Answer: Copper reacts with concentrated nitric acid to produce nitrogen dioxide. study of compounds ammonia and nitric acid. Unlike other dilute acids only very dilute nitric acid (1%) reacts exclusively with Magnesium or … All the solutions of - Chemistry explained in detail by experts to help students prepare for their Maharashtra exams. (b) Copper when reacts with dilute HNO3 forms Copper nitrate, Nitric oxide and water. P 4 +20HNO 3 → 4H 3 PO 4 + 4H 2 O + 20NO 2. State your observation when copper is heated with concentrated nitric acid in a hard glass test tube. Solution 1 (2007). Write the equation for the same. Acid + Metal Oxide ⇨ Salt + Water Nitric acid | HNO3 | CID 944 - structure, chemical names, physical and chemical properties, classification, patents, literature, biological activities, safety/hazards/toxicity information, supplier lists, and more. Nitric acid on exposure to sunlight, slowly decomposes to form nitrogen dioxide gas which is reddish brown in color/. When nitric acid is prepared by the action of concentrated sulphuric acid on potassium nitrate, what is the special feature of the apparatus used. Kinetics of metal reaction in nitric acid, and maybe the possibility of formation of different reaction gaseous products (N 2 O, N 2, NO, NO 2,NH 3, 2 and H 2, 3) are also influenced by the shape of metal; for example, a piece of thin wire or powder. Name the gas evolved (formula is not acceptable). The yellow colour of nitric acid obtained in the laboratory is removed by babbling air through it. ; Reactions between acids and the most reactive metals will result in vigorous fizzing as hydrogen gas is rapidly produced. Sodium Bisuiphate + Nitric acid NaNO3 + H2S04 (conc.) Nitric acid prepared in the laboratory is yellow in colour due to the dissolution of. → Cu (NO3)2 + 2H2O + 2NO2. Question 2. Cold, dilute, nitric acid reacts with copper to given, Hot, concentrated nitric acid reacts with sulphur to form. Answer: Question 15. Give equations for the action of heat on – (1) NH4Cl (2) NH4NO3. It turns yellow because cone. The nitrogen dioxide dissolves in atmospheric moisture forming nitric acid. Fe (OH)3 + 3HNO3→ Fe (NO3)3 + 3H2O. Brown coloured pungent smelling gas – nitrogen dioxide (NO. Answer: Copper Nitrate. Name the gas evolved when acidified iron (II) sulphate reacts with dilute nitric acid in the brown ring test. Answer: Cu + 4HNO3 → Cu(NO3)2 + 2H2O + 2NO2, Question 4. Magnesium, manganese, and zinc liberate H 2 : Mg + 2 HNO 3 → Mg (NO 3) 2 + H 2 (Magnesium nitrate) Answer: [NO–] Nitrate, Question 2. During the process, nitric acid itself gets reduced to various products (NO, NO2, N2O, NH3, etc.) Give a balanced equation for the reactions: Dilute nitric acid and Copper carbonate. Answer: Question 1. C + 4HNO 3 → CO 2 + 2H 2 O + 4NO 2 (b) Copper when reacts with dilute HNO3 forms Copper nitrate, Nitric oxide and water. HNO3. Question 1. Zn(NO3)2 3. State two conditions which affect the decomposition of nitric acid. Thus, when an acid reacts with a metal oxide both neutralize each other. Name the chemical constituent of the brown ring ‘Y’. The compound which is responsible for the brown ring in the brown ring test for identify the nitrate ion. → ZnCl2 + H2 However, when zinc reacts with dil HNO3, no hydrogen is obtained. Question 3. Explosives (T.N.T., picric acid, nitrocellulose etc. 5. Reaction of zinc with dil. Give balanced equations for: Oxidation of carbon with concentrated nitric acid. Answer: Cu + 4HNO3 (cone.) Choose the correct word from the brackets to complete the sentence. Understand concepts from this chapter such as aqua regia, passive iron, aqua fortis, nitrogen fixation etc. 10HNO 3 … Copper metal reacts with nitric acid according to the reaction 3Cu + 8HNO 3 ----> 3Cu(NO3 )2 + 2NO + 4H2O If 18.75 g Cu(NO3 )2 is eventually obtained, then how many grams of nitric oxide (NO) would have also formed according to the preceeding equation. Question 2. Write an equation for the following reaction: Copper and concentrated nitric acid. Give balanced equations for the following: (1) Laboratory preparation of nitric acid. Experiment 2A – Reaction of Acid and Base. This salt gives nitrogen dioxide on heating. Write equation for the same. Question 2. When a metal react with dilute nitric acid,then hydrogen gas is not evolved.Nitric acid is a strong oxidising agent.As soon as hydrogen gas is formed in reaction between metal and dilute nitric acid,the nitric acid oxidises this hydrogen to water.Nitric acid itself is reduced to nitrogen oxides such as nitrogen monoxide,dinitrogen monoxide. It does, if the nitric acid is dilute. HNO3 when added to copper turnings kept in a beaker. Write a balanced equation for the reaction of – sulphur and hot concentrated nitric acid. State the cone, acid which will oxidise sulphur directly to H2SO4. nitric acid. Related Questions to study. Question 4. Excess of air carries the reactions in forward direction as oxygen is needed in all the three reactions, leading to the formation of nitric acid. The p-Block Elements. The first step in the manufacture of HNO3 is the catalytic oxidation of NH3. Question 1. 202 Qs. nitric acid) in which nitric acid……….. (reduces/oxidises) hydrochloric acid to chlorine. Extra Questions for Class 10 Science Chapter 3 Metals and Non-metals with Answers Solutions. State a reason for the inactivity of iron and aluminium on reaction with fuming HNO3. The common anion is the ion. 288 Views. Answer: Cu + 4HNO3 (cone.) ), Fertilizers (Ammonium nitrate, calcium ammonium nitrate or C.A.N.). Solution 3 (2006). Metal oxides are basic in nature. Answer: Formation of a hard residual crust of the corresponding sulphate [Na2SO4 or K2SO4] which being a -poor conductor of heat, sticks to the glass and cannot be easily removed from the apparatus. (2) Action of heat on a mixture of copper and concentrated nitric acid. When metal reacts with nitric acid (HNO 3), ... Identify the metal and its ore and give the reaction involved. It is due to the following reasons: Question 4(2). Question 17. Answer: Nitric acid oxidises iron(II) sulphate to iron (III) sulphate with the liberation of nitric oxide gas. Give a word equation and balanced molecular equation for the laboratory preparation of nitric acid from (1) KN03 (2) NaNO3. In case of nitric acid which is a strong oxidising agent, hydrogen produced in the nascent state reduces excess nitric acid and produces water and a reduction productof nitric acid. In the laboratory preparation of nitric acid, an all glass apparatus is used. If you have any doubts, please comment below. A mnemonic device has been designed for writing reactions of metals with nitric acid. In the laboratory preparation of nitric acid: Name the reactants A (a liquid) and B (a solid) used. Nitric acid obtained in laboratory is pale yellow in colour. If the HNO3 is concentrated the gas produced is a mixture of oxides of nitrogen, because concentrated nitric acid is a powerful oxidizing agent and can oxidize free hydrogen to water. Answer: 3Cu + 8HNO3 → 3Cu(NO3)2 + 4H2O + 2NO. Silver reacts with nitric acid to give silver nitrate (AgNO 3), NO 2 and H 2 O. 05. If the conditions are right, just about any metal will burn. → 3Fe2(SO4)3 + 4H2O +2NO The nitric oxide so formed reacts wtih more of iron(II) sulphate to form nitrosoferrous sulphate, which appears in the form of brown ring at the junction of liquids. Control the temperature carefully at nearly 200 °C. When a metal react with dilute nitric acid,then hydrogen gas is not evolved.Nitric acid is a strong oxidising agent.As soon as hydrogen gas is formed in reaction between metal and dilute nitric acid,the nitric acid oxidises this hydrogen to water.Nitric acid itself is reduced to nitrogen oxides such Question 5. Acid + Metal Word Equations Chemistry Tutorial Key Concepts. 5H2O, KNO3, NaCl, NaHSO,, Pb(NO3)2, ZnCO3, ZnSO4.7H2O. Question 3. Question 5. 6FeSO4 +3H2SO4 + 2HNO3 (dil. ) Answer: Platinum. Question 1. (a) Reaction of nitric acid with non-metals: C + 4HNO 3 → CO 2 + 2H 2 O + 4 NO 2. Give reasons for the following: Question 6. Ans: Nitric acid is strong oxidizing agent thus it can oxidize the hydrogen gas liberated in the reaction into water. It should Table of Contents. It does, if the nitric acid is dilute. Question 2. acid). Nitric acid affects the skin if it accidently falls on it, staining the skin yellow. State the cation responsible for turning moist neutral litmus red on reaction with dil. The device utilizes a left hand and schematically indicates the product of reduction of nitric acid as a function of two factors: the activity of metal and the concentration of acid. Answer: In the presence of sunlight nitric acid decomposes even at room temperature to give nitrogen dioxide, water and oxygen. HNO3. What do you see when concentrated nitric acid is added to copper. Write a balanced equation for the reaction of cone. Read the Nitric Acid Carefully to understand the concept in better way .After reading the Nitric Acid solve all example of your text book with ICSE Specimen Sample Paper for Class-10 Exam of Council. Question 1. Calcium starts floating because the bubbles of hydrogen gas formed stick to the surface of the metal. Answer: Pure or fuming nitric acid renders metals like iron (Fe) and Al- passive i. e., inactive. State two relevant observations for : Lead nitrate crys­tals are heated in a hard glass test tube. S + 6HNO3 → H2SO4 + 2H2O + 6NO2, Question 1. Question 5. Question 3. Acidified iron (II) sulphate (with dil. Action of heat on a mixture of copper and concentrated nitric acid. Answer: Nitric oxide (NO). Ans. Answer: Question 1. It is a powerful oxidizing agent and the nascent oxygen oxidises hydrogen in water. Answer: Platinum. Equation 3 2Fe 2 (SO 4 ) 3 + 2H 2 + 4NO → 4[Fe(H 2 O)5NO]SO 4 + 2H 2 SO 4 The [Fe(H 2 O) 5 NO]SO 4 forms a brown ring in the middle of the solution produced by the reaction, making it easy to identify the presence of nitrates in the water. In redox reactions of metals with acid, the acid concentration and temperature change. (1) The reaction between a metal and an acid can be represented by the general word equation shown below: acid + metal → salt + hydrogen gas HCl is not used as a reactant in the laboratory preparation of nitric acid. Question 1. Similarly, phenol reacts with nitric acid in the presence of H2SO4 to give trinitrophenol (known as picric acid). Add – cone, sulphuric acid carefully from the sides of the test tube. Give examples, alongwith equations to illustrate the reaction of the add. It is because at 68% concentration it forms a constant boiling mixture, i.e., if heated beyond this concentration then proportion of water vapour and nitric acid vapour, leaving the dilute acid does not change. 3Cu + 8HNO 3 → 3Cu (NO 3) 2 + 4H 2 O + 2NO Select the correct word from the list in bracket to complete each statement. Nitric acid oxidises the hydrogen produced to water and hence no hydrogen is liberated. More Resources for Selina Concise Class 10 ICSE Solutions H2SO4 4.Fe2(SO4)3 CO2. Question 18. Choose from the list substances – Acetylence gas, aqua fortis, coke, brass, barium chloride, bronze, platinum. The brown coloured NO2 dissolves in HNO3 to give it a yellow colour. Question 2. dilute nitric acid is generally considered a typical acid but not so in its reaction with metals. Question 3. HNO3 with (1) carbon (2) copper. Nitric acid is a stronger oxidising agent in the cone, state of the acid than in the dilute state. HNO 3 acid dissociate completely in the water and release hydronium ion (H 3 O +) in the water to form strong acid … Answer: C + 4HNO3 → 2H2O + 4NO2 + CO2. The second class of metals includes zinc, magnesium, aluminium, cadmium, tin, lead, iron, and the alkali metals, and no nitrous acid is required to start their reaction with nitric acid. Silver is oxidized to +1 oxidation state. Answer: Yellowish brown colour is changed to dark yellowish brown colour on prolonged decomposition. Answer: Question 1. Also, learn the properties of nitric acid … Answer: Pb(NO3)2. Solution 2 (2006). The NO2 so produced dissolves in cone. During the reaction it produces Nitrous acid and Zinc nitrate. Give two general uses of HNO3. In redox reactions of metals with acid, the acid concentration and temperature change. Answer: All glass apparatus is used in the laboratory preparation of nitric acid. → H2O + 2NO + 3[O] This nascent oxygen oxidises metals, non-metals, organic and inorganic compounds. Nitric acid combines with protein of the skin forming a yellow compound Xanthoproteic acid, stains skin yellow. Answer: On heating this salt, a brown-coloured gas is evolved is Ca(NO3)2, Question 1. Nitric acid act as solvent for large number of metals. Question 4(3). Answer: S + 6HNO3 → H2SO4 + 2H2O + 6NO2. Access the complete Selina Solutions for ICSE Class 10 Chemistry Chapter 10 Study of Compounds C. Nitric Acid at TopperLearning. State why a yellow colour that appears in concentrated  nitric acid when it is left standing in an ordinary glass bottle. HCl. Answer: Cold, dilute nitric acid reacts with copper to form nitric oxide. Question 5. Dilute nitric acid behaves as a typical acid in its reaction with most metals. Zn + 2HCl(dil.) Answer: Nitric acid works as an oxidising agent. A reddish-brown gas is obtained when X, Y and Z are separately warmed with concentrated sulphuric acid and copper turnings added to the mixture. Match each substance A to E listed below with the appropriate description given below.| (A) Sulphur (B) Silver chloride (C) Hydrogen chloride (D) Copper (II) sulphate (E) Graphite. In the laboratory preparation of nitric acid from – KNO3 or NaNO3 State. Copper metal reacts with aqueous nitric acid to produce copper (II) nitrate, nitrogen dioxide and (b) Iron becomes inert when reacted with nitric acid due to the formation of extremely thin layer of insoluble metallic oxide which stops the reaction. Question 2. HNO 3 reaction with water. Convert ammonia to nitric acid by the above process giving all conditions. The reaction temperature is maintained below 200°C Answer: The reaction temperature is maintained below 200°C. → H2O + 2NO2 + [O] 2HNO3 (dil.) Answer: Metals, lying above hydrogen in the electro chemical series, give hydrogen from the acid. State why hydrogen is liberated when zinc reacts with dil.HCl but not with dil. Question 1. The vapours obtained in the receiver on heating alone or with copper turnings evolve – reddish brown fumes of nitrogen dioxide which turns acidified ferrous sulphate solution brown – proving that the vapours are of nitric acid. Answer: At once reddish brown fumes of nitrogen dioxide gas are evolved. Answer: Reddish brown gas is liberated residue is yellow when hot and white when cold. Give a reason why the brown ring does not settle down at the bottom of the test tube. Answer: Potassium nitrate and cone, sulphuric acid. Answer: The complete apparatus is made of glass only – since the vapours of nitric acid being highly corrosive and attack rubber, cork, etc. Question 3. Nitric acid, (HNO 3), is a colourless, fuming, and highly corrosive acid … (b) A freshly prepared ferrous sulphate solution is used because on exposure to the atmosphere, it is oxidized to ferric sulphate which will not give the brown ring. Answer: Cu + 4HNO3 → Cu(NO3)2 + 2H2O + 2NO2  ↑, Question 2. The precautions to be taken during the preparation. }. Nitric acid is a powerful oxidising agent and hence corrodes rubber or any other stoppers to avoid corrosion, we use all glass apparatus. D. N 2 O and NO 2. Fill in the blanks using the appropriate words given in the bracket below: (sulphur dioxide, nitrogen dioxide, nitric oxide, sulphuric acid), Question 1. Reaction of manganese with cold very dil. 3. Write a balanced equation for – Ferric hydroxide reacts with nitric acid. Question 2. Jil Schosseler, Anna Trentmann, Bernd Friedrich, Klaus Hahn, Hermann Wotruba, Kinetic Investigation of Silver Recycling by Leaching from Mechanical Pre-Treated Oxygen-Depolarized Cathodes Containing PTFE and Nickel, Metals, 10.3390/met9020187, 9, 2, (187), (2019). State the concentration of nitric acid used in each case. The reduction product depends on the dilution of the acid. Get … At high temperatures the sodium sulphate or phtassium sulphate formed, forms a crust and sticks to the glass apparatus. Cold, dil. From the formulae listed below, choose, one, corresponding to the salt having the given description: AgCl, CuCO3, CuSO4. State whether each reaction is an example of thermal decomposition   or thermal dissociation. It oxidises the hydrogen gas to form water. (c) Zinc reacts with nitric acid to form Zinc nitrate, nitric oxide and water. Give reasons for the following: Iron is rendered passive with fuming nitric acid. Convert nitric acid to sulphuric acid using a non-metal. Answer: The first step of Ostwald’s process involves catalytic oxidation of ammonia to nitric oxide and water (steam). Ans. It should Ans. → Cu (NO3)2 + 2H2O + 2NO2. From the list of the following salts — AgCl, MgCl2, NaHSO4, PbCO3, ZnCO3, KNO3, Ca(NO3)2 State the salt which on heating, evolves a brown coloured gas. The skin if it accidently falls on it, staining the skin a! 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