A titration was performed on 50.0 ml of .250 M NaOH. After the addition of 71.4 ml of HCl,the phenolphthalein indicator changed from pink to colorless. What was the concentration of the HCl? im not sure how to figure this one out but here goes
200*.250*1000=50000
1000*121.4=121400
50000/121400=.412?
that was my best shot
I don't know what you did and since you didn't explain the steps you took OR use any units, I'm clueless.
Here is how you do it.
mols NaOH = mols HCl
M x mL = M x mL
0.250 M x 50 mL = M x 71.4 mL
Solve for M HCl.
Im sorry, that was very stupid of me for not explaining anything. Is this right?
0.250 M x 50 mL= 12.5ml
12.5 M x 71.4ml= 893
no if I solve for m I would have to
0.250 M x 50 mL = M x 71.4 mL
.250M*50=12.5ml
12.5ml=M*71.4
12.5ml=71.4M
12.5/71.4=.175ml
right number, wrong unit.
You are solving for M so M = 0.175M
To solve for the concentration of HCl, you can use the concept of stoichiometry. In a balanced chemical equation, the ratio of moles of reactants and products is constant.
First, calculate the moles of NaOH used in the titration. This can be determined using the formula:
moles of NaOH = Molarity x Volume (in liters)
Given that the volume of NaOH used is 50.0 mL (or 0.050 L) and the molarity of NaOH is 0.250 M:
moles of NaOH = 0.250 M x 0.050 L = 0.0125 moles
Since the reaction is balanced, the moles of HCl consumed will be equal to the moles of NaOH.
Now, using the volume of HCl added (71.4 mL or 0.0714 L), you can calculate the concentration of HCl:
concentration of HCl = moles of HCl / volume of HCl (in liters)
concentration of HCl = 0.0125 moles / 0.0714 L = 0.175 M
So, the concentration of HCl is 0.175 M.