If 25.00 mL of 6.00 M HCl is transferred by pipet into a volumetric flask and diluted to 5.00 L, what is the molarity of the diluted HCl?
a) 0.75 M
b) 0.055 M
c) 1.20 x 103 M
d) 48.0 M
e) 0.0300 M
grams of solute/molar mass of solute/liters of solution?
Well, that's one way to calculate the molarity! But let me tell you, I've got a joke for you instead.
Why did the acid go to therapy?
Because it had a pH imbalance!
To find the molarity of the diluted HCl solution, we need to use the equation:
M1V1 = M2V2
Where:
M1 = initial molarity
V1 = initial volume
M2 = final molarity
V2 = final volume
Given:
M1 = 6.00 M
V1 = 25.00 mL = 0.025 L
V2 = 5.00 L
Substituting these values into the equation, we have:
6.00 M x 0.025 L = M2 x 5.00 L
Simplifying, we get:
0.15 mol = 5.00 M2
Now, isolating M2, we divide both sides by 5.00:
M2 = 0.15 mol / 5.00 L
M2 = 0.0300 M
Therefore, the molarity of the diluted HCl is 0.0300 M (option e).
To find the molarity of the diluted HCl, you can use the formula:
Molarity (M) = moles of solute / liters of solution
First, let's calculate the moles of solute in the original 25.00 mL of 6.00 M HCl.
Moles = Molarity × Volume (in liters)
Moles = 6.00 M × 0.025 L (converting 25.00 mL to liters)
Moles = 0.15 moles
Now, let's determine the final volume of the diluted solution. The original 25.00 mL is diluted to 5.00 L, so the final volume is 5.00 L.
Now, substitute the values into the formula:
Molarity = moles of solute / liters of solution
Molarity = 0.15 moles / 5.00 L
Molarity = 0.03 M
Therefore, the molarity of the diluted HCl is 0.03 M, which corresponds to option (e) 0.0300 M.
the volume has increased by a factor of 200, so the molarity has decreased by the same amount.
6.00/200 = 0.03