[{"data":1,"prerenderedAt":-1},["ShallowReactive",2],{"doc-detail-207931-en":3,"doc-seo-207931-105":30,"detail-sidebar-cat-0-en-105":89},{"code":4,"msg":5,"data":6},0,"success",{"doc_id":7,"user_id":8,"nickname":9,"user_avatar":10,"doc_module":4,"category_id":11,"category_name":12,"doc_title":13,"doc_description":14,"doc_content":15,"file_id":16,"file_url":17,"file_type":18,"file_size":19,"view_count":4,"is_deleted":4,"is_public":20,"is_downloadable":20,"audit_status":20,"page_count":21,"language":22,"language_code":23,"site_id":24,"html_lang":23,"table_of_contents":25,"faqs":26,"seo_title":27,"seo_description":14,"update_tm":28,"read_time":29},207931,8796095462418,"Noah","https://ap-avatar.wpscdn.com/avatar/80000253c1241d02b47?x-image-process=image/resize,m_fixed,w_180,h_180&k=1778826106357471780",4,"Exam","AQA GCSE Chemistry - Topic 8 - Chemical analysis - Identification of ions by chemical and spectroscopic means","Topic 8 focuses on chemical analysis for identifying ions using practical tests and instrumental methods. It covers flame tests for metal ions and explains how mixed ions can mask flame colours. It then describes precipitation reactions with metal hydroxides, carbonate reactions producing CO2 for limewater confirmation, and halide testing using dilute nitric acid followed by silver nitrate. Finally, it introduces instrumental methods, including flame emission spectroscopy, for producing a line spectrum to identify metal ions and determine concentrations.","AQA GCSE Chemistry  \nTopic 8: Chemical analysis  \nIdentification of ions by chemical and spectroscopic  \nmeans  \nNotes  \n(Content in bold is for Higher Tier only)  \nFlame tests  \n● Flame tests can be used to identify metal ions.  \n\n| Lithium | Crimson |\n| --- | --- |\n| Sodium | Yellow |\n| Potassium | Lilac |\n| Calcium | Orange-Red |\n| Copper | Green |\n\n● However, if a sample containing a mixture of ions is used some flame colours can be masked (you won’t be able to see them)  \nMetal hydroxides  \n● Aluminium, calcium and magnesium ions form a white precipitate with NaOH.  \n● Only aluminium’s precipitate dissolves when excess NaOH is added.  \n● Copper(II) produces a blue precipitate  \n● Iron(II) produces a green precipitate  \n● Iron(III) produces a brown precipitate  \n● equations: e.g. Cu2+ + 2OH- -> Cu(OH)2  \no you need as many OH- ions as the charge on the metal ion  \no the Na from the NaOH and whatever the metal ion was bonded to will react to form a compound together: e.g. CuCl2 + 2NaOH-> Cu(OH)2 + 2NaCl  \nCarbonates  \n● Carbonates react with dilute acids to create carbon dioxide.  \n● This gas can be bubbled through limewater, if the limewater goes cloudy, the gas is CO2.  \nHalides  \n● First add dilute nitric acid, followed by silver nitrate solution  \n● Chloride gives a white precipitate  \n● Bromide gives a cream precipitate  \n● Iodide gives a yellow precipitate  \n● (catswithbrainscanideallyyodel)  \nSulfates  \n● First add dilute hydrochloric acid, followed by barium chloride solution  \n● A white precipitate will form when sulfate ions are in this solution  \nInstrumental methods  \n● Elements and compounds can be detected and identified using instrumental methods  \no These are: accurate, sensitive and rapid, making them advantageous compared to chemical tests  \nFlame emission spectroscopy  \n● Example of an instrumental method used to analyse metal ions in solutions  \n● Sample is put into a flame and the light given out is passed through a spectroscope  \n● Output is a line spectrum that can be analysed to identify the metal ions in the solution and measure their concentrations","cbCaibzLc9IYrGjY","https://ap.wps.com/l/cbCaibzLc9IYrGjY","pdf",169645,1,3,"English","en",105,"# Topic 8: Chemical analysis\n## Identification of ions by chemical and spectroscopic means\n## Flame tests\n## Metal hydroxides\n## Carbonates\n## Halides\n## Sulfates\n## Instrumental methods\n## Flame emission spectroscopy","[{\"question\":\"How can flame tests be used to identify metal ions?\",\"answer\":\"Metal ions produce characteristic flame colours, such as lithium (crimson), sodium (yellow), potassium (lilac), calcium (orange-red), and copper (green). For mixtures, some colours can be masked.\"},{\"question\":\"What observations confirm carbonate ions during chemical analysis?\",\"answer\":\"Carbonates react with dilute acids to produce carbon dioxide. Bubbling the gas through limewater that turns cloudy indicates CO2.\"},{\"question\":\"How does flame emission spectroscopy identify ions and measure concentration?\",\"answer\":\"A sample is placed into a flame and the emitted light is passed through a spectroscope. The resulting line spectrum is analysed to identify metal ions and determine their concentrations.\"}]","AQA GCSE Chemistry - Topic 8 - Chemical analysis - Identification of ions by chemical and spectroscopic means | PDF",1788601776,8,{"code":4,"msg":31,"data":32},"ok",{"site_id":24,"language":23,"slug":33,"title":13,"keywords":34,"description":14,"schema_data":35,"social_meta":84,"head_meta":86,"extra_data":88,"updated_unix":28},"aqa-gcse-chemistry-topic-8-chemical-analysis-identification-of-ions-by-chemical-and-spectroscopic-means","",{"@graph":36,"@context":83},[37,52,66],{"@type":38,"itemListElement":39},"BreadcrumbList",[40,44,48,50],{"item":41,"name":42,"@type":43,"position":20},"https://docshare.wps.com","Home","ListItem",{"item":45,"name":46,"@type":43,"position":47},"https://docshare.wps.com/document/","Document",2,{"item":49,"name":12,"@type":43,"position":21},"https://docshare.wps.com/document/exam/",{"item":51,"name":13,"@type":43,"position":11},"https://docshare.wps.com/document/aqa-gcse-chemistry-topic-8-chemical-analysis-identification-of-ions-by-chemical-and-spectroscopic-means/207931/",{"url":51,"name":13,"@type":53,"author":54,"headline":13,"publisher":56,"fileFormat":59,"inLanguage":23,"description":14,"dateModified":60,"datePublished":60,"encodingFormat":59,"isAccessibleForFree":61,"interactionStatistic":62},"DigitalDocument",{"name":9,"@type":55},"Person",{"url":41,"name":57,"@type":58},"DocShare","Organization","application/pdf","2026-09-05",true,{"@type":63,"interactionType":64,"userInteractionCount":4},"InteractionCounter",{"@type":65},"ViewAction",{"@type":67,"mainEntity":68},"FAQPage",[69,75,79],{"name":70,"@type":71,"acceptedAnswer":72},"How can flame tests be used to identify metal ions?","Question",{"text":73,"@type":74},"Metal ions produce characteristic flame colours, such as lithium (crimson), sodium (yellow), potassium (lilac), calcium (orange-red), and copper (green). For mixtures, some colours can be masked.","Answer",{"name":76,"@type":71,"acceptedAnswer":77},"What observations confirm carbonate ions during chemical analysis?",{"text":78,"@type":74},"Carbonates react with dilute acids to produce carbon dioxide. Bubbling the gas through limewater that turns cloudy indicates CO2.",{"name":80,"@type":71,"acceptedAnswer":81},"How does flame emission spectroscopy identify ions and measure concentration?",{"text":82,"@type":74},"A sample is placed into a flame and the emitted light is passed through a spectroscope. 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