The ionic product of water is 10⁻¹⁴ . The H⁺  ion concentration in 0.1M NaOH  solution is

To calculate the ^H+ ion concentration in a 0.1M NaOH solution, we use the relation between the ionic product of water (K_w) and the concentrations of ^H+ and ^OH−:

Formula:

K_w = [H⁺][OH⁻]

Here, the ionic product of water is given as 10⁻¹⁴, and the concentration of ^OH− in the NaOH solution is equal to its molarity (0.1 M) because NaOH fully dissociates in water:

[OH⁻] = 0.1 M = 10⁻¹ M

Now, substitute these values into the formula to find ^H+:

[H⁺] = K_w / [OH⁻] = 10⁻¹⁴ / 10⁻¹

[H⁺] = 10^{−14 + 1} = 10⁻¹³ M

Final Answer

In a strong base like NaOH, the ^OH− ion concentration is high, resulting in a correspondingly low ^H+ ion concentration due to the inverse relationship described by K_w. Thus, in this case, the ^H+ ion concentration is 10⁻¹³ M.