magnesium and iron nitrate equation

4.4: Oxidation-Reduction Reactions is shared under a CC BY-NC-SA 3.0 license and was authored, remixed, and/or curated by LibreTexts. It only takes a minute to sign up. The nitrate compounds are generally soluble in water. Magnesium nitrate is also known as magniosan, magnesium dinitrate or Nntromagnesite. The nitrate compounds tend to form a flammable mixture when it is combined with the hydrocarbons. When iron is exposed to air in the presence of water, for example, the iron turns to rustan iron oxide. Mandatory experiment 1.2 - Redox reactions of group VII elements - halogens as oxidising agents (reactions with bromides, iodides, Fe and sulfites). Thanks for contributing an answer to Chemistry Stack Exchange! Assigning oxidation states allows us to see that there has been a net transfer of electrons from hydrogen (0 +1) to copper (+1 0). Differentiated worksheets guide learners to consider word equations, symbol equations and conservation of mass linked to simple decomposition reactions, Introduce your students to some applications ofdecomposition reactions: clean energy, bleach and baking, Use this fresh, fast approach to demonstratethe colourful oxidation states of vanadium, Practical experiment where learners produce gold coins by electroplating a copper coin with zinc, includes follow-up worksheet. 1. barium chloride + sodium sulfate metathesis BaCl2 + Na2SO4 2NaCl + BaSO4 2. calcium + hydrochloric acid replacement Ca + 2HCl H2 + Ca Cl2 3. iron ( II) sulfide + hydrochloric acid hydrogen sulfide (g) + metathesis Example $\PageIndex{2}$ demonstrates how a familiarity with the activity series allows you to predict the products of many single-displacement reactions. It can also be prepared by mixing the magnesium sulfate, also known as Epsom salt with calcium nitrate. Watch on. Asking for help, clarification, or responding to other answers. The metals at the top of the series, which have the greatest tendency to lose electrons, are the alkali metals (group 1), the alkaline earth metals (group 2), and Al (group 13). To identify oxidationreduction reactions in solution. WebIdentify the type of reaction and write a balanced chemical equation for each of the following reactions. For a neutral compound, one Fe+3 is needed for every 3 Cl-1 The formula of the compound is FeCl3. If we add the two reactions together, we get an effective reaction: $$\ce{Mg + Zn^2+ + Zn + Cu^2+ -> Mg^2+ + Zn + Zn^2+ + Cu}$$. Observe andrecord your observations. Zinc powder, Zn(s) see CLEAPSS HazcardHC107. We can balance oxidationreduction reactions in solution using the oxidation state method (Table $\PageIndex{1}$), in which the overall reaction is separated into an oxidation equation and a reduction equation. Both carbonic acid and sulfurous acid are unstable and will decompose to form carbon dioxide and sulfur dioxide gases, respectively: sulfuric acid + aqueous lithium hydroxide. If you determine that a reaction will not occur, write no reaction after the arrow. cation = iron (III) = Fe+3 anion = chloride = Cl-1 The basic rules for writing names of ionic compounds: 1. Both types of reactions are called single-displacement reactions, in which the ion in solution is displaced through oxidation of the metal. In any chemical reaction, the net charge must be conserved; that is, in a chemical reaction, the total number of electrons is constant, just like the total number of atoms. In any redox reaction, the total number of electrons lost must equal the total of electrons gained to preserve electrical neutrality. What were the poems other than those by Donne in the Melford Hall manuscript? Hydrogen is included in the series, and the tendency of a metal to react with an acid is indicated by its position relative to hydrogen in the activity series. In the formation of Al2O3, electrons are transferred as follows (the small overset number emphasizes the oxidation state of the elements): \[ 4 \overset{0}{\ce{Al}} + 3 \overset{0}{\ce{O2}} \rightarrow \ce{4 Al^{3+} + 6 O^{2-} }\label{4.4.3} \]. The best answers are voted up and rise to the top, Not the answer you're looking for? Another process would be by mixing the anhydrous calcium or barium nitrate that is dissolved in anhydrous methanol or ethanol, with anhydrous magnesium sulfate. For every oxidation, there must be an associated reduction. Galvanic cell involving a hydrogen electrode and copper electrode in sodium hydroxide. We have grown leaps and bounds to be the best Online Tuition Website in India with immensely talented Vedantu Master Teachers, from the most reputed institutions. Active metals lie at the top of the activity series, whereas inert metals are at the bottom of the activity series. Always name the cation first, then the anion. Fe3+ (aq) + 3OH- (aq) ----> Fe (OH)3 (s) Salts of alkali metals and ammonia Soluble Exceptions: some lithium compounds Be especially cautious when using the 6M HCl, 3M H2SO4 and 6M NaOH as they can burn your skin. So what's the answer? In fact, Fe3O4 can be viewed as having two Fe3+ ions and one Fe2+ ion per formula unit, giving a net positive charge of +8 per formula unit. So the oxidation state of oxygen is +2 in OF2 but in KO2. Add two drops of copper(II) sulfate solution to each metal in the first column. Mg (s) + 2 HNO3 (aq) --> H2 (g) + Mg(NO3)2 (aq). Be sure to include the physical states of all reactants and products in your final equation. Due to the hygroscopic nature, Magnesium nitrate is used as a desiccant. In the preparation of nitric acid, it is used as a dehydrating agent. It is used in fertilizers too. Magnesium nitrate is used in hair conditioning products. It is used in preservatives and antioxidants. WebThe formula of magnesium nitrate is Mg (NO3)2. Thus the sum of the oxidation states of the two carbon atoms is indeed zero. Making statements based on opinion; back them up with references or personal experience. Hence, heating it would result to decomposition of magnesium oxide, oxygen, and nitrogen oxides. This gives us: Each neutral aluminum atom loses three electrons to produce an aluminum ion with an oxidation state of +3 in the product, so aluminum has been oxidized. How much is a biblical shekel of silver worth in us dollars? Did Billy Graham speak to Marilyn Monroe about Jesus? Mg(NO3)2 is a type of an inorganic nitrate salt of the element magnesium that has a chemical name magnesium nitrate. feasible redox reactions), the reaction with the least potential difference takes place (since $1.51 0.19 < 1.51 0.05$). \ce{MnO4- & Mn^2+} & \pu{1.51 V} \\ When exposed to air, aluminum metal develops a continuous, transparent layer of aluminum oxide on its surface. To learn more, see our tips on writing great answers. H2SO4 + MgO ---> H2O + MgSO4 .This is a balanced equation . Accessibility StatementFor more information contact us atinfo@libretexts.org. Equation $\ref{4.4.1}$ and Equation $\ref{4.4.2}$ are examples of oxidationreduction (redox) reactions. Review: Chemical Formulas and Names of Ionic Compounds What time does normal church end on Sunday? Experimentally, it is found that zinc reacts with both copper salts and silver salts, producing $\ce{Zn2+}$. Balancing Strategies: In this single displacement reaction the Mg replaces the H in the HNO3. \end{align}. I wonder if an answer could be in antioxidant in the body. Ionic compounds are formed when positive cations and negative anions are attracted to each. There are many types of redox reactions. Certain metals are oxidized by aqueous acid, whereas others are oxidized by aqueous solutions of various metal salts. The resources originally appeared in the bookMicroscale chemistry: experiments in miniature, published by the Royal Society of Chemistry in 1998. When using the activity series to predict the outcome of a reaction, keep in mind that any element will reduce compounds of the elements below it in the series. Locate the reactants in the activity series in Figure $\PageIndex{4}$ and from their relative positions, predict whether a reaction will occur. What is the median age of the following 36 27 31 35 22 28 27 34 30 21 23? Examine the reactions between various metals and metal salt solutions in this class practical. 2Fe(aq) + 6e 2Fe(s), Educator app for Therefore, the overall reaction seems to be one where ethanol only reacted with permanganate to only form ethanal, while in fact ethanoic acid was formed, but in the end the equilibrium favoured ethanal. iPad. It is also used for helping in the process of ammonium nitrate for the coating and prilling. Hence fluorine provides a reference for calculating the oxidation states of other atoms in chemical compounds. Aqueous sodium carbonate + cobalt(II) nitrate, 8. decompose) which decomposes into Magnesium and Oxygen. Identify the reaction type precipitation, neutralization or gas forming. Now how does this differ from the ethanol case? Displacement reactions of metals (Zn with Cu, Mg with Cu). WebThe equation can be rewritten without them: Mg (s) + Cu2+(aq) Mg2+(aq) + Cu (s) This equation is an example of a balanced ionic equation. The oxidation state of fluorine in chemical compounds is always 1. For example, metallic zinc reacts with iron salts, and metallic copper reacts with silver salts. Was Aristarchus the first to propose heliocentrism? \end{array}. \tag{anode} \ce{Cu &-> Cu^2+ + 2e-} & (E_0 &= +0.34)\\ Example 1: aqueous lead (II) nitrate + aqueous sodium chloride. In these reactions one of the products (AD or CB) after the double replacement is in the gaseous state, such as hydrogen sulfide (H2S) or ammonia (NH3). Nitrogen gas and bromide ions are formed. Can the game be left in an invalid state if all state-based actions are replaced? Who makes the plaid blue coat Jesse stone wears in Sea Change? Identify all of the phases in your answer. This must be balanced by the positive charge on three iron atoms, giving an oxidation state of +8/3 for iron: Fractional oxidation states are allowed because oxidation states are a somewhat arbitrary way of keeping track of electrons. If metals want to "lose" electrons, then why will copper ions take electrons from a zinc electrode? The equation for this reaction is:, The reaction between solid silicon dioxide and Write equations for any reactions that you observe. \begin{align} What is the balanced equation for magnesium metal and iron III nitrate? Magnesium dinitrate is a type of hygroscopic and crystalline solid which is white in colour. Add two drops of magnesium nitrate solution to each metal in the second column. Determine products of redox-reaction (KMnO4) by Standard electrode potential. In NaCl, for example, Na has an oxidation state of +1 and Cl is 1. Single-displacement reactions are reactions of metals with either acids or another metal salt that result in dissolution of the first metal and precipitation of a second (or evolution of hydrogen gas). Aqueous sodium phosphate + aqueous copper(II) sulfate, 7. I do not point out that the solid AgNO 3 is not the aqueous solution mentioned earlier. The predicted products are water and lithium sulfate. Any metal will reduce metal ions below it in the activity series. Swallowing larger doses of this may result in weakness, dizziness, vomiting, bloody diarrhoea, abdominal pain, and convulsions. 3Mg(s) 3Mg(aq) + 6e (I am aware that a reaction may or may not be feasible as redox, and this is according the reduction potential of the two half-equations), \begin{array}{l|l|r} Use IUPAC nomenclature rules to write the chemical formula or the chemical name. \ce{Cu + Mg^2+ &-> Mg + Cu^2+}\\ Then use a seed crystal for obtaining crystals of the compound and then remove the excess water using a vacuum. Magnesium is a metal with a very low electronegativity, It is highly soluble in water and ethanol and it occurs naturally in the caverns and mines. thermit reaction), Unit 2: Further Chemical Reactions, Rates and Equilibrium, Calculations and Organic Chemistry. Lead(II) sulfate is the white solid that forms on corroded battery terminals. Example: Fe {3+} + I {-} = Fe {2+} + I2 Substitute immutable groups in chemical compounds to avoid ambiguity. Magnesium nitrate is often used in the pyrotechnics and in the manufacturing of the concentrated nitric acid in which it extracts water and the concentrates of the acid vapors to 90 to 95 percent HNO3. The change in Gibbs free energy- given by the expression $-nFE_0$, is thus positive for this reaction, implying that it is not feasible - i.e. The chemical formula for magnesium peroxide is MgO2. Iron also reacts but the change is not so clear. Because each carbon atom has a different set of atoms bonded to it, they are likely to have different oxidation states. The numbers of each element present in the compound become subscripts in the chemical formula. 2MgO --> 2Mg + 02. the chemical equation between magnesium sulfate and water can be given as below . The physics of restoration and conservation, RSC Yusuf Hamied Inspirational Science Programme, How to prepare for the Chemistry Olympiad, guidance on apparatus and techniques for microscale chemistry. \end{array}. In contrast, the metals at the bottom of the series, which have the lowest tendency to be oxidized, are the precious metals or coinage metalsplatinum, gold, silver, and copper, and mercury, which are located in the lower right portion of the metals in the periodic table. Rule 6 states that the sum of the oxidation states in a molecule or formula unit must equal the net charge on that compound. First, the full When all the pieces of metal are in place: The zinc granules and magnesium ribbon rapidly darken in copper sulfate solution as they becomecovered with a layer of copper. WebWrite balanced net ionic equations for the following reactions in acid solution. $\ce{Mg^2+}$ will undergo a redox reaction with both the species. Since one of the predicted products is insoluble, a precipitation reaction is will occur. Product Names & States (if none, why not? other via strong electrostatic forces. Copper turnings see CLEAPSS HazcardHC026. Also be aware that skin discoloration will result from contact with AgNO3. The $E_0$ of the net reaction is $E(\text{cathode})-E(\text{anode})$ which turns out to be negative. For example, it has been proposed that one factor that contributed to the fall of the Roman Empire was the widespread use of lead in cooking utensils and pipes that carried water. What is wrong with reporter Susan Raff's arm on WFSB news? When solid copper(I) oxide is heated with hydrogen, for example, its mass decreases because the formation of pure copper is accompanied by the loss of oxygen atoms as a volatile product (water vapor). Most phosphates, carbonates, chromates and sulfides are insoluble (except those of the alkali metals and ammonium). Asked for: overall reaction and net ionic equation, \[ \ce{ Al(s) + 3Ag^+(aq) \rightarrow Al^{3+}(aq) + 3Ag(s)} \nonumber \]. However, we can still assign oxidation states to the elements involved by treating them as if they were ionic (that is, as if all the bonding electrons were transferred to the more attractive element). The practical should take approximately 20 minutes. reaction. Identify the spectator ions and write a balance net ionic equation for the reaction. One of the products could also be carbonic acid (H2CO3) or sulfurous acid (H2SO3). Identify all of the phases in your answer. WebThe chemical formula for Magnesium Nitrate is Mg (NO 3) 2. This means that each Cu atom in Cu2O must have a charge of +1: 2(+1) + (2) = 0. By adding nitric acid to magnesium oxide, hydroxide or carbonate it will give you magnesium nitrate. Magnesium is a metal with a very low electronegativity, and only Oxygen is normally assigned an oxidation state of 2 in compounds, with two exceptions: in compounds that contain oxygenfluorine or oxygenoxygen bonds, the oxidation state of oxygen is determined by the oxidation states of the other elements present. Perhaps this explains why the Roman Emperor Caligula appointed his favorite horse as consul! In the presence of these acids, lead dissolves: \[ \ce{Pb(s) + 2H^+(aq) \rightarrow Pb^{2+}(aq) + H_2(g) } \label{4.4.83} \]. Inform your instructor of any chemical contact as soon as possible. Magnesium Includes kit list and safety instructions. As a result, the oxygen atoms acquire a negative charge and form oxide ions (O2). Magnesium can do a redox reaction with C u X 2 + as well as with Z n X 2 +, since Mg has the lowest reduction potential E 0. The oxidation state of an atom in any pure element, whether monatomic, diatomic, or polyatomic, is zero. The six fluorine atoms in sulfur hexafluoride give a total negative charge of 6. Magnesium and zincreact with the iron(III) nitrate, the solution gradually darkens. Also, the nitrate products are known to be the oxidizing agents. The outcome of these reactions can be predicted using the activity series (Figure $\PageIndex{4}$), which arranges metals and H2 in decreasing order of their tendency to be oxidized. \begin{align} It is widely used in the field of pyrotechnics. Nitrates are the excellent precursors for the production of the ultra-high purity compounds and a certain catalyst and the nanoscale materials. From rule 4, hydrogen in H2O has an oxidation state of +1, and from rule 5, oxygen in both Cu2O and H2O has an oxidation state of 2. Remember that oxidation states are useful for visualizing the transfer of electrons in oxidationreduction reactions, but the oxidation state of an atom and its actual charge are the same only for simple ionic compounds. The predicted products are carbonic acid and sodium nitrate. Zinc metal plus copper II nitrate yields zinc nitrate plus The carbon atom of the methyl group (CH3) is bonded to three hydrogen atoms and one carbon atom. Which was the first Sci-Fi story to predict obnoxious "robo calls"? Determine the formulas and charges on the cation and anion involved in the compound. copper balanced equation? Pairwise reactions of this sort are the basis of the activity series (Figure $\PageIndex{4}$), which lists metals and hydrogen in order of their relative tendency to be oxidized. Skip to main content Skip to navigation Mast navigation Register Sign In Search our site All What is the mean for 21 23 27 28 32 32 34 43. \ce{Zn^2+ & Zn} &\pu{-0.76 V} \\ The sum of the oxidation states of all the atoms in a neutral molecule or ion must equal the charge on the molecule or ion. It can be split into two half equations: Once again, the number of electrons lost equals the number of electrons gained, and there is a net conservation of charge: \[ \text{electrons lost} = 2 \, H \, \text{atoms} \times {1 \, e^- \, \text{lost} \over H \, \text{atom} } = 2 \, e^- \, \text{lost} \label{4.4.6a} \], \[ \text{electrons gained} = 2 \, Cu \, \text{atoms} \times {1 \, e^- \, \text{gained} \over Cu \, \text{atom}} = 2 \, e^- \, \text{gained} \label{4.4.6b} \]. WebPlace an iron nail in each box in the iron row. How to Balance Mg + O2 = MgO (Magnesium plus Oxygen Gas) Share. Read our standard health and safety guidance. The nitrate compounds are generally soluble in water. Filter off the insoluble calcium sulfate from this mixture for obtaining a solution of Mg(NO3)2. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. Because rule 1 requires that the sum of the oxidation states of all atoms be zero in a neutral molecule (here SF6), the oxidation state of sulfur must be +6: [(6 F atoms)(1)] + [(1 S atom) (+6)] = 0. b. )copper (II) chloride and magnesium sulfide Express your answer as a chemical equation. Place an iron nail in each box in the iron row. (located at the top of the series) and which are inert metals, which have the least tendency to be oxidized. Oxidationreduction reactions are balanced by separating the overall chemical equation into an oxidation equation and a reduction equation. Zinc powderis FLAMMABLE and hazardous to the aquatic environment. Using the activity series, predict what happens in each situation. the chemical symbols are Magnesium mg iron nitrate Magnesiun nitrate iron Fe thankies? Write balanced chemical equations for each double replacement reaction studied. Thus, this is a redox reaction. 3[Mg(s) Mg(aq) + 2e] In this article, we will learn about magnesium nitrate, the magnesium nitrate formula, use of magnesium nitrate, the magnesium nitrate structure, and the health hazards of magnesium nitrate. Originally, the term reduction referred to the decrease in mass observed when a metal oxide was heated with carbon monoxide, a reaction that was widely used to extract metals from their ores. Example 6: Name the ionic compound Al(NO3)3. Assign oxidation states to all atoms in each compound. For instance equation C6H5C2H5 + O2 = C6H5OH + CO2 + H2O will not be balanced, (a) Liquid hydrazine reacts with an aqueous solution of sodium bromate. What will be the reaction between tin (II) chloride and copper (II) chloride? When a double replacement reaction occurs, the cations and anions switch partners, resulting in the formation of water and a new ionic compound (or salt), which is usually soluble. So, in response to your question - $\ce{Mg^2+}$ will participate in a redox reaction with both the species in which $\ce{Mg}$ gets oxidized while simultaneously reducing the other species. 2.1.4 explain and describe the displacement reactions of metals with other metal ions in solution; Unit C2: Further Chemical Reactions, Rates and Equilibrium, Calculations and Organic Chemistry. In this case, the nitrate ions are spectator ions and are not involved in the reaction. WebStudy with Quizlet and memorize flashcards containing terms like During photosynthesis plants use carbon dioxide and water to make glucose and release oxygen. The basic rules for writing the chemical formulas of ionic compounds: total charge of all the positive cations must equal the total charge of all the negative anions in the compound. They are usually due to the presence of two or more atoms of the same element with different oxidation states. Each neutral oxygen atom gains two electrons and becomes negatively charged, forming an oxide ion; thus, oxygen has an oxidation state of 2 in the product and has been reduced. Atoms in their elemental form, such as O2 or H2, are assigned an oxidation state of zero. Do you have pictures of Gracie Thompson from the movie Gracie's choice. The oxidation state of each atom in a compound is the charge an atom would have if all its bonding electrons were transferred to the atom with the greater attraction for electrons. Therefore, these reactions are known as oxidation-reduction reactions, or "redox" reactions for short. The same pattern is seen in all oxidationreduction reactions: the number of electrons lost must equal the number of electrons gained. A widely encountered class of oxidationreduction reactions is the reaction of aqueous solutions of acids or metal salts with solid metals. Rule 1 states that atoms in their elemental form have an oxidation state of zero, which applies to H2 and Cu. To determine whether a product ionic compound will be soluble or insoluble, consult the Solubility Rules provided at the end of the Background section. For NH4+, hydrogen has an oxidation state of +1 (rule 4), so nitrogen must have an oxidation state of 3: [(4 H atoms)(+1)] + [(1 N atom)(3)] = +1, the charge on the NH4+ ion. Assigning oxidation states to the elements in binary ionic compounds is straightforward: the oxidation states of the elements are identical to the charges on the monatomic ions. What time does normal church end on Sunday? Identify the products formed in each of these reactions. Can you still use Commanders Strike if the only attack available to forego is an attack against an ally? Yes, zinc and copper can react according to the well-known and often-displayed electrochemical reaction (depositing copper on a blank piece of zinc metal). MgO + 2HNO 3 Mg (NO 3) 2 + H 2 O [ Check the balance ] Magnesium react with nitric acid to produce nitrate magnesium and water. \begin{array}{l|l|r} If total energies differ across different software, how do I decide which software to use? What you'll find is that the half reaction of $\ce{Mg^2+}$ has a highly negative electrode potential $-2.37$ while the $\ce{Zn^2+}$ and $\ce{Cu^2+}$ half reactions have less negative $E_0$ values [$-0.76$ and $0.34$ respectively]. Nitrate compounds are usually dissolved in water. By a reaction analogous to the reverse Cannizarro reaction, these can comproportionate: $$\ce{CH3CH2OH + CH3COOH <=>> 2 CH3CHO}$$. Students should observe nochange between any of the metals and a salt solution of the same metal. \ce{CH3CHO & CH3CH2OH} & \pu{0.19 V} \\ \ce{Mg^2+ & Mg} &\pu{-2.37V} \\ 2. When all the pieces of metal are in place: Add two drops of copper(II) sulfate solution to each metal in the first column. Alkali metal compounds, acetates, nitrates, and ammonium compounds are all soluble. The predicted products are lead (II) chloride (insoluble) and sodium nitrate (soluble). For a neutral compound, three Mg+2 are needed for every 2 PO4 -3 The formula of the compound is Mg3(PO4)2. Zinc therefore has a greater tendency to be oxidized than does iron, copper, or silver. Hydrochloric acid + solid sodium bicarbonate, 4. 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. You notice that the zinc is little more than a spectator ion. Magnesium nitrate refers to inorganic compounds with the formula Mg (NO 3) 2 (H 2 O) x, where x = 6, 2, and 0. All are white solids. [2] The anhydrous material is hygroscopic, quickly forming the hexahydrate upon standing in air. All of the salts are very soluble in both water and ethanol . Aqueous iron (III) chloride + aqueous ammonium hydroxide, 5. \tag{anode} \ce{Cu &-> Cu^2+ + 2e-} & (E_0 &= +0.34)\\ Aqueous nickel(II) nitrate + aqueous sodium hydroxide. The reaction is given as follows: MgO + 2HNO3 ---> Mg (NO3)2 + The complete ionic equation for this reaction is as follows: 2Ag + (aq) + 2F (aq) + 2NH + 4 (aq) + Cr 2O2 7 (aq) Ag 2Cr 2O 7(s) + 2NH + 4 (aq) + 2F (aq) Because two NH + 4 (aq) and two F (aq) ions appear on both \ce{CH3CHO & CH3CH2OH} & \pu{0.19 V} \\ Exposure to magnesium nitrate leads to mild irritation in the mucous membranes. A strip of aluminum foil is placed in an aqueous solution of silver nitrate. Describe each of the following compounds as ionic, covalent, or acid. So the possible reactants are: $\ce{Cu^2+}$, $\ce{Zn^2+}$, and $\ce{Mg}$. Then determine the oxidation states of other atoms present according to rule 1. a. Aqueous sodium chloride + aqueous silver nitrate, Aqueous sodium phosphate + aqueous copper (II) sulfate, Hydrochloric acid + solid sodium bicarbonate (just a small scoop), Aqueous nickel (II) nitrate + aqueous sodium hydroxide, Hydrochloric acid + aqueous sodium hydroxide, Aqueous sodium carbonate + aqueous cobalt (II) nitrate, Aqueous sodium chloride + aqueous potassium nitrate, Aqueous iron (III) chloride + aqueous ammonium hydroxide. Displacement reactions of metals - student sheet, Displacement reactions of metals - teacher notes.