1.1. Calculate the volume of water, in cm³, required to raise the pH of 25.0 cm³ of hydrochloric acid from 0.80 to 0.90 at 298K.

1.2. After a neutralization reaction between sodium hydroxide and hydrochloric acid, a solution of sodium chloride is evaporated and 3.45 g of pure sodium chloride is produced.

Determine the volume, in cm³, of 0.30 mol dm^-3 of hydrochloric acid required in the reaction to produce this mass of sodium chloride.

1.3. 32.00 cm³ of 0.30 mol dm^-3 hydrochloric acid is added to 30.00 cm³ of 0.50 mol dm^-3 sodium hydroxide. Calculate the pH of the resulting solution at 298 K. Give your answer to 2 decimal places.

(K_w = 1.00 x 10^-14 mol² dm^-6 at 298 K)

1.4. 20.00 cm³ of 0.40 mol dm^-3 barium hydroxide solution, Ba(OH)₂ (aq), is added to the 35.00 cm³ of 0.30 mol dm^-3 of hydrochloric acid. What is the pH of the new solution at 298 K?

Give your answer to 2 decimal places. 

(K_w = 1.00 x 10^-14 mol² dm^-6 at 298 K)