What is the molar concentration of sulfate ions in a 0.150 M #Na_2SO_4# solution?

1 Answer
May 28, 2016

Answer:

#M_(SO_4^(2-))=0.150M#

Explanation:

In solution, sodium sulfate dissociates according to the following equation:

#Na_2SO_4(s)->2Na^(+)(aq)+SO_4^(2-)(aq)#

Therefore, #1mol# of #Na_2SO_4# will give #1mol# of #SO_4^(2-)# and thus, the molarity of sulfate ions will be equal to that of the sodium sulfate.

#M_(SO_4^(2-))=0.150M#

However, the molarity of sodium ions is the double of that of sodium sulfate since #1mol# of #Na_2SO_4# will give #2mol# of #Na^(+)#:

#M_(Na^(+))=0.300M#