10mL of 0.1 M HCl solution reacts completely with 10 mL of 0.1 M NaOH solution. What will be the pH of the resulting solution?

What is the pH of 0.1M NaOH solution?

Calculate the pH of 0.005 M NaOH solution.

2.5 litre of 1 M NaOH solution are mixed and another 3 litre of 0.5 M NaOH solution. Then the molarity of the resulting solution is

20 mL of 0.2 M NaOH(aq) solution is mixed with 35 mL of this 0.1 ML NaOH (aq) solution and the resultant solution is diluted to 100 mL. 40 mL of this diluted solution reacted with 10% impure sample of oxalic acid (H_(2)C_(2)O_(4)) The mass of impure is:

100 mL of a solution containing 5 g of NaOH are mixed with 200 mL of M/5 NaOH solution. Calculate the molarity of the resulting solution.

4L of water is added to 2L of 6M HCl solution. What is the molarity of resulting solution .

At 90^(@) C, pure water has [H^(+)]=10^(-6) M.If 100 mL of 0.2 M HCl is added to 200 mL of 0.1 M KOH at 90^(@) C then pH of the resulting solution will be :

What is the pH of 0.1 M HCl ?

A solution of weak acid HA was titrated with base NaOH. The equivalent point was reached when 40 mL. Of 0.1 M NaOH has been added. Now 20 mL of 0.1 M HCl were added to titrated solution, the pH was found to be 5.0 What will be the pH of the solution obtained by mixing 20 mL of 0.2 M NaOH and 20 mL of 0.2 M HA?

pH of 10^-5 M HCl solution is……………..