An experiment calls for you to use 100 mL of 0.65 M HNO3 solution. All you have available is a bottle of 2.7 M HNO3. How many milliliters of the 2.7 M HNO3 solution do you need to prepare the desired solution?
To determine how many milliliters of the 2.7 M HNO3 solution you need to prepare the desired solution, you can use the following formula:
C1V1 = C2V2
where:
C1 = concentration of the initial solution (2.7 M)
V1 = volume of the initial solution (unknown)
C2 = concentration of the final solution (0.65 M)
V2 = volume of the final solution (100 mL or 0.1 L)
Rearranging the formula to solve for V1, we have:
V1 = (C2 * V2) / C1
Let's substitute the given values into the formula:
V1 = (0.65 M * 0.1 L) / 2.7 M
V1 ≈ 0.024 L
To convert the volume from liters to milliliters, multiply by 1000:
V1 ≈ 0.024 L * 1000 mL/L
V1 ≈ 24 mL
Therefore, you would need approximately 24 mL of the 2.7 M HNO3 solution to prepare the desired solution.
To determine the number of milliliters of the 2.7 M HNO3 solution needed to prepare the desired solution, we can use the concept of moles and the formula:
Moles = Volume (in Liters) * Concentration (in Molarity)
First, let's calculate the moles of HNO3 needed for the desired solution:
Moles = Volume (in Liters) * Concentration (in Molarity)
Moles = 0.100 L * 0.65 mol/L
Moles = 0.065 moles
Now, let's calculate the volume of the 2.7 M HNO3 solution required:
Moles = Volume (in Liters) * Concentration (in Molarity)
0.065 moles = Volume (in Liters) * 2.7 mol/L
Rearranging the equation:
Volume (in Liters) = 0.065 moles / 2.7 mol/L
Volume (in Liters) = 0.0241 L
Finally, convert the volume from liters to milliliters:
Volume (in mL) = 0.0241 L * 1000 mL/L
Volume (in mL) ≈ 24.1 mL
Therefore, you would need approximately 24.1 mL of the 2.7 M HNO3 solution to prepare the desired 100 mL solution of 0.65 M HNO3.
mL1 x M1 = mL2 x M2
100 x 0.65 = mL2 x 2.7M
Solve for mL2.