[{"data":1,"prerenderedAt":-1},["ShallowReactive",2],{"detail-sidebar-cat-1-en-105":3,"doc-seo-573092-105":53,"doc-detail-573092-en":118},{"code":4,"msg":5,"data":6},0,"success",[7,14,19,24,29,34,39,44,49],{"id":8,"doc_module":9,"doc_module_name":10,"category_name":11,"show_sort_weight":12,"slug":13},11,1,"Template","Presentations",90,"presentations",{"id":15,"doc_module":9,"doc_module_name":10,"category_name":16,"show_sort_weight":17,"slug":18},12,"Resumes",80,"resumes",{"id":20,"doc_module":9,"doc_module_name":10,"category_name":21,"show_sort_weight":22,"slug":23},14,"Invoices",70,"invoices",{"id":25,"doc_module":9,"doc_module_name":10,"category_name":26,"show_sort_weight":27,"slug":28},15,"Posters",60,"posters",{"id":30,"doc_module":9,"doc_module_name":10,"category_name":31,"show_sort_weight":32,"slug":33},16,"Social Media",50,"social-media",{"id":35,"doc_module":9,"doc_module_name":10,"category_name":36,"show_sort_weight":37,"slug":38},17,"Forms",40,"forms",{"id":40,"doc_module":9,"doc_module_name":10,"category_name":41,"show_sort_weight":42,"slug":43},18,"Letters",30,"letters",{"id":45,"doc_module":9,"doc_module_name":10,"category_name":46,"show_sort_weight":47,"slug":48},21,"Paper Templates",5,"papers-templates",{"id":50,"doc_module":9,"doc_module_name":10,"category_name":51,"show_sort_weight":4,"slug":52},158,"General","general-158",{"code":4,"msg":54,"data":55},"ok",{"site_id":56,"language":57,"slug":58,"title":59,"keywords":60,"description":61,"schema_data":62,"social_meta":111,"head_meta":113,"extra_data":115,"updated_unix":117},105,"en","cheat-sheet-c1-acids-and-bases-printable-quick-reference","Cheat Sheet C1 - Acids and Bases - printable quick reference","","Cheat Sheet C1, C2, C3, and C4 provides concise revision formulas and worked-style multiple-choice questions covering key chemistry foundations. It summarizes acid-base dissociation and pH/pOH relationships, mole conversions and major gas laws, and equilibrium expressions for aqueous and gaseous systems using KC/KP alongside Dalton’s, Raoult’s, and Henry’s laws. It further outlines reaction rate laws with Arrhenius and Michaelis–Menten, plus thermodynamics via heat calculations, Hess’ law, and entropy changes.",{"@graph":63,"@context":110},[64,80,101],{"@type":65,"itemListElement":66},"BreadcrumbList",[67,71,74,77],{"item":68,"name":69,"@type":70,"position":9},"https://docshare.wps.com","Home","ListItem",{"item":72,"name":10,"@type":70,"position":73},"https://docshare.wps.com/template/",2,{"item":75,"name":51,"@type":70,"position":76},"https://docshare.wps.com/template/general/",3,{"item":78,"name":59,"@type":70,"position":79},"https://docshare.wps.com/template/cheat-sheet-c1-acids-and-bases-printable-quick-reference/573092/",4,{"url":78,"name":59,"@type":81,"image":82,"author":87,"headline":59,"publisher":90,"fileFormat":93,"inLanguage":57,"description":61,"dateModified":94,"datePublished":95,"encodingFormat":93,"isAccessibleForFree":96,"interactionStatistic":97},"DigitalDocument",{"url":83,"@type":84,"width":85,"height":86},"https://docshare.wps.com/thumbnails/cheat-sheet-c1-acids-and-bases-printable-quick-reference/573092.png","ImageObject",442,249,{"name":88,"@type":89},"\tJames","Person",{"url":68,"name":91,"@type":92},"DocShare","Organization","application/pdf","2026-10-19","2026-10-13",true,{"@type":98,"interactionType":99,"userInteractionCount":79},"InteractionCounter",{"@type":100},"ViewAction",{"@type":102,"mainEntity":103},"FAQPage",[104],{"name":105,"@type":106,"acceptedAnswer":107},"How are equilibrium constants expressed for aqueous versus gaseous systems?","Question",{"text":108,"@type":109},"For aqueous species, KC is written using concentrations as KC = [C]c[D]d / ([A]a[B]b). For gaseous species, KP is written using partial pressures: KP = (pC)c(pD)d / (pA)a(pB)b.","Answer","https://schema.org",{"og:url":78,"og:type":112,"og:title":59,"og:site_name":91,"og:description":61},"article",{"robots":114,"canonical":78},"index,follow",{"doc_id":116,"site_id":56},573092,1792086183,{"code":4,"msg":5,"data":119},{"doc_id":116,"user_id":120,"nickname":88,"user_avatar":121,"doc_module":9,"category_id":50,"category_name":51,"doc_title":59,"doc_description":61,"doc_content":122,"file_id":123,"file_url":124,"file_type":125,"file_size":126,"view_count":79,"is_deleted":4,"is_public":9,"is_downloadable":9,"audit_status":9,"page_count":15,"language":127,"language_code":57,"site_id":56,"html_lang":57,"table_of_contents":128,"faqs":129,"seo_title":130,"seo_description":61,"update_tm":131,"read_time":79},2336474466412,"https://ap-avatar.wpscdn.com/davatar_155a257f0dc6eb9ab79c44ca47cae57d","Cheat Sheet C1: Acids and Bases  \nThe general equation for acid dissociation is: HA + H20 ⇌ H30 +A –  \nThe acid dissociation constant, Ka, is given by:[H 0+][A–]  \nKa = ~~ ~~~~ ~~ pKa= −logKa  \npH and pOH are defined as:  \npH = −log[H30+] pOH = −log[OH–]  \nThe ionic product of water is given by:  \nKw= [OH–][H30+] = 10 − 14 pKw = pH + pOH = 14  \nat 298 K at 298 K  \nBu􀀝er solutions obey the Henderson-Hasselbach equation: pH = pKa + log [[AHA–]]  \nAll concentrations are in mol dm − 3.  \n1  \nA solution is made by dissolving 28 g of potassium hydroxide (molar mass = 56) in 100 mL of water. The solution is allowed to cool to 25°C.  \nWhat is the pH of this solution?  \nA. Less than 14  \nB. 14  \nC. Greater than 14 but less than 15  \nD. 15  \n2  \nAt 25°C the pKa of H2 PO4- is 7.21. In order to maintain a system at pH 6.2, the amount of NaH2 PO4 sodium hydrogen phosphate in the bu er should be:  \nA. Twice the amount of Na2 HPO4  \nB. Equal to the amount of Na2 HPO4  \nC. One fifth the amount of Na2 HPO4  \nD. Ten times the amount of Na2 HPO4  \nAnswers: 1 C, 2D  \nWant more questions and expert tips to prepare for the GAMSAT?  [medify.co.uk](medify.co.uk)  \nSign up to Medify's GAMSAT Online Course now.  [medify.com.au](medify.com.au)  \nCheat Sheet C2: Moles and Gas Laws  \nA mole means 6.022 × 1023 particles.  \nRelative atomic mass of a sample of an element made of di􀀝erent isotopes:  \nm1 abundance1 + m2 abundance2 + m3 abundance3 +   A =    \nr  \nabundance1 + abundance2 + abundance3 +   Conversion between mass and moles.  \nmass (g)  \nAmount (mol) =  relative formula (or molecular) mass × Mu (g mol−1)  \nwhere Mu = 1 g mol−1  \nGas laws: Boyle’s law p1 V1 = p2 V2  \n\n| Charles’ law |  V1\u003Cbr>T1\u003Cbr>=\u003Cbr> V2\u003Cbr>T2 |\n| --- | --- |\n| Gay-Lussac‘s law |  p1\u003Cbr>T1\u003Cbr>=\u003Cbr>p2\u003Cbr>T2 |\n| Avogadro’s law | V\u003Cbr>n |\n| Ideal Gas law | pV = nRT |\n| Kinetic Gas equation | pV = mnC3RMS2 |\n| Graham’s law of di􀀝usion | Rate1 ∝  1  M1\u003Cbr>|\n\nGraham’s law of di􀀝usion 2 Rate~~ ~~1Rate~~ ~~2 = ~~ ~~MM21  \nWhere m = mass, p = pressure, V = volume, n = number of molecules, T = temperature, R = the gas constant, CRMS = root mean squared velocity, Mx is the molecular mass of gas x  \n1  \nAt standard temperature and pressure, fluorine gas has a density of 1.696 gL−1 and chlorine gas has a density of 3.214 gL−1 . Which of these is the best estimate of the relative rates of di usion of fluorine and chlorine?  \n1  \nA. RateCl =  RateF  \n2  \nB. RateCl = 12 RateF  \nC. RateCl = 2 RateF  \nD. RateCl = 2 RateF  \n| 2\u003Cbr>An ideal gas is heated from 400 K to 900 K. What will happen the the root mean squared velocity (CRMS)?\u003Cbr>A. The root mean squared velocity will not change\u003Cbr>B. The root mean squared velocity will increase by a factor of 49\u003Cbr>C. The root mean squared velocity will increase by a factor of 32\u003Cbr>D. The root mean squared velocity 3\u003Cbr>will increase by a factor of 3 × 2\u003Cbr>| Answers: 1A, 2C |\n| --- | --- |\n\nWant more questions and expert tips to prepare for the GAMSAT?  [medify.co.uk](medify.co.uk)  \nSign up to Medify's GAMSAT Online Course now.  [medify.com.au](medify.com.au)  \nCheat Sheet C3: Equilibrium  \naA + bB ⇌ cC + dD  \nWhen all species are aqueous, the equilibrium constant, KC, can be expressed as:  \n[C]c [D]d Kc = [A]a [B]b  \nWhen all species are gaseous, the equilibrium constant, KP, can be expressed as:  \n(pC)c (pD)d  \nKP =  \n(pA)a (pB)b  \nwhere pA=xA × ptot ; xA= totnalon.~~ ~~moooles~~ ~~off~~ ~~molgesasofAgas ; xtot = xA + xB + xC + xD = 1  \nDalton’s law: ptot + pA + pB + pC + pD  \nRaoult’s law: the vapour pressure of a solution, p, is equal to the vapour pressure of the pure solvent, p°solv, multiplied by the mole fraction of the pure solvent, xsolv:  \n°  \np = xsolv × psolv  \nRaoult’s law applied to a mixture of two volatile liquids, A and B, at equilibrium:  \n°  \np = xA × pA + xB + p°B  \nHenry’s law: for real solutions at low concentrations:  \npC = xC × KH  \nNote: KC and KP = equilibrium constants,[X] = concentration of X, pA = partial pressure of A, xA = m","cbCairWWxYtfblH8","https://ap.wps.com/l/cbCairWWxYtfblH8","pdf",2518028,"English","# Cheat Sheet C1: Acids and Bases\n## Acid dissociation, Ka and pKa\n## pH, pOH, Kw and pKw\n## Buffer solutions (Henderson–Hasselbalch)\n## Practice questions\n# Cheat Sheet C2: Moles and Gas Laws\n## Mole and relative atomic mass concepts\n## Converting mass and moles\n## Boyle’s, Charles’, Gay-Lussac’s and related gas laws\n## Ideal gas and kinetic gas relations\n## Diffusion (Graham’s law)\n## Practice questions\n# Cheat Sheet C3: Equilibrium\n## Equilibrium expressions (KC and KP)\n## Dalton’s, Raoult’s and Henry’s laws\n## Mole fraction and partial pressure links\n## Practice questions\n# Cheat Sheet C4: Rates and Thermodynamics\n## Rate law and Arrhenius equation\n## Enzyme kinetics (Michaelis–Menten)\n## Thermodynamics: heat, Hess’ law, entropy","[{\"question\":\"How are equilibrium constants expressed for aqueous versus gaseous systems?\",\"answer\":\"For aqueous species, KC is written using concentrations as KC = [C]c[D]d / ([A]a[B]b). For gaseous species, KP is written using partial pressures: KP = (pC)c(pD)d / (pA)a(pB)b.\"}]","Cheat Sheet C1 - Acids and Bases - printable quick reference | PDF",1791932017]