{"id":2489,"date":"2023-10-03T08:05:09","date_gmt":"2023-10-03T08:05:09","guid":{"rendered":"http:\/\/localhost\/ecole9ja\/?p=2489"},"modified":"2023-10-03T08:07:01","modified_gmt":"2023-10-03T08:07:01","slug":"week-2-ad-3-ss1-third-term-chemistry-notes","status":"publish","type":"post","link":"https:\/\/ecolebooks.com\/nigeria\/posts\/week-2-ad-3-ss1-third-term-chemistry-notes\/","title":{"rendered":"Week 2 ad 3 &#8211; SS1 Third Term Chemistry Notes"},"content":{"rendered":"<p><strong>WEEK TWO AND THREE<\/strong><br \/>\n\t\t<strong>TOPIC: BASES AND SALTS<\/strong><br \/>\n\t\t<strong>CONTENT<\/strong><\/p>\n<ul>\n<li>Bases\n<\/li>\n<li>Salts\n<\/li>\n<li>Efflorescence, deliquescence and hygroscopic\n<\/li>\n<\/ul>\n<p>\u00a0<strong>BASES AND ALKALIS<\/strong><br \/>\n\t\tA base is a substance which will neutralize an acid to yield a salt and water only. Most oxide and hydroxide of metals are bases e.g. Na<sub>2<\/sub>O, K<sub>2<\/sub>O, MgO, NaOH, KOH e.t.c.<\/p>\n<p>\u00a0An alkalis is a basic hydroxide which is soluble in water NaOH, KOH, Ca(OH)<sub>2<\/sub>. A basic oxide (or hydroxide) is a metallic oxide (or hydroxide) which contains ions (O<sup>2<\/sup> or OH<sup\/>) and will react with an acid to form a salt and water only.<\/p>\n<p>\u00a0Note: An exception to this definition is the reaction of lead (IV) oxide with hydrochloric acid to produce lead (ii) chloride (a salt), water and chlorine gas.<br \/>\n<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S1.png\" alt=\"\"\/>PbO<sub>2(s)<\/sub> +   4HCl<sub> (aq)<\/sub>        PbCl<sub>2 (aq) +<\/sub>    2H<sub>2<\/sub>O<sub> (l)<\/sub>   +   Cl<sub>2 (g)<\/sub><\/p>\n<p>\u00a0From the equation above, PbO<sub>2<\/sub> is not a base.    The nature of the hydroxides of the metals varies according to the position of the metal in the electrochemical series, as illustrated below.<\/p>\n<div>\n<table>\n<tbody>\n<tr>\n<td>Metal\u00a0<\/td>\n<td>Solubility\u00a0<\/td>\n<td>Decomposition by heat.\u00a0<\/td>\n<\/tr>\n<tr>\n<td>K<br \/>\nNa<br \/>\nCa\u00a0<\/td>\n<td>The hydroxides of these metals are soluble in water and are alkalis.\u00a0<\/td>\n<td>Hydroxide of sodium and potassium can<br \/>\nnot be decomposed by heat.\u00a0<\/td>\n<\/tr>\n<tr>\n<td>Mg, Al, Zn<br \/>\nFe, Pb, Cu<\/td>\n<td>These metals form hydroxides which are insoluble in water. They are amphoteric except the three hydroxides of Magnesium, iron, and copper.\u00a0<\/td>\n<td>Decomposed on heating to form oxide and water.\u00a0<\/td>\n<\/tr>\n<tr>\n<td>Hg, Ag, Au.<\/td>\n<td>Hydroxides of these metals do not exist.\u00a0<\/td>\n<td>\u00a0<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<\/div>\n<p>\u00a0<strong>STRENGTH OF BASE<\/strong><br \/>\n\t\tLike an acid, we have strength of a base. The strength of a base can either be weak or strong.<br \/>\nWeak base: Weak base are base that ionizes slightly in aqueous solution to produce positively charged metallic ion and negatively charged hydroxide ion e.g. CaO, NH<sub>3<\/sub>.<\/p>\n<p>\u00a0<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S2.png\" alt=\"\"\/>NH<sub>3 (g)<\/sub>    +   H<sub>2<\/sub>O<sub> (l)<\/sub>        NH<sub>4<\/sub><sup>+<\/sup>(<sub>aq<\/sub>) OH<sup>&#8211;<\/sup><sub>(aq)<\/sub><br \/>\n\t\tStrong bases: Strong base are base that ionizes completely in aqueous solution to produce positively charged metallic ion and negatively charged hydroxide ion e.g. Na<sub>2<\/sub>O, K<sub>2<\/sub>O.<br \/>\n<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S3.png\" alt=\"\"\/>Na<sub>2<\/sub>O<sub>(s)<\/sub>   +      H<sub>2<\/sub>O<sub> (l)<\/sub>          2NaOH<sub>(aq)<\/sub><br \/>\n\t\t<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S4.png\" alt=\"\"\/>K<sub>2<\/sub>O<sub>(s)<\/sub>      +     H<sub>2<\/sub>O<sub> (l)<\/sub>         2KOH<sub>(aq)<\/sub><br \/>\n\t\t<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S5.png\" alt=\"\"\/>NaOH<sub> (aq)<\/sub>       Na<sup>+<\/sup><sub>(aq)<\/sub>    +       OH<sup>&#8211;<\/sup><sub>(aq)<\/sub><br \/>\n\t\t<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S6.png\" alt=\"\"\/>KOH<sub> (aq)<\/sub>         K<sup>+<\/sup><sub>(aq)         <\/sub>+       OH<sup>&#8211;<\/sup><sub>(aq)<\/sub><\/p>\n<p>\u00a0<strong>PHYSICAL PROPERTIES OF ALKALIS<\/strong><br \/>\n\t\t1. Alkalis have a bitter taste.<br \/>\n2. Alkalis are soapy to the touch.<br \/>\n3. Alkalis turn red litmus blue.<br \/>\n4. Concentrated form of the caustic alkalis of NaOH and KOH are corrosive.<\/p>\n<p>\u00a0<strong>CHEMICAL PROPERTIES OF ALKALIS<\/strong><br \/>\n\t\t1.\u00a0Reaction with acid: All base react with acid to form salt and water only.<br \/>\n<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S7.png\" alt=\"\"\/>NaOH<sub>(aq)<\/sub>   +    HCl<sub>(aq)<\/sub>         NaCl<sub>(aq)<\/sub>       +    H<sub>2<\/sub>O<sub>(l)<\/sub><br \/>\n\t\t<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S8.png\" alt=\"\"\/>MgO<sub>(s)<\/sub>      +   2HNO<sub>3(aq)<\/sub>     \u00a0\u00a0\u00a0\u00a0Mg(NO<sub>3<\/sub>)<sub>2(aq)<\/sub>   +   H<sub>2<\/sub>O<sub>(l)<\/sub><br \/>\n\t\t2. Displacement of volatile ammonia from ammonium salt by a non volatile alkali: if an ammonium salt is warmed with an alkali (in the presence of water) ammonia gas is liberated<br \/>\n<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S9.png\" alt=\"\"\/>NaOH<sub> (aq<\/sub>)   +      NH<sub>4<\/sub>Cl<sub> (aq)<\/sub>       NaCl<sub> (aq)<\/sub>    +     H<sub>2<\/sub>O<sub>(l)<\/sub>   +     NH<sub>3(g)<\/sub><br \/>\n\t\t<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S10.png\" alt=\"\"\/>Ca (OH)<sub>2(aq)<\/sub>  +  (NH<sub>4<\/sub>)<sub>2<\/sub>SO<sub>4(aq)<\/sub>       CaSO<sub>4(aq)<\/sub>   +    2H<sub>2<\/sub>O<sub>(l)<\/sub>  +   2NH<sub>3(g)<\/sub><\/p>\n<p>\u00a0<strong>USES OF ALKALIS\/BASE<\/strong><\/p>\n<div>\n<table>\n<tbody>\n<tr>\n<td>Names\u00a0<\/td>\n<td>Uses\u00a0<\/td>\n<\/tr>\n<tr>\n<td>NaOH<\/td>\n<td>Used in the manufacture of soap, Na salts and plastic<br \/>\nUsed in petrol refining.\u00a0<\/td>\n<\/tr>\n<tr>\n<td>KOH\u00a0<\/td>\n<td>Used in the manufacture of liquid soap<br \/>\nUsed in dyeing and electroplating.\u00a0<\/td>\n<\/tr>\n<tr>\n<td>Ca(OH)<sub>2<\/sub><\/td>\n<td>Used in manufacture of  mortar, cement and plaster<br \/>\nUsed in dissolving acidic soil.\u00a0<\/td>\n<\/tr>\n<tr>\n<td>Mg(OH)<sub>2<\/sub><\/td>\n<td>Used in the manufacture of toothpaste<br \/>\nUsed as a laxative.\u00a0<\/td>\n<\/tr>\n<tr>\n<td>Aqueous NH<sub>3<\/sub><\/td>\n<td>Used for bleaching cloth<br \/>\nUsed as detergent.\u00a0<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<\/div>\n<p>\u00a0<strong>EVALUATION<\/strong><br \/>\n\t\t1. Define alkali giving examples<br \/>\n2. State three physical properties of alkalis<br \/>\n3.\u00a0Using balanced equations, state two chemical properties of bases<br \/>\n4.\u00a0State the uses of bases<\/p>\n<p>\u00a0<strong>NEUTRALIZATION REACTION<\/strong><br \/>\n\t\tNeutralization reaction can be defined in three major ways.<br \/>\n1. In terms of acid and the base present.<br \/>\n2. In terms of H<sup>+<\/sup> ion and OH<sup>&#8211;<\/sup> present in the acid and base.<br \/>\n3. In terms of oxonium ions (H<sub>3<\/sub>O<sup>+<\/sup>) and hydroxide ion (OH<sup>&#8211;<\/sup>).<br \/>\nNeutralization is the process whereby an acid react completely with an alkalis\/bases to form salt and water.<br \/>\n<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S11.png\" alt=\"\"\/>HCl<sub>(aq)<\/sub>   +   NaOH<sub>(aq)<\/sub>          NaCl<sub>(aq)<\/sub>    +    H<sub>2<\/sub>O<sub>(l)<\/sub><br \/>\n\t\tNeutralization is the combination of hydrogen ion (H<sup>+<\/sup>) and hydroxide ions (OH<sup>&#8211;<\/sup>) to form water molecules. A salt is also form at the same time.<br \/>\n<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S12.png\" alt=\"\"\/>H<sup>+<\/sup><sub>(aq)<\/sub>    +     OH<sup>&#8211;<\/sup>            H<sub>2<\/sub>O<sub>(l)<\/sub><br \/>\n\t\tNeutralization can also be defined as the combination of oxonium ions (H<sub>3<\/sub>O<sup>+<\/sup>) and hydroxide ions (OH<sup>&#8211;<\/sup>) to form water molecule. A salt is also formed at the same time.<br \/>\n<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S13.png\" alt=\"\"\/>H<sub>3<\/sub>OCl<sub>(aq)<\/sub>        +      KOH<sub>(aq)<\/sub>            KCl<sub>(aq)<\/sub>    +    H<sub>2<\/sub>O<sub>(l)<\/sub><br \/>\n\t\t<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S14.png\" alt=\"\"\/>(H<sub>3<\/sub>O)<sub>2<\/sub>SO<sub>4(aq)<\/sub>   +      2NaOH<sub>(aq)<\/sub>          Na<sub>2<\/sub>SO<sub>4(aq)    <\/sub>+     4H<sub>2<\/sub>O<sub>(l)<\/sub><br \/>\n\t\t<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S15.png\" alt=\"\"\/>H<sub>3<\/sub>O<sup>+<\/sup><sub>(aq)              <\/sub>+      OH<sup>&#8211;<\/sup><sub>(aq)<\/sub>             2H<sub>2<\/sub>O<sub>(l)<\/sub><\/p>\n<p>\u00a0<strong>OXONIUM ION<\/strong><br \/>\n\t\tIn aqueous solution, the hydrogen ion become associated with a water molecule to form oxonium ion (H<sub>3<\/sub>O<sup>+<\/sup>).This is an example of a coordinate covalent combination.<br \/>\n<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S16.png\" alt=\"\"\/>H<sup>+<\/sup>    +   H<sub>2<\/sub>O           H<sub>3<\/sub>O<sup>+<\/sup><br \/>\n\t\tDuring neutralization, oxonium ion H<sub>3<\/sub>O<sup>+<\/sup> behaves as hydrogen ion and thus reacts with hydroxide ion (OH<sup>&#8211;<\/sup>) to form water molecules.<\/p>\n<p>\u00a0<strong>EVALUATION<\/strong><br \/>\n\t\t1.\u00a0Define the term neutralization.<br \/>\n2.\u00a0Write TWO balanced equations to show neutralization reactions.<\/p>\n<p>\u00a0<strong>SALTS<\/strong><br \/>\n\t\tA salt is referred to as the compound formed when all or part of the ionisable hydrogen ion in an acid is replaced by a metallic or ammonium ion e.g.<br \/>\nHCl<sub>(aq)<\/sub> + NaOH<sub>(aq)<\/sub> \u2192 NaCl<sub>(aq)<\/sub> + H<sub>2<\/sub>O<sub>(l)<\/sub><br \/>\n\t\tH<sub>2<\/sub>SO<sub>4(aq)<\/sub> + KOH<sub>(aq)<\/sub> \u2192 KHSO<sub>4(aq)<\/sub> + H<sub>2<\/sub>O<sub>(l)<\/sub><\/p>\n<p>\u00a0<strong>TYPES OF SALTS<\/strong><br \/>\n\t\tThere are five main types of salts namely:<br \/>\n1. Normal salt.<br \/>\n2. Acid salts<br \/>\n3. Basic salts<br \/>\n4. Double salts.<br \/>\n5. Complex salts.<\/p>\n<p>\u00a01. <strong>Normal salts<\/strong>: are the salts formed when all the replaceable hydrogen ion in the acid has been completely replaced by a metal ion e.g. NaCl, K<sub>2<\/sub>SO<sub>4<\/sub>, Na<sub>3<\/sub>PO<sub>4<\/sub>, NaNO<sub>3<\/sub> etc. Normal salts are neutral to litmus<br \/>\n<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S17.png\" alt=\"\"\/>HCl<sub>(aq)<\/sub>   +    NaOH<sub>(aq)<\/sub>              NaCl<sub>(aq)<\/sub>  +    H<sub>2<\/sub>O<sub>(l)<\/sub><br \/>\n\t\t<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S18.png\" alt=\"\"\/>H<sub>2<\/sub>SO<sub>4(aq)  <\/sub>+  KOH<sub>(aq)<\/sub>                K<sub>2<\/sub>SO<sub>4(aq)  <\/sub>+   H<sub>2<\/sub>O<sub>(aq)<\/sub><\/p>\n<p>\u00a02. <strong>Acid salt<\/strong>s: Acid salts are formed when the replaceable hydrogen ion in the acids are only partially replaced by a metal e.g. NaHSO<sub>4<\/sub>, Na<sub>2<\/sub>HPO<sub>4<\/sub>, NaH<sub>2<\/sub>PO<sub>4<\/sub>, NaHCO<sub>3<\/sub>. They can be produce from acids which contain more than one replaceable hydrogen ion. Acids with two replaceable hydrogen ions can form only one acid salt while acid with three replaceable hydrogen ions can form two different acid salts<br \/>\n<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S19.png\" alt=\"\"\/>H<sub>2<\/sub>SO<sub>4(aq)    <\/sub>+    NaOH<sub>(aq)<\/sub>              NaHSO<sub>4(aq)  <\/sub>+  H<sub>2<\/sub>O<sub>(l)<\/sub><br \/>\n\t\t<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S20.png\" alt=\"\"\/>2H<sub>3<\/sub>PO<sub>4(aq)   <\/sub>+   3NaOH<sub>(aq)<\/sub>              NaH<sub>2<\/sub>PO<sub>4(aq)  <\/sub>+ Na<sub>2<\/sub>HPO<sub>4(aq)  <\/sub>+3H<sub>2<\/sub>O<sub>(l)<\/sub><br \/>\n\t\tAcid salts turn blue litmus red. Acid salts can be converted to normal salt if the remaining replaceable hydrogen ions in the acid salt are replaced in with metallic ions.<br \/>\n<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S21.png\" alt=\"\"\/>KHSO<sub>4(aq)   <\/sub>+    KOH<sub>(aq)<\/sub>               K<sub>2<\/sub>SO<sub>4(aq)<\/sub>  +  H<sub>2<\/sub>O<sub>(l)<\/sub><\/p>\n<p>\u00a03. <strong>Basic salts<\/strong>: Basic salts are formed when only part of the hydroxide ions of a base are replaced by the negative ions from an acid. It can occur when there is insufficient supply of acid for complete neutralization of the base e.g Zn(OH)Cl , Mg(OH)Cl, Mg(OH)NO<sub>3<\/sub>, Bi(OH)<sub>2<\/sub>NO<sub>3<\/sub> e. t .c.<br \/>\n<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S22.png\" alt=\"\"\/>Zn(OH)<sub>2(aq)<\/sub>   +   HCl<sub>(aq)<\/sub>              Zn(OH)Cl<sub>(aq)<\/sub>  +   H<sub>2<\/sub>O<sub>(l)<\/sub><\/p>\n<p>\u00a0Because of the presence of hydroxide ion in the salt, it has basic properties. Basic salts turn red litmus blue. Basic salts react with excess acid to form a normal salt and water only.<br \/>\n<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S23.png\" alt=\"\"\/>Mg(OH)NO<sub>3(aq)   <\/sub>+  HNO<sub>3(aq)<\/sub>              Mg(NO<sub>3<\/sub>)<sub>2(aq)<\/sub>   +  H<sub>2<\/sub>O<sub>(l)<\/sub><\/p>\n<p>\u00a04. <strong>Double salts<\/strong>: Double salts are salt which ionize to produce three different types of ions in solution. Usually two of these are positively charged (metallic or NH4<sup>+<\/sup> ion) while the other is negatively charged e.g. (NH<sub>4<\/sub>)<sub>2<\/sub>Fe(SO<sub>4<\/sub>)<sub>2<\/sub>.6H<sub>2<\/sub>O, KAl(SO<sub>4<\/sub>)<sub>2<\/sub>.12H<sub>2<\/sub>O, KCr(SO<sub>4<\/sub>)<sub>2<\/sub>.12H<sub>2<\/sub>O.<br \/>\n(NH<sub>4<\/sub>)<sub>2<\/sub>Fe(SO<sub>4<\/sub>)<sub>2<\/sub>.6H<sub>2<\/sub>O: Ammonium iron (II) tetraoxosulphate (VI) hexahydrate.<br \/>\nKAl (SO<sub>4<\/sub>)<sub>2<\/sub>.12H<sub>2<\/sub>O: Aluminium Potassium tetraoxosulphate (V) dodecahydrate (Potash alum).<br \/>\nKCr (SO<sub>4<\/sub>)<sub>2<\/sub>.12H<sub>2<\/sub>O: Chromium (III) Potassium tetraoxosulphate (VI) dodecahydrate (Chrome alum).<\/p>\n<p>\u00a05. <strong>Complex salts<\/strong>: Complex salts contains complex ion i.e ion consisting of a charged group of atom e.g. Na<sub>2<\/sub>Zn(OH)<sub>4<\/sub>, K<sub>4<\/sub>Fe(CN)<sub>6<\/sub>, NaAl(OH)<sub>4<\/sub>.<br \/>\nNa<sub>2<\/sub>Zn(OH)<sub>4<\/sub>: Sodium tetrahydroxozincate (ii)<br \/>\nK<sub>4<\/sub>Fe(CN)<sub>6 <\/sub>:<sub><br \/>\n\t\t\t<\/sub>Potassium hexacyanoferrate (iii)<br \/>\nNaAl(OH)<sub>4<\/sub>:<sub><br \/>\n\t\t\t<\/sub>Sodium tetrahydroxoaluminate (iii)<br \/>\n<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S24.png\" alt=\"\"\/>Na<sub>2<\/sub>Zn(OH)<sub>4<\/sub>              2Na<sup>+<\/sup>   +   [Zn(OH)<sub>4<\/sub>]<sup>2-<\/sup><br \/>\n\t\t<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S25.png\" alt=\"\"\/>K<sub>4<\/sub>Fe(CN)<sub>6  <\/sub>               4K<sup>+<\/sup>    +     [Fe(CN)<sub>6<\/sub>]<sup>4-<\/sup>.<\/p>\n<p>\u00a0<strong>HYDROLYSIS OF SALT<\/strong><br \/>\n\t\tSome salts undergoes hydrolysis in water to give an acidic or alkaline medium (solution) e.g. Na<sub>2<\/sub>CO<sub>3<\/sub>, NaHCO<sub>3<\/sub>, AlCl<sub>3<\/sub>, Na<sub>2<\/sub>S, NH<sub>4<\/sub>Cl, CH<sub>3<\/sub>COONa e.t.c.<br \/>\n<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S26.png\" alt=\"\"\/>Na<sub>2<\/sub>CO<sub>3<\/sub> + H<sub>2<\/sub>O                   NaOH   +   H<sub>2<\/sub>CO<sub>3<\/sub>.<br \/>\n<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S27.png\" alt=\"\"\/>AlCl<sub>3<\/sub>   +   H<sub>2<\/sub>O                  Al (OH)<sub>3<\/sub>  +   HCl.<br \/>\n<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S28.png\" alt=\"\"\/>Na<sub>2<\/sub>S    +   H<sub>2<\/sub>O                  NaOH    +    H<sub>2<\/sub>S<br \/>\nHydrolysis of salt occurs when a salt react with water e.g salt of strong acid and weak base gives acidic solution. The change in PH of solution is due to hydrolysis.<\/p>\n<p>\u00a0<strong>USES OF SALTS<\/strong><br \/>\n\t\t1. NH<sub>4<\/sub>Cl is used as an electrolyte in dry cell (Leclanche cell)<br \/>\n2. CaCO<sub>3<\/sub> is used as medicine to neutralise acidity in the stomach<br \/>\n3. CaCl<sub>2<\/sub> is used as antifreeze while fused CaCl<sub>2<\/sub> is used as a drying agent and also in dessicator.<br \/>\n4. CaSO<sub>4<\/sub> is used for making plaster of Paris.<br \/>\n5. CuSO<sub>4<\/sub> is used in dyeing and calico printing.<br \/>\n6. MgSO<sub>4<\/sub> is used as a laxative.<br \/>\n7. KNO<sub>3<\/sub> is used for making gunpowder, matches and soil fertilizer.<br \/>\n8. NaCl is used for preserving food and in glazing pottery.<br \/>\n9. ZnCl<sub>2<\/sub> is used in petroleum refining<\/p>\n<p>\u00a0<strong>EVALUATION<\/strong><br \/>\n\t1. Define salt?<br \/>\n2.\u00a0\u00a0\u00a0\u00a0List the five main types of salts giving two examples each<br \/>\n3. Name four salts and state the use of each of them<\/p>\n<p>\u00a0<strong>SOLUBILITY RULE<\/strong><\/p>\n<div>\n<table>\n<tbody>\n<tr>\n<td><strong>S\/NO<\/strong><\/td>\n<td><strong>SOLUBLE SALTS<\/strong><\/td>\n<td><strong>INSOLUBLE SALTS<\/strong><\/td>\n<\/tr>\n<tr>\n<td>1.\u00a0<\/td>\n<td>All Na<sup>+<\/sup>, K<sup>+<\/sup> and NH<sub>4<\/sub><sup>+<\/sup> salt<\/td>\n<td>\u00a0<\/td>\n<\/tr>\n<tr>\n<td>2.\u00a0<\/td>\n<td>All trioxonitrate (v)\u00a0<\/td>\n<td>\u00a0<\/td>\n<\/tr>\n<tr>\n<td>3.\u00a0<\/td>\n<td>All chloride except\u00a0<\/td>\n<td>PbCl<sub>2<\/sub>, HgCl<sub>2<\/sub> and AgCl are soluble in hot water.<\/td>\n<\/tr>\n<tr>\n<td>4.\u00a0<\/td>\n<td>Trioxocarbonate (iv) of Na<sup>+<\/sup>, K<sup>+<\/sup> and NH<sub>4<\/sub><sup>+<\/sup><\/td>\n<td>All other trioxocarbonate (iv).\u00a0<\/td>\n<\/tr>\n<tr>\n<td>5.\u00a0<\/td>\n<td>Trioxosulphate (vi) of Na<sup>+<\/sup>, K<sup>+<\/sup>, NH<sub>4<\/sub><sup>+<\/sup> &amp; Cu<sup>2+<\/sup><\/td>\n<td>All other trioxosulphate (IV)\u00a0<\/td>\n<\/tr>\n<tr>\n<td>6.\u00a0<\/td>\n<td>Sulphide of Na<sup>+<\/sup>, K<sup>+<\/sup> and NH<sub>4<\/sub><sup>+<\/sup><\/td>\n<td>All other sulphide.\u00a0<\/td>\n<\/tr>\n<tr>\n<td>7.\u00a0<\/td>\n<td>All tetraoxosulphate (vi) except\u00a0<\/td>\n<td>PbSO<sub>4<\/sub>, BaSO<sub>4<\/sub> and CaSO<sub>4<\/sub> are slightly soluble in H<sub>2<\/sub>O<\/td>\n<\/tr>\n<tr>\n<td>8.\u00a0<\/td>\n<td>All hydrogen trioxocarbonate (iv)\u00a0<\/td>\n<td>\u00a0<\/td>\n<\/tr>\n<tr>\n<td><strong>S\/NO<\/strong><\/td>\n<td><strong>SOLUBLE BASE\/ALKALIS<\/strong><\/td>\n<td><strong>INSOLUBLE BASE\/ALKALIS<\/strong><\/td>\n<\/tr>\n<tr>\n<td>1.\u00a0<\/td>\n<td>K<sub>2<\/sub>O, Na<sub>2<\/sub>O are very soluble<br \/>\nMgO, CaO are slightly soluble\u00a0<\/td>\n<td>Other oxide are insoluble\u00a0<\/td>\n<\/tr>\n<tr>\n<td>2.\u00a0<\/td>\n<td>NaOH, KOH, Ca(OH)<sub>2<\/sub> are very soluble<br \/>\nMg (OH)<sub>2<\/sub> is slightly soluble.<\/td>\n<td>Other hydroxides are insoluble.\u00a0<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<\/div>\n<p>\u00a0<strong>METHOD OF PREPARATION OF SALTS<\/strong><br \/>\n\t\tThe method of preparing a particular salt depends on its:<br \/>\n1. Solubility in water<br \/>\n2. Stability to heat.<br \/>\nIt is necessary, therefore, for us to become familiar with the simple rules of solubility indicated above. Knowing the solubility of the salt enables us to determine which method to be used.<\/p>\n<p>\u00a0<strong>SOLUBLE SALT<br \/>\n<\/strong>Soluble salts can be prepared by the following method:<br \/>\n1. Neutralization of an acid by an alkali<br \/>\n2. Action of dilute acid on a metal.<br \/>\n3. Action of dilute acid on an insoluble base.<br \/>\n4. Action of dilute acid on trioxocarbonate (IV).<\/p>\n<p>\u00a0<strong>RECOVERING SOLUBLE SALTS FROM SOLUTION<\/strong><br \/>\n\t\tThis can be done by:<br \/>\n1. Heating to dryness: This is used to prepare soluble salts which are not destroyed or decomposed by heat e.g. most chlorides such as NaCl, ZnCl<sub>2<\/sub>, FeCl<sub>2<\/sub> and FeCl<sub>3<\/sub> are recovered by heating.<br \/>\n2. Crystallization: This is used to prepare salt which are easily decomposed or destroyed by dry heating. All trioxonitrate (V) and tetraoxosulphate (VI) are recovered by crystallization.<\/p>\n<p>\u00a0<strong>INSOLUBLE SALTS<br \/>\n<\/strong>Insoluble salts can be prepared by the following method:<br \/>\n1. Double decomposition or precipitation.<br \/>\n<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S29.png\" alt=\"\"\/>Pb (NO<sub>3<\/sub>)<sub>2(aq)<\/sub>    +    2NaCl<sub> (aq)<\/sub>                  2NaNO<sub>3 (aq)<\/sub>   + PbCl<sub>2(s)<\/sub><br \/>\n\t\t<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S30.png\" alt=\"\"\/>AgNO<sub>3 (aq)<\/sub>       +      NH<sub>4<\/sub>Cl<sub> (aq)<\/sub>                 NH<sub>4<\/sub>NO<sub>3 (aq)   <\/sub>+ AgCl<sub>(s)<\/sub><\/p>\n<p>\u00a02. Direct combination of 2 elements.<br \/>\n<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S31.png\" alt=\"\"\/>Fe<sub>(s)<\/sub>    +    S<sub>(s)<\/sub>                    FeS<sub>(s)<\/sub><br \/>\n\t\t<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S32.png\" alt=\"\"\/>2Fe(<sub>s)<\/sub> +   3Cl<sub>2(g)<\/sub>                 2FeCl<sub>3(s)<\/sub><\/p>\n<p>\u00a0<strong>ANHYDROUS AND HYDRATED SALT<br \/>\n<\/strong>Anhydrous salts: are salts which do not contain water and cannot be crystallized out from aqueous solution.<\/p>\n<p>\u00a0Hydrated salts\/salts with water of crystallization: are salts which combine chemically with water. The water molecule is loosely held to the salt molecule and when heated, such salt lose their water of crystallization. The water attached is known as water of crystallization e.g<\/p>\n<p>\u00a0Cu(NO<sub>3<\/sub>)<sub>2<\/sub>.3H<sub>2<\/sub>O:  Copper (ii) trioxonitrate (v) trihydrate.<br \/>\nMgSO<sub>4<\/sub>.7H<sub>2<\/sub>O: Magnesium tetraoxosulphate (vi) heptahydrate.<br \/>\nFeSO<sub>4<\/sub>.7H<sub>2<\/sub>O: Iron (ii) tetraoxosulphate (vi) heptahydrate.<\/p>\n<p>\u00a0<\/p>\n<div>\n<table>\n<tbody>\n<tr>\n<td>Salts without water of crystallization\u00a0<\/td>\n<td>Salts with water of crystallization\u00a0<\/td>\n<\/tr>\n<tr>\n<td>NaCl\u00a0<\/td>\n<td>CuSO<sub>4<\/sub>.5H<sub>2<\/sub>O<\/td>\n<\/tr>\n<tr>\n<td>KNO<sub>3<\/sub><\/td>\n<td>FeSO<sub>4<\/sub>.7H<sub>2<\/sub>O<\/td>\n<\/tr>\n<tr>\n<td>KMnO<sub>4<\/sub><\/td>\n<td>ZnSO<sub>4<\/sub>.7H<sub>2<\/sub>O<\/td>\n<\/tr>\n<tr>\n<td>(NH<sub>4<\/sub>)<sub>2<\/sub>SO<sub>4<\/sub><\/td>\n<td>Na<sub>2<\/sub>CO<sub>3<\/sub>.10H<sub>2<\/sub>O<\/td>\n<\/tr>\n<tr>\n<td>K<sub>2<\/sub>SO<sub>4<\/sub><\/td>\n<td>Cu(NO<sub>3<\/sub>)<sub>2<\/sub>.3H<sub>2<\/sub>O<\/td>\n<\/tr>\n<tr>\n<td>Pb(NO<sub>3<\/sub>)<sub>2<\/sub><\/td>\n<td>MgSO<sub>4<\/sub>.7H<sub>2<\/sub>O<\/td>\n<\/tr>\n<tr>\n<td>AgNO<sub>3<\/sub><\/td>\n<td>Zn(NO<sub>3<\/sub>)<sub>2<\/sub>.6H<sub>2<\/sub>O.<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<\/div>\n<p>\u00a0Calculation of water of crystallization<br \/>\n14g of hydrated H<sub>2<\/sub>C<sub>2<\/sub>O<sub>4<\/sub>.xH<sub>2<\/sub>O was heated to give an anhydrous salt weighing 9.99g.<br \/>\n(a). Calculate the value of x.<br \/>\n(b). Give the formula of the hydrated salt.<br \/>\n(c). Calculate the % of water of crystallization.<\/p>\n<p>\u00a0Solution<br \/>\n(a).\u00a0\u00a0\u00a0\u00a0Mass of hydrated salt \u00a0\u00a0\u00a0\u00a0 =\u00a0\u00a0\u00a0\u00a0 Molar mass of hydrated salt<br \/>\nMass of water molecule \u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0Molar mass of water molecule<br \/>\n14           =    (90+18x)<br \/>\n(14-9.99)              18x<br \/>\n14     =    (90 +18x)<br \/>\n4.01            18x<br \/>\n14(18x) = 4.01 (90 + 18x)<br \/>\n252x = 360.9 + 72.18x<br \/>\n252x \u2013 72.18x = 360.9<br \/>\n179.82x = 360.9<br \/>\nx = 360.9\/179.82<br \/>\nx = 2.007<br \/>\nx = 2 to the nearest whole number.<br \/>\n(b) Formula of hydrated salt = H<sub>2<\/sub>C<sub>2<\/sub>0<sub>4<\/sub>.2H<sub>2<\/sub>0.<br \/>\n(c) To calculate the % of water of crystallization:<br \/>\n% of water of crystallization = Mass of water x 100%<br \/>\nTotal mass<br \/>\n=        36        x 100<br \/>\n(90 + 36)<br \/>\n=   36    x   100<br \/>\n126<br \/>\n= 3600<br \/>\n126<br \/>\n= 28.57%<\/p>\n<p>\u00a0<strong>EFFLORESCENCE, DELIQUESCENCE AND HYGROSCOPIC<\/strong><br \/>\n\tWhen certain compound is exposed to the air, they either lose their water of crystallization or they absorb moisture from their surroundings. The term efflorescent, deliquescent and hygroscopic are used to describe such compound.<\/p>\n<p>\u00a0<strong>EFFLORESCENTS<\/strong>: are substances which on exposure to air, lose some or all of their water of crystallization. The phenomenon or process is efflorescence. There is loss of weight or mass of the substances.<br \/>\n<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S33.png\" alt=\"\"\/>e.g Na<sub>2<\/sub>CO<sub>3<\/sub>.10H<sub>2<\/sub>O             Na<sub>2<\/sub>CO<sub>3<\/sub>.H<sub>2<\/sub>O     +       9H<sub>2<\/sub>O<br \/>\nOther examples are Na<sub>2<\/sub>SO<sub>4<\/sub>.10H<sub>2<\/sub>O, MgSO<sub>4<\/sub>.7H<sub>2<\/sub>O and CuSO<sub>4<\/sub>.5H<sub>2<\/sub>O e.t.c<\/p>\n<p>\u00a0<strong>DELIQUESCENTS<\/strong>: are substances that absorb so much water from air and form a solution e.g. NaOH, CaCl<sub>2<\/sub>, FeCl<sub>3<\/sub>, MgCl<sub>2<\/sub>, KOH and P<sub>4<\/sub>O<sub>10<\/sub>. There is a gain in weight.<\/p>\n<p>\u00a0<strong>HYGROSCOPIC<\/strong>: are substances which absorb moisture on exposure to the atmosphere without forming a solution. If they are solids, no solution will be formed but if a liquid absorb water, it gets diluted. There is little or no difference in mass e.g Conc. H<sub>2<\/sub>SO<sub>4<\/sub>, NaNO<sub>3<\/sub>, CuO, CaO and anhydrous Na<sub>2<\/sub>CO<sub>3<\/sub>.<\/p>\n<p>\u00a0<strong>DRYING AGENTS<\/strong><br \/>\n\tThese are substances which have high affinity for water or moisture. They are either deliquescent or hygroscopic. They remove water molecules to effect physical change. Drying agents are different from dehydrating agents which removes elements of water i.e hydrogen and oxygen atoms or intra-molecular water.<br \/>\nDrying agents which react with gases are not used to dry the gas e.g conc. H<sub>2<\/sub>SO<sub>4<\/sub> is not used to dry NH<sub>3<\/sub> and H<sub>2<\/sub>S gas.<br \/>\n<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S34.png\" alt=\"\"\/>NH<sub>3(g)        <\/sub>+      H<sub>2<\/sub>SO<sub>4(aq)<\/sub>         (NH<sub>4<\/sub>)<sub>2<\/sub>SO<sub>4(aq)<\/sub><br \/>\n\t<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100323_0805_Week2ad3S35.png\" alt=\"\"\/>H<sub>2<\/sub>S<sub>(g)<\/sub>     +      H<sub>2<\/sub>SO<sub>4(aq)<\/sub>          2H<sub>2<\/sub>O<sub>(l)  <\/sub>+    SO<sub>2(g)   <\/sub>+    S<sub>(s)<\/sub><\/p>\n<div>\n<table>\n<tbody>\n<tr>\n<td>Drying agent\u00a0<\/td>\n<td>Gases\u00a0<\/td>\n<\/tr>\n<tr>\n<td>Conc. H<sub>2<\/sub>SO<sub>4<\/sub><\/td>\n<td>All gases except NH<sub>3<\/sub> &amp; H<sub>2<\/sub>S<\/td>\n<\/tr>\n<tr>\n<td>Fused CaCl<sub>2<\/sub><\/td>\n<td>All gases except NH<sub>3<\/sub><\/td>\n<\/tr>\n<tr>\n<td>CaO or quicklime\u00a0<\/td>\n<td>For ammonia\u00a0<\/td>\n<\/tr>\n<tr>\n<td>P<sub>2<\/sub>O<sub>5<\/sub><\/td>\n<td>All gases except ammonia\u00a0<\/td>\n<\/tr>\n<tr>\n<td>Silica gel\u00a0<\/td>\n<td>All gases\u00a0<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<\/div>\n<p>Salts are usually dried in dessicator.<\/p>\n<p>\u00a0<strong>EVALUATION<\/strong><br \/>\n\t1.\u00a0Using balanced equations, state two methods of preparing: (a) Soluble salt (b) insoluble salt<br \/>\n2.\u00a0How can soluble salts be recovered from their solution?<\/p>\n<p>\u00a0<strong>GENERAL EVALUATION\/REVISION<\/strong><br \/>\n\t1.\u00a0\u00a0\u00a0\u00a0Calculate the percentage of water in sodium trioxocarbonate (iv) heptahydrate<br \/>\n2.\u00a0\u00a0\u00a0\u00a0What is the number of molecules in 6.4g of sulphur (iv) oxide (N<sub>A<\/sub>=6.0X10<sup>23<\/sup>\/mol)<br \/>\n3.\u00a0\u00a0\u00a0\u00a0Write an equation to show the acid formed when phosphorus (v) oxide is dissolved in cold water and name the acid formed<br \/>\n4.\u00a0\u00a0\u00a0\u00a0Differentiate between a base and an alkali<br \/>\n5.\u00a0\u00a0\u00a0\u00a0Define: Efflorescence, Deliquescence and Hygroscopy<\/p>\n<p>\u00a0<strong>READING ASSIGNMENT<\/strong><br \/>\n\tNew School Chemistry for Senior Secondary Schools by O.Y Ababio pages 100-101 and 108-115.<\/p>\n<p>\u00a0<strong>WEEKEND ASSIGNMENT<\/strong><br \/>\n\t1.\u00a0\u00a0\u00a0\u00a0The two types of bonds that exist in H<sub>3<\/sub>O<sup>+<\/sup> are a. covalent and ionic b. co-ordinate covalent and covalent c. metallic and ionic d. polar covalent and metallic<br \/>\n2.  How many moles of hydrogen ions are there in 50cm<sup>3<\/sup> of 0.20moldm<sup>-3<\/sup> H<sub>2<\/sub>SO<sub>4<\/sub>?<br \/>\na. 0.01 b 0.02 c 0.10 d 0.20<br \/>\n3.  Which of these is not recovered through dry heating (evaporation)?<br \/>\na. NaClO<sub>3<\/sub> b. NH<sub>4<\/sub>NO<sub>3<\/sub> c. CuHSO<sub>4 <\/sub>d. NaHCO<sub>3<\/sub>.<br \/>\n4.  Which pH value indicates a basic solution? a. -1 b.3 c.9 d.7<br \/>\n5. All common gases are dried using P<sub>2<\/sub>O<sub>5<\/sub> except a. NO<sub>2<\/sub> b. NH<sub>3<\/sub> c. SO<sub>2<\/sub> d. H<sub>2<\/sub>S<\/p>\n<p>\u00a0<strong>THEORY<\/strong><br \/>\n\t1.  Give the reason for each of the following:<br \/>\na. Sodium salts cannot be prepared by double decomposition<br \/>\nb. Na<sub>2<\/sub>CO<sub>3(aq)<\/sub> which is a salt solution, turns red litmus blue.<br \/>\n2.  1.34g of hydrated Na<sub>2<\/sub>SO<sub>4<\/sub> was heated to give an anhydrous salt weighing<br \/>\n0.71g.<br \/>\na. Calculate the number of molecules of water of crystallization<br \/>\nb. Give the formula of the hydrated salt [Na=23, S=32, O=16, H=1].<\/p>\n<p>\u00a0<br \/>\n\t\t\u00a0<\/p>\n","protected":false},"excerpt":{"rendered":"<p>WEEK TWO AND THREE TOPIC: BASES AND SALTS CONTENT Bases Salts Efflorescence, deliquescence and hygroscopic&#8230;<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[1,209],"tags":[],"class_list":["post-2489","post","type-post","status-publish","format-standard","hentry","category-posts","category-third-term-ss1-chemistry"],"aioseo_notices":[],"_links":{"self":[{"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/posts\/2489","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/comments?post=2489"}],"version-history":[{"count":1,"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/posts\/2489\/revisions"}],"predecessor-version":[{"id":2490,"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/posts\/2489\/revisions\/2490"}],"wp:attachment":[{"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/media?parent=2489"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/categories?post=2489"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/tags?post=2489"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}