A student titrates a 10.00mL sample of an HCl solution, using 0.359 M solution of NaOH. She finds that 24.75mL of sodium hydroxi
de solution are needed for the titration. Calculate the molarity of the HCl solution. (Can someone explain how to solve this question I don't know how to set up the question. Step by step please)
HCl and NaOH react in a 1:1 ratio, meaning that 1 H+ from HCl will react with 1 OH- from NaOH. Knowing this, and that molarity is mol/liter, all we need to do is use what we have available. First we must find the mols of HCl in our solution, so we set up the following equation in the following steps: 1. 24.75mL x (0.359mol NaOH / 1000mL) = 8.885 x 10^-3mol NaOH This is done in order to find the mols of NaOH to convert to mols of HCl. 2. 8.885x10^-3mol NaOH x (1 mol HCl/1mol NaOH) = 8.885 x 10^-3mol HCl Here we just used the mols of NaOH we found to convert to mols of HCl using the 1:1 ratio described earlier.
From the mols of HCl all we have to do is divide by the amount of liters in the solution. Since we started with 10mL HCl and added 24.75mL NaOH, the total volume is 34.75mL = 0.03475L. So: 8.885 x 10^-3mol HCl/0.03475L = 2.557 x 10^-1M HCl However, this is the molarity of the HCl and NaOH solution, not the original HCl solution. Using the dilution equation M1V1=M2V2, we can solve for the original molarity. M1 = the molarity of our HCl in the titrated mixture (2.557 x 10^-1M HCl) V1 = the total volume that our mixture has (34.75mL = 0.03475L) M2 = what we're trying to find V2 = the amount of the original HCl that we had (10mL = 0.010L) Simply solving for M2 gives us: M2 = (M1V1) / V2 or: M2=((2.557 x 10^-1) x 0.03475L) / 0.010L = 8.89 x 10^-1M HCl. That is your answer.
