CHEMISTRY

posted by .

Consider an aqueous solution prepared from 250.0 mL of water and 1.27 g of potassium bromide. Express the amount of potassium bromide in this solution in terms of
(a) mass percent
(b) mole fraction
(c) molarity
assume the density of the solution is equal to that of water, 1.00 g mL-1.........help!

  • CHEMISTRY -

    Surely you don't want me to work all three. Surely you know SOMETHING about SOME of them. Just remember the definitions:
    1. mass percent. grams solute/100 g solution.
    2. mole fraction. moles solute/total mules.
    3. molarity = moles/L of solution.
    Apply those three definitions and you will have your answer(s).
    Post your work if you get stuck.

  • CHEMISTRY -

    I surely do, and don't call me Shirley! LOL yessss i'm sorry I don't know much about chemistry that's why i'm here!!

    1. Mass percent= grams solute/100solution 1.27g/250.0mL = 5.08x10^-03 is my answer but the correct one is 0.505%

    2. Mole fraction= moles solute/total moles ?/119.002

    3. Molarity 1.27g/119.002= 0.0107moles
    than 0.0107/0.25L = 0.048 that's my answer but the correct one is 4.25x10^-2

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chemistry

    Need Help On This Question.! Potassium chloride reacts with bromine forming potassium bromide plus chlorine. If 500g of potassium bromide are produced, how many grams of potassium chloride reacted?
  2. chemistry

    Determine the number of bromide ions in solution when 4.23 g of magnesium bromide and 1.21 g of potassium bromide are dissolved in 120mL of water. Please explain not sure how to even start this problem, thanks!
  3. chemisty

    Posted by STACY on Monday, December 13, 2010 at 7:56pm. Consider an aqueous solution prepared from 250.0 mL of water and 1.27 g of potassium bromide. Express the amount of potassium bromide in this solution in terms of (a) mass percent …
  4. chem

    The mole fraction of an aqueous solution of potassium perchlorate is 0.125. Assuming that the density of this solution is 1.20g mL-1, calculate the following: (A) the mass percent of potassium perchlorate in the solution. (B) the molarity …
  5. chemistry needs another look plz

    Posted by Lori on Tuesday, December 14, 2010 at 5:38pm. The mole fraction of an aqueous solution of potassium perchlorate is 0.125. Assuming that the density of this solution is 1.20g mL-1, calculate the following: (A) the mass percent …
  6. Chemistry(Please Check)

    You dissolve 6.55 g of potassium nitrate in enough water to make a 250. ML solution. 1.What is the molarity of this solution?
  7. chemistry

    If 50.0 mL of 0.150 M magnesium bromide is combined with 200 mL of 0.110 M sodium bromide what is the molarity of the bromide ion in the resulting solution?
  8. Chemistry

    Suppose 26.0g of sodium bromide is dissolved in 150mL of a 0.60M aqueous solution of silver nitrate. Calculate the final molarity of bromide anion in the solution. You can assume the volume of the solution doesn't change when the sodium …
  9. Chemistry2

    12.) Chlorine reacts with potassium bromide to produce potassium chloride and bromine. a.) write a chemical equation, using words, to represent the above chemical reaction. Answer: Chlorine + potassium bromide ==> potassium chloride …
  10. chemistry

    When aqueous solutions of chromium(III) bromide and potassium phosphate are combined, solid chromium(III) phosphate and a solution of potassium bromide are formed. The net ionic equation for this reaction is:

More Similar Questions