To solve this problem, we can use the formula M1V1 = M2V2, where M1 is the molarity of the initial solution, V1 is the volume of the initial solution, M2 is the molarity of the final solution, and V2 is the volume of the final solution.

Given:
M1 = 6.00 M (molarity of the initial solution)
M2 = 1.50 M (molarity of the final solution)
V2 = 125.0 mL (volume of the final solution)

We need to find V1 (volume of the initial solution).

Rearranging the formula to solve for V1 gives us V1 = (M2 * V2) / M1.

Substituting the given values into the formula gives us V1 = (1.50 M * 125.0 mL) / 6.00 M = 31.25 mL.

Therefore, the T.A. needs 31.25 mL of the 6.00 M HCl solution to make 125.0 mL of a 1.50 M HCl solution.

Question

To solve this problem, we can use the formula M1V1 = M2V2, where M1 is the molarity of the initial solution, V1 is the volume of the initial solution, M2 is the molarity of the final solution, and V2 is the volume of the final solution.

Given:
M1 = 6.00 M (molarity of the initial solution)
M2 = 1.50 M (molarity of the final solution)
V2 = 125.0 mL (volume of the final solution)

We need to find V1 (volume of the initial solution).

Rearranging the formula to solve for V1 gives us V1 = (M2 * V2) / M1.

Substituting the given values into the formula gives us V1 = (1.50 M * 125.0 mL) / 6.00 M = 31.25 mL.

Therefore, the T.A. needs 31.25 mL of the 6.00 M HCl solution to make 125.0 mL of a 1.50 M HCl solution.

Knowee AI · Accepted Answer

To solve this problem, we can use the formula M1V1 = M2V2, where M1 is the molarity of the initial solution, V1 is the volume of the initial solution, M2 is the molarity of the final solution, and V2 is the volume of the final solution.

Given:
M1 = 6.00 M (molarity of the initial solution)
M2 = 1.50 M (molarity of the final solution)
V2 = 125.0 mL (volume of the final solution)

We need to find V1 (volume of the initial solution).

Rearranging the formula to solve for V1 gives us V1 = (M2 * V2) / M1.

Substituting the given values into the formula gives us V1 = (1.50 M * 125.0 mL) / 6.00 M = 31.25 mL.

Therefore, the T.A. needs 31.25 mL of the 6.00 M HCl solution to make 125.0 mL of a 1.50 M HCl solution.

A T.A. decides to prepare a more dilute solution from a stock solution. What volume of a 6.00 M HCl in milliliters is required to make 125.0 mL of a 1.50 M HCl solution? Express your answer to the correct number of significant figures.

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