State that pH is dependent on the concentration of hydrogen ions in solution.

A student measures the hydrogen ion concentration, $[\text{H}^{+}]$, of three aqueous solutions at $298\text{ K}$ and obtains the following results: • Solution A: $[\text{H}^{+}] = 1 \times 10^{-3}\text{ mol L}^{-1}$ • Solution B: $[\text{H}^{+}] = 1 \times 10^{-5}\text{ mol L}^{-1}$ • Solution C: $[\text{H}^{+}] = 1 \times 10^{-7}\text{ mol L}^{-1}$ (a) State which solution is the most acidic. (1 mark) (b) Explain why the pH of solution C is different from that of solution B, using a statement about the dependence of pH on hydrogen ion concentration. (1 mark)

A student prepares two aqueous solutions. Solution A has a hydrogen ion concentration of $[\text{H}^{+}] = 1.0 \times 10^{-3}$ mol/L, and Solution B has $[\text{H}^{+}] = 1.0 \times 10^{-5}$ mol/L. Which statement correctly describes the relationship between the hydrogen ion concentration and pH of these solutions?

Which statement correctly describes the relationship between pH and hydrogen ion concentration in an aqueous solution?