Two solutions are available as sample.
Solution A - 2 L of 0.1 M $$\text{H}_2\text{SO}_4$$ solution, and
Solution B - 1 L of 0.2 M NaOH solution
Then the correct statement(s) is/are 

This is a multiple-correct question, and the correct options are (a) and (b). Dilution lowers $$[\text{H}^+]$$ in the acid and $$[\text{OH}^-]$$ in the base, so the acid's pH rises and the base's pH falls, both approaching 7 at infinite dilution. On mixing, A gives $$2 \times 0.2 = 0.4$$ mol $$\text{H}^+$$ while B gives only 0.2 mol $$\text{OH}^-$$, so the mixture is acidic, not neutral. A slight rise in temperature increases $$K_w$$, which lowers the pH of the base but leaves $$[\text{H}^+]$$ of the strong acid practically unchanged, so (d) is wrong.