Question 15.2: What is the molarity of each ion in a solution of (a) 2.0 M ...

What is the molarity of each ion in a solution of (a) 2.0 M NaCl and (b) 0.40 M K2SO4K_2SO_4 Assume complete dissociation.

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(a) According to the dissociation equation,

NaClH2ONa+(aq)+Cl(aq)NaCl \xrightarrow[]{H_2O} Na^+(aq) + Cl^-(aq)

1 mol                                  1 mol                    1 mol

the concentration of Na+Na^+ is equal to that of NaCl : 1 mol NaCl → 1 mol Na+Na^+ and the concentration of ClCl^-  is also equal to that of NaCl Therefore the concentrations of the ions in 2.0 M NaCl are 2.0 M Na+Na^+  and 2.0 M  ClCl^-

(b) According to the dissociation equation

K2SO4H2O2K+(aq)+SO42(aq)K_2SO_4 \xrightarrow[] {H_2O} 2K^+(aq) + SO^{2-}_4(aq)

1 mol                                     2 mol                           1 mol

the concentration of K+K^+ is twice that of K2SO4K_2SO_4 and the concentration of SO42SO_4^{2-} is equal to that of K2SO4K_2SO_4 .Therefore the concentrations of the ions in 0.40 M K2SO4K_2SO_4 are 0.80 M K+K^+ and 0.40 M SO42SO_4^{2-}

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