To what volume must 10.0ml of 5.00 M HCL be diluted to make a 0.500 M HCL solution ?

10.0*5.0/0.500=100ml

mL1 x M1 = mL2 x M2

To calculate the volume of the 5.00 M HCl solution that needs to be diluted to make a 0.500 M HCl solution, you can use the dilution formula:

C1V1 = C2V2

Where:
C1 = initial concentration of the solution
V1 = initial volume of the solution
C2 = final concentration of the solution
V2 = final volume of the solution (unknown)

Let's plug in the values:

C1 = 5.00 M
V1 = 10.0 mL (convert to liters by dividing by 1000: 10.0 mL / 1000 = 0.010 L)
C2 = 0.500 M
V2 = unknown

Using the formula C1V1 = C2V2, we can rearrange it to solve for V2:

V2 = (C1V1) / C2

Plugging in the values:

V2 = (5.00 M * 0.010 L) / 0.500 M

V2 = 0.1 L

Therefore, you must dilute 10.0 mL of 5.00 M HCl to a volume of 0.1 L (or 100 mL) to make a 0.500 M HCl solution.

To determine the volume of 5.00 M HCl solution needed, we can use the formula:

C1V1 = C2V2

Where:
C1 = initial concentration of HCl (5.00 M)
V1 = initial volume of HCl (10.0 mL)
C2 = final concentration of HCl (0.500 M)
V2 = final volume of the diluted solution (unknown)

Rearranging the equation to solve for V2:

V2 = (C1 * V1) / C2

Plugging in the values:

V2 = (5.00 M * 10.0 mL) / 0.500 M

V2 = 100 mL

Therefore, you need to dilute 10.0 mL of 5.00 M HCl with water to a final volume of 100 mL to obtain a 0.500 M HCl solution.