The figure plots the molar conductivity $\Lambda_m$ against $\sqrt{c}$ at $298\ \text{K}$ for potassium chloride and for acetic acid. Four points are marked. For KCl, $\Lambda_m$ is $147.1$ at $c = 0.00100\ \text{mol L}^{-1}$ and $141.2$ at $c = 0.0100\ \text{mol L}^{-1}$. For acetic acid at the same two concentrations it is $48.2$ and $16.0$. All molar conductivities are in $\text{S cm}^2\ \text{mol}^{-1}$. Both solutions are made with very pure water whose own conductivity can be ignored. NCERT's limiting molar ionic conductivities are $\lambda^\circ(\text{K}^+) = 73.5$, $\lambda^\circ(\text{Cl}^-) = 76.3$, $\lambda^\circ(\text{H}^+) = 349.6$ and $\lambda^\circ(\text{CH}_3\text{COO}^-) = 40.9$, in the same unit. Which of the following statements are correct?

Fig. 1: A graph of molar conductivity, in siemens square centimetres per mole, against the square root of the concentration. Potassium chloride gives a high, nearly flat straight line with points marked 147.1 and 141.2. Acetic acid gives a low curve that rises steeply towards the left, with points marked 48.2 and 16.0. Both pairs of points are at concentrations of 0.00100 and 0.0100 mol per litre.