The acidity of a solution is measured by its pH . If \( \left[\mathrm{H}^{+}\right] \)represents the concentration of hydrogen ions (in moles/liter) in the solution, the pH is defined by \( \mathrm{pH}=-\log \left[\mathrm{H}^{+}\right] \) Based on careful measurements and calculations, a chemist examines two solutions and asserts: "The hydrogen ion concentration of Solution A is 6.22 times greater than the hydrogen ion concentration of Solution B." If the pH of solution B is 3.3 , determine the pH of Solution A. Report your answer to one decimal place. Solution A has pH equal to Number

To find the pH of Solution A, we start by determining the hydrogen ion concentration of Solution B. The formula for pH is given by: \[ \text{pH} = -\log \left[\mathrm{H}^{+}\right] \] Given that the pH of Solution B is 3.3, we can calculate \(\left[\mathrm{H}^{+}\right]_B\): \[ \left[\mathrm{H}^{+}\right]_B = 10^{-\text{pH}} = 10^{-3.3} \approx 0.0005012 \, \text{moles/liter} \] According to the chemist, the hydrogen ion concentration of Solution A is 6.22 times greater than that of Solution B: \[ \left[\mathrm{H}^{+}\right]_A = 6.22 \times \left[\mathrm{H}^{+}\right]_B = 6.22 \times 0.0005012 \approx 0.003123 \, \text{moles/liter} \] Now we can find the pH of Solution A: \[ \text{pH}_A = -\log \left[\mathrm{H}^{+}\right]_A = -\log(0.003123) \approx 2.5 \] So, the pH of Solution A is approximately **2.5**.