500 mL of water is added to 25 mL of 6.0 M hydrochloric acid. What is the final concentration of this solution in mol/L?

6.0 x (25/525) = ??

Assuming the volumes are additive.

To find the final concentration of the solution, we need to use the principle of dilution, which states that the moles of solute in the solution remain constant before and after dilution.

First, we need to calculate the moles of hydrochloric acid (HCl) in the 25 mL solution. We can use the formula:

moles = concentration × volume

Given that the initial volume is 25 mL and the initial concentration is 6.0 M, we have:

moles of HCl = 6.0 M × 0.025 L (converting mL to L) = 0.15 moles

When the 500 mL of water is added, the total volume of the solution becomes 525 mL (25 mL + 500 mL). To find the final concentration, we divide the moles of HCl by the final volume:

final concentration = moles of HCl / final volume

Converting the final volume to liters, we have:

final volume = 525 mL ÷ 1000 mL/L = 0.525 L

Now, we can calculate the final concentration:

final concentration = 0.15 moles / 0.525 L = 0.29 M

Therefore, the final concentration of the solution is 0.29 mol/L.