A student measured the concentration of H2SO4 by titrating it with 3 L of NH3 at 646 torr and 305 K. The experiment revealed that 144 mL of H2SO4 was required to neutralize the NH3. Calculate the concentration of the acid in terms of normality.

It was found that 19.60 mL of NaOH solution were required to neutralize 10.00 mL of HCl. If the concentration of the base solution was 0.1051 M, calculate the concentration of the acid solution.

In the acid-base titration experiment, a measured volume of oxalic acid is titrated with sodium hydroxide solution to determine the concentration of sodium hydroxide solution. The balance chemical equation for the reaction is given below: H2C2O4(aq) + 2 NaOH(aq) → Na2C2O4(aq) + 2 H2O(l) If 18.65 mL of NaOH solution is required to neutralize 10.00 mL of 0.1089 M of H2C2O4, what is the concentration (in mol/L) of the NaOH solution?

Calculate the concentration of 20.00 ml of H2SO4 needed to neutralize 21.33 ml of a NaOH solution having a concentration of 0.60 M. H2SO4(aq) + NaOH(aq) Ã H2O(l) + Na2SO4(aq) (unbalanced)

Please EXPLAIN!