formate. Does a precipitate form, and if so, what is it? Hydrogen fluoride will also react with sand (silicon dioxide). Write the balanced equation for the reaction that occurs between barium chloride and sodium sulfate. a. hydrochloric acid and aqueous sodium cyanide, with production of hydrogen cyanide gas (HCN), b. sulfuric acid (H2SO4) and aqueous rubidium sulfide, with production of hydrogen sulfide gas. From the balanced molecular equations, write the complete ionic and net ionic equations for the following: [latex]{\text{K}}_{2}{\text{C}}_{2}{\text{O}}_{4}\text{(}aq\text{)}+\text{Ba}{\text{(OH)}}_{2}\text{(}aq\text{)}\rightarrow 2\text{KOH(}aq\text{)}+{\text{BaC}}_{2}{\text{O}}_{2}\text{(}s\text{)}[/latex], [latex]{\text{Pb(NO}}_{3}{\text{)}}_{2}\text{(}aq\text{)}+{\text{H}}_{2}{\text{SO}}_{4}\text{(}aq\text{)}\rightarrow{\text{PbSO}}_{4}\text{(}s\text{)}+2{\text{HNO}}_{3}\text{(}aq\text{)}[/latex], [latex]{\text{CaCO}}_{3}\text{(}s\text{)}+{\text{H}}_{2}{\text{SO}}_{4}\text{(}aq\text{)}\rightarrow{\text{CaSO}}_{4}\text{(}s\text{)}+{\text{CO}}_{2}\text{(}g\text{)}+{\text{H}}_{2}\text{O(}l\text{)}[/latex], [latex]{\text{CaCO}}_{3}\text{(}s\text{)}\rightarrow\text{CaO(}s\text{)}+{\text{CO}}_{2}\text{(}g\text{)}[/latex], [latex]2{\text{C}}_{4}{\text{H}}_{10}\text{(}g\text{)}+13{\text{O}}_{2}\text{(}g\text{)}\rightarrow 8{\text{CO}}_{2}\text{(}g\text{)}+10{\text{H}}_{2}\text{O(}g\text{)}[/latex], [latex]{\text{MgC1}}_{2}\text{(}aq\text{)}+2\text{NaOH(}aq\text{)}\rightarrow\text{Mg}{\text{(OH)}}_{2}\text{(}s\text{)}+2\text{NaCl(}aq\text{)}[/latex], [latex]2{\text{H}}_{2}\text{O(}g\text{)}+2\text{Na(}s\text{)}\rightarrow 2\text{NaOH(}s\text{)}+{\text{H}}_{2}\text{(}g\text{)}[/latex], [latex]2{\text{KClO}}_{3}\text{(}s\text{)}\rightarrow 2\text{KCl(}s\text{)}+3{\text{O}}_{2}\text{(}g\text{)}[/latex], [latex]2\text{Ba}{\text{(}{\text{NO}}_{3}\text{)}}_{2}\text{(}s\text{)}\rightarrow 2\text{BaO(}s\text{)}+2{\text{N}}_{2}\text{(}g\text{)}+5{\text{O}}_{2}\text{(}g\text{)}[/latex], [latex]\begin{array}{l}2\text{Mg(}s\text{)}+{\text{O}}_{2}\text{(}g\text{)}\rightarrow 2\text{MgO(}s\text{)}\\ 4\text{Al(}s\text{)}+3{\text{O}}_{2}\text{(}g\text{)}\rightarrow 2{\text{Al}}_{2}{\text{O}}_{3}\text{(}g\text{)}\\ 4\text{Fe(}s\text{)}+3{\text{O}}_{2}\text{(}g\text{)}\rightarrow 2{\text{Fe}}_{2}{\text{O}}_{3}\text{(}s\text{)}\end{array}[/latex], [latex]4\text{HF(}aq\text{)}+{\text{SiO}}_{2}\text{(}s\text{)}\rightarrow{\text{SiF}}_{4}\text{(}g\text{)}+2{\text{H}}_{2}\text{O(}l\text{);}[/latex], complete ionic equation: [latex]2{\text{Na}}^{\text{+}}\text{(}aq\text{)}+2{\text{F}}^{\text{-}}\text{(}aq\text{)}+{\text{Ca}}^{\text{2+}}\text{(}aq\text{)}+2{\text{Cl}}^{\text{-}}\text{(}aq\text{)}\rightarrow\text{Ca}{\text{F}}_{2}\text{(}s\text{)}+2{\text{Na}}^{\text{+}}\text{(}aq\text{)}+2{\text{Cl}}^{\text{-}}\text{(}aq\text{),}[/latex] net ionic equation: [latex]2{\text{F}}^{\text{-}}\text{(}aq\text{)}+{\text{Ca}}^{\text{2+}}\text{(}aq\text{)}\rightarrow{\text{CaF}}_{2}\text{(}s\text{)}[/latex], [latex]\begin{array}{l}{}2{\text{K}}^{\text{+}}\text{(}aq\text{)}+{\text{C}}_{2}{\text{O}}_{4}{}^{\text{2-}}\text{(}aq\text{)}+{\text{Ba}}^{\text{2+}}\text{(}aq\text{)}+2{\text{OH}}^{\text{-}}\text{(}aq\text{)}\rightarrow 2{\text{K}}^{\text{+}}\text{(}aq\text{)}+2{\text{OH}}^{\text{-}}\text{(}aq\text{)}+{\text{BaC}}_{2}{\text{O}}_{4}\text{(}s\text{)}\text{(complete)}\\ {\text{Ba}}^{\text{2+}}\text{(}aq\text{)}+{\text{C}}_{2}{\text{O}}_{4}{}^{\text{2-}}\text{(}aq\text{)}\rightarrow{\text{BaC}}_{2}{\text{O}}_{4}\text{(}s\text{)}\text{(net)}\end{array}[/latex], [latex]\begin{array}{l}{\text{Pb}}^{\text{2+}}\text{(}aq\text{)}+2{\text{NO}}_{3}{}^{\text{-}}\text{(}aq\text{)}+2{\text{H}}^{+}\text{(}aq\text{)}+{\text{SO}}_{4}{}^{\text{2-}}\text{(}aq\text{)}\rightarrow{\text{PbSO}}_{4}\text{(}s\text{)}+2{\text{H}}^{\text{+}}\text{(}aq\text{)}+2{\text{NO}}_{3}{}^{\text{-}}\text{(}aq\text{)}\text{(complete)}\\ {\text{Pb}}^{\text{2+}}\text{(}aq\text{)}+{\text{SO}}_{4}{}^{\text{2-}}\text{(}aq\text{)}\rightarrow{\text{PbSO}}_{4}\text{(}s\text{)}\text{(net)}\end{array}[/latex], [latex]\begin{array}{l}{}{\text{CaCO}}_{3}\text{(}s\text{)}+2{\text{H}}^{\text{+}}\text{(}aq\text{)}+{\text{SO}}_{4}{}^{\text{2-}}\text{(}aq\text{)}\rightarrow{\text{CaSO}}_{4}\text{(}s\text{)}+{\text{CO}}_{2}\text{(}g\text{)}+{\text{H}}_{2}\text{O(}l\text{)}\text{(complete)}\\ {\text{CaCO}}_{3}\text{(}s\text{)}+2{\text{H}}^{\text{+}}\text{(}aq\text{)}+{\text{SO}}_{4}{}^{\text{2-}}\text{(}aq\text{)}\rightarrow{\text{CaSO}}_{4}\text{(}s\text{)}+{\text{CO}}_{2}\text{(}g\text{)}+{\text{H}}_{2}\text{O(}l\text{)}\text{(net)}\end{array}[/latex].