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To calculate the molarity (M) of the \( K_2CO_3 \) solution, we use the formula for molarity:

\[
\text{Molarity (M)} = \frac{\text{moles of solute}}{\text{volume of solution in liters}}
\]

From the problem:

- Moles of \( K_2CO_3 \) = 6.44 moles
- Volume of the solution = 5.00 L

Now, substituting the values:

\[
\text{Molarity} = \frac{6.44 \, \text{moles}}{5.00 \, \text{L}} = 1.288 \, \text{M}
\]

So, the molarity of the \( K_2CO_3 \) solution is **1.29 M** (rounded to three significant figures).

Would you like further details on how molarity works or have any questions?

Here are 5 related questions you might consider:
1. What is the definition of molarity in chemistry?
2. How would you prepare a solution if only the molarity and volume are given?
3. How do you calculate molarity if you are given grams instead of moles of solute?
4. What is the relationship between molarity and dilution of a solution?
5. Can molarity change with temperature, and if so, why?

**Tip:** Always ensure the volume is in liters (L) when calculating molarity; if given in milliliters, convert it by dividing by 1000.

An aqueous potassium carbonate solution is made by dissolving 6.44 moles of K2CO3 in sufficient water so that the final volume of the solution is 5.00 L. Calculate the molarity of the K2CO3 solution.

Learn how to calculate the molarity of a K2CO3 solution when 6.44 moles of solute is dissolved in 5.00 L of solution. This solution covers key chemistry concepts such as molarity, moles, and volume relationships. Ideal for students in Grades 10-12.

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