What is the concentration of a solution of HCL in which a 10.0 mL sample of acid required 50.0 mL of 0.150 M NaOH for neutralization?
HCL stands for "a" and NaOH stands for "b"
0.050Lb*0.150molb/1Lb*0.010La/1molb*1mola/1La = o.oo33moles of the acid (HCL)
To find the concentration of the HCl solution, we can use the relationship between moles, volume, and concentration.
We know that the moles of NaOH used for neutralization is equal to the moles of HCl present in the 10.0 mL sample. The number of moles can be calculated using the equation:
moles = concentration × volume
Let's calculate the moles of NaOH used:
moles of NaOH = concentration of NaOH × volume of NaOH
= 0.150 M × 50.0 mL
= 7.50 mmol (millimoles)
Since HCl and NaOH react in a 1:1 ratio, the number of moles of HCl in the 10.0 mL sample is also 7.50 mmol.
Next, we need to calculate the concentration of the HCl solution. The concentration is given in moles per liter (M), so we need to convert the volume to liters:
volume of HCl = 10.0 mL = 10.0 mL × (1 L/1000 mL) = 0.0100 L
Finally, we can calculate the concentration of the HCl solution:
concentration of HCl = moles of HCl / volume of HCl
= 7.50 mmol / 0.0100 L
= 750 mmol/L
Therefore, the concentration of the HCl solution is 750 mmol/L (or 0.750 M).