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

1. First, convert the initial volume from mL to L: 50.0 mL = 0.050 L
2. Convert the final volume from mL to L: 450.0 mL = 0.450 L
3. Substitute the known values into the formula: (0.660 M)(0.050 L) = M2(0.450 L)
4. Solve for M2: M2 = (0.660 M)(0.050 L) / 0.450 L
5. M2 = 0.0733 M

So, the molarity of the diluted solution is 0.0733 M.

Question

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

1. First, convert the initial volume from mL to L: 50.0 mL = 0.050 L
2. Convert the final volume from mL to L: 450.0 mL = 0.450 L
3. Substitute the known values into the formula: (0.660 M)(0.050 L) = M2(0.450 L)
4. Solve for M2: M2 = (0.660 M)(0.050 L) / 0.450 L
5. M2 = 0.0733 M

So, the molarity of the diluted solution is 0.0733 M.

Knowee AI · Accepted Answer

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

1. First, convert the initial volume from mL to L: 50.0 mL = 0.050 L
2. Convert the final volume from mL to L: 450.0 mL = 0.450 L
3. Substitute the known values into the formula: (0.660 M)(0.050 L) = M2(0.450 L)
4. Solve for M2: M2 = (0.660 M)(0.050 L) / 0.450 L
5. M2 = 0.0733 M

So, the molarity of the diluted solution is 0.0733 M.

Enough water is added to 50.0 mL of a 0.660 M NaOH solution in order to bring the total volume to 450.0 mL. What is the molarity of this diluted solution?

Question

Enough water is added to 50.0 mL of a 0.660 M NaOH solution in order to bring the total volume to 450.0 mL. What is the molarity of this diluted solution?

Solution

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