In undergraduate chemistry teaching labs, an Fe2+ solution, normally of unknown concentration, is titrated with a...
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In undergraduate chemistry teaching labs, an Fe2+ solution, normally of unknown concentration, is titrated with a KMNO4 solution of exact concentration (assume 0.062 M). The 'endpoint is detected when the purple color of permanganate persists. Give the (balanced) reactions that are occurring and explain the titration experiment at various stages, using the Nernst equation. In undergraduate chemistry teaching labs, an Fe2+ solution, normally of unknown concentration, is titrated with a KMNO4 solution of exact concentration (assume 0.062 M). The 'endpoint is detected when the purple color of permanganate persists. Give the (balanced) reactions that are occurring and explain the titration experiment at various stages, using the Nernst equation.
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