{"id":4404,"date":"2026-04-07T08:29:24","date_gmt":"2026-04-07T08:29:24","guid":{"rendered":"https:\/\/ksquareinstitute.in\/blog\/?p=4404"},"modified":"2026-04-07T08:29:25","modified_gmt":"2026-04-07T08:29:25","slug":"top-5-chemical-equilibrium-questions","status":"publish","type":"post","link":"https:\/\/ksquareinstitute.in\/blog\/top-5-chemical-equilibrium-questions\/","title":{"rendered":"Top 5 Chemical Equilibrium Questions for NEET (Most Repeated PYQs)"},"content":{"rendered":"\n

Top Chemical Equilibrium Questions for NEET <\/h2>\n\n\n\n

Chemical equilibrium is one of the most scoring and concept-driven chapters in NEET Chemistry. Every year, multiple questions are directly asked from equilibrium constants, Le Chatelier\u2019s principle, and ionic equilibrium. If you prepare the Top 5 Chemical Equilibrium Questions, you can easily secure those marks with accuracy and confidence.<\/p>\n\n\n\n

In this article, we will go through the Top 5 Chemical Equilibrium Questions that are frequently repeated in NEET PYQs, along with clear explanations and solving strategies. Understanding these problems will strengthen your conceptual clarity and improve your problem-solving speed.<\/p>\n\n\n\n

\"Top<\/figure>\n\n\n\n

Question 1: Relation Between Kp and Kc<\/h2>\n\n\n\n

For a gaseous reaction:N<\/mi>2<\/mn><\/msub>(<\/mo>g<\/mi>)<\/mo>+<\/mo>3<\/mn>H<\/mi>2<\/mn><\/msub>(<\/mo>g<\/mi>)<\/mo>\u21cc<\/mo>2<\/mn>N<\/mi>H<\/mi>3<\/mn><\/msub>(<\/mo>g<\/mi>)<\/mo><\/mrow>N_2(g) + 3H_2(g) \\rightleftharpoons 2NH_3(g)<\/annotation><\/semantics><\/math>N2\u200b(g)+3H2\u200b(g)\u21cc2NH3\u200b(g)<\/p>\n\n\n\n

Find the relation between K<\/mi>p<\/mi><\/msub><\/mrow>K_p<\/annotation><\/semantics><\/math>Kp\u200b and K<\/mi>c<\/mi><\/msub><\/mrow>K_c<\/annotation><\/semantics><\/math>Kc\u200b.<\/p>\n\n\n\n

Solution<\/h3>\n\n\n\n

The relation between equilibrium constants is:K<\/mi>p<\/mi><\/msub>=<\/mo>K<\/mi>c<\/mi><\/msub>(<\/mo>R<\/mi>T<\/mi>)<\/mo>\u0394<\/mi>n<\/mi><\/mrow><\/msup><\/mrow>K_p = K_c (RT)^{\\Delta n}<\/annotation><\/semantics><\/math>Kp\u200b=Kc\u200b(RT)\u0394n<\/p>\n\n\n\n

Where:<\/p>\n\n\n\n

    \n
  • \u0394<\/mi>n<\/mi>=<\/mo>moles of gaseous products<\/mtext>\u2212<\/mo>moles of gaseous reactants<\/mtext><\/mrow>\\Delta n = \\text{moles of gaseous products} – \\text{moles of gaseous reactants}<\/annotation><\/semantics><\/math>\u0394n=moles\u00a0of\u00a0gaseous\u00a0products\u2212moles\u00a0of\u00a0gaseous\u00a0reactants<\/li>\n<\/ul>\n\n\n\n

    Here:\u0394<\/mi>n<\/mi>=<\/mo>2<\/mn>\u2212<\/mo>(<\/mo>1<\/mn>+<\/mo>3<\/mn>)<\/mo>=<\/mo>\u2212<\/mo>2<\/mn><\/mrow>\\Delta n = 2 – (1 + 3) = -2<\/annotation><\/semantics><\/math>\u0394n=2\u2212(1+3)=\u22122<\/p>\n\n\n\n

    So,K<\/mi>p<\/mi><\/msub>=<\/mo>K<\/mi>c<\/mi><\/msub>(<\/mo>R<\/mi>T<\/mi>)<\/mo>\u2212<\/mo>2<\/mn><\/mrow><\/msup><\/mrow>K_p = K_c (RT)^{-2}<\/annotation><\/semantics><\/math>Kp\u200b=Kc\u200b(RT)\u22122<\/p>\n\n\n\n

    Final Answer:<\/h3>\n\n\n\n

    K<\/mi>p<\/mi><\/msub>=<\/mo>K<\/mi>c<\/mi><\/msub>(<\/mo>R<\/mi>T<\/mi>)<\/mo>2<\/mn><\/msup><\/mrow><\/mfrac><\/mrow>K_p = \\frac{K_c}{(RT)^2}<\/annotation><\/semantics><\/math>Kp\u200b=(RT)2Kc\u200b\u200b<\/p>\n\n\n\n

    This is one of the most important problems in the Top 5 Chemical Equilibrium Questions<\/strong>, as NEET frequently tests this concept.<\/p>\n\n\n\n

    Question 2: Le Chatelier\u2019s Principle Application<\/h2>\n\n\n\n

    What happens to equilibrium when pressure is increased for the reaction:2<\/mn>S<\/mi>O<\/mi>2<\/mn><\/msub>(<\/mo>g<\/mi>)<\/mo>+<\/mo>O<\/mi>2<\/mn><\/msub>(<\/mo>g<\/mi>)<\/mo>\u21cc<\/mo>2<\/mn>S<\/mi>O<\/mi>3<\/mn><\/msub>(<\/mo>g<\/mi>)<\/mo><\/mrow>2SO_2(g) + O_2(g) \\rightleftharpoons 2SO_3(g)<\/annotation><\/semantics><\/math>2SO2\u200b(g)+O2\u200b(g)\u21cc2SO3\u200b(g)<\/p>\n\n\n\n

    Solution<\/h3>\n\n\n\n

    According to Le Chatelier\u2019s principle:<\/p>\n\n\n\n

      \n
    • Increase in pressure favors the side with fewer moles of gas.<\/li>\n<\/ul>\n\n\n\n

      Reactants: 3 moles
      Products: 2 moles<\/p>\n\n\n\n

      So equilibrium shifts towards products.<\/p>\n\n\n\n

      Final Answer:<\/h3>\n\n\n\n

      Equilibrium shifts to the right, increasing S<\/mi>O<\/mi>3<\/mn><\/msub><\/mrow>SO_3<\/annotation><\/semantics><\/math>SO3\u200b formation.<\/p>\n\n\n\n

      This concept appears repeatedly in the Top 5 Chemical Equilibrium Questions<\/strong>, especially in conceptual MCQs.<\/p>\n\n\n\n

      Question 3: Degree of Dissociation<\/h2>\n\n\n\n

      For a weak electrolyte, the degree of dissociation \u03b1<\/mi><\/mrow>\\alpha<\/annotation><\/semantics><\/math>\u03b1 is related to equilibrium constant K<\/mi><\/mrow>K<\/annotation><\/semantics><\/math>K and concentration C<\/mi><\/mrow>C<\/annotation><\/semantics><\/math>C as:K<\/mi>=<\/mo>C<\/mi>\u03b1<\/mi>2<\/mn><\/msup><\/mrow>1<\/mn>\u2212<\/mo>\u03b1<\/mi><\/mrow><\/mfrac><\/mrow>K = \\frac{C\\alpha^2}{1 – \\alpha}<\/annotation><\/semantics><\/math>K=1\u2212\u03b1C\u03b12\u200b<\/p>\n\n\n\n

      If \u03b1<\/mi><\/mrow>\\alpha<\/annotation><\/semantics><\/math>\u03b1 is very small, simplify the expression.<\/p>\n\n\n\n

      Solution<\/h3>\n\n\n\n

      Since \u03b1<\/mi>\u226a<\/mo>1<\/mn><\/mrow>\\alpha \\ll 1<\/annotation><\/semantics><\/math>\u03b1\u226a1, we approximate:1<\/mn>\u2212<\/mo>\u03b1<\/mi>\u2248<\/mo>1<\/mn><\/mrow>1 – \\alpha \\approx 1<\/annotation><\/semantics><\/math>1\u2212\u03b1\u22481<\/p>\n\n\n\n

      Thus:K<\/mi>=<\/mo>C<\/mi>\u03b1<\/mi>2<\/mn><\/msup><\/mrow>K = C\\alpha^2<\/annotation><\/semantics><\/math>K=C\u03b12 \u03b1<\/mi>=<\/mo>K<\/mi>C<\/mi><\/mfrac><\/msqrt><\/mrow>\\alpha = \\sqrt{\\frac{K}{C}}<\/annotation><\/semantics><\/math>\u03b1=CK\u200b\u200b<\/p>\n\n\n\n

      Final Answer:<\/h3>\n\n\n\n

      \u03b1<\/mi>=<\/mo>K<\/mi>C<\/mi><\/mfrac><\/msqrt><\/mrow>\\alpha = \\sqrt{\\frac{K}{C}}<\/annotation><\/semantics><\/math>\u03b1=CK\u200b\u200b<\/p>\n\n\n\n

      This formula is a must-remember shortcut from the Top 5 Chemical Equilibrium Questions<\/strong>.<\/p>\n\n\n\n

      Question 4: Ionic Equilibrium \u2013 pH Calculation<\/h2>\n\n\n\n

      Calculate the pH of a 0.01 M HCl solution.<\/p>\n\n\n\n

      Solution<\/h3>\n\n\n\n

      HCl is a strong acid, so it dissociates completely:[<\/mo>H<\/mi>+<\/mo><\/msup>]<\/mo>=<\/mo>0.01<\/mn>=<\/mo>10<\/mn>\u2212<\/mo>2<\/mn><\/mrow><\/msup><\/mrow>[H^+] = 0.01 = 10^{-2}<\/annotation><\/semantics><\/math>[H+]=0.01=10\u22122 p<\/mi>H<\/mi>=<\/mo>\u2212<\/mo>log<\/mi>\u2061<\/mo>[<\/mo>H<\/mi>+<\/mo><\/msup>]<\/mo><\/mrow>pH = -\\log[H^+]<\/annotation><\/semantics><\/math>pH=\u2212log[H+] p<\/mi>H<\/mi>=<\/mo>\u2212<\/mo>log<\/mi>\u2061<\/mo>(<\/mo>10<\/mn>\u2212<\/mo>2<\/mn><\/mrow><\/msup>)<\/mo>=<\/mo>2<\/mn><\/mrow>pH = -\\log(10^{-2}) = 2<\/annotation><\/semantics><\/math>pH=\u2212log(10\u22122)=2<\/p>\n\n\n\n

      Final Answer:<\/h3>\n\n\n\n

      pH = 2<\/p>\n\n\n\n

      Direct pH-based questions are very common in the Top 5 Chemical Equilibrium Questions<\/strong>, especially from strong acids and bases.<\/p>\n\n\n\n

      Question 5: Common Ion Effect<\/h2>\n\n\n\n

      What happens when ammonium chloride (NH\u2084Cl) is added to ammonium hydroxide (NH\u2084OH)?<\/p>\n\n\n\n

      Solution<\/h3>\n\n\n\n

      NH\u2084OH \u21cc NH\u2084\u207a + OH\u207b<\/p>\n\n\n\n

      Adding NH\u2084Cl increases NH\u2084\u207a concentration.<\/p>\n\n\n\n

      According to Le Chatelier\u2019s principle:<\/p>\n\n\n\n

        \n
      • Increase in product shifts equilibrium to the left.<\/li>\n<\/ul>\n\n\n\n

        Thus:<\/p>\n\n\n\n

          \n
        • Ionization of NH\u2084OH decreases.<\/li>\n<\/ul>\n\n\n\n

          Final Answer:<\/h3>\n\n\n\n

          Ionization decreases due to the common ion effect.<\/p>\n\n\n\n

          This is a classic conceptual problem included in the Top 5 Chemical Equilibrium Questions<\/strong> every year.<\/p>\n\n\n\n

          Why These Top 5 Chemical Equilibrium Questions Matter for NEET<\/h2>\n\n\n\n

          The Top 5 Chemical Equilibrium Questions<\/strong> covered here are not random\u2014they represent the exact pattern followed in NEET. Questions are usually:<\/p>\n\n\n\n

            \n
          • Concept-based rather than lengthy<\/li>\n\n\n\n
          • Formula-driven with small calculations<\/li>\n\n\n\n
          • Focused on equilibrium shifts, constants, and pH<\/li>\n<\/ul>\n\n\n\n

            If you master these Top 5 Chemical Equilibrium Questions<\/strong>, you can confidently attempt most equilibrium problems in the exam.<\/p>\n\n\n\n

            Preparation Tips for Chemical Equilibrium<\/h2>\n\n\n\n

            To fully utilize the Top 5 Chemical Equilibrium Questions<\/strong>, keep these strategies in mind:<\/p>\n\n\n\n

            Focus on formulas like K<\/mi>p<\/mi><\/msub>=<\/mo>K<\/mi>c<\/mi><\/msub>(<\/mo>R<\/mi>T<\/mi>)<\/mo>\u0394<\/mi>n<\/mi><\/mrow><\/msup><\/mrow>K_p = K_c (RT)^{\\Delta n}<\/annotation><\/semantics><\/math>Kp\u200b=Kc\u200b(RT)\u0394n and pH calculations. Practice approximation methods such as 1<\/mn>\u2212<\/mo>\u03b1<\/mi>\u2248<\/mo>1<\/mn><\/mrow>1 – \\alpha \\approx 1<\/annotation><\/semantics><\/math>1\u2212\u03b1\u22481. Understand Le Chatelier\u2019s principle deeply rather than memorizing it. Pay special attention to ionic equilibrium, especially pH, pOH, and buffer solutions.<\/p>\n\n\n\n

            Repeated revision of these Top 5 Chemical Equilibrium Questions<\/strong> will help you build speed and accuracy.<\/p>\n\n\n\n

            FAQs on Top 5 Chemical Equilibrium Questions<\/h2>\n\n\n\n

            What is the weightage of equilibrium in NEET?<\/h3>\n\n\n\n

            Chemical equilibrium usually carries 2\u20133 questions in NEET, making it a high-weightage chapter.<\/p>\n\n\n\n

            Are numerical questions difficult in equilibrium?<\/h3>\n\n\n\n

            No, most numerical problems are formula-based and can be solved quickly if concepts are clear.<\/p>\n\n\n\n

            Is ionic equilibrium important for NEET?<\/h3>\n\n\n\n

            Yes, ionic equilibrium is extremely important and often asked in the form of pH calculations and buffer problems.<\/p>\n\n\n\n

            How to revise Top 5 Chemical Equilibrium Questions effectively?<\/h3>\n\n\n\n

            Revise formulas daily, solve PYQs multiple times, and focus on conceptual clarity.<\/p>\n\n\n\n

            Conclusion<\/h2>\n\n\n\n

            The Top 5 Chemical Equilibrium Questions<\/strong> discussed in this article cover the most repeated and high-yield concepts for NEET. By practicing these questions regularly, you can strengthen your fundamentals and improve your score significantly.<\/p>\n\n\n\n

            Make sure to revise these Top 5 Chemical Equilibrium Questions<\/strong> multiple times before the exam, as they form the backbone of equilibrium-related problems in NEET.<\/p>\n","protected":false},"excerpt":{"rendered":"

            Top Chemical Equilibrium Questions for NEET Chemical equilibrium is one of the most scoring and concept-driven chapters in NEET Chemistry. Every year, multiple questions are directly asked from equilibrium constants, Le Chatelier\u2019s principle, and ionic equilibrium. If you prepare the Top 5 Chemical Equilibrium Questions, you can easily secure those marks with accuracy and confidence. […]<\/p>\n","protected":false},"author":1,"featured_media":4388,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[127,69],"tags":[732,734,735,736,629,733],"class_list":["post-4404","post","type-post","status-publish","format-standard","has-post-thumbnail","hentry","category-free-study-material","category-chemistry","tag-chemical-equilibrium-neet","tag-equilibrium-questions-with-solutions","tag-ionic-equilibrium-neet","tag-le-chatelier-principle-neet","tag-neet-chemistry-pyqs","tag-top-5-chemical-equilibrium-questions"],"blocksy_meta":{"page_structure_type":"type-1","styles_descriptor":{"styles":{"desktop":"","tablet":"","mobile":""},"google_fonts":[],"version":6}},"_links":{"self":[{"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/posts\/4404","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/comments?post=4404"}],"version-history":[{"count":1,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/posts\/4404\/revisions"}],"predecessor-version":[{"id":4405,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/posts\/4404\/revisions\/4405"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/media\/4388"}],"wp:attachment":[{"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/media?parent=4404"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/categories?post=4404"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/tags?post=4404"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}