[{"data":1,"prerenderedAt":-1},["ShallowReactive",2],{"doc-seo-343687-105":3,"detail-sidebar-cat-0-en-105":81,"doc-detail-343687-en":130},{"code":4,"msg":5,"data":6},0,"ok",{"site_id":7,"language":8,"slug":9,"title":10,"keywords":11,"description":12,"schema_data":13,"social_meta":74,"head_meta":76,"extra_data":78,"updated_unix":80},105,"en","topic-8-acids-and-bases-theories-properties-and-the-ph-scale","Topic 8 - Acids and bases - Theories, properties, and the pH scale","","Topic 8 covers acids and bases, starting with the Brønsted-Lowry theory that defines acids as proton (H+) donors and bases as proton (H+) acceptors. It explains amphiprotic species and conjugate acid-base pairs, including how to deduce conjugates and label pairs in reactions. The topic then summarizes neutralization reactions, including salt formation with water, exothermic behavior, and how to derive salt formulas for hydroxyl, carbonate, and metal-related base reactions. Finally, it introduces the pH scale, the relationships between pH, [H+], pOH, and Kw, and the self-ionization equilibrium of water.",{"@graph":14,"@context":73},[15,34,56],{"@type":16,"itemListElement":17},"BreadcrumbList",[18,23,27,31],{"item":19,"name":20,"@type":21,"position":22},"https://docshare.wps.com","Home","ListItem",1,{"item":24,"name":25,"@type":21,"position":26},"https://docshare.wps.com/document/","Document",2,{"item":28,"name":29,"@type":21,"position":30},"https://docshare.wps.com/document/exam/","Exam",3,{"item":32,"name":10,"@type":21,"position":33},"https://docshare.wps.com/document/topic-8-acids-and-bases-theories-properties-and-the-ph-scale/343687/",4,{"url":32,"name":10,"@type":35,"image":36,"author":41,"headline":10,"publisher":44,"fileFormat":47,"inLanguage":8,"description":12,"dateModified":48,"datePublished":49,"encodingFormat":47,"isAccessibleForFree":50,"interactionStatistic":51},"DigitalDocument",{"url":37,"@type":38,"width":39,"height":40},"https://docshare.wps.com/thumbnails/topic-8-acids-and-bases-theories-properties-and-the-ph-scale/343687.png","ImageObject",300,407,{"name":42,"@type":43},"Ivy","Person",{"url":19,"name":45,"@type":46},"DocShare","Organization","application/vnd.openxmlformats-officedocument.wordprocessingml.document","2026-10-23","2026-09-22",true,{"@type":52,"interactionType":53,"userInteractionCount":55},"InteractionCounter",{"@type":54},"ViewAction",6,{"@type":57,"mainEntity":58},"FAQPage",[59,65,69],{"name":60,"@type":61,"acceptedAnswer":62},"What are Brønsted-Lowry acids and bases?","Question",{"text":63,"@type":64},"A Brønsted-Lowry acid donates a proton (H+), while a Brønsted-Lowry base accepts a proton (H+).","Answer",{"name":66,"@type":61,"acceptedAnswer":67},"What is a conjugate acid-base pair and how do you find conjugates?",{"text":68,"@type":64},"A conjugate pair consists of two species that differ by a single proton. The acid becomes the conjugate base, and the base becomes the conjugate acid; add one H+ to find the conjugate acid and remove one H+ to find the conjugate base.",{"name":70,"@type":61,"acceptedAnswer":71},"How does the pH scale relate to hydrogen ion concentration?",{"text":72,"@type":64},"pH is defined as pH = −log[H+], so [H+] = 10^(−pH). Changing pH by 1 unit corresponds to a 10-fold change in hydrogen ion concentration.","https://schema.org",{"og:url":32,"og:type":75,"og:title":10,"og:site_name":45,"og:description":12},"article",{"robots":77,"canonical":32},"index,follow",{"doc_id":79,"site_id":7},343687,1790492294,{"code":4,"msg":82,"data":83},"success",[84,88,92,95,100,104,109,114,119,122,126],{"id":22,"doc_module":4,"doc_module_name":25,"category_name":85,"show_sort_weight":86,"slug":87},"Story & Novel",90,"story-novel",{"id":26,"doc_module":4,"doc_module_name":25,"category_name":89,"show_sort_weight":90,"slug":91},"Literature",80,"literature",{"id":33,"doc_module":4,"doc_module_name":25,"category_name":29,"show_sort_weight":93,"slug":94},70,"exam",{"id":96,"doc_module":4,"doc_module_name":25,"category_name":97,"show_sort_weight":98,"slug":99},5,"Comic",60,"comic",{"id":55,"doc_module":4,"doc_module_name":25,"category_name":101,"show_sort_weight":102,"slug":103},"Technology",50,"technology",{"id":105,"doc_module":4,"doc_module_name":25,"category_name":106,"show_sort_weight":107,"slug":108},7,"Healthcare",40,"healthcare",{"id":110,"doc_module":4,"doc_module_name":25,"category_name":111,"show_sort_weight":112,"slug":113},8,"Research & Report",30,"research-report",{"id":115,"doc_module":4,"doc_module_name":25,"category_name":116,"show_sort_weight":117,"slug":118},9,"Religion & Spirituality",20,"religion-spirituality",{"id":117,"doc_module":4,"doc_module_name":25,"category_name":120,"show_sort_weight":117,"slug":121},"World Cup","world-cup",{"id":123,"doc_module":4,"doc_module_name":25,"category_name":124,"show_sort_weight":123,"slug":125},10,"Lifestyle","lifestyle",{"id":127,"doc_module":4,"doc_module_name":25,"category_name":128,"show_sort_weight":96,"slug":129},19,"General","general",{"code":4,"msg":82,"data":131},{"doc_id":79,"user_id":132,"nickname":42,"user_avatar":133,"doc_module":4,"category_id":33,"category_name":29,"doc_title":10,"doc_description":12,"doc_content":134,"file_id":135,"file_url":136,"file_type":137,"file_size":138,"view_count":55,"is_deleted":4,"is_public":22,"is_downloadable":22,"audit_status":22,"page_count":115,"language":139,"language_code":8,"site_id":7,"html_lang":8,"table_of_contents":140,"faqs":141,"seo_title":142,"seo_description":12,"update_tm":143,"read_time":144,"preview_page_count":4},549758252649,"https://ap-avatar.wpscdn.com/avatar/8000253669c5317157?_k=1778319167496531819","Topic 8: Acids and bases\n8.1\nTheories of acids and bases\n8.1.1\nA Brønsted-Lowry acid is a proton/H+ donor and a Brønsted-Lowry base is a proton/H+ acceptor\n8.1.2\nAmphiprotic species can act as both Brønsted-Lowry acids and bases\n8.1.3\nA pair of species differing by a single proton is called a conjugate acid-base pair\n8.1.4\nDeduction of the Brønsted-Lowry acid and base in a chemical reaction\n8.1.5\nDeduction of the conjugate acid or conjugate base in a chemical reaction\nBrønsted-Lowry theory\nAccording to the Brønsted-Lowry theory, a substance behaves as an acid when it donates a proton to a base. A substance behaves as a base when it accepts a proton from an acid. Thus:\nA Brønsted-Lowry acid is a proton (H+) donor\nA Brønsted-Lowry base is a proton (H+) acceptor\nAcids can be a combination of hydrogen ions (\u001a𝑯\u001b+\u001b) and an anion. Examples include: 𝐻𝐶𝑙, \u001a𝐻𝑁𝑂\u001b3\u001b, 𝐻\u001a𝐶\u001b2\u001b\u001a𝐻\u001b3\u001b\u001a𝑂\u001b2\u001b\nBases can be a combination of hydroxide ions (\u001a𝑶𝑯\u001b−\u001b) and metal cations. Examples include: 𝑁𝑎𝑂𝐻, 𝐾𝑂𝐻\nHowever, sometimes a hydrogen next to a metal signifies a base such as 𝑁𝑎𝐻\nAcid-Base Conjugate Pairs: A conjugate pair is two species which differ by a single proton:\nThe acid will become the conjugate base\nThe base will become the conjugate acid\nConjugate-Base Pair Question:\nLabel the conjugate acid-base pairs in the following reactions:\n\u001aCH\u001b3\u001bCOOH+\u001aH\u001b2\u001bO\u001ag\u001b⇌\u001aCH\u001b3\u001b𝐶𝑂\u001a𝑂\u001b−\u001b+\u001aH\u001b3\u001b\u001aO\u001b+\u001b\nConjugate pair 1: \u001aCH\u001b3\u001bCOOH/\u001aCH\u001b3\u001b𝐶𝑂\u001a𝑂\u001b−\u001b\n\u001a𝐶𝐻\u001b3\u001b𝐶𝑂𝑂𝐻 is the acid because it donates a \u001aH\u001b+\u001b, so \u001aCH\u001b3\u001b𝐶𝑂\u001a𝑂\u001b−\u001b is conjugate base\nConjugate pair 2: \u001aH\u001b2\u001bO/\u001aH\u001b3\u001b\u001aO\u001b+\u001b\n\u001aH\u001b2\u001bO is the base because it accepts a  \u001aH\u001b+\u001b, so  \u001aH\u001b3\u001b\u001aO\u001b+\u001b is the conjugate acid\nTo find the conjugate acid of a species, add one \u001aH\u001b+\u001b\nTo find the conjugate base of a species, takeaway one \u001aH\u001b+\u001b\nBefore the Brønsted-Lory theory acids and bases were distinguished by their taste, acids tasted sour\nAmphiprotic\nSome substances can behave as either acids and bases, depending on what they react with, and can therefore donate or receive protons. Such substances are said to be amphiprotic\nAmphiprotic: A chemical species capable of accepting and donating protons, thus able to act as a Brønsted-Lowry acid and a base\nThis means the species must be able to accept or donate a proton to another species\nH2O is amphiprotic as it is able to donate a proton to form a \u001aOH\u001b−\u001b or accept a proton to form \u001aH\u001b3\u001b\u001aO\u001b+\u001b therefore acting as a Brønsted-Lowry acid or base\nAmphiprotic Species Question:\nWrite an equation to show hydrogen phosphate acting as and an acid and a base in water\nActing like an Acid: \u001a\u001aHPO\u001b4\u001b\u001b2−\u001b+\u001aH\u001b2\u001bO\u001ag\u001b⇌\u001a\u001aPO\u001b4\u001b\u001b3−\u001b+\u001aH\u001b3\u001b\u001aO\u001b+\u001b\nActing like a Base: \u001a\u001aHPO\u001b4\u001b\u001b2−\u001b+\u001aH\u001b2\u001bO\u001ag\u001b⇌\u001a\u001aHPO\u001b4\u001b\u001b−\u001b+\u001aOH\u001b−\u001b\nAmphoteric\nAmphoteric: A species that can act as an acid or base, including reactions that do not involve a proton\nAmphiprotic specifically relates to the Brønsted-Lowry acid-base theory, where the emphasis is on the transfer of a proton. Amphoteric is a more general term that isn’t just confined to proton transfer\nAll amphiprotic species are also amphoteric but not all amphoteric species are amphiprotic\n8.2\nProperties of acids and bases\n8.2.1\nMost acids have observable characteristic chemical reactions with reactivate metals, metal oxides, metal hydroxides, hydrogen carbonates and carbonates\n8.2.2\nSalt and water are produced in exothermic neutralization reactions\n8.2.3\nBalancing chemical equations for the reaction of acids\n8.2.4\nIdentification of the acid and base needed to make different salts\nNeutralization Reactions\nNeutralization: A chemical reaction where a base and an acid react to form a salt and water\nSalt: An ionic Compound\nAcid base reactions will always produce a salt and water\nSalt and water are neither acidic nor basic. They are called neutral solutions\nNeutralization reactions are exothermic as heat is released\nThere are different types of bases that acids react with to form salt:\nHydroxyl Base:\nEquation: 𝐴𝑐𝑖𝑑+𝐵𝑎𝑠𝑒→𝑆𝑎𝑙𝑡+𝑊𝑎𝑡𝑒𝑟\nTo find the salt formula, take away the hydrogen from the acid and the hydroxyl group from the b","cbCaikBq4utO1U55","https://ap.wps.com/l/cbCaikBq4utO1U55","docx",441080,"English","# 8.1 Theories of acids and bases\n## Brønsted-Lowry acids and bases\n## Amphiprotic species and conjugate pairs\n# 8.2 Properties of acids and bases\n## Neutralization reactions\n## Types of bases and salt formation\n# 8.3 The pH scale\n## pH equations and interpretation\n## Kw, pH/pOH relationships, and water self-ionization","[{\"question\":\"What are Brønsted-Lowry acids and bases?\",\"answer\":\"A Brønsted-Lowry acid donates a proton (H+), while a Brønsted-Lowry base accepts a proton (H+).\"},{\"question\":\"What is a conjugate acid-base pair and how do you find conjugates?\",\"answer\":\"A conjugate pair consists of two species that differ by a single proton. The acid becomes the conjugate base, and the base becomes the conjugate acid; add one H+ to find the conjugate acid and remove one H+ to find the conjugate base.\"},{\"question\":\"How does the pH scale relate to hydrogen ion concentration?\",\"answer\":\"pH is defined as pH = −log[H+], so [H+] = 10^(−pH). Changing pH by 1 unit corresponds to a 10-fold change in hydrogen ion concentration.\"}]","Topic 8 - Acids and bases - Theories, properties, and the pH scale | DOCX",1790051811,23]