The intermolecular forces that exist between molecules of NH3, H2O, and HF are hydrogen bonding, dipole-dipole interactions, and London dispersion forces.
The intermolecular forces that exist between molecules of NH3, H2O, and HF are called hydrogen bonding, dipole-dipole interactions, and London dispersion forces. Hydrogen bonding occurs between a hydrogen atom bonded to a highly electronegative atom (such as O, N, or F) and a lone pair of electrons on a nearby molecule. Dipole-dipole interactions occur between molecules with permanent dipole moments, while London dispersion forces occur due to the temporary formation of induced dipoles in adjacent molecules.
The right response is that, Using the 0.200 M KBr solution, about 43.31 mL should be mixed with water to create a 0.0495 M solution with a volume of 175.0 mL.
175.0 mL is the final volume needed for a 0.0495 M solution. To achieve this, we can use the dilution formula and calculate the amount of 0.200 M KBr solution necessary.
V2C2 is equivalent to V1C1, as depicted by the formula C1V1 = C2V2.
Where:
Starting at 0.200 M, C1 indicates the concentration of the solution.
Unknown is the designation for the volume of the first solution that will be used.
The diluted solution's final volume is V2, and its ultimate concentration is marked as C2 (0.0495 M).
To determine V1, rewrite the equation as V1 = (C2 * V2) / C1.
Based on these values:
V2 is 175.0 mL, C1 is 0.200 M, and C2 is 0.0495 M.
Enter the corresponding values to establish V1:
= (0.0495 * 175.0) / 0.200 V1 = 43.3125 mL
You would need around 43.31 mL of the 0.200 M KBr solution to make a 0.0495 M solution (rounded to two decimal places) when diluted to 175.0 mL with water.
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Final answer:
To prepare a 0.0495 M solution of KBr by dilution to 175.0 mL with water, you would need 2.744 mL of 0.200 M KBr solution.
Explanation:
When diluting a solution, the equation M1V1 = M2V2 holds true, where M1 is the initial concentration, V1 is the initial volume, M2 is the final concentration, and V2 is the final volume. In this case, the final concentration (M2) is 0.0495 M, and the final volume (V2) is 175.0 mL.
Rearranging the equation to solve for V1, the initial volume of the concentrated solution needed, we have:
V1 = (M2 * V2) / M1
Substituting the given values:
V1 = (0.0495 M * 175.0 mL) / 0.200 M
V1 ≈ 43.3125 mL
This means you need 43.3125 mL of the 0.200 M KBr solution to achieve a concentration of 0.0495 M. However, since you have the concentrated solution at 0.200 M, you can dilute it further. The volume you take from the concentrated solution (V1) and the volume of water you add (V_water) should sum up to the final volume of 175.0 mL:
V1 + V_water = 175.0 mL
Rearranging to find V_water:
V_water = 175.0 mL - V1
V_water ≈ 175.0 mL - 43.3125 mL
V_water ≈ 131.6875 mL
So, you would take 43.3125 mL of the 0.200 M KBr solution and dilute it with approximately 131.6875 mL of water to get a total volume of 175.0 mL, resulting in a final concentration of 0.0495 M.
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