[{"data":1,"prerenderedAt":127},["ShallowReactive",2],{"cheatsheet-acids-bases-and-ph":3},{"sheet":4},{"sheetSlug":5,"topicSlugs":6,"primaryTopic":7,"title":8,"subtitle":9,"sections":10},"acids-bases-and-ph",[5],22,"Acids, Bases & pH","Acid-base models, pH/pOH, conjugate pairs, strong vs weak, Ka/Kb, salt hydrolysis, and polyprotic acids.",[11,39,48,56,64,72,80,88,111,119],{"heading":12,"kind":13,"columns":14,"items":18},"Three models","data",[15,16,17],"Model","Acid","Base",[19],{"ref":20,"mode":23,"provenance":24,"rows":25,"source_hash":38},{"type":21,"topic":7,"id":22,"field":21},"rule","AB-R001","transform","owned_workbook",[26,30,34],[27,28,29],"Arrhenius","makes H⁺ in water","makes OH⁻ in water",[31,32,33],"Brønsted-Lowry","donates H⁺","accepts H⁺",[35,36,37],"Lewis","accepts an e⁻ pair","donates an e⁻ pair","6fe61e23e51f7d544e2cde2c971c92a0b08532e80692c91529aa546349dff292",{"heading":40,"kind":41,"items":42},"pH, pOH, Kw","rules",[43],{"ref":44,"mode":23,"provenance":24,"text":46,"source_hash":47},{"type":21,"topic":7,"id":45,"field":21},"AB-R003","Kw = [H₃O⁺][OH⁻] = 1.0 × 10⁻¹⁴ at 25 °C. pH = −log[H₃O⁺], pOH = −log[OH⁻], pH + pOH = 14.00. [H⁺] = 10^(−pH). pH 7 neutral, \u003C7 acidic, >7 basic.","171db0c6f97a5fb158c468b36106c984b517479fb25769db4ff052d165ab0e6d",{"heading":49,"kind":41,"items":50},"Conjugate pairs",[51],{"ref":52,"mode":23,"provenance":24,"text":54,"source_hash":55},{"type":21,"topic":7,"id":53,"field":21},"AB-R004","A conjugate pair differs by one H⁺. In HA + B ⇌ A⁻ + BH⁺: (HA, A⁻) and (B, BH⁺). Amphiprotic species (H₂O, HCO₃⁻, H₂PO₄⁻) act as acid or base depending on the partner.","d6a4619c7522227106e5827afe7022c62bd00c145b2a04c0dfee0b52192e11f7",{"heading":57,"kind":41,"items":58},"Strong acids & bases",[59],{"ref":60,"mode":23,"provenance":24,"text":62,"source_hash":63},{"type":21,"topic":7,"id":61,"field":21},"AB-R005","Ionize completely. Strong acids: HCl, HBr, HI, HNO₃, HClO₃, HClO₄, H₂SO₄ (1st only). Strong bases: group 1 hydroxides; Ca/Sr/Ba(OH)₂ (2 OH⁻). Monoprotic: [H⁺] = [HA]₀. n-OH base: [OH⁻] = n[B]₀.","bd6b0f43bc0890ebdb4b4c8043461aa92ff14cbb1a64281faeb5397b1462bc55",{"heading":65,"kind":41,"items":66},"Weak acid (Ka)",[67],{"ref":68,"mode":23,"provenance":24,"text":70,"source_hash":71},{"type":21,"topic":7,"id":69,"field":21},"AB-R006","HA ⇌ H₃O⁺ + A⁻, Ka = [H₃O⁺][A⁻]/[HA]. ICE gives x²/([HA]₀ − x) = Ka. If 100·Ka \u003C [HA]₀, x ≈ √(Ka·[HA]₀); pH = −log x. Otherwise use the quadratic.","aaf8dbe7a790522f34b57fc5352196912322398ed21ce970d421edbd25ecbee6",{"heading":73,"kind":41,"items":74},"Weak base (Kb)",[75],{"ref":76,"mode":23,"provenance":24,"text":78,"source_hash":79},{"type":21,"topic":7,"id":77,"field":21},"AB-R007","B + H₂O ⇌ BH⁺ + OH⁻, Kb = [BH⁺][OH⁻]/[B]. ICE: x²/([B]₀ − x) = Kb; if 100·Kb \u003C [B]₀, x ≈ √(Kb·[B]₀); [OH⁻] = x, pOH = −log x, pH = 14 − pOH.","c692a5c73c8418712257cc32a197b7f0b49f263bd9bc5885b051da3b840bc5e5",{"heading":81,"kind":41,"items":82},"Ka · Kb = Kw",[83],{"ref":84,"mode":23,"provenance":24,"text":86,"source_hash":87},{"type":21,"topic":7,"id":85,"field":21},"AB-R008","For a conjugate pair: Ka·Kb = Kw = 1.0 × 10⁻¹⁴, so pKa + pKb = 14. Stronger acid → weaker conjugate base. Get a salt anion's Kb = Kw/Ka, or a cation's Ka = Kw/Kb.","2b439c0c3cbc410d403d3bc9a62dbabe23ed02877ec2577f3504a20cbe86220a",{"heading":89,"kind":13,"columns":90,"items":93},"Salt hydrolysis",[91,92],"Salt (from)","Solution",[94],{"ref":95,"mode":23,"provenance":24,"rows":97,"source_hash":110},{"type":21,"topic":7,"id":96,"field":21},"AB-R009",[98,101,104,107],[99,100],"strong acid + strong base (NaCl)","neutral",[102,103],"strong acid + weak base (NH₄Cl)","acidic",[105,106],"weak acid + strong base (NaCH₃COO)","basic",[108,109],"weak acid + weak base","compare Ka vs Kb","0155dfac1b6af61155d48bb4f97f9f4e761b92ed209872a17c66677aa6bdb7d0",{"heading":112,"kind":41,"items":113},"Percent ionization",[114],{"ref":115,"mode":23,"provenance":24,"text":117,"source_hash":118},{"type":21,"topic":7,"id":116,"field":21},"AB-R010","% ionization = (x / [HA]₀) × 100, x from the ICE table. Larger Ka → more ionized; more dilute → more ionized (Le Chatelier on dilution).","f634258229fc2748d3848100616e696c9074ce646dca95b8e86bab1bcd2e54b1",{"heading":120,"kind":41,"items":121},"Polyprotic acids",[122],{"ref":123,"mode":23,"provenance":24,"text":125,"source_hash":126},{"type":21,"topic":7,"id":124,"field":21},"AB-R011","Stepwise: Ka1 ≫ Ka2 ≫ Ka3 (by ~10⁴-10⁵). When Ka1 ≥ 20·Ka2, treat as monoprotic for pH (Ka1 ICE alone). Then [X²⁻] ≈ Ka2, independent of concentration. E.g. H₃PO₄: Ka1 7.5 × 10⁻³, Ka2 6.2 × 10⁻⁸, Ka3 4.8 × 10⁻¹³.","15099624706754e276d281a9bc542c59fd525ca117ab1b8ee8819582d4b9a9d5",1787246032994]