Help with Textbook problem G.21

Moderators: Chem_Mod, Chem_Admin

Ellen Amico 2L
Posts: 101
Joined: Thu Sep 19, 2019 12:16 am

Help with Textbook problem G.21

Postby Ellen Amico 2L » Tue Oct 08, 2019 3:38 pm

The question is: "A solution is prepared by dissolving 0.500 g of KCl, 0.500 g of K2S, and 0.500 g of K3PO4 in 500. mL of water. What is the concentration in the final solution of (a) potassium ions; (b) sulfide ions?"
I calculated the molarity of the solution, but how do I find the concentration of the individual ions?

LNgo 1G
Posts: 100
Joined: Sat Aug 24, 2019 12:16 am

Re: Help with Textbook problem G.21

Postby LNgo 1G » Tue Oct 08, 2019 3:43 pm

You can use the mole ratios of the individual ions to the compounds given to find the moles of each ion in the solution and divide by volume to get the concentration from there.

Lauren Tanaka 1A
Posts: 109
Joined: Sat Aug 17, 2019 12:18 am

Re: Help with Textbook problem G.21

Postby Lauren Tanaka 1A » Wed Oct 09, 2019 10:52 am

To find the concentration of the individual ions you take the moles of each compound and multiply it by the mole ratio of the ions in that compound. This will leave you with the number of moles of the particular ion. From there you are able to use the molarity equation c = n/v (where n is the calculated moles of the particular ion and v is the volume given). Plug those numbers in and you should end up with the concentration of the particular ions.


Return to “Molarity, Solutions, Dilutions”

Who is online

Users browsing this forum: No registered users and 1 guest