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id="menu-item-108"><a href="#"><span>FAQ</span></a></li> <li class="menu-item menu-item-type-post_type menu-item-object-page" id="menu-item-104"><a href="#"><span>Contact</span></a></li> </ul></nav> </div><div class="secondary_menu_wrapper"> </div> <div class="banner_wrapper"> </div> </div> </div> </div> </div> </header> </div> {{ text }} <br> <br> {{ links }} <footer class="clearfix" id="Footer"> <div class="footer_copy"> <div class="container"> <div class="column one"> <div class="copyright"> {{ keyword }} 2021</div> <ul class="social"></ul> </div> </div> </div> </footer> </div> </body> </html>";s:4:"text";s:13868:"Answer: Question 12: How many types of salts can be prepared from orthophosphoric acid ? The solubility guidelines indicate BaSO4 is insoluble, and so a precipitation reaction is expected. —> CaCO3 (White ppt) + 2NaCl (aq.). Answer: (i) Take about 50 cm3 of dilute sulphuric acid in a beaker and heat it on a wire gauge. (iii) How does pH value of a solution and hydrogen ion concentration of solution vary ? Question 7: An aqueous solution of the zinc sulphate acidic in nature. (iv) Give two practical application of Neutralization. Both negative and positive biases can be acute, so greater care must be taken in ignition temperature and time. Oxidation-reduction (redox) reactions are those in which one or more elements involved undergo a change in oxidation number. (d) This is not a redox reaction, since oxidation numbers remain unchanged for all elements. Answer: Three different classes of substances are a metal, a base and a metallic carbonate, which react with an acid to form salts. (b) [latex]\text{H}_2(g) + \text{Br}_2(l) \longrightarrow 2\text{HBr}(g)[/latex]; Molten sodium and chlorine. During the preparation of hydrogen chloride gas on a humid day, the gas is usually passed through the guard tube containing calcium chloride. Question 11: You are provided with the following chemicals : Ammonium hydroxide, chlorine, copper oxide, iron, lead nitrate and dilute sulphuric acid; using only chemicals of this given list, write equation for the following salt preparations: (i) A salt by direct combination. Answer: (i) Water of crystallization. The iron half-reaction does not contain O atoms. Base   Acid       Salt   water In the reaction of neutralization, the hydrogen ions of an acid combines with the hydroxyl ions of an alkali to form water, at the same time a salt is formed. Single-displacement (replacement) reactions are redox reactions in which an ion in solution is displaced (or replaced) via the oxidation of a metallic element. (iv) Zinc sulphate. Answer: Calcium chloride is a deliquescent substance, it absorbs water up to such an extent that it finally dissolves in it and more over, it does not react with water. A far greater number of compounds behave as weak acids and only partially react with water, leaving a large majority of dissolved molecules in their original form and generating a relatively small amount of hydronium ions. Zn + H2SO4 —> ZnSO4 (Zinc sulphate) + H2 (ii) Sulphur dioxide is an acidic oxide, because it is an oxide of non-metal, which dissolves in water to form an acidlcnown as sulphurous acid. For those reactions identified as redox, name the oxidant and reductant. Which one of them is acidic, neutral and alkaline in nature ? 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. (iii) What can you say about the pH of a solution that liberates carbon dioxide from sodium carbonate. 4. The reducing agent is Ga(l). (While the vast majority of redox reactions involve changes in oxidation number for two or more elements, a few interesting exceptions to this rule do exist Example 4.) (c) Silver chloride. Gallium is oxidized, its oxidation number increasing from 0 in Ga(l) to +3 in GaBr3(s). (d) Boric acid. The term oxidation was originally used to describe chemical reactions involving O2, but its meaning has evolved to refer to a broad and important reaction class known as oxidation-reduction (redox) reactions. [latex]\text{H}_2 \text{O}(s) \longrightarrow \text{H}_2 \text{O}(l)[/latex], ii. of calcium carbonate appears when the solutions of CaCl2 and Na2CO3 are mixed. Sodium sulphate from sodium carbonate. What is the balanced equation for this reaction? 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. (iii) contain solute molecules and ions ? Solution : The chemical formula of ammonium chloride is NH 4 Cl. (iii) Neutral solutions: potassium nitrate; (KNO3), sodium chloride (NaCl). Name the phenomenon exhibited. Answer: A universal indicator is better than an ordinary indicator as it not only shows whether the solution is acidic or basic but also gives the pH values (approx.) The pH number less than 7 indicates acidity, while pH number more than 7 indicates alkalinity. Which solution will (i) liberate sulphur dioxide from sodium sulphite. (ii) (a) Water of crystallization is that definite number of water molecules which are to a crystal when it is crystallizing out from an aqueous solution, e.g. 5. Sodium sulphate is dissolved in water and barium chloride solution is added, an insoluble white precipitate of barium sulphate is obtained. (iv) (a) Acidity of soil is reduced by adding slaked lime. A few examples of such reactions will be used to develop a clear picture of this classification. 7. (They burn!) Give examples. (vi) Give the name of a soluble lead salt and write the equation for the action of heat on this salt. (b) A solution of Sr(OH)2 is added to a solution of HNO3. MgO is a white solid, but in these experiments it often looks gray, due to small amounts of Mg, Lithium hydroxide may be used to absorb carbon dioxide in enclosed environments, such as manned spacecraft and submarines. Answer: Strong acids, strong bases and their salts ionize completely in the solution. 4. 1.5 Measurement Uncertainty, Accuracy, and Precision, 1.6 Mathematical Treatment of Measurement Results, Chapter 3. (c) A is a soluble acidic oxide, B is a soluble base compared to the pH of pure water, what will be the pH of: (A) a solution of A, (B) a solution of B. (v) Name an acid used : (a) as a flavour and to preserve food (b) in a drink (c) to remove ink spots (d) as an eye wash. Answer: (i) The number of replaceable hydrogen atoms, present in one molecule of an acid is known as basicity of the acid. Zn + H2SO4 —> ZnSO4 (Zinc sulphate) + H2 More zinc filings are added, till dilute sulphuric acid is completely consumed and effervescence of hydrogen stops. Ferric hydroxide reacts with nitric acid. (iii) Give an example of a solution which is a weak alkali. Question 5: Solution A is a sodium hydroxide solution. Calcium carbonqfe from calcium chloride. More information on these important concepts is provided in the text chapter on solutions. (d) [latex]\text{Fe}^{2+}(aq) + \text{Ce}^{4+}(aq) \longrightarrow \text{Fe}^{3+}(aq) + \text{Ce}^{3+}(aq)[/latex] Application for TC in English | How to Write an Application for Transfer Certificate? Answer: (i) (a) Hydrochloric acid and sodium hydroxide solution react to form sodium chloride. Iron (in) chloride from iron. Answer: When zinc sulphate is dissolved in water, it is hydrolysed to form sulphuric acid and zinc hydroxide. Oxidation numbers for common nonmetals are usually assigned as follows: Hydrogen: +1 when combined with nonmetals, −1 when combined with metals, Oxygen: −2 in most compounds, sometimes −1 (so-called peroxides, O, Halogens: −1 for F always, −1 for other halogens except when combined with oxygen or other halogens (positive oxidation numbers in these cases, varying values). The gaseous product then reacts with liquid water to produce liquid hydrogen sulfate as the only product. (e) This is a redox reaction (combustion). (v) A soluble salt from a metal. (ii) Copper sulphate. These reactions are common in nature and are responsible for the formation of coral reefs in ocean waters and kidney stones in animals. Explain. Sodium sulphate from sodium hydroxide. When they exchange blows with their fists or feet, we say they are fighting. (c) [latex]\text{Hg}_2 \text{Cl}_2(s) + 2\text{e}^{-} \longrightarrow 2\text{Hg}(l) + 2\text{Cl}^{-}(aq)[/latex] When dissolved in water, ammonia reacts partially to yield hydroxide ions, as shown here: This is, by definition, an acid-base reaction, in this case involving the transfer of H+ ions from water molecules to ammonia molecules. (d) Sodium sulphate. A large number of important reactions are included in three categories: precipitation, acid-base, and oxidation-reduction (redox). Question 3: Acetic acid is monobasic. Preparation: ... NH 4 Cl, Ammonium Chloride will have pH less than 7. (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. 2. Under typical conditions, only about 1% of the dissolved ammonia is present as NH4+ ions. The solubility guidelines indicate PbCO3 is insoluble, and so a precipitation reaction is expected. 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