10mL of 2(M) NaOH solution is added to 200mL of 0.5 (M) of NaOH solution. What is the final concentration?

10 mL of 2(M) NaOH solution is added to 200 mL of 0.5 (M) of NaOH solution. What is the final concentration of the resultant solution?

100 mL of 30% (m/v) NaOH solution is mixed with 100 mL of 90% (m/v) NaOH solution then the molarity of final solution will be-

If 100mL of 1M HCl is added to 150mL of 1M NaOH, What is the final nature and concentration of resultant solution.

The equivalent point in titration of 40.0 ml of a solution of a weak monoprotic acid occurs when 35.0 of a 0.10 M NaOH solution has been added . The pH of the solution is 5.75 after the addition of 20.0 ml of NaOH solution . What is the dissociation constant of the acid ?

100 ml of 5 M NaOH solution (density 1.2 g/ml) added to 200 mL of another NaOH solution which has a density of 1.5 g/ml and contains 20 mass percent of NaOH. What will be the volume of the gas (at STP) in litres liberated when aluminium reacts with this (final) solution? [Give answer excluding decimal places] The reaction is Al+NaOH+H_(2)OrarrNaAlO_(2)+H_(2) (At. wt. Na=23, 0=16, H=1)

What volume of 0.2 M NaOH (in ml) solution should be mixed to 500 ml of 0.5 M NaOH solution so that 300 ml of final solution is completely neutralised by 20 ml of 2 M H_(3) PO_(4) solution [Assuming 100% dissociation]

What volume of 0.2 M NaOH (in ml) solution should be mixed to 500 ml of 0.5 M NaOH solution so that 300 ml of final solution is completely neutralised by 20 ml of 2 M H_(3) PO_(4) solution [Assuming 100% dissociation]

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?

The equivalent point in a titration of 40.0mL of a sodium of a weak monoprotic acid occurs when 35.0mL of a 0.10M NaOH solutio has been added. The pH of the solution is 5.5 after the addition of 20.0mL of NaOH solution. What is the dissociation constant of the acid ?