Calculate the volume in mL of a 1.420M NaOH solution to tirarte the following solutions
25.00mL of a 2.430M HCl solution
Well, well, well, looks like we have a chemistry problem here. Alrighty then, let's get to it!
To calculate the volume of a solution needed to titrate another solution, we need to use the equation:
M1V1 = M2V2
Where:
M1 = molarity of solution 1
V1 = volume of solution 1
M2 = molarity of solution 2
V2 = volume of solution 2
So in this case, we're trying to find the volume of the NaOH solution (V1) that will titrate with 25.00 mL of the HCl solution (V2). The molarity of NaOH (solution 1) is 1.420M and the molarity of HCl (solution 2) is 2.430M.
Using the equation, we have:
(1.420M)(V1) = (2.430M)(25.00 mL)
Now, let's solve for V1:
V1 = (2.430M)(25.00 mL) / 1.420M
V1 ≈ 42.57 mL
So, the volume of the 1.420M NaOH solution needed to titrate 25.00 mL of the 2.430M HCl solution is approximately 42.57 mL. Voilà!
To calculate the volume of a 1.420M NaOH solution needed to titrate 25.00mL of a 2.430M HCl solution, you can use the equation:
Molarity of Acid x Volume of Acid = Molarity of Base x Volume of Base
Let's substitute the given values into the equation:
(2.430M) x (25.00mL) = (1.420M) x Volume of NaOH
Solving for the Volume of NaOH:
(2.430M x 25.00mL) / 1.420M = Volume of NaOH
Volume of NaOH = 42.842mL
Therefore, you would need 42.842mL of the 1.420M NaOH solution to titrate the 25.00mL of 2.430M HCl solution.
To calculate the volume of a solution required to titrate another solution, we need to use the concept of stoichiometry and the balanced chemical equation between the two reactants.
The balanced chemical equation for the reaction between NaOH and HCl is:
NaOH + HCl -> NaCl + H2O
From the equation, we can see that the ratio between NaOH and HCl is 1:1. This means that 1 mole of NaOH reacts with 1 mole of HCl.
First, let's calculate the number of moles of HCl in the 25.00 mL of 2.430 M HCl solution using the formula:
moles = concentration (M) * volume (L)
Converting the volume from mL to L:
volume (L) = 25.00 mL * (1 L / 1000 mL) = 0.0250 L
Now, we can calculate the number of moles of HCl:
moles HCl = 2.430 M * 0.0250 L = 0.0608 moles
Since the reaction is 1:1, we need an equal number of moles of NaOH to react with the HCl, which is 0.0608 moles.
Next, we need to calculate the volume of a 1.420 M NaOH solution required to supply 0.0608 moles of NaOH.
Using the same formula as before, but rearranged to solve for volume:
volume (L) = moles / concentration (M)
volume NaOH (L) = 0.0608 moles / 1.420 M = 0.0429 L
Finally, we can convert the volume from liters to milliliters:
volume NaOH (mL) = 0.0429 L * (1000 mL / 1 L) = 42.9 mL
Therefore, you would need approximately 42.9 mL of a 1.420 M NaOH solution to titrate 25.00 mL of a 2.430 M HCl solution.
25mL * 2.43M/L = 0.06075 moles
The equation HCl + NaOH = NaCl + H2O
tells you you will need that many moles of NaOH
x mL * 1.42 moles/1000mL = 0.06075 moles