{"id":37343,"date":"2026-11-02T02:30:15","date_gmt":"2026-11-02T02:30:15","guid":{"rendered":"https:\/\/www.vedprep.com\/exams\/?p=37343"},"modified":"2026-11-02T02:30:15","modified_gmt":"2026-11-02T02:30:15","slug":"calcium-oxide-reaction-with-water","status":"publish","type":"post","link":"https:\/\/www.vedprep.com\/exams\/csir-net\/calcium-oxide-reaction-with-water\/","title":{"rendered":"Calcium Oxide Reaction With Water: Ultimate Guide for CSIR"},"content":{"rendered":"<article>\n<h1>Calcium Oxide Reaction with Water: Ultimate Guide for CSIR NET<\/h1>\n<p>Master the <strong>calcium oxide reaction with water<\/strong>\u2014a high-yield topic for CSIR NET\u2014with balanced equations, thermodynamic data, safety protocols, and exam-focused problem-solving techniques.<\/p>\n<p>The <strong>calcium oxide reaction with water<\/strong> is a cornerstone of inorganic chemistry, producing calcium hydroxide while releasing 64.8 kJ\/mol of heat. This exothermic reaction appears frequently in CSIR NET exams, requiring precise stoichiometric calculations and thermodynamic understanding.<\/p>\n<\/p>\n<h2>Why the Calcium Oxide Reaction with Water Matters for CSIR NET<\/h2>\n<p>The <strong>calcium oxide reaction with water<\/strong> is a staple in the CSIR NET Physical Chemistry syllabus, specifically under Reaction Kinetics and Thermodynamics. It exemplifies exothermic hydration, a concept tested through:<\/p>\n<ul>\n<li>Balanced chemical equations (CaO + H\u2082O \u2192 Ca(OH)\u2082)<\/li>\n<li>Enthalpy change calculations (\u0394H\u00b0 = \u201364.8 kJ\/mol)<\/li>\n<li>Stoichiometric problems involving heat release<\/li>\n<li>Safety considerations in laboratory settings<\/li>\n<\/ul>\n<p>Refer to <em>Physical Chemistry<\/em> by O.P. Tandon (Chapter 3) and <em>Modern Approach to Chemical Calculations<\/em> by B.K. Sharma for detailed worked examples. These resources provide thermodynamic tables and step-by-step stoichiometric guidance, essential for solving CSIR NET numerical problems efficiently.<\/p>\n<p>Exam patterns typically include:<\/p>\n<ul>\n<li>Two multiple-choice questions on reaction mechanisms<\/li>\n<li>One numerical problem requiring heat-of-reaction calculations<\/li>\n<li>Descriptive questions on safety protocols<\/li>\n<\/ul>\n<p>Understanding the <strong>calcium oxide reaction with water<\/strong> ensures you can confidently tackle these questions within the exam\u2019s time constraints.<\/p>\n<\/p>\n<h2>Step-by-Step: The Calcium Oxide Reaction with Water Mechanism<\/h2>\n<p>When water is added to calcium oxide (quicklime), an instantaneous exothermic reaction occurs, forming calcium hydroxide (slaked lime):<\/p>\n<div class=\"chemical-equation\">CaO(s) + H\u2082O(l) \u2192 Ca(OH)\u2082(s) \u0394H\u00b0 = \u201364.8 kJ\/mol<\/div>\n<p>The reaction demonstrates a classic oxide-to-base conversion, where the solid calcium oxide reacts vigorously with water to produce a white, moist slurry of calcium hydroxide. This process is highly exothermic, releasing enough heat to raise the mixture\u2019s temperature to ~200\u00b0C if unchecked.<\/p>\n<p>The product, calcium hydroxide, is a strong base that dissociates completely in water, releasing OH\u207b ions. This property makes it invaluable for neutralizing acids in laboratory and industrial settings. The reverse reaction (dehydration of Ca(OH)\u2082 to CaO) requires temperatures exceeding 500\u00b0C, making the hydration process effectively irreversible under normal conditions.<\/p>\n<p><strong>Safety Note:<\/strong> Always wear protective gloves and goggles when performing this reaction, as the sudden heat release can cause burns and the caustic slurry can irritate skin and eyes.<\/p>\n<p>The <strong>calcium oxide reaction with water<\/strong> is a prime example of an acid-base neutralization, where a basic oxide converts to a soluble hydroxide. This concept is frequently tested in CSIR NET inorganic chemistry sections.<\/p>\n<\/p>\n<h2>Laboratory Procedure: Performing the Calcium Oxide Reaction with Water Safely<\/h2>\n<p>To conduct the <strong>calcium oxide reaction with water<\/strong> safely and effectively, follow these steps:<\/p>\n<ol>\n<li><strong>Equipment:<\/strong> Use a heat-resistant borosilicate glass beaker to contain the reaction mixture.<\/li>\n<li><strong>Safety Gear:<\/strong> Wear protective gloves, safety goggles, and a lab coat to prevent exposure to the hot, caustic slurry.<\/li>\n<li><strong>Reaction Setup:<\/strong> Add water dropwise to the calcium oxide using a glass rod. This controlled addition prevents violent splattering and allows you to observe the reaction\u2019s exothermic nature.<\/li>\n<li><strong>Observation:<\/strong> Vigorous bubbling and a noticeable temperature rise (recorded with a thermometer) indicate the reaction\u2019s progress. The temperature change can be used to calculate the enthalpy change (\u0394H) using the formula:<\/p>\n<div class=\"formula\">\u0394H = \u2013m\u00b7c\u00b7\u0394T<\/div>\n<p>where <em>m<\/em> is the mass of water, <em>c<\/em> is the specific heat capacity of water (4.18 J\/g\u00b7\u00b0C), and <em>\u0394T<\/em> is the temperature change.<\/li>\n<li><strong>Post-Reaction:<\/strong> After the reaction completes, filter and weigh the solid calcium hydroxide to confirm stoichiometric conversion. This step provides empirical validation of the theoretical yield.<\/li>\n<li><strong>Volume Control:<\/strong> Limit the water volume to approximately half the mass of calcium oxide to avoid overflow and ensure manageable reaction conditions.<\/li>\n<\/ol>\n<p>This procedure ensures both safety and accuracy in demonstrating the <strong>calcium oxide reaction with water<\/strong>.<\/p>\n<\/p>\n<h2>Industrial Applications of the Calcium Oxide Reaction with Water<\/h2>\n<p>The <strong>calcium oxide reaction with water<\/strong> is foundational to several key industries:<\/p>\n<ul>\n<li><strong>Cement Manufacturing:<\/strong> Quicklime (CaO) is slaked to produce hydrated lime (Ca(OH)\u2082), a critical binding agent in mortar and concrete.<\/li>\n<li><strong>Water Treatment:<\/strong> Quicklime raises pH levels and precipitates impurities, while the exothermic reaction provides useful thermal energy.<\/li>\n<li><strong>Thermal Energy Storage:<\/strong> The heat released during hydration is captured and stored for later use in industrial processes.<\/li>\n<li><strong>Flue-Gas Desulfurization:<\/strong> Calcium hydroxide reacts with sulfur dioxide to form gypsum, a safe byproduct used in construction.<\/li>\n<li><strong>Paper and Textile Industries:<\/strong> Slaked lime breaks down lignin in paper pulp and neutralizes acidic dyes in textiles, improving fabric strength.<\/li>\n<\/ul>\n<p>In all these applications, the <strong>calcium oxide reaction with water<\/strong> underpins large-scale chemical processes, highlighting its industrial significance.<\/p>\n<p><strong>Safety Protocols:<\/strong> Industrial settings require protective clothing, proper ventilation, and automated water feed systems to control heat release and prevent hazards.<\/p>\n<\/p>\n<h2>Worked Example: Calculating Heat Released in the Calcium Oxide Reaction with Water<\/h2>\n<p><strong>Problem:<\/strong> A 5.0 g sample of calcium oxide is mixed with excess water. Calculate the amount of heat evolved in kilojoules, indicating whether the process is exothermic or endothermic.<\/p>\n<p><strong>Solution:<\/strong><\/p>\n<ol>\n<li><strong>Calculate moles of CaO:<\/strong><\/li>\n<div class=\"formula\">n = mass \/ molar mass = 5.0 g \/ 56.08 g\/mol \u2248 0.0892 mol<\/div>\n<li><strong>Use the standard enthalpy change:<\/strong> The <strong>calcium oxide reaction with water<\/strong> has \u0394H\u00b0 = \u201364.8 kJ\/mol.<\/li>\n<li><strong>Calculate heat evolved:<\/strong><\/li>\n<div class=\"formula\">q = n \u00d7 \u0394H\u00b0 = 0.0892 mol \u00d7 (\u201364.8 kJ\/mol) \u2248 \u20135.77 kJ<\/div>\n<li><strong>Interpret the result:<\/strong> The negative sign indicates heat is released, confirming the process is exothermic. Thus, 5.77 kJ of energy is given off during the reaction.<\/li>\n<\/ol>\n<p>This calculation demonstrates how the <strong>calcium oxide reaction with water<\/strong> releases significant thermal energy, a key concept for CSIR NET thermodynamics questions.<\/p>\n<\/p>\n<h2>Common Misconceptions About the Calcium Oxide Reaction with Water<\/h2>\n<p>A prevalent misconception is that calcium oxide (quicklime) is inert until heated. However, the <strong>calcium oxide reaction with water<\/strong> occurs spontaneously at room temperature, producing calcium hydroxide and releasing heat. This reaction can raise the mixture\u2019s temperature to over 100\u00b0C, posing safety risks if water is added too quickly.<\/p>\n<p>Ignoring the exothermic nature of the <strong>calcium oxide reaction with water<\/strong> can lead to:<\/p>\n<ul>\n<li>Incorrect stoichiometric calculations<\/li>\n<li>Safety hazards, such as burns or equipment damage<\/li>\n<li>Misinterpretation of thermodynamic data<\/li>\n<\/ul>\n<p>Understanding that quicklime is highly reactive with moisture ensures proper laboratory techniques, such as slow water addition and protective gear use.<\/p>\n<\/p>\n<h2>Real-World Applications: Calcium Hydroxide in Construction<\/h2>\n<p>The product of the <strong>calcium oxide reaction with water<\/strong>, calcium hydroxide (hydrated lime), is a vital component in construction. When mixed with sand and water, it forms a paste that hardens through carbonation, trapping CO\u2082 from the air. This process raises the pH of the matrix, suppressing microbial growth and protecting embedded steel from corrosion.<\/p>\n<p>In concrete curing, engineers add lime to adjust pH and enhance the pozzolanic reaction between cement and silica. This accelerates the formation of calcium silicate hydrate, the compound responsible for concrete\u2019s strength. Recycled lime from waste sources can also replace a portion of Portland cement, reducing CO\u2082 emissions.<\/p>\n<p>Stoichiometric calculations are critical in construction to determine the exact amount of lime needed for optimal water-to-lime ratios, ensuring proper setting time and structural integrity.<\/p>\n<\/p>\n<h2>CSIR NET Exam Strategy: Mastering the Calcium Oxide Reaction with Water<\/h2>\n<p>To excel in CSIR NET questions on the <strong>calcium oxide reaction with water<\/strong>, follow this structured approach:<\/p>\n<ol>\n<li><strong>Memorize Key Data:<\/strong> Recall the balanced equation <em>CaO + H\u2082O \u2192 Ca(OH)\u2082<\/em> and its enthalpy change (\u0394H\u00b0 = \u201364.8 kJ\/mol). Recognize that the reaction is exothermic, indicating heat loss.<\/li>\n<li><strong>Practice Stoichiometry:<\/strong> Solve numerical problems linking moles of reactants to heat evolved. Use the formula <em>q = m\u00b7c\u00b7\u0394T<\/em> to calculate temperature rises, allocating 3 minutes per problem.<\/li>\n<li><strong>Focus on Safety:<\/strong> Highlight the vigorous heat generation and the necessity of protective eyewear in descriptive answers.<\/li>\n<li><strong>Use VedPrep Resources:<\/strong> Utilize <a href=\"https:\/\/www.vedprep.com\/\">VedPrep<\/a> flashcards for \u0394H\u00b0 values and reaction steps, and watch this <a href=\"https:\/\/www.youtube.com\/watch?v=4kgyTSQnB9o\" target=\"_blank\" rel=\"noopener nofollow\">free lecture on the calcium oxide reaction with water<\/a> for visual reinforcement.<\/li>\n<li><strong>Spaced Repetition:<\/strong> Review enthalpy tables daily, solve two problems weekly, and test recall after 48 hours to reinforce long-term memory.<\/li>\n<\/ol>\n<p>This strategy ensures comprehensive preparation for CSIR NET questions on the <strong>calcium oxide reaction with water<\/strong>.<\/p>\n<\/p>\n<h2>Frequently Asked Questions About the Calcium Oxide Reaction with Water<\/h2>\n<section class=\"vedprep-faq\">\n<h3>Core Understanding<\/h3>\n<div class=\"faq-item\">\n<h4>What is the chemical reaction when water is added to calcium oxide?<\/h4>\n<div>\n<p>The <strong>calcium oxide reaction with water<\/strong> produces calcium hydroxide (Ca(OH)\u2082) and releases 64.8 kJ\/mol of heat. The resulting slurry, known as lime water, has a pH of around 12 due to its strong basic nature.<\/p>\n<\/div>\n<\/div>\n<div class=\"faq-item\">\n<h4>Why does the calcium oxide reaction with water generate heat?<\/h4>\n<div>\n<p>The reaction releases approximately 64.8 kJ\/mol due to the formation of strong O-H bonds in calcium hydroxide. This exothermic process can heat the mixture to temperatures dangerous to skin without proper protection.<\/p>\n<\/div>\n<\/div>\n<div class=\"faq-item\">\n<h4>Is calcium oxide the same as red oxide?<\/h4>\n<div>\n<p>No. Red oxide typically refers to iron(III) oxide (Fe\u2082O\u2083), a reddish pigment, while calcium oxide is a white, caustic solid derived from limestone. Their chemical properties and industrial uses differ significantly.<\/p>\n<\/div>\n<\/div>\n<div class=\"faq-item\">\n<h4>How does the ionic product of water relate to the calcium oxide reaction with water?<\/h4>\n<div>\n<p>The ionic product of water (Kw = 1.0 \u00d7 10\u207b\u00b9\u2074 at 25\u00b0C) describes water\u2019s auto-ionization. In the <strong>calcium oxide reaction with water<\/strong>, water dissociates to supply OH\u207b ions, which combine with Ca\u00b2\u207a to form Ca(OH)\u2082, driving the reaction forward.<\/p>\n<\/div>\n<\/div>\n<div class=\"faq-item\">\n<h4>Can calcium hydroxide react with carbon dioxide after hydration?<\/h4>\n<div>\n<p>Yes. Calcium hydroxide reacts with CO\u2082 to regenerate calcium carbonate (CaCO\u2083) and water, a reversible process used in lime cycle experiments and carbon capture technologies.<\/p>\n<\/div>\n<\/div>\n<\/section>\n<section class=\"vedprep-faq\">\n<h3>Exam Application<\/h3>\n<div class=\"faq-item\">\n<h4>How is the calcium oxide reaction with water relevant for CSIR NET?<\/h4>\n<div>\n<p>CSIR NET frequently tests the thermodynamics of the <strong>calcium oxide reaction with water<\/strong>, including stoichiometry, heat evolution, and the role of lime in neutralization. Mastering this reaction helps solve both multiple-choice and numerical problems efficiently.<\/p>\n<\/div>\n<\/div>\n<div class=\"faq-item\">\n<h4>What numerical problem can be derived from the calcium oxide reaction with water?<\/h4>\n<div>\n<p>A common problem involves calculating temperature rise using <em>q = m\u00b7c\u00b7\u0394T<\/em>, where <em>q<\/em> is the enthalpy of hydration (\u224864.8 kJ\/mol), <em>m<\/em> is the mass of water, and <em>c<\/em> is water\u2019s specific heat. Students must balance moles of CaO with water volume for accurate results.<\/p>\n<\/div>\n<\/div>\n<div class=\"faq-item\">\n<h4>Compare the reaction of sodium with water to the calcium oxide reaction with water.<\/h4>\n<div>\n<p>Sodium reacts violently with water, producing Na\u207a, OH\u207b, and H\u2082 gas while releasing ~368 kJ\/mol. In contrast, the <strong>calcium oxide reaction with water<\/strong> is milder, forming Ca(OH)\u2082 without gas evolution and releasing only ~64.8 kJ\/mol. Both are exothermic but differ in kinetics and products.<\/p>\n<\/div>\n<\/div>\n<div class=\"faq-item\">\n<h4>Which exam question links lime water reacting with chlorine?<\/h4>\n<div>\n<p>A CSIR NET question might ask: \u201cLime water (Ca(OH)\u2082) reacts with chlorine gas to produce which compounds?\u201d The answer is calcium hypochlorite (Ca(OCl)\u2082) and calcium chloride (CaCl\u2082), demonstrating oxidation-reduction chemistry.<\/p>\n<\/div>\n<\/div>\n<div class=\"faq-item\">\n<h4>How does the decomposition of calcium carbonate relate to the calcium oxide reaction with water?<\/h4>\n<div>\n<p>Calcium carbonate (CaCO\u2083) decomposes thermally to yield CaO and CO\u2082. The resulting CaO can then undergo the <strong>calcium oxide reaction with water<\/strong> to form Ca(OH)\u2082. This lime cycle\u2014calcination followed by slaking\u2014is a key topic in inorganic chemistry.<\/p>\n<\/div>\n<\/div>\n<\/section>\n<section class=\"vedprep-faq\">\n<h3>Common Mistakes<\/h3>\n<div class=\"faq-item\">\n<h4>Do students often confuse calcium oxide with calcium carbonate?<\/h4>\n<div>\n<p>Yes. Many incorrectly write CaO + H\u2082O \u2192 CaCO\u2083, overlooking the intermediate Ca(OH)\u2082. The correct pathway is CaO + H\u2082O \u2192 Ca(OH)\u2082, followed by CO\u2082 addition to form CaCO\u2083.<\/p>\n<\/div>\n<\/div>\n<div class=\"faq-item\">\n<h4>Is it correct to assume no heat is released in the calcium oxide reaction with water?<\/h4>\n<div>\n<p>No. The <strong>calcium oxide reaction with water<\/strong> is highly exothermic, releasing ~64.8 kJ\/mol. Ignoring this heat can lead to incorrect thermodynamic calculations and safety oversights.<\/p>\n<\/div>\n<\/div>\n<div class=\"faq-item\">\n<h4>Do learners incorrectly think calcium oxide dissolves completely in water?<\/h4>\n<div>\n<p>Calcium oxide does not dissolve; it reacts to form a suspension of Ca(OH)\u2082 particles. Assuming complete dissolution can mislead predictions about solution clarity and conductivity.<\/p>\n<\/div>\n<\/div>\n<div class=\"faq-item\">\n<h4>Why is comparing sodium\u2019s reaction with water to the calcium oxide reaction with water incorrect?<\/h4>\n<div>\n<p>Sodium reacts instantaneously with gas evolution, while CaO hydrates slowly via solid-liquid contact. Equating their rates ignores surface area and activation energy differences, leading to inaccurate kinetic conclusions.<\/p>\n<\/div>\n<\/div>\n<div class=\"faq-item\">\n<h4>What error arises when using the ionic product of water for strong bases like Ca(OH)\u2082?<\/h4>\n<div>\n<p>Kw applies only to pure water. In strong base solutions like Ca(OH)\u2082, [OH\u207b] exceeds 10\u207b\u2077 M, making Kw ineffective for pH prediction. Relying on Kw alone underestimates the alkalinity of slaked lime.<\/p>\n<\/div>\n<\/div>\n<\/section>\n<section class=\"vedprep-faq\">\n<h3>Advanced Concepts<\/h3>\n<div class=\"faq-item\">\n<h4>How does the calcium oxide reaction with water illustrate Le Chatelier\u2019s principle?<\/h4>\n<div>\n<p>Adding water shifts the equilibrium CaO \u21cc Ca(OH)\u2082 toward Ca(OH)\u2082 formation. The exothermic nature means increasing temperature reverses the reaction, demonstrating Le Chatelier\u2019s principle.<\/p>\n<\/div>\n<\/div>\n<div class=\"faq-item\">\n<h4>What role does calcium hydroxide play in CO\u2082 capture?<\/h4>\n<div>\n<p>Ca(OH)\u2082 reacts with CO\u2082 to form solid CaCO\u2083, effectively sequestering carbon dioxide. This reversible cycle is explored for sustainable CO\u2082 capture and lime regeneration.<\/p>\n<\/div>\n<\/div>\n<div class=\"faq-item\">\n<h4>Explain the thermodynamic cycle involving CaO, Ca(OH)\u2082, and CaCO\u2083.<\/h4>\n<div>\n<p>The cycle begins with CaCO\u2083 \u2192 CaO + CO\u2082 (endothermic calcination), followed by CaO + H\u2082O \u2192 Ca(OH)\u2082 (exothermic hydration), and finally Ca(OH)\u2082 + CO\u2082 \u2192 CaCO\u2083 + H\u2082O (exothermic carbonation). Balancing enthalpies reveals net energy requirements for lime production.<\/p>\n<\/div>\n<\/div>\n<div class=\"faq-item\">\n<h4>How can the reaction of lime water with chlorine be used in water treatment?<\/h4>\n<div>\n<p>Chlorinating Ca(OH)\u2082 produces calcium hypochlorite, a solid disinfectant releasing HOCl in water. This controlled chlorine source enhances microbial kill while minimizing free chlorine spikes, a key water treatment principle.<\/p>\n<\/div>\n<\/div>\n<div class=\"faq-item\">\n<h4>What experimental setup demonstrates the heat of hydration of calcium oxide?<\/h4>\n<div>\n<p>Use a calorimeter with a known mass of water and a temperature probe. Quickly add pre-weighed CaO, record the temperature rise, and calculate \u0394H using <em>q = m\u00b7c\u00b7\u0394T<\/em>. This verifies the theoretical enthalpy of the <strong>calcium oxide reaction with water<\/strong>.<\/p>\n<\/div>\n<\/div>\n<\/section>\n<\/article>\n","protected":false},"excerpt":{"rendered":"<p>Understand the exothermic hydration of quicklime, key for CSIR NET, IIT JAM, and GATE. This guide covers stoichiometry, thermodynamics, and practical tips.<\/p>\n","protected":false},"author":12,"featured_media":37342,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"_acf_changed":false,"footnotes":"","_debug_hook_fired":"2026-11-02 02:30:16","rank_math_seo_score":0},"categories":[29],"tags":[2923,26579,26576,26577,26578,2922],"class_list":["post-37343","post","type-post","status-publish","format-standard","has-post-thumbnail","hentry","category-csir-net","tag-competitive-exams","tag-quicklime-hydration-reaction","tag-to-pour-water-on-calcium-oxide","tag-to-pour-water-on-calcium-oxide-notes","tag-to-pour-water-on-calcium-oxide-questions","tag-vedprep","entry","has-media"],"acf":[],"rank_math_title":"Calcium Oxide Reaction With Water: Ultimate Guide for CSIR","rank_math_description":"Calcium oxide reaction with water explained: balanced equation, enthalpy, safety tips, and CSIR NET exam strategies. Master this reaction today!","rank_math_focus_keyword":"calcium oxide reaction with water","_links":{"self":[{"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/posts\/37343","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/users\/12"}],"replies":[{"embeddable":true,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/comments?post=37343"}],"version-history":[{"count":1,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/posts\/37343\/revisions"}],"predecessor-version":[{"id":37347,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/posts\/37343\/revisions\/37347"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/media\/37342"}],"wp:attachment":[{"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/media?parent=37343"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/categories?post=37343"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/tags?post=37343"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}