March 29, 2024, 11:09:07 AM
Forum Rules: Read This Before Posting


Topic: titration  (Read 7375 times)

0 Members and 1 Guest are viewing this topic.

Offline dirknathan

  • Regular Member
  • ***
  • Posts: 37
  • Mole Snacks: +1/-1
titration
« on: September 20, 2012, 04:50:50 PM »
How many milliliters of 8.34×10−2 M Ba(OH)2 are required to titrate 54.40 mL of 5.24×10−2 M HNO3?

I can't figure out where the M of Ba(OH)3 comes into play?

Offline fledarmus

  • Chemist
  • Sr. Member
  • *
  • Posts: 1675
  • Mole Snacks: +203/-28
Re: titration
« Reply #1 on: September 20, 2012, 05:17:45 PM »
What reaction is occurring when you do the titration?

Offline dirknathan

  • Regular Member
  • ***
  • Posts: 37
  • Mole Snacks: +1/-1
Re: titration
« Reply #2 on: September 20, 2012, 05:42:55 PM »
I assume they are reacting with each other.  This is the only information I've been given.

Offline Arkcon

  • Retired Staff
  • Sr. Member
  • *
  • Posts: 7367
  • Mole Snacks: +533/-147
Re: titration
« Reply #3 on: September 20, 2012, 05:47:33 PM »
To begin to figure this out properly, you will need to determine the balanced chemical reaction these reagents undergo.  We'd like to see it from you, and then we'll try to give you more hints to relate the various molarities to each other.
Hey, I'm not judging.  I just like to shoot straight.  I'm a man of science.

Offline Borek

  • Mr. pH
  • Administrator
  • Deity Member
  • *
  • Posts: 27635
  • Mole Snacks: +1799/-410
  • Gender: Male
  • I am known to be occasionally wrong.
    • Chembuddy
Re: titration
« Reply #4 on: September 20, 2012, 05:49:56 PM »
I assume they are reacting with each other.  This is the only information I've been given.

I suppose you are expected to know what kind of reaction to expect when you mix strong acid and strong base.
ChemBuddy chemical calculators - stoichiometry, pH, concentration, buffer preparation, titrations.info

Offline dirknathan

  • Regular Member
  • ***
  • Posts: 37
  • Mole Snacks: +1/-1
Re: titration
« Reply #5 on: September 20, 2012, 06:39:55 PM »
How many milliliters of 8.34×10−2 M Ba(OH)2 are required to titrate 54.40 mL of 5.24×10−2 M HNO3?

Ba(OH)2 + HNO3  :rarrow: BaNO3+ + H2O + OH-

Does that look correct?

Offline Arkcon

  • Retired Staff
  • Sr. Member
  • *
  • Posts: 7367
  • Mole Snacks: +533/-147
Re: titration
« Reply #6 on: September 20, 2012, 06:51:41 PM »
NO, that's not correct.  An acid and base should neutralize each other completely.  And no, we can't create negative ions singly.  Why does barium no longer need its charge balanced in the product?
Hey, I'm not judging.  I just like to shoot straight.  I'm a man of science.

Offline dirknathan

  • Regular Member
  • ***
  • Posts: 37
  • Mole Snacks: +1/-1
Re: titration
« Reply #7 on: September 20, 2012, 07:14:07 PM »
Every strong acid,strong base reaction has the same net ionic equation correct?

Why won't M1V1=M2V2 work for this problem?

I assume the ratio of moles isn't one to one (or is it), but if the net ionic equation is the same...

Offline dirknathan

  • Regular Member
  • ***
  • Posts: 37
  • Mole Snacks: +1/-1
Re: titration
« Reply #8 on: September 20, 2012, 07:14:41 PM »
This (OH)2 is rocking my world.

Offline dirknathan

  • Regular Member
  • ***
  • Posts: 37
  • Mole Snacks: +1/-1
Re: titration
« Reply #9 on: September 20, 2012, 07:25:43 PM »
2HNO3 + Ba(OH)2 --> Ba(NO3)2 + 2 H2O

Offline Arkcon

  • Retired Staff
  • Sr. Member
  • *
  • Posts: 7367
  • Mole Snacks: +533/-147
Re: titration
« Reply #10 on: September 20, 2012, 07:25:55 PM »
Every strong acid,strong base reaction has the same net ionic equation correct?

I suppose, but that won't help you here, since you will have to use the molarity of the the actual reagents.

Quote
Why won't M1V1=M2V2 work for this problem?

No.  I suppose you could test that by filling all the values in your formula, if you're missing too many, then you'll know it won't work.

Quote
I assume the ratio of moles isn't one to one (or is it), but if the net ionic equation is the same...
You'll know when you balance the equation

2HNO3 + Ba(OH)2 --> Ba(NO3)2 + 2 H2O

Good.  Now, you have a balanced chemical equation.  What are the units understood in a chemical equation?   There are some units understood to be there, 'tho this is somtimes hard for a new student to see.
Hey, I'm not judging.  I just like to shoot straight.  I'm a man of science.

Offline dirknathan

  • Regular Member
  • ***
  • Posts: 37
  • Mole Snacks: +1/-1
Re: titration
« Reply #11 on: September 20, 2012, 07:32:25 PM »
I see coefficients and charges.  Not sure what your are asking for?

Offline Arkcon

  • Retired Staff
  • Sr. Member
  • *
  • Posts: 7367
  • Mole Snacks: +533/-147
Re: titration
« Reply #12 on: September 20, 2012, 07:43:27 PM »
Yes, the coefficient '2' before the nitric acid, that means two ... what?
Hey, I'm not judging.  I just like to shoot straight.  I'm a man of science.

Offline dirknathan

  • Regular Member
  • ***
  • Posts: 37
  • Mole Snacks: +1/-1
Re: titration
« Reply #13 on: September 20, 2012, 07:46:08 PM »
atoms.  I did notice that, I've been working with the titration on a piece of paper.  Back to my orignal problem, how to use Ba(OH)2's molarity.

Offline dirknathan

  • Regular Member
  • ***
  • Posts: 37
  • Mole Snacks: +1/-1
Re: titration
« Reply #14 on: September 20, 2012, 07:49:58 PM »
I actually found a sample problem just like this, only problem, mole ratio is one to one.  they used the formula I previously stated.  This is a different story.

Sponsored Links