{"id":148949,"date":"2024-02-27T18:32:50","date_gmt":"2024-02-27T13:02:50","guid":{"rendered":"https:\/\/www.mapsofindia.com\/my-india\/?p=148949"},"modified":"2024-02-27T18:32:50","modified_gmt":"2024-02-27T13:02:50","slug":"can-copper-sulphate-solution-be-stored-in-a-pot-made-of-zine-explain","status":"publish","type":"post","link":"https:\/\/www.mapsofindia.com\/my-india\/quiz\/can-copper-sulphate-solution-be-stored-in-a-pot-made-of-zine-explain","title":{"rendered":"Can copper sulphate solution be stored in a pot made of zine? Explain…"},"content":{"rendered":"

Can copper sulphate solution be stored in a pot made of zine?
\nExplain with the help of the value of E\u00b0 cell.
\n(E\u00b0 Cu2+ \/ Cu = 0.34 V)
\n(E\u00b0 Zn2+ \/ Zn = \u2013 0.76 V)<\/h2>\n

Ans.<\/h3>\n

No, copper sulfate solution cannot be stored in a pot made of zinc. This is due to the potential for a galvanic cell reaction to occur between zinc and copper ions in the copper sulfate solution, leading to corrosion of the zinc pot.<\/h3>\n

The standard electrode potential (\ufffd\u00b0<\/span>E<\/span>\u00b0<\/span><\/span><\/span><\/span><\/span>) values provided for the reactions involving copper (\ufffd\ufffd2+\/\ufffd\ufffd<\/span>C<\/span>u<\/span>2+<\/span><\/span><\/span><\/span><\/span><\/span><\/span>\/<\/span>C<\/span>u<\/span><\/span><\/span><\/span><\/span>) and zinc (\ufffd\ufffd2+\/\ufffd\ufffd<\/span>Z<\/span>n<\/span>2+<\/span><\/span><\/span><\/span><\/span><\/span><\/span>\/<\/span>Z<\/span>n<\/span><\/span><\/span><\/span><\/span>) ions are as follows:<\/h3>\n
    \n
  • \n

    \ufffd\u00b0\ufffd\ufffd2+\/\ufffd\ufffd=0.34\u2009V<\/span>E<\/span>\u00b0C<\/span>u<\/span>2+<\/span><\/span>\/C<\/span>u<\/span><\/span><\/span><\/span>\u200b<\/span><\/span><\/span><\/span><\/span>=<\/span><\/span>0.34<\/span>V<\/span><\/span><\/span><\/span><\/span><\/span><\/h3>\n<\/li>\n
  • \n

    \ufffd\u00b0\ufffd\ufffd2+\/\ufffd\ufffd=\u22120.76\u2009V<\/span>E<\/span>\u00b0Z<\/span>n<\/span>2+<\/span><\/span>\/Z<\/span>n<\/span><\/span><\/span><\/span>\u200b<\/span><\/span><\/span><\/span><\/span>=<\/span><\/span>\u2212<\/span>0.76<\/span>V<\/span><\/span><\/span><\/span><\/span><\/span><\/h3>\n<\/li>\n<\/ul>\n

    For a galvanic cell reaction, the overall cell potential (\ufffd\u00b0cell<\/span>E<\/span>\u00b0cell<\/span><\/span><\/span><\/span>\u200b<\/span><\/span><\/span><\/span><\/span><\/span><\/span><\/span><\/span>) is determined by the difference between the standard electrode potentials of the two half-cells:<\/h3>\n

    \ufffd\u00b0cell=\ufffd\u00b0cathode\u2212\ufffd\u00b0anode<\/span>E<\/span>\u00b0cell<\/span><\/span><\/span><\/span>\u200b<\/span><\/span><\/span><\/span><\/span>=<\/span><\/span>E<\/span>\u00b0cathode<\/span><\/span><\/span><\/span>\u200b<\/span><\/span><\/span><\/span><\/span>\u2212<\/span><\/span>E<\/span>\u00b0anode<\/span><\/span><\/span><\/span>\u200b<\/span><\/span><\/span><\/span><\/span><\/span><\/span><\/span><\/span><\/h3>\n

    In this case, copper ions (\ufffd\ufffd2+<\/span>C<\/span>u<\/span>2+<\/span><\/span><\/span><\/span><\/span><\/span><\/span><\/span><\/span><\/span><\/span>) from the copper sulfate solution would act as the cathode, and zinc metal (\ufffd\ufffd<\/span>Z<\/span>n<\/span><\/span><\/span><\/span><\/span>) from the zinc pot would act as the anode.<\/h3>\n

    Given the standard electrode potentials, the overall cell potential (\ufffd\u00b0cell<\/span>E<\/span>\u00b0cell<\/span><\/span><\/span><\/span>\u200b<\/span><\/span><\/span><\/span><\/span><\/span><\/span><\/span><\/span>) for the reaction would be:<\/h3>\n

    \ufffd\u00b0cell=\ufffd\u00b0\ufffd\ufffd2+\/\ufffd\ufffd\u2212\ufffd\u00b0\ufffd\ufffd2+\/\ufffd\ufffd<\/span>E<\/span>\u00b0cell<\/span><\/span><\/span><\/span>\u200b<\/span><\/span><\/span><\/span><\/span>=<\/span><\/span>E<\/span>\u00b0C<\/span>u<\/span>2+<\/span><\/span>\/C<\/span>u<\/span><\/span><\/span><\/span>\u200b<\/span><\/span><\/span><\/span><\/span>\u2212<\/span><\/span>E<\/span>\u00b0Z<\/span>n<\/span>2+<\/span><\/span>\/Z<\/span>n<\/span><\/span><\/span><\/span>\u200b<\/span><\/span><\/span><\/span><\/span><\/span><\/span><\/span><\/span> \ufffd\u00b0cell=(0.34\u2009V)\u2212(\u22120.76\u2009V)<\/span>E<\/span>\u00b0cell<\/span><\/span><\/span><\/span>\u200b<\/span><\/span><\/span><\/span><\/span>=<\/span><\/span>(<\/span>0.34<\/span>V<\/span><\/span>)<\/span>\u2212<\/span><\/span>(<\/span>\u2212<\/span>0.76<\/span>V<\/span><\/span>)<\/span><\/span><\/span><\/span><\/span> \ufffd\u00b0cell=1.10\u2009V<\/span>E<\/span>\u00b0cell<\/span><\/span><\/span><\/span>\u200b<\/span><\/span><\/span><\/span><\/span>=<\/span><\/span>1.10<\/span>V<\/span><\/span><\/span><\/span><\/span><\/span><\/h3>\n

    The positive value of \ufffd\u00b0cell<\/span>E<\/span>\u00b0cell<\/span><\/span><\/span><\/span>\u200b<\/span><\/span><\/span><\/span><\/span><\/span><\/span><\/span><\/span> indicates that the reaction is spontaneous, and thus, there would be a tendency for zinc metal to undergo oxidation (loss of electrons) and dissolve into the copper sulfate solution. This would result in corrosion of the zinc pot.<\/h3>\n

    To prevent such corrosion, it’s important to avoid storing copper sulfate solution in a container made of zinc or any other metal with a higher negative standard electrode potential than zinc.<\/h3>\n","protected":false},"excerpt":{"rendered":"

    Can copper sulphate solution be stored in a pot made of zine? Explain with the help of the value of E\u00b0 cell. (E\u00b0 Cu2+ \/ Cu = 0.34 V) (E\u00b0 Zn2+ \/ Zn = \u2013 0.76 V) Ans. No, copper sulfate solution cannot be stored in a pot made of zinc. This is due to […]<\/p>\n","protected":false},"author":21830,"featured_media":114041,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[12119],"tags":[],"class_list":{"0":"post-148949","1":"post","2":"type-post","3":"status-publish","4":"format-standard","5":"has-post-thumbnail","7":"category-quiz"},"aioseo_notices":[],"_links":{"self":[{"href":"https:\/\/www.mapsofindia.com\/my-india\/wp-json\/wp\/v2\/posts\/148949","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.mapsofindia.com\/my-india\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.mapsofindia.com\/my-india\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.mapsofindia.com\/my-india\/wp-json\/wp\/v2\/users\/21830"}],"replies":[{"embeddable":true,"href":"https:\/\/www.mapsofindia.com\/my-india\/wp-json\/wp\/v2\/comments?post=148949"}],"version-history":[{"count":1,"href":"https:\/\/www.mapsofindia.com\/my-india\/wp-json\/wp\/v2\/posts\/148949\/revisions"}],"predecessor-version":[{"id":148950,"href":"https:\/\/www.mapsofindia.com\/my-india\/wp-json\/wp\/v2\/posts\/148949\/revisions\/148950"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/www.mapsofindia.com\/my-india\/wp-json\/wp\/v2\/media\/114041"}],"wp:attachment":[{"href":"https:\/\/www.mapsofindia.com\/my-india\/wp-json\/wp\/v2\/media?parent=148949"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.mapsofindia.com\/my-india\/wp-json\/wp\/v2\/categories?post=148949"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.mapsofindia.com\/my-india\/wp-json\/wp\/v2\/tags?post=148949"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}