**Calculating the Volume of Water to Add to 50cm³ 0.02M Solution**

**Introduction**

In chemistry, calculating the volume of water to add to a solution is an essential skill. In this article, we will explore how to calculate the volume of water needed to add to 50cm³ of 0.02M solution.

**The Problem**

You have 50cm³ of a 0.02M solution, and you want to know how much water you need to add to achieve a certain concentration or volume. To solve this problem, we need to understand the concept of molarity and how it relates to the volume of a solution.

**Molarity**

Molarity (M) is a measure of the concentration of a solution, defined as the number of moles of solute per liter of solution. In our case, we have a 0.02M solution, which means that there are 0.02 moles of solute per liter of solution.

**Calculating the Volume of Water**

To calculate the volume of water needed to add to the solution, we need to know the desired concentration or volume of the final solution. Let's assume we want to add water to achieve a final volume of 100cm³.

**Step 1: Calculate the Number of Moles of Solute**

First, we need to calculate the number of moles of solute in the 50cm³ of 0.02M solution:

**Number of moles = Molarity x Volume (in liters)**

Since 50cm³ is equal to 0.05 liters, we can plug in the values:

**Number of moles = 0.02M x 0.05L = 0.001 moles**

**Step 2: Calculate the Volume of Water Needed**

Next, we need to calculate the volume of water needed to achieve the desired final volume of 100cm³. Since we want to maintain the same concentration of 0.02M, we can set up the following equation:

**Number of moles = Molarity x Volume (in liters)**

Rearranging the equation to solve for volume, we get:

**Volume = Number of moles / Molarity**

Plugging in the values, we get:

**Volume = 0.001 moles / 0.02M = 0.05L**

Since we want to add water to achieve a final volume of 100cm³, we can convert the volume from liters to cm³:

**Volume of water needed = 0.05L x 1000cm³/L = 50cm³**

Therefore, we need to add **50cm³ of water** to the 50cm³ of 0.02M solution to achieve a final volume of 100cm³.

**Conclusion**

In this article, we have demonstrated how to calculate the volume of water needed to add to a solution to achieve a desired concentration or volume. By understanding the concept of molarity and how it relates to the volume of a solution, we can solve problems like this with ease.