Answer: a) The molarity of the solution is 0.348 M
b) The concentration of the chromium(II) cation is 0.348 M
c) The concentration of the acetate anion is 0.696 M
Explanation:
Molarity of a solution is defined as the number of moles of solute dissolved per Liter of the solution.
[tex]Molarity=\frac{n\times 1000}{V_s}[/tex]
where,
n = moles of solute
[tex]V_s[/tex] = volume of solution in ml = 150 ml
moles of solute =[tex]\frac{\text {given mass}}{\text {molar mass}}=\frac{14.8g}{170g/mol}=0.0870moles[/tex]
Now put all the given values in the formula of molality, we get
[tex]Molality=\frac{0.0870\times 1000}{250}=0.348M[/tex]
Thus molarity of solution is 0.348 M
[tex]Cr(CH_3COO)_2\rightarrow Cr^{2+}+2CH_3COO^-[/tex]
According to stoihiometry;
1 mole of chromium acetate gives 1 mole of chromium ions
Thus molarity of [tex]Cr^{2+}[/tex] ions = 0.348 M
1 mole of chromium acetate gives 2 moles of acetate ions
Thus molarity of [tex]CH_3COO^- ions =2\times 0.348 M=0.696M[/tex]
