🤓 Based on our data, we think this question is relevant for Professor Daly's class at ARIZONA.

Problem

How many milliliters of a 6.00 M NaOH solution are needed to provide 0.355 mol of NaOH?

Solution

We’re being asked to **calculate the milliliter of 6.00 M NaOH **needed to provide **0.355 mol NaOH solution**.

The given values are:

Moles of NaOH needed = **0.355 mol NaOH**

Molarity of NaOH = **6.00 M NaOH**

Recall that * molarity* is the ratio of the moles of solute and the volume of solution (in liters).

In other words:

$\overline{){\mathbf{Molarity}}{\mathbf{\left(}}{\mathbf{M}}{\mathbf{\right)}}{\mathbf{=}}\frac{\mathbf{moles}\mathbf{}\mathbf{of}\mathbf{}\mathbf{solute}}{\mathbf{Liters}\mathbf{}\mathbf{of}\mathbf{}\mathbf{solution}}}$

Molarity

→ Molarity

→ Molarity