A community for students.
Here's the question you clicked on:
 0 viewing
anonymous
 one year ago
When 0.054 moles of aluminum sulfate are
dissolved in enough water to make 459
milliliters of solution, what is the molarity
of sulfate ions?
Answer in units of M.
anonymous
 one year ago
When 0.054 moles of aluminum sulfate are dissolved in enough water to make 459 milliliters of solution, what is the molarity of sulfate ions? Answer in units of M.

This Question is Open

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Molarity = moles of solute (aluminum sulfate) divided by the volume of the solution in L. So, to calculate the molarity, divide the moles of aluminum sulfate by the volume of solution in L.

Jhannybean
 one year ago
Best ResponseYou've already chosen the best response.0\[\sf \frac{0.054 ~mol~Al_2(SO_4)_3}{459~mL~soln}~\times ~ \frac{1~mL}{10^{3}~L~ soln}~\times \frac{3~mol~SO_4^{2+}~ions}{1~mol~Al_2(SO_4)_3}\]\[\sf=\frac{(0.054 \cdot 3)~ mol~ SO_4^{2+} ~ions}{(459 \cdot 10^{3}) ~L~ soln} \]\[=~?\]

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0.4 or .35 or .353 ??? depending on what you used for sig figs? @Jhannybean

Jhannybean
 one year ago
Best ResponseYou've already chosen the best response.0The answer I got was: \[\sf \frac{0.35 ~mol~ SO_$^{2+}~ions }{1~L~soln}\] 2 sig figs because you started with 0.054 moles aluminum sulfate
Ask your own question
Sign UpFind more explanations on OpenStudy
Your question is ready. Sign up for free to start getting answers.
spraguer
(Moderator)
5
→ View Detailed Profile
is replying to Can someone tell me what button the professor is hitting...
23
 Teamwork 19 Teammate
 Problem Solving 19 Hero
 Engagement 19 Mad Hatter
 You have blocked this person.
 ✔ You're a fan Checking fan status...
Thanks for being so helpful in mathematics. If you are getting quality help, make sure you spread the word about OpenStudy.