chemistry

posted by .

Purpose: The purpose of this experiment is to determine the Ksp for calcium hydroxide.

Materials are:
*50.0 mL of 0.10 M HCl(aq)
*bromophenol blue indicator
*50.0 mLsaturated calcium hydroxide
*50.0 mL buret
*125 mL Erlynmyer Flask
*50.0 mL of distilled water
*10.0 mL pipet with pump
*waste beaker

The procedure for the lab is:
1.Fill the buret with the acid solution.
2.Pipet 10.0 mL of calcium hydroxide into the flask.
3.Add approximately 10.0 mL of water to the flask.
4.Add 4 drops of bromophenol blue to the flask.
5.Titrate the base to an endpoint and record the volume of acid added.
6.Dispose of the flask contents into a waste beaker.
7.Repeat steps 2-6 four more times.

The following is what I am having trouble with.

Present your data in a table.Use the following table as a guide:
Trial 1 Trial 2 Trial 3
*Initial volume
of HCL(mL)

*Final volume
of HCL (mL)

*Volume of
HCL added (mL)

I am having difficulty regarding the trial 1 column. What is my initial volume of HCL(mL) supposed to be?

  • chemistry -

    Could it be the reading on the burette? As 50mL which was called for?

  • chemistry -

    Here are my results:


    *Initial volume
    of HCL(mL)
    Trial 1- 0.0
    Trial 2- 2.51
    Trial 3- 4.95
    Trial 4- 7.4
    Trial 5- 9.9

    *Final volume
    of HCL (mL)
    Trial 1- 2.51
    Trial 2- 4.95
    Trial 3- 7.4
    Trial 4- 9.9
    Trial 5- 12.39

    *Volume of
    HCL added (mL)
    Trial 1- 2.51
    Trial 2- 2.44
    Trial 3- 2.45
    Trial 4- 2.50
    Trial 5- 2.49

    But now the next question is asking me to calculate the solubility product for calcium hydroxide. How do I do this? I would be very thankful for your help

  • chemistry -

    I think the instructions are not too good, if I interpret them correctly. I THINK the initial volume is the initial READING OF THE BURET. Then I think the final volume is the FINAL READING OF THE BURET. Subtract the initial reading from the final reading to obtain the volume of HCl added (in mL).
    For example:
    The initial reading of the buret may have been something like 0.72 mL. Then the titration is performed and the final reading at the end point of the indicator is 4.52 mL. The volume of HCl used for the titration then is 4.52 - 0.72 = ?? Just as a side note, when I do a titration, I ALWAYS make the initial reading 0.00 although teachers have told me through the years that I'm wasting time to do that. But it has some advantages, at least for me.
    1. I ALWAYS know what the initial reading was since it never changes.
    2. I don't need to make an entry into the notebook of the initial volume.
    3. I need not make a big deal out of subtracting (a possible source of a math error) because the final reading IS the volume of titrant used.
    I always advise students to follow the instructions provided by their prof. Personally, I prefer the way I do it.

  • chemistry -

    Ca(OH)2 ==> Ca^+2 + 2OH^-
    Ksp = (Ca+2)(OH^-)^2 = ??
    You know volume of HCl. You know the molarity of the HCl.
    mols HCl = L x M = ??
    The equation for the titration is
    Ca(OH)2 + 2HCl ==> CaCl2 + 2H2O

    So take 1/2 mols HCl to give you mol OH^-.
    mols OH^-/volume of the sample = (OH^-) in mols/L. Plug that into Ksp expression. 1/2 of the (OH^-) is Ca^+2.

  • chemistry -

    To get volume of HCL, would I do this?

    2.51+2.44+2.45+2.50+2.49 / 5

    = 2.48

    ?

  • chemistry -

    No, although that would give you an average and in the end you will want to calculate an average anyway. However, I think you want to use each one as a separate experiment because you will want to see how good the precision is. That way you will have five experimental determinations of Ksp. Use 2.51 mL for the first one.

  • chemistry -

    I see, so for the first trial my volume would be 2.51 ml

    For the second trial, the volume would be 2.44 ml

    For the third trial, the volume will be
    2.45 mL

    For the fourth trial, the volume will be 2.50 mL


    For the fifth trial, the volume will be 2.49 mL

    ?

  • chemistry -

    right.

  • chemistry -

    Im going to try to solve for the first trial please let me know if I am correct. I will send it within the next 10 minutes

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. chemistry

    Hi Cna someone please tell me what I must out into the Trial 1 column?
  2. chemistry

    Let me repost the important information only: Purpose: The purpose of this experiment is to determine the Ksp for calcium hydroxide. Materials are: *50.0 mL of 0.10 M HCl(aq) *bromophenol blue indicator *50.0 mLsaturated calcium hydroxide …
  3. Chemistry

    a solution saturated in calcium hydroxide(limewater) has a pH of 12.35. What is Ksp for calcium hydroxide?
  4. chemistry

    Determine the number of moles of calcium per mole of calcium hydroxide. My answer is: Because there is only one calcium ion per mole of calcium hydroxide, the mole of calcium ion is equal to the mole of calcium hydroxide. Is this a …
  5. chemistry

    A 0.500 L solution of 7.50 M hydrochloric acid is used to neutralize a 250.0 g sample of calcium hydroxide. Calcium chloride – a chemical used to control highway dust, strengthen concrete mixes, and add flavor to foods – is produced …
  6. Chemistry - Ksp

    i did an experiment where we titrated HCl on calcium hydroxide, and now i am confused with the calculations, i do not know if i am correct, so please help me out... Trial One volume of HCl used - 11.20mL concentration of HCl - 0.04mol/L …
  7. Chemistry

    1.Write a mathematical equation that can be used to calculate the concentration of the HCl solution after the standardization procedure (Titration #1). 2. Using LeChatelier’s principle, predict whether [OH-] in the calcium hydroxide/0.050 …
  8. Chemistry

    Calcium hydroxide has Ksp = 5.5 x 10-5 at 25 oC and a molar mass of 74.10 g/mol. How many grams of calcium hydroxide are needed to create 365 mL of a saturated solution of calcium hydroxide at 25 oC?
  9. Chemistry

    We did a titration of calcium hydroxide lab in chemistry, once with and once with edta, we have to calculate the solubility for both, and the ksp, for the hcl I did (concentration)*(Volume of hcl used) then that answer divided by two …
  10. Chemistry

    10. Use the accepted Ksp value of Calcium hydroxide to calculate the following: a. What is the most calcium hydroxide that can be dissolved in 1.0 Liters of de-ionized water?

More Similar Questions