Answer: Question 2: Some methods used for the laboratory preparation of salts are : A : metal + acid B : carbonate + acid C : precipitation (double decomposition) D : direct combination E: titration Copy and complete the following table: Question 1: Hydrochloric acid is considered as a strong acid whereas acetic acid is a weak acid. Zinc is heated with sodium hydroxide solution. 7. 6. Balancing Redox Reactions in Acidic Solution 4. Write the two equations which represent these reactions. (c) [latex]\text{P}_4(s) + 5\text{O}_2(g) \longrightarrow \text{P}_4 \text{O}_{10}(s)[/latex]; Which solution will (i) liberate sulphur dioxide from sodium sulphite. The substances are: Chlorine, iron, lead, le&d nitrate solution, sodium nitrate solutions, iron (III) carbonate, lead carbonate, iron (III) chloride, sodium hydroxide solution and dilute hydrochloric add. Answer: Question 3: Study the following conversion schemes: 1. 5. Question 20: Why fused calcium chloride is used in the preparation of FeCl3 ? Sodium sulphate from sodium carbonate. (i) Which solution contains solute molecules in addition to water molecules. If water is used as a solvent, write the reactants and products as aqueous ions. Adding one electron to the right side bring that side’s total charge to (3+) + (1−) = 2+, and charge balance is achieved. NaOH + HNO3 —> NaNO3 + H2O. Write the net ionic equation representing the neutralization of any strong acid with an ionic hydroxide. H2O + 9H2O. Add iron fillings with constant stirring till effervescence of hydrogen stops. Substances with relatively large solubilities are said to be soluble. (a) [latex]2\text{HCl}(g) + \text{Ca(OH)}_2(s) \longrightarrow \text{CaCl}_2(s) + 2\text{H}_2 \text{O}(l)[/latex]; Iron (IK) chloride is also dissolved in water and then sodium hydroxide solution is added. The net ionic equation for this reaction, derived in the manner detailed in the previous module, is, (c) The two possible products for this combination are PbCO3 and NH4NO3. Stoichiometry of Chemical Reactions, 4.1 Writing and Balancing Chemical Equations, Chapter 6. Since the substance is reported to be an acid, its reaction with water will involve the transfer of H+ from HOCl to H2O to generate hydronium ions, H3O+ and hypochlorite ions, OCl−. (Hint: Consider the ions produced when a strong acid is dissolved in water. Write the two half-reactions representing the redox process. Students who are preparing for their Class 10 exams must go through NCERT Solutions for Class 10 Science Chapter 1 Chemical Reactions and Equations. Use the following equations to answer the next five questions: Indicate what type, or types, of reaction each of the following represents: Silver can be separated from gold because silver dissolves in nitric acid while gold does not. (i) Lead sulphate. (b) Degree of ionisation to H+ ion. PbO+C  ⟶   Pb+CO [B] Lead (II) oxide, when dissolved in the dilute nitric acid, lead nitrate is formed. Is there any difference in the salts formed by the acid ? To avoid this, the acid is always slowly added to water. (a) [latex]\text{Sn}^{2+}(aq) + 2\text{Cu}^{2+}(aq) \longrightarrow \text{Sn}^{4+}(aq) + 2\text{Cu}^{+}(aq)[/latex] (b) [latex]\text{SO}_3(g) + 2\text{H}_2 \text{O}(l) \longrightarrow \text{H}_3 \text{O}^{+}(aq) + {\text{HSO}_4}^{-}(aq), \text{(a solution of)} \; \text{H}_2 \text{SO}_4);[/latex] Iron (II) chloride and Iron (III) chloride. (iii) Copper (II) carbonate from copper (II) sulphate. Write a balanced equation for this reaction. For example, mixing solutions of silver nitrate and sodium fluoride will yield a solution containing Ag+, NO3−, Na+, and F− ions. Iron and dilute sulphuric acid. (ii) Crystals of zinc sulphate from zinc carbonate. Filter to remove excess of iron fillings and evaporate the solution till a saturated solution is formed. (a) [latex]\text{Mg(OH)}_2(s) + 2\text{HClO}_4(aq) \longrightarrow \text{Mg}^{2+}(aq) + 2{\text{ClO}_4}^{-}(aq) + 2\text{H}_2 \text{O}(l);[/latex] Potassium hydroxide, 7. Iron, 4. Finally, check to see that both the number of atoms and the total charges[2] are balanced. Answer: Carbonic acid (H2CO3) is a dibasic acid because it has two replaceable hydrogen atoms and hence it combines with two hydroxyl groups of the bases to form two kinds of salt and water. (a) [latex]\text{ZnCO}_3(s) \longrightarrow \text{ZnO}(s) + \text{CO}_2(g)[/latex], (b) [latex]2\text{Ga}(l) + 3\text{Br}_2(l) \longrightarrow 2\text{GaBr}_3(s)[/latex], (c) [latex]2\text{H}_2 \text{O}_2(aq) \longrightarrow 2\text{H}_2 \text{O}(l) + \text{O}_2(g)[/latex], (d) [latex]\text{BaCl}_2(aq) + \text{K}_2 \text{SO}_4(aq) \longrightarrow \text{BaSO}_4(s) + 2\text{KCl}(aq)[/latex], (e) [latex]\text{C}_2 \text{H}_4(g) + 3\text{O}_2(g) \longrightarrow 2\text{CO}_2(g) + 2\text{H}_2 \text{O}(l)[/latex]. (iv) A white precipitate of calcium carbonate is seen. Question 3: (i) What is acidity of a base. 2. The reducing agent (fuel) is C2H4(g). [A] Lead (II) oxide, when heated with powdered coke, reduced to metallic lead and carbon monoxide is formed. Why? (iv) Calcium chloride. 4. [A] Copper (II) oxide, when heated with coke powder is reduced to metallic copper. Question 10: (i) The pH value is utilised in medicine and agriculture. According to guideline 2, the oxidation number for sodium is +1. [B] Copper (II) oxide is dissolved in dilute sulphuric acid to form copper sulphate. (iii) What is reaction of neutralization ? A double-arrow is appropriate in this equation because it indicates the HOCl is a weak acid that has not reacted completely. [latex]2\text{LiOH}(aq) + \text{CO}_2(g) \longrightarrow \text{Li}_2 \text{CO}_3(aq) + \text{H}_2 \text{O}(l)[/latex], 22. Answer: Ammonium acetate, when dissolved in water is hydrolysed to form ammonium hydroxide and acetic acid. Question 4: Name the kind of particles present in: (i) Sodium hydroxide solution. Complete and balance the equations of the following reactions, each of which could be used to remove hydrogen sulfide from natural gas: Copper(II) sulfide is oxidized by molecular oxygen to produce gaseous sulfur trioxide and solid copper(II) oxide. The net ionic equation for this reaction, derived in the manner detailed in the previous module, is. i. When dissolved in water, NaOH dissociates to yield Na+ and OH− ions. The extent to which a substance may be dissolved in water, or any solvent, is quantitatively expressed as its solubility, defined as the maximum concentration of a substance that can be achieved under specified conditions. (ii) Which compound is blue in colour ? 3 s (green flame) use a liquid fuel/oxidant mixture, and the second, more powerful engines firing at 4 s (yellow flame) use a solid mixture. Classify the following as acid-base reactions or oxidation-reduction reactions: Identify the atoms that are oxidized and reduced, the change in oxidation state for each, and the oxidizing and reducing agents in each of the following equations: Complete and balance the following acid-base equations: Complete and balance the following oxidation-reduction reactions, which give the highest possible oxidation state for the oxidized atoms. ∴   The phenomenon is called efflorescence. (iv) On what factors the strength of an acid depend ? 6. (a) Which equation describes a physical change? Assigning Oxidation Numbers Why ? This heat is liberated due to the hydration of hydrogen ions derived from the acid. (iii) Which salt is hydroscopic in nature ? Question 16: Sodium sulphite (Na2SO3) and sodium hydrogen sulphite (NaHSO3) are salts of sodium but sodium sulphite is called a normal salt and sodium hydrogen sulphite is called an acid salt. 24. Write balanced chemical equations for the acid-base reactions described here: (a) the weak acid hydrogen hypochlorite reacts with water, (b) a solution of barium hydroxide is neutralized with a solution of nitric acid. Answer: (i) The number of hydroxyl ions that one molecule of a base gives on dissociation is known as acidity of a base. 3. (iii) pH of solution is less than 7. Several subclasses of redox reactions are recognized, including combustion reactions in which the reductant (also called a fuel) and oxidant (often, but not necessarily, molecular oxygen) react vigorously and produce significant amounts of heat, and often light, in the form of a flame. With silver nitrate HCl gives white precipitate of silver chloride. Redox reactions that take place in aqueous media often involve water, hydronium ions, and hydroxide ions as reactants or products. As an example, consider the equation shown here: The process represented by this equation confirms that hydrogen chloride is an acid. (b) [latex][{\text{Ag(NH}_3)_2}]^{+}(aq) + \text{e}^{-} \longrightarrow \text{Ag}(s) + 2\text{NH}_3(aq)[/latex] Sodium hydroxide, also known as lye and caustic soda, is an inorganic compound with the formula NaOH. If so, provide a more specific name for the reaction if appropriate, and identify the oxidant and reductant. The iron half-reaction is already balanced, but the chromium half-reaction shows two Cr atoms on the left and one Cr atom on the right. To the solution of calcium chloride, sodium hydroxide solution is added, a white precipitate of calcium hydroxide is obtained, which is insoluble even in the excess of sodium hydroxide. Question 1: Draw the structure of the stable positive ion formed when an acid dissolves in water. For purposes of predicting the identities of solids formed by precipitation reactions, one may simply refer to patterns of solubility that have been observed for many ionic compounds (Table 8). (d) Boric acid. (v) CaCl2(aq.) Consider as an example the dissolution of lye (sodium hydroxide) in water: This equation confirms that sodium hydroxide is a base. Zn + H2SO4 —> ZnSO4 (Zinc sulphate) + H2 More zinc filings are added, till dilute sulphuric acid is completely consumed and effervescence of hydrogen stops. We provide step by step Solutions for ICSE Chemistry Class 10 Solutions Pdf. You can download the Class 10 Chemistry ICSE Textbook Solutions with Free PDF download option. Dilute sulphuric acid is poured over sodium sulphate 9. (c) The loss of water by a hydrate on exposure to air is called efflorescence, e.g. (b) [latex]\text{H}_2 \text{S}(g) + {\text{Hg}_2}^{2+}(aq) + 2\text{H}_2 \text{O}(l) \longrightarrow 2\text{Hg}(l) + \text{S}(s) + 2\text{H}_3 \text{O}^{+}(aq)[/latex] (b) [latex]\text{H}_2(g) + \text{Br}_2(l) \longrightarrow 2\text{HBr}(g)[/latex]; Question 27: (i) Give chemical names of the following: (a) Green vitriol (b) Blue vitriol (c) White vitriol. Sn(s) is the reductant, HCl(g) is the oxidant. [latex]\text{H}_2 \text{O}(s) \longrightarrow \text{H}_2 \text{O}(l)[/latex], ii. Answer: Three different classes of substances are a metal, a base and a metallic carbonate, which react with an acid to form salts. This convention aims to emphasize the distinction between these two related properties. Explain. The displacement of two hydrogen atoms takes place in two steps. Is the dissolution of silver in nitric acid an acid-base reaction or an oxidation-reduction reaction? This compound can be prepared by the reaction of calcium carbonate, CaCO. Likewise, chlorine functions as an oxidizing agent (oxidant), as it effectively removes electrons from (oxidizes) sodium. Question 9: An aqueous solution of sodium carbonate is alkaline and that of ammonium chloride is acidic in behaviour. AgNO 3 + HCl AgCl + HNO 3 . Give balanced chemical equations only. Balance charge[1] by adding electrons. Some redox processes, however, do not involve the transfer of electrons. pH value > 7 indicates an alkaline solution. Determine the oxidation states of the elements in the following compounds: Determine the oxidation states of the elements in the compounds listed. Now add a concentrated solution of sodium carbonate to this solution. The precipitate is insoluble in nitric acid but soluble in ammonium hydroxide. Cool the solution to obtain the crystals of zinc sulphate with seven molecules of water of crystallization. Multiply the two half-reactions so the number of electrons in one reaction equals the number of electrons in the other reaction. Sodium hydroxide is a highly caustic base and alkali that decomposes proteins at ordinary ambient temperatures and may cause severe chemical burns.It is highly … Substances with relatively low solubilities are said to be insoluble, and these are the substances that readily precipitate from solution. (iii) How does pH value of a solution and hydrogen ion concentration of solution vary ? 10H2O is heated, the water of crystallization is evaporated leaving anhydrous sodium carbonate Na2CO3. Answer: Take about 50 cm3 of dilute sulphuric acid in a beaker and add 5 gm of zinc filings and heat it on a wire gauge with constant stirring. Lead nitrate and copper nitrate. 19. The iron half-reaction does not contain H atoms. Chemical reactions are classified according to similar patterns of behavior. An equation must represent equal numbers of electrons on the reactant and product sides, and so both atoms and charges must be balanced. 2. Answer: (i) Acidic solutions: ammonium sulphate; (NH4)2SO4, copper sulphate (CuSO4). Question 12: Lime juice has a sour taste while lime water is slightly bitter. Compare the pH values of sulphur dioxide solution and ammonia solution with that of pure water. These salts are obtained by the stepwise replacement of hydrogen atom from orthophosphoric acid. Composition of Substances and Solutions, 3.2 Determining Empirical and Molecular Formulas, 3.4 Other Units for Solution Concentrations, Chapter 4. Answer: (i) (B) Neutralisation (ii) (E) Direct synthesis (iii) (D) Double decomposition (iv) (A) Simple displacement (v) (C) Decomposition by acid. Answer: Sodium carbonate when dissolved in water is hydrolysed to form a weak acid, carbonic acid and a strong base sodium hydroxide. Question 23: (i) What happens to the crystals of washing soda when exposed to air ? In these reactions, water serves as both a solvent and a reactant. Answer: (i) pH value of a solution is the negative logarithm to the base 10 of hydrogen ion concentration expressed in gram-ions per litre. Complete and balance each of the following half-reactions (steps 2–5 in half-reaction method): Balance each of the following equations according to the half-reaction method: The requirement of “charge balance” is just a specific type of “mass balance” in which the species in question are electrons. (g) [latex]8\text{H}^{+}(aq) + {\text{MnO}_4}^{-}(aq) + 5\text{e}^{-} \longrightarrow \text{Mn}^{2+}(aq) + 4\text{H}_2 \text{O}(l)[/latex] (iv) For zinc sulphate zinc and dilute sulphuric acid are required. Lithium hydroxide may be used to absorb carbon dioxide in enclosed environments, such as manned spacecraft and submarines. The pH number less than 7 indicates acidity, while pH number more than 7 indicates alkalinity. Answer: (i) Zinc sulphate is a salt, because it is formed by the complete replacement of the hydrogen of sulphuric acid by zinc. Ammonium hydrogen carbonate crystals separate and they are heated to form sodium carbonate. The role of calcium chloride taken in the guard tube is to (a) absorb the evolved gas (b) moisten the gas (c) absorb moisture from the gas (v) (a) Citric add. Changing the coefficient on the right side of the equation to 2 achieves balance with regard to Cr atoms. Zinc metal reacts with dilute sulphuric acid to liberate hydrogen gas and zinc sulphate is formed. Question 8: (i) (a) What is the purpose of the pH scale ? Unlike ionic hydroxides, some compounds produce hydroxide ions when dissolved by chemically reacting with water molecules. Faced with a wide range of varied interactions between chemical substances, scientists have likewise found it convenient (or even necessary) to classify chemical interactions by identifying common patterns of reactivity. (d) [latex]2\text{H}_2 \text{O}(l) \longrightarrow \text{O}_2 + 4\text{H}^{+}(aq) + 4\text{e}^{-}[/latex] (h) [latex]\text{Cl}^{-}(aq) + 6 \text{OH}^{-}(aq) \longrightarrow {\text{ClO}_3}^{-}(aq) + 3\text{H}_2 \text{O}(l) + 6\text{e}^{-}[/latex], 28. 17. Ammonium carbamate when heated to 473K gives a mixture ofNH3 and CO2 vapour with a … Answer: Question 2: Write the equation for the laboratory preparation of the following salts 1. A base is a substance that will dissolve in water to yield hydroxide ions, OH−. 13. Give examples. A vivid example of precipitation is observed when solutions of potassium iodide and lead nitrate are mixed, resulting in the formation of solid lead iodide: This observation is consistent with the solubility guidelines: The only insoluble compound among all those involved is lead iodide, one of the exceptions to the general solubility of iodide salts. For example: The acidic salts obtained from orthophosphoric acid have the capacity to ionize further to yield hydrogen ion and thus they can change blue litmus paper red, whereas normal salt does not. (iv) It is a number assigned to express the acidity or alkalinity of a solution which varies from 1 to 14. Question 7: An aqueous solution of the zinc sulphate acidic in nature. Volunteer Certificate | Format, Samples, Template and How To Get a Volunteer Certificate? Zn + H2SO4 —> ZnSO4 + H2 (ii) Sodium hydroxide, a base reacts with dilute nitric acid to form sodium nitrate and water. (ii) (a) Calcium carbonate. Give the equations for the following conversions A to E. 2. (Hint: Water is one of the products.) The temperature of the water rose to reach a final temperature of 35°C. Calcium carbonqfe from calcium chloride. Answer: (i) Water of crystallization. 4. Write the balanced equation for this reaction. Follow the guidelines in this section of the text to assign oxidation numbers to all the elements in the following species: Solution Lithium hydroxide may be used to absorb carbon dioxide in enclosed environments, such as manned spacecraft and submarines. Answer: There are three types of salts prepared from orthophosphoric acid [H3PO4], two acidic salts and one normal salt. Chemistry by Rice University is licensed under a Creative Commons Attribution 4.0 International License, except where otherwise noted. Answer: Hydrochloric acid is consMered as a strong acid because it dissociates completely in water. Acid-base reactions involve the transfer of hydrogen ions between reactants. (The use of a double-arrow in the equation above denotes the partial reaction aspect of this process, a concept addressed fully in the chapters on chemical equilibrium.). (a) [latex]\text{Al}(s) + \text{F}_2(g) \longrightarrow[/latex], (b) [latex]\text{Al}(s) + \text{CuBr}_2(aq) \longrightarrow \;\text{(single displacement)}[/latex], (c) [latex]\text{P}_4(s) + \text{O}_2(g) \longrightarrow[/latex], (d) [latex]\text{Ca}(s) + \text{H}_2 \text{O}(l) \longrightarrow \;\text{(products are a strong base and a diatomic gas)}[/latex], (a) [latex]\text{K}(s) + \text{H}_2 \text{O}(l) \longrightarrow[/latex], (b) [latex]\text{Ba}(s) + \text{HBr}(aq) \longrightarrow[/latex], (c) [latex]\text{Sn}(s) + \text{I}_2(s) \longrightarrow[/latex], (a) [latex]\text{Mg(OH)}_2(s) + \text{HClO}_4(aq) \longrightarrow[/latex], (b) [latex]\text{SO}_3(g) + \text{H}_2 \text{O}(l) \longrightarrow \;\text{(assume an excess of water and that the product dissolves)}[/latex], (c) [latex]\text{SrO}(s) + \text{H}_2 \text{SO}_4(l) \longrightarrow[/latex], (a) [latex]\text{Ca(OH)}_2 + \text{HC}_2 \text{H}_3 \text{O}_2(aq) \longrightarrow[/latex], (b) [latex]\text{H}_3 \text{PO}_4(aq) + \text{CaCl}_2(aq) \longrightarrow[/latex], (a) [latex]\text{Ca(OH)}_2(s) + \text{H}_2 \text{S}(g) \longrightarrow[/latex], (b) [latex]\text{Na}_2 \text{CO}_3(aq) + \text{H}_2 \text{S}(g) \longrightarrow[/latex], (a) solid ammonium nitrate from gaseous molecular nitrogen via a two-step process (first reduce the nitrogen to ammonia, then neutralize the ammonia with an appropriate acid), (b) gaseous hydrogen bromide from liquid molecular bromine via a one-step redox reaction, (c) gaseous H2S from solid Zn and S via a two-step process (first a redox reaction between the starting materials, then reaction of the product with a strong acid), (a) [latex]\text{Sn}^{4+}(aq) \longrightarrow \text{Sn}^{2+}(aq)[/latex], (b) [latex][{\text{Ag(NH}_3)_2}]^{+}(aq) \longrightarrow \text{Ag}(s) + \text{NH}_3(aq)[/latex], (c) [latex]\text{Hg}_2 \text{Cl}_2(s) \longrightarrow \text{Hg}(l) + \text{Cl}^{-}(aq)[/latex], (d) [latex]\text{H}_2 \text{O}(l) \longrightarrow \text{O}_2(g) \;\text{(in acidic solution)}[/latex], (e) [latex]{\text{IO}_3}^{-}(aq) \longrightarrow \text{I}_2(s)[/latex], (f) [latex]{\text{SO}_3}^{2-}(aq) \longrightarrow {\text{SO}_4}^{2-}(aq) \text{(in acidic solution)}[/latex], (g) [latex]{\text{MnO}_4}^{-}(aq) \longrightarrow \text{Mn}^{2+}(aq) \;\text{(in acidic solution)}[/latex], (h) [latex]\text{Cl}^{-}(aq) \longrightarrow {\text{ClO}_3}^{-}(aq) \;\text{(in basic solution)}[/latex], (a) [latex]\text{Cr}^{2+}(aq) \longrightarrow \text{Cr}^{3+}(aq)[/latex], (b) [latex]\text{Hg}(l) + \text{Br}^{-}(aq) \longrightarrow {\text{HgBr}_4}^{2-}(aq)[/latex], (c) [latex]\text{ZnS}(s) \longrightarrow \text{Zn}(s) + \text{S}^{2-}(aq)[/latex], (d) [latex]\text{H}_2(g) \longrightarrow \text{H}_2 \text{O}(l) \text{(in basic solution)}[/latex], (e) [latex]\text{H}_2(g) \longrightarrow \text{H}_3 \text{O}^{+}(aq) \text{(in acidic solution)}[/latex], (f) [latex]{\text{NO}_3}^{-}(aq) \longrightarrow \text{HNO}_2(aq) \;\text{(in acidic solution)}[/latex], (g) [latex]\text{MnO}_2(s) \longrightarrow {\text{MnO}_4}^{-}(aq) \;\text{(in basic solution)}[/latex], (h) [latex]\text{Cl}^{-}(aq) \longrightarrow {\text{ClO}_3}^{-}(aq) \;\text{(in acidic solution)}[/latex], (a) [latex]\text{Sn}^{2+}(aq) + \text{Cu}^{2+}(aq) \longrightarrow \text{Sn}^{4+}(aq) + \text{Cu}^{+}(aq)[/latex], (b) [latex]\text{H}_2 \text{S}(g) + {\text{Hg}_2}^{2+}(aq) \longrightarrow \text{Hg}(l) + \text{S}(s) \;\text{(in acid)}[/latex], (c) [latex]\text{CN}^{-}(aq) + \text{ClO}_2(aq) \longrightarrow \text{CNO}^{-}(aq) + \text{Cl}^{-}(aq) \text{(in acid)}[/latex], (d) [latex]\text{Fe}^{2+}(aq) + \text{Ce}^{4+}(aq) \longrightarrow \text{Fe}^{3+}(aq) + \text{Ce}^{3+}(aq)[/latex], (e) [latex]\text{HBrO}(aq) \longrightarrow \text{Br}^{-}(aq) + \text{O}_2(g) \;\text{(in acid)}[/latex], (a) [latex]\text{Zn}(s) + {\text{NO}_3}^{-}(aq) \longrightarrow \text{Zn}^{2+}(aq) + \text{N}_2(g) \;\text{(in acid)}[/latex], (b) [latex]\text{Zn}(s) + {\text{NO}_3}^{-}(aq) \longrightarrow \text{Zn}^{2+}(aq) + \text{NH}_3(aq) \;\text{(in base)}[/latex], (c) [latex]\text{CuS}(s) + {\text{NO}_3}^{-}(aq) \longrightarrow \text{Cu}^{2+} + \text{S}(s) + \text{NO}(g) \;\text{(in acid)}[/latex], (d) [latex]\text{NH}_3(aq) + \text{O}_2(g) \longrightarrow \text{NO}_2(g) \;\text{(gas phase)}[/latex], (e) [latex]\text{Cl}_2(g) + \text{OH}^{-}(aq) \longrightarrow \text{Cl}^{-}(aq) + {\text{ClO}_3}^{-}(aq) \;\text{(in base)}[/latex], (f) [latex]\text{H}_2 \text{O}_2(aq) + {\text{MnO}_4}^{-}(aq) \longrightarrow \text{Mn}^{2+}(aq) + \text{O}_2(g) \;\text{(in acid)}[/latex], (g) [latex]\text{NO}_2(g) \longrightarrow {\text{NO}_3}^{-}(aq) + {\text{NO}_2}^{-}(aq) \;\text{(in base)}[/latex], (h) [latex]\text{Fe}^{3+}(aq) + \text{I}^{-}(aq) \longrightarrow \text{Fe}^{2+}(aq) + \text{I}_2(aq)[/latex], (a) [latex]{\text{MnO}_4}^{-}(aq) + {\text{NO}_2}^{-}(aq) \longrightarrow \text{MnO}_{2}(s) + {\text{NO}_3}^{-}(aq) \;\text{(in base)}[/latex], (b) [latex]{\text{MnO}_4}^{2-}(aq) \longrightarrow {\text{MnO}_4}^{-}(aq) + {\text{MnO}_2}(s) \;\text{(in base)}[/latex], (c) [latex]\text{Br}_2(l) + \text{SO}_2(g) \longrightarrow \text{Br}^{-}(aq) + {\text{SO}_4}^{2-}(aq) \;\text{(in acid)}[/latex], Answers to Chemistry End of Chapter Exercises, 2.