If a student used 11.54mL of their NaOH solution to neutralize 10.00mL of a 0.445M KHP solution, then what is the concentration of the student's NaOH solution (in Molarity)?
NaOH + KHP ==> NaKP + H2O
moles KHP = M x L = ??
moles NaOH = same (from the equation)
M NaOH = moles NaOH/L NaOH
0.01L KHP * 0.445M KHP = 0.00445 molKHP
KHP and NaOH are in 1 to 1 ratio so, moles NaOH = 0.00445
so,
0.00445mol NaOH/ 0.01154L NaOH = 0.386M NaOH
To determine the concentration of a solution, we can use the equation:
Molarity (M) = moles of solute / volume of solution (in liters)
In this case, we need to find the concentration (M) of the NaOH solution used by the student.
To start, we need to find the moles of KHP (potassium hydrogen phthalate) neutralized by the NaOH solution.
The balanced equation for the reaction is:
NaOH + KHP -> NaKP + H2O
From the equation, we can see that the mole ratio between NaOH and KHP is 1:1.
To find the moles of KHP, we need to use its concentration and volume.
Moles of KHP = concentration (M) x volume (L)
Given that the volume of KHP solution is 10.00 mL and its concentration is 0.445 M, we can find the moles of KHP as follows:
Moles of KHP = 0.445 M x 0.01000 L = 0.00445 mol
Since the mole ratio between NaOH and KHP is 1:1, the moles of NaOH used by the student will also be 0.00445 mol.
Next, we can use the volume of NaOH solution used (11.54 mL) to find the concentration of NaOH:
Concentration of NaOH solution = moles of NaOH / volume of NaOH solution (in liters)
Converting the volume from milliliters to liters:
Volume of NaOH solution = 11.54 mL / 1000 mL/L = 0.01154 L
Now, we can calculate the concentration of the NaOH solution:
Concentration of NaOH solution = 0.00445 mol / 0.01154 L ≈ 0.385 M
Therefore, the concentration of the student's NaOH solution is approximately 0.385 M.