If you add enough water to 175.0 mL of a .15 M NaCl solution until the final volume is 350.0 mL, what will the molarity of the diluted solution be?

If you could do step by step it would be appreciated :)

0.15M x (175.0/350.0) = ?

To find the molarity of the diluted solution, you need to use the formula:

M1V1 = M2V2

where:
M1 = initial molarity of the solution (before dilution)
V1 = initial volume of the solution (before dilution)
M2 = final molarity of the solution (after dilution)
V2 = final volume of the solution (after dilution)

In this case, the initial molarity (M1) is 0.15 M, and the initial volume (V1) is 175.0 mL. The final volume (V2) is 350.0 mL.

Now, we can plug in the values into the formula:

(0.15 M)(175.0 mL) = (M2)(350.0 mL)

To solve for M2, divide both sides of the equation by 350.0 mL:

(0.15 M)(175.0 mL) / 350.0 mL = M2

Calculate the solution:

M2 = 0.075 M

Therefore, the molarity of the diluted solution is 0.075 M.