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

1 Answer
May 28, 2016

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