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
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 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

right number, wrong unit.
You are solving for M so M = 0.175M

  1. 👍
  2. 👎
  3. 👁

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    The following data were collected at the endpoint of a titration performed to find the molarity of an HCl solution: Volume of acid (HCl) used = 14.4 mL; Volume of base (NaOH) used = 22.4 mL; Molarity of standard base (NaOH) =

  2. Chemistry

    A weak acid with a Ka of 1.8 × 10–5 is titrated with a strong base. During the titration,12.5 mL of 0.10 M NaOH is added to 50.0 mL of 0.100 M acetic acid. What is the pH after the addition of the NaOH? A. 7.22 B. 5.13 C. 4.26

  3. Chemistry

    A titration setup was used to determine the unknown molar concentration of a solution of NaOH. A .025 M HCl solution was used as the titration standard. The following data were collected. Trial 1 Trial 2 Trial 3 Initial NaOH Buret

  4. chemistry

    Find the pH during the titration of a 20.00mL of 0.1000 M butanoic acid, CH3CH2CH2COOH (Ka=1.54 x10^-5), with the addition of 10 mL of 0.1000 M NaOH solution??

  1. Chemistry

    1. Calculate the pH for each of the following cases in the titration of 25.0 mL of 0.240 M pyridine, C5H5N(aq) with 0.240 M HBr(aq): (a) before addition of any HBr (b) after addition of 12.5 mL of HBr (c) after addition of 22.0 mL

  2. Chemistry

    Why is it important to keep the NaOH solution (being used during titration) stoppered at all times when it is not in use? And why is it all right to use a wet flask for a titration experiment?

  3. Chemistry

    HC2H3O2 + NaOH --> NaC2H3O2 + H2O? a. when the titration is only half over, what species are present in the reaction flask b. what can be said about the pH at this point when the titration is half over? c. what is the pH at the

  4. Chemistry

    If you had added 50 mL of distilled water to one the vinegar sample instead of 30 mL, would the titration have required more NaOH, less NaOH or the same amount of NaOH? Why?

  1. Chemistry

    Calculate the pH for each of the following points in the titration of 50.0 mL of a 2.7 M H3PO3(aq) with 2.7 M KOH(aq). pKa1 = 1.3 and pKa2 = 6.7 a) before addition of any KOH b) after addition of 25.0 mL of KOH c) after addition

  2. Chemistry

    How to solve titration problem for HC2H3O2 + NaOH= NaC2H3O2 + H2O The M of NaOH= 0.427 The volume of NaOH= 17.30mL 10.00mL of acid The second titration calculation is: The M of NaOH= 0.427 The volume of NaOH=34.60mL 20.00mL of

  3. College Chemistry

    The Question Is: "A student weighs 0.347 g of KHP on a laboratory balance. The KHP was titrated with NaOH and the concentration of the NaOH determined to be 0.110 M. For the second titration, the student correctly diluted 6 M HCl

  4. Chemistry

    Use the dilution relationship (Mi x Vi = Mf x Vf) to calculate the volume of 0.500 M NaOH needed to prepare 500 mL of .250 M NaOH. This is my work ? L Solution = 500mL x (1L/1000mL) = .500L ? mol NaOH = .500 L Solution x (0.250 M

You can view more similar questions or ask a new question.