Explanation:
The ionic strength of a solution, I, is defined as
I=1/2 Σ m_i z_i^2
Where m_i is the concentration of the ion, and z_i is the charge of the ion.
For 1 M NaCl solution, Ionic strength I = ½ (1*12 + 1*12) = 1.00;
For, 1 M (NH4)2SO4, concentration of [NH4] = 2 M and [SO4] = 1 M;
I = ½ (2*12 + 1*22) = 3.00;
so ionic strength of 1 M (NH4)2SO4 is different, therefore it is a serious error.
Explanation:
It is known that the ionic strength of a solution, I, is represented as follows.
[tex]I = \frac{1}{2} \sum m_{i}z^{2}_{i}[/tex]
where, [tex]m_{i}[/tex] = the concentration of the ion,
[tex]z_{i}[/tex] = the charge of the ion
Now, for 1 M NaCl solution, the ionic strength will be calculated as follows.
I = [tex]\frac{1}{2} [(1 \times 1^{2}) + (1 \times 1^{2})][/tex]
= 1.00
And, for 1 M [tex](NH_{4})_{2}SO_{4}[/tex], concentration of [tex][NH_{4}][/tex] = 2 M and [tex][SO_{4}][/tex] = 1 M.
I = [tex]\frac{1}{2} [(2 \times 1^{2}) + ((1 \times 2^{2})][/tex]
= 3.00
As the ionic strength of 1 M [tex](NH_{4})_{2}SO_{4}[/tex], is different therefore it is a serious error.
