chemistry

My problem is calculate the molarity of HCl and NaOH.

(molarity of acid)x(volume of acid)=(molarity of base)+(volume of added base)

HCl=acid NaOH=base

HCl volume = 25mL=0.025L
NaOH=67.05mL=0.06705

molarity = moles of solute
Liters of a solution
M=0.015000 moles of NaOH
0.06705L
M1V1=M2V2
M1V1=M2V2
V1
M1=M2V2
V1
M1=0.223713647 M of NaOH * 0.06705L
0.025L
M1=0.600000001M of HCl

0.600000001 M of HCl* 0.025L =
0.223713647 M of NaOH * 0.06705L

Am I even close?

  1. 👍
  2. 👎
  3. 👁
  1. You would have done much better to type in the problem before showing your solution. It's good to show your work, however, you have no data (at least none identifiable). For example, where did the 0.01500 mols come from? Finally, you have made a typo in the second sentence (the formula). You show a + sign and it should be a x sign. If you will post the problem someone will go through and check it for you. Thanks for using Jiskha.

    1. 👍
    2. 👎
  2. Calculate the molarity of the HCl from the volumes of acid and base and the molarity of the NaOH. Use the following equation:

    (molarity of acid)x(volume of acid)=(molarity of base)x(volume of added base)

    equivalance point=number of mL of base to an acid

    1mL=0.001L

    HCl volume=25 mL=0.025L
    NaOH=67.05mL=0.06705L

    Molarity=Moles of solute
    ---------------
    Liters of a solution

    M=0.015000 moles of NaOH
    ----------------------
    0.06705L

    M=0.223713647M of NaOH

    M1V1=M2V2

    M1=M2V2
    ----
    V1

    M1=0.223713647M of NaOH * 0.06705L
    ---------
    0.025L

    M1= 0.600000001 M of HCl

    0.600000001 M of HCl * 0.025L=
    0.223713647 M of NaOH * 0.06705L

    1. 👍
    2. 👎

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

    commercially available concentrated Hydrochloric acid is 37.0% w/w Hcl.its density is 1.18g/ml.using this information calculate (a)the molarity of concentrated Hcl,and (b)the mass and volume (in ml)of solution containing 0.315 mol

  3. Chemistry

    A BS Medical Technology student was asked to determine the molecular weight of a diprotic acid using acid-base titration. This student performed four trials. Firstly, the student used potassium hydrogen phthalate (KHP, 204.22

  4. chemistry help asap

    Please check these thanks. 1. In a titration, 33.21 mL 0.3020M rubidium hydroxide solution is required to exactly neutralize 20.00 mL hydrofluroic acid solution. What is the molarity of the hydrofluroic acid solution? Answer:

  1. Chemistry

    1. You have been given a sample of unknown molarity. Calculate the molarity of a solution which has been prepared by dissolving 8.75 moles of sodium chloride in enough water to produce a solution of 6.22l. 2. You have a sample

  2. CHECK MY CHEMISTRY WORK PLEASE ASAP

    1. You have been given a sample of unknown molarity. Calculate the molarity of a solution which has been prepared by dissolving 8.75 moles of sodium chloride in enough water to produce a solution of 6.22l. 2. You have a sample

  3. Chemistry

    7.0 ml of 6.0 M NaOH are diluted with water to a volume of 400 ml. You are asked to find the molarity of the resulting solution. The total number of moles of NaOH is not changed on dilution. Calulate the molarity. Work:

  4. Chemistry 12

    Hi, I did the acid-base titration lab with HCl and 0.5M NaOH. I need to calculate the moles of NaOH from molarity of NaOH and the average volume used. My English isn't good but is it asking me to find the moles of NaOH using the

  1. Chemistry

    1.) Watch the animation, and observe the titration process using a standard 0.100 M sodium hydroxide solution to titrate 50.0 mL of a 0.100 M hydrochloric acid solution. Identify which of the following statements regarding

  2. CHEMISTRY

    You have been given a sample of unknown molarity. Calculate the molarity of a solution which has been prepared by dissolving 8.75 moles of sodium chloride in enough water to produce a solution of 6.22l. 2. You have a sample which

  3. Chemistry

    How do you calculate the volume of titrant needed to reach the endpoint of a reaction when you are given the mls and molarity of a strong base and only the molarity of a weak acid?

  4. chemistry

    commercially available concentrated hydrochloric acid is 37.0% w/w HCl. Its density is 1.18 g/mL. Using this information calculate (a) the molarity of concentrated HCl, and (b) the mass and volume (in mL) of solution containing

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