[{"data":1,"prerenderedAt":-1},["ShallowReactive",2],{"detail-sidebar-cat-0-en-105":3,"doc-seo-343377-105":59,"doc-detail-343377-en":130},{"code":4,"msg":5,"data":6},0,"success",[7,13,18,23,28,33,38,43,48,51,55],{"id":8,"doc_module":4,"doc_module_name":9,"category_name":10,"show_sort_weight":11,"slug":12},1,"Document","Story & Novel",90,"story-novel",{"id":14,"doc_module":4,"doc_module_name":9,"category_name":15,"show_sort_weight":16,"slug":17},2,"Literature",80,"literature",{"id":19,"doc_module":4,"doc_module_name":9,"category_name":20,"show_sort_weight":21,"slug":22},4,"Exam",70,"exam",{"id":24,"doc_module":4,"doc_module_name":9,"category_name":25,"show_sort_weight":26,"slug":27},5,"Comic",60,"comic",{"id":29,"doc_module":4,"doc_module_name":9,"category_name":30,"show_sort_weight":31,"slug":32},6,"Technology",50,"technology",{"id":34,"doc_module":4,"doc_module_name":9,"category_name":35,"show_sort_weight":36,"slug":37},7,"Healthcare",40,"healthcare",{"id":39,"doc_module":4,"doc_module_name":9,"category_name":40,"show_sort_weight":41,"slug":42},8,"Research & Report",30,"research-report",{"id":44,"doc_module":4,"doc_module_name":9,"category_name":45,"show_sort_weight":46,"slug":47},9,"Religion & Spirituality",20,"religion-spirituality",{"id":46,"doc_module":4,"doc_module_name":9,"category_name":49,"show_sort_weight":46,"slug":50},"World Cup","world-cup",{"id":52,"doc_module":4,"doc_module_name":9,"category_name":53,"show_sort_weight":52,"slug":54},10,"Lifestyle","lifestyle",{"id":56,"doc_module":4,"doc_module_name":9,"category_name":57,"show_sort_weight":24,"slug":58},19,"General","general",{"code":4,"msg":60,"data":61},"ok",{"site_id":62,"language":63,"slug":64,"title":65,"keywords":66,"description":67,"schema_data":68,"social_meta":123,"head_meta":125,"extra_data":127,"updated_unix":129},105,"en","chapter-14-acids-and-bases-acids-and-bases","Chapter 14 - Acids and Bases - Acids and Bases","","Chapter 14 covers the fundamental concepts of acids and bases, starting from the Arrhenius and Bronsted-Lowry models and moving to conjugate acid-base pairs. It introduces acid dissociation through Ka, distinguishes strong versus weak acids, and explains water’s self-ionization and the ion-product constant Kw. The pH scale and solution problem-solving methods are developed, including strong and weak acid calculations, percent dissociation, and pH of weak acid mixtures. It also covers bases, polyprotic acids, and acid-base properties of salts.",{"@graph":69,"@context":122},[70,84,105],{"@type":71,"itemListElement":72},"BreadcrumbList",[73,77,79,82],{"item":74,"name":75,"@type":76,"position":8},"https://docshare.wps.com","Home","ListItem",{"item":78,"name":9,"@type":76,"position":14},"https://docshare.wps.com/document/",{"item":80,"name":20,"@type":76,"position":81},"https://docshare.wps.com/document/exam/",3,{"item":83,"name":65,"@type":76,"position":19},"https://docshare.wps.com/document/chapter-14-acids-and-bases-acids-and-bases/343377/",{"url":83,"name":65,"@type":85,"image":86,"author":91,"headline":65,"publisher":94,"fileFormat":97,"inLanguage":63,"description":67,"dateModified":98,"datePublished":99,"encodingFormat":97,"isAccessibleForFree":100,"interactionStatistic":101},"DigitalDocument",{"url":87,"@type":88,"width":89,"height":90},"https://docshare.wps.com/thumbnails/chapter-14-acids-and-bases-acids-and-bases/343377.png","ImageObject",300,407,{"name":92,"@type":93},"Himbo","Person",{"url":74,"name":95,"@type":96},"DocShare","Organization","application/pdf","2026-10-23","2026-09-22",true,{"@type":102,"interactionType":103,"userInteractionCount":52},"InteractionCounter",{"@type":104},"ViewAction",{"@type":106,"mainEntity":107},"FAQPage",[108,114,118],{"name":109,"@type":110,"acceptedAnswer":111},"How do the Arrhenius and Bronsted-Lowry models define acids and bases?","Question",{"text":112,"@type":113},"In the Arrhenius model, acids produce hydrogen ions in aqueous solution and bases produce hydroxide ions. In the Bronsted-Lowry model, acids are proton donors and bases are proton acceptors.","Answer",{"name":115,"@type":110,"acceptedAnswer":116},"What is a conjugate acid-base pair?",{"text":117,"@type":113},"A conjugate base is what remains after an acid donates a proton, and a conjugate acid forms when a base accepts a proton. Example relationships such as Cl- being the conjugate base of HCl are given.",{"name":119,"@type":110,"acceptedAnswer":120},"How is pH calculated for strong and weak acid solutions?",{"text":121,"@type":113},"For strong acids, the document assumes complete ionization of HA and focuses on major species. For weak acids, it outlines steps using equilibrium constants, dominant equilibria, solving for x, applying the 5% rule, and then computing [H+] and pH.","https://schema.org",{"og:url":83,"og:type":124,"og:title":65,"og:site_name":95,"og:description":67},"article",{"robots":126,"canonical":83},"index,follow",{"doc_id":128,"site_id":62},343377,1790369406,{"code":4,"msg":5,"data":131},{"doc_id":128,"user_id":132,"nickname":92,"user_avatar":133,"doc_module":4,"category_id":19,"category_name":20,"doc_title":65,"doc_description":67,"doc_content":134,"file_id":135,"file_url":136,"file_type":137,"file_size":138,"view_count":52,"is_deleted":4,"is_public":8,"is_downloadable":8,"audit_status":8,"page_count":29,"language":139,"language_code":63,"site_id":62,"html_lang":63,"table_of_contents":140,"faqs":141,"seo_title":142,"seo_description":67,"update_tm":143,"read_time":144,"preview_page_count":4},687197100911,"https://ap-avatar.wpscdn.com/avatar/a000239b6f1da00475?x-image-process=image/resize,m_fixed,w_180,h_180&k=1785132997149421697","Chapter 14-Acids and Bases  \n14.1 The Nature of Acids and Bases  \nA. Arrhenius Model  \n1. Acids produce hydrogen ions in aqueous solutions  \n2. Bases produce hydroxide ions in aqueous solutions  \nB. Bronsted-Lowry Model  \n1. Acids are proton donors  \n2. Bases are proton acceptors  \n3. H3O+ is called the hydronium ion  \nC. Conjugate Acid-Base Pairs  \n1. A conjugate base is what remains after an acid has donated a proton  \na. Cl- is the conjugate base of HCl  \n2. A conjugate acid is what is formed when a base accepts a proton  \nbase acid acid base  \n3. HCl is a stronger base than H3O+ (H+) so the equilibrium lies far to the right  \nD. Acid Dissociation Constant  \n1. Ka = [H[+H]C[Cll]~~ ~~−~~ ~~]  \na. water is not included because, in dilute solution, the concentration of water is high, and changes so little it is assumed to be constant  \nb. The dissociation constant is the same as for the dissociation equation here:  \nHCl(aq) 􀀧 H+(aq) + Cl- (aq)  \nc. Ka is used only for this type of expression  \nd. For strong acids such as HCl, the equilibrium lies so far to the right that [HCl] cannot be measured accurately, and an accurate calculation of Ka is not possible  \n14.2 Acid Strength  \nA. Strong Acids  \n1. Acids for which the equilibrium lies far to the right  \na. Strong acids yield weak conjugate bases  \n2. Common strong acids  \na. sulfuric, hydrochloric, nitric, perchloric  \nB. Weak Acids  \n1. Acids for which the equilibrium lies far to the left  \na. Weak acids yield relatively strong conjugate bases  \nC. Acid Terminology  \n1. Monoprotic-one acidic proton  \n2. Diprotic-two acidic protons  \n3. Triprotic-three acidic protons  \n4. Oxyacids-acids in which the acidic proton is attached to an oxygen atom  \n5. Organic acids-acids containing the mildly acidic carboxyl group  \na. Generally weak acids  \nb. Equilibrium lies far to the left  \nD. Water as an Acid and a Base  \n1. Water can act as an acid or as a base  \na. Autoionization of water (Self-ionization)  \n2. Ion-product constant, Kw (dissociation constant)  \na. At 25°C, [H+] = [OH-] = 1.0 x 10-7  \nb. Kw = [H+][OH-] = (1 .0 x 10-7 mol/L)( 1.0 x 10-7 mol/L)  \n(1) Kw = 1.0 x 10-14 mol2/L2 (units often dropped)  \n3. Solution characteristics  \na. Neutral solution,[H+] = [OH-] = 1.0 x 10-7  \nb. Acid solution,[H+] > [OH-]  \nc. Basic solution,[H+] \u003C [OH-]  \n14.4 The pH Scale  \nA. pH and pOH  \n1. pH = -log[H+]  \na. The number of decimal places in the log is equal to the number of  \nsignificant figures in the original number  \n2. pOH = -log[OH-]  \n3. pH + pOH = 14  \nB. Solving Acid and Base Problems  \n1. Please take time to read the advice at the end of this section (Page 658) . It applies to far more than acid-base problems!  \n14.4 Calculating the pH of Strong Acid Solutions  \nA. What are the components of the solution?  \n1. HA 􀃆 H+(aq) + A- (aq)  \nor  \nHA + H2O 􀃆 H3O+(aq) + A- (aq)  \n2. H2O + H2O 􀃆 H3O+(aq) + OH- (aq)  \nor  \nH2O 􀃆 H+(aq) + OH- (aq)  \nB. Focus on the major species  \n1. At high concentrations of strong acids, the autoionization of water is insignificant  \n2. For strong acids, the assumption is that HA is completely ionized  \n14.5 Calculating the pH of Weak Acid Solutions  \nA. Steps (from page 662)  \n1. List the major species in the solution  \n2. Choose the species that can produce H+ , and write the balanced equations for the reactions producing H+  \n3. Using the values of the equilibrium constants for the reactions you have written decide which equilibrium will dominate in producing H+  \n4. Write the equilibrium expression for the dominant equilibrium  \n5. List the initial concentrations of the species participating in the dominant equilibrium  \n6. Define the change needed to achieve equilibrium; that is, define x  \n7. Write the equilibrium concentrations in terms of x  \n8. Substitute the equilibrium concentrations into the equilibrium expression  \n9. Solve for x the \"easy\" way; that is, by assuming that [HA]0-x ≈ [HA]0  \n10. Use the 5% rule to verify whether the approximation ","cbCaitFB58DNrgWQ","https://ap.wps.com/l/cbCaitFB58DNrgWQ","pdf",66239,"English","# Chapter 14: Acids and Bases\n## 14.1 The Nature of Acids and Bases\n## 14.2 Acid Strength\n## 14.4 The pH Scale\n## 14.5 Calculating the pH of Weak Acid Solutions\n## 14.6 Bases\n## 14.7 Polyprotic Acids\n## 14.8 Acid-Base Properties of Salts","[{\"question\":\"How do the Arrhenius and Bronsted-Lowry models define acids and bases?\",\"answer\":\"In the Arrhenius model, acids produce hydrogen ions in aqueous solution and bases produce hydroxide ions. In the Bronsted-Lowry model, acids are proton donors and bases are proton acceptors.\"},{\"question\":\"What is a conjugate acid-base pair?\",\"answer\":\"A conjugate base is what remains after an acid donates a proton, and a conjugate acid forms when a base accepts a proton. Example relationships such as Cl- being the conjugate base of HCl are given.\"},{\"question\":\"How is pH calculated for strong and weak acid solutions?\",\"answer\":\"For strong acids, the document assumes complete ionization of HA and focuses on major species. For weak acids, it outlines steps using equilibrium constants, dominant equilibria, solving for x, applying the 5% rule, and then computing [H+] and pH.\"}]","Chapter 14 - Acids and Bases - Acids and Bases | PDF",1790050965,15]