November 23, 2024, 10:35:17 PM
Forum Rules: Read This Before Posting


« previous next »
Pages: [1]   Go Down

Topic: buffer  (Read 6426 times)

0 Members and 2 Guests are viewing this topic.

tulth

  • Guest
buffer
« on: July 16, 2005, 02:33:22 AM »
I used 50 ml of 0.2 M Na2HPO4 and 4.1 ml of 0.1 M NaOH  and make volume to 100 ml. (I copy from a book for preparing phosphate buffer pH 11)
What is  the concentration of this buffer?  
How to calculated pH of this buffer? (Please show the ion dissociation)
 and If you sent the answer to me at **** it very good. Thank you very much for your kindness
« Last Edit: July 16, 2005, 04:14:05 AM by Borek »
Logged

Offline Borek

  • Mr. pH
  • Administrator
  • Deity Member
  • *
  • Posts: 27858
  • Mole Snacks: +1813/-412
  • Gender: Male
  • I am known to be occasionally wrong.
    • Chembuddy
Re:buffer
« Reply #1 on: July 16, 2005, 04:13:22 AM »
You are violating forum rules.

At least show us that you tried to do the calculations by yourself.

And never ask on the forum fro the answers to be sent elsewhere. Asked on forum, answered on forum.
Logged
ChemBuddy chemical calculators - stoichiometry, pH, concentration, buffer preparation, titrations.info

Offline Donaldson Tan

  • Editor, New Asia Republic
  • Retired Staff
  • Sr. Member
  • *
  • Posts: 3177
  • Mole Snacks: +261/-13
  • Gender: Male
    • New Asia Republic
Re:buffer
« Reply #2 on: July 16, 2005, 07:16:56 PM »
for starters, use the related Ka expressions and solve them simultaneously
Logged
"Say you're in a [chemical] plant and there's a snake on the floor. What are you going to do? Call a consultant? Get a meeting together to talk about which color is the snake? Employees should do one thing: walk over there and you step on the friggin� snake." - Jean-Pierre Garnier, CEO of Glaxosmithkline, June 2006
Pages: [1]   Go Up
« previous next »
Sponsored Links