Final answer:
The molarity of the diluted HCl solution after adding 50 ml of water to 300 ml of a 0.54 m HCl solution is approximately 0.4629 M.
Step-by-step explanation:
When 50 ml of water is added to 300 ml of a 0.54 m HCl solution, the molarity of the diluted solution can be calculated using the dilution formula M1 × V1 = M2 × V2, where M1 and V1 are the initial molarity and volume, M2 is the final molarity, and V2 is the final volume of the solution after dilution.
In this case, the initial molarity (M1) is 0.54 M, the initial volume (V1) is 300 ml, the final volume (V2) after adding 50 ml of water is 350 ml (300 ml + 50 ml). To find the new molarity (M2), we rearrange the formula to M2 = (M1 × V1) / V2 and substitute the known values to get M2 = (0.54 M × 300 ml) / 350 ml.
By calculating this, we get a new molarity of approximately 0.4629 M for the diluted HCl solution. It's important to remember that molarity is defined as moles of solute per liter of solution, and when we dilute a solution, the number of moles of solute remains unchanged while the total volume of the solution increases.