Answer :
By calculating the number of moles and using the mole ratio from the balanced equation, we can determine the number of moles of KI needed. Finally, using the concentration of the KI solution, we can find the volume in mL. The volume of the 0.150 N KI solution required is approximately 9.83 mL.
The balanced equation for the reaction between KI and KMnO4 in basic solution is:
2 KMnO4 + 10 KI + H2O → 2 MnO2 + 5 I2 + 10 KOH
The mole ratio between KMnO4 and KI is 2:10. Given that the volume of the KMnO4 solution is 34.1 mL and its concentration is 0.216 N, we can calculate the number of moles of KMnO4:
moles KMnO4 = volume (in L) × concentration = 34.1 mL × (1 L/1000 mL) × (0.216 mol/L) = 0.00737056 mol
From the balanced equation, we can see that 2 moles of KMnO4 react with 10 moles of KI. Therefore, the number of moles of KI needed is:
moles KI = (2/10) × moles KMnO4 = (2/10) × 0.00737056 mol = 0.001474112 mol
Now, we can calculate the volume of the KI solution using its concentration:
volume (in L) = moles/volume (in L) = 0.001474112 mol / 0.150 mol/L = 0.00982741 L = 9.82741 mL ≈ 9.83 mL
Therefore, the volume of a 0.150 N KI solution required to react with 34.1 mL of a 0.216 N solution of KMnO4 in basic solution is approximately **9.83 mL**.
To learn more about Volume click here:
https://brainly.com/question/14710169
#SPJ11
