The ratio of number of moles of `KMnO_4 and K _2 Cr _2 O _7`required to oxidise 0.1mol `Sn^ (+4)`in acidic medium :

Explanation

To solve the problem of finding the ratio of the number of moles of \( KMnO_4 \) and \( K_2Cr_2O_7 \) required to oxidize 0.1 moles of \( Sn^{4+} \) in acidic medium, we will follow these steps:

### Step 1: Determine the n-factor for \( KMnO_4 \)
In acidic medium, \( KMnO_4 \) reduces from \( Mn^{+7} \) to \( Mn^{+2} \). The change in oxidation state is:
\[ n_{\text{factor}} = 7 - 2 = 5 \]

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