March 03, 2024, 04:41:20 AM
Forum Rules: Read This Before Posting


Topic: Aqueous solutions of Silver Nitrate and Copper II Chloride  (Read 6415 times)

0 Members and 1 Guest are viewing this topic.

Offline tdean

  • Very New Member
  • *
  • Posts: 1
  • Mole Snacks: +0/-0
Aqueous solutions of Silver Nitrate and Copper II Chloride
« on: March 06, 2010, 04:30:12 PM »
I have .5 mole solution of Ag(NO3) but its in limited supply. I only need a .1 m solution. Is it possible to dilute the .5 mole solution to make a .1 mole? I'd say I have about 100 mL of .5 mole. Is it as simple as adding 400 mL of water to 100 mL of .5 mole solution?

0.1 mole => 16.988 g
16.988 g + enough water to reach the volume of 1 L

0.5 mole => 84.935 g
84.935 g + enough water to reach the volume of 1 L

Also, I'm looking to make an aqueous solution of copper II nitrate to observe single replacement reactions of zinc and of iron.
What concentration of copper II nitrate would work best? What ratio of copper II nitrate crystals to water do I use to make that soltution?
Will the reactions work with Zinc dust rather than zinc wire? and iron fillings rather than iron wire?

Offline Borek

  • Mr. pH
  • Administrator
  • Deity Member
  • *
  • Posts: 27604
  • Mole Snacks: +1797/-410
  • Gender: Male
  • I am known to be occasionally wrong.
    • Chembuddy
ChemBuddy chemical calculators - stoichiometry, pH, concentration, buffer preparation, titrations.info

Sponsored Links