Consider the following species at standard conditions- Na+- Cl-- Ag+-.docx

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Consider the following species at standard conditions: Na+, Cl-, Ag+, Zn2+, Zn, Pb Please explain why as well! i) What is the strongest reducing agent? ii) Which is the strongest oxidizing agent? iii) Which species can be oxidized by acidic SO4 2-(aq)? iv) Which species can be reduced by Al(s)? v) Which of the solids dissolve in HCl? Solution i) The strongest reducing agent is Zn. Because it can easily under go oxidation and reduce other species. ii) The strongest oxidizing agent is Ag + ion. Becasue it is placed at bottom of the electrochemical series. We know that the ions or elements placed bottom of the series can accept electrons easily and under go reduction. iii) Zn can be oxidized by sulfate iion. Because it is placed top in electrochemical series than remaining elements iv) Ag + ion can be reduced easily be aluminium metal. Due to high SRP values of silver ion v) Zn,Pd and sodium metals can dissolve in acids. .

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