HNO 3 reaction with water. 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. Answer: At once reddish brown fumes of nitrogen dioxide gas are evolved. Write a balanced equation for the reaction of cone. Control the temperature carefully at nearly 200 °C. When ammonium nitrate is heated the products formed are nitrous oxide and steam. Give reasons for the following: Question 6. Get the detailed answer: Reactions of copper Experiment. Nitric acid obtained in laboratory is pale yellow in colour. Question 3. (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. Solutions for Class 9 Chemistry Maharashtra, 10 Nitric Acid. Answer: The oxidising property of nitric acid is based on the fact that when nitric acid undergoes decomposition, it yields nascent oxygen, which is very reactive. H2SO4 4.Fe2(SO4)3 CO2. Special Case of Nitric Acid: Nitric acid does not react with metals in the same way as hydrochloric acid or sulphuric acid do. Answer: Question 1. (a) Reaction of nitric acid with non-metals: C + 4HNO 3 → CO 2 + 2H 2 O + 4 NO 2. COVID-19 is an emerging, rapidly evolving situation. (1) The reaction between a metal and an acid can be represented by the general word equation shown below: acid + metal → salt + hydrogen gas 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. 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. 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. For refinning of noble metals like gold, platinum etc. H2SO4 2. → H2O + 2NO2 + [O] 2HNO3 (dil.) Nitric acid is a strong oxidising agent. The characteristics of copper, and the reaction of the metal with nitric acid Stable metal Vs. Strong oxidizer. State whether each reaction is an example of thermal decomposition   or thermal dissociation. H2SO4. Question 17. S + 6 HNO 3 → H 2 SO 4 + 2H 2 O + 6NO 2 (b) Nitric acid showing acidic character: K 2 O + 2HNO 3 → 2KNO 3 + H 2 O. ZnO + 2HNO 3 → Zn(NO 3) 2 + H 2 O (c) Nitric acid acting as oxidizing agent. (b) Most of the metals do not give hydrogen while reacting with nitric acid because HNO 3 is a strong oxidising agent. State two conditions which affect the decomposition of nitric acid. Sodium Bisuiphate + Nitric acid NaNO3 + H2S04 (conc.) You can refer to NCERT Solutions for Class 10 Science Chapter 3 Metals and Non-metals to revise the concepts in the syllabus effectively and improve your chances of securing high marks in your board exams. Silver is oxidized to +1 oxidation state. Fe (OH)3 + 3HNO3→ Fe (NO3)3 + 3H2O. That is why dilute nitric acid is considered a typical acid for its reaction with metals. It is used to create an inert atmosphere for welding and for carrying certain chemical reactions. Output refers to the product of the process not the intermediate steps. Nitric acid attacks proteins giving a yellow nitro compound known as xantho protein. 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. Fill in the blank from the choices given in the bracket: Question 1. Nitric acid is a powerful oxidising agent and hence corrodes rubber or any other stoppers to avoid corrosion, we use all glass apparatus. 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. Reaction of zinc with dilute nitric acid gives _____ gas. HNO3 decomposes by the action of sunlight to give brown coloured NO2 The brown coloured NO2 dissolves in cone. In particular dilute nitric acid (< 0.5 M) does produce hydrogen with moderately reactive metals such as magnesium and zinc, even though reactions are different at higher concentrations, and with other metals. ... Aluminium is a reactive metal , yet is is used to make utensils for cooking. 1. Identify the acid — The acid which is prepared by cata­lytic oxidation of ammonia. Write balanced chemical equation for: Action of hot and concentrated nitric acid on copper. → H2O + 2NO + 3[O] This nascent oxygen oxidises metals, non-metals, organic and inorganic compounds. The brown coloured NO2 dissolves in HNO3 to give it a yellow colour. (b) Nitric acid is kept in reagent bottle because nitric acid is a highly fuming liquid; it spreads in air and is highly corrosive. State why a yellow colour that appears in concentrated  nitric acid when it is left standing in an ordinary glass bottle. Convert nitric acid to sulphuric acid using a non-metal. Nitric acid, as a rule, does not carry on as an acid with metals to shape the comparing salt and free hydrogen. Question 18. If the conditions are right, just about any metal will burn. 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. }. Answer: Nitric acid oxidises iron(II) sulphate to iron (III) sulphate with the liberation of nitric oxide gas. Answer: Question 2. State the concentration of nitric acid used in each case. Answer: Hydrogen |H+| ions and Nitrate ions. Calcium starts floating because the bubbles of hydrogen gas formed stick to the surface of the metal. HNO3. nitric acid) in which nitric acid……….. (reduces/oxidises) hydrochloric acid to chlorine. State the cation responsible for turning moist neutral litmus red on reaction with dil. Answer: Question 1. FeSO4 + NO → FeSO4.NO. A non-metal which reacts with concentrated nitric acid to form its own acid as one of the product. This is due to the formation of a thin oxide coating on the surface of the metal which prevents further action. Identify the gas evolved when: Question 2. Question 3. The reaction temperature is maintained below 200°C Answer: The reaction temperature is maintained below 200°C. HNO 3 acid dissociate completely in the water and release hydronium ion (H 3 O +) in the water to form strong acid … (d) The temperature of the mixture of concentrated sulphuric acid and sodium nitrate should not exceed 200°C because sodium sulphate formed at higher temperature forms a hard crust which sticks to the walls of the retort and is difficult to remove. HN03 when added to copper turnings kept in a beaker. State how addition of nitric acid to acidified FeSO, serves as a test for the former. Solution 1 (2008). Question 4(3). → Cu (NO3)2 + 2H2O + 2NO2. Answer: (A) Cone, sulphuric acid (B) Potassium nitrate (Nitre). Zn + 2HCl(dil.) In this reaction, salt and water are formed. Give examples, alongwith equations to illustrate the reaction of the add. HCl is not used as a reactant in the laboratory preparation of nitric acid. State the type of reaction involved. Answer: Cone. Table of Contents. Question 4. 4. Give reasons for the following: Iron is rendered passive with fuming nitric acid. In the laboratory preparation of nitric acid from – KNO3 or NaNO3 State. It is a powerful oxidizing agent and the nascent oxygen oxidises hydrogen in water. Question 2. e) Reaction with Metallic Sulphites. Rewrite the correct statement with the missing word/s: Magnesium reacts with nitric acid to liberate hydrogen gas. → 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. Answer: Nitric acid, Question 4. Question 1. HNO 3 reaction with water. Heat on nitric acid. Answer: Cu + 4HNO3 → Cu(NO3)2 + 2NO2 + 2H2O, Question 3. When metal reacts with nitric acid (HNO 3), ... Identify the metal and its ore and give the reaction involved. Answer. Question 2. The ability of metals to be drawn into thin wires is known as 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. Therefore, all glass apparatus should be used for the preparation of nitric acid in the laboratory. Which of the two solutions – iron (II) sulphate or cone, sulphuric acid, do ‘X’ and ‘Z’ represent. Choose the correct answer from the choices given – The brown ring test is used for detection of: (A) C02–3 (B) NO-3 (c) SO23– (D) cl-. Nitric acid is not manufactured from atmospheric nitrogen. Concentrated nitric acid vapours – condense and are collected in the water-cooled receiver. Question 1. Answer: Pure or fuming nitric acid renders metals like iron (Fe) and Al- passive i. e., inactive. This salt gives nitrogen dioxide on heating. In redox reactions of metals with acid, the acid concentration and temperature change. Copy and complete the corresponding inferences in. concentrated hydrochloric acid is not used as a reactant in the laboratory preparation. HNO3 when added to copper turnings kept in a beaker. Observing Acid-Metal Reactions. Metal oxides are basic in nature. Answer: Nitric acid works as an oxidising agent. Answer: Question 3. Write the equation for the same. Question 1. Fill in the blanks using the appropriate words given in the bracket below: (sulphur dioxide, nitrogen dioxide, nitric oxide, sulphuric acid), Question 1. In particular dilute nitric acid (< 0.5 M) does produce hydrogen with moderately reactive metals such as magnesium and zinc, even though reactions are different at higher concentrations, and with other metals. 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