To find the volume of solution required to prepare a 1.13 M solution containing 1 mole of $KMnO_4$, use the formula for molarity:

$M = \frac{\text{moles of solute}}{\text{liters of solution}}$

Rearrange the formula to solve for the volume of solution:

$\text{Liters of solution} = \frac{\text{moles of solute}}{M}$

Substitute the given values:

$\text{Liters of solution} = \frac{1}{1.13}$

Perform the calculation:

$\text{Liters of solution} = 0.885$

To the nearest hundredth, the answer is:

0.89

Would you like further clarification or additional examples?
Here are five related questions:

1. How would you prepare a 2.5 M solution of NaCl if you need 3 moles?
2. What is the molarity of a solution with 0.5 moles of solute in 0.25 liters?
3. If you dilute 2 liters of a 5 M solution to 10 liters, what is the new molarity?
4. How many moles of $KMnO_4$ are needed to prepare 0.5 L of a 0.75 M solution?
5. What is the volume required to dilute a 10 M solution to 1 M with 1 liter of water?

Tip: Always ensure to convert units (like milliliters to liters) when using the molarity formula!