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Jan. 28, 2023•0 likes•2 views

Jan. 28, 2023•0 likes•2 views

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what amount of 0.50 mol/L NaOH is required to titrate 10.0 ml of a 2.00 moll/L H2SO4 solution? Solution volume of H2SO4 solution = 10 ml = 0.01 L concentration of H2SO4 solution = 2 mol / L now moles of H2SO4 = 0.01 L x 2 mol / L = 0.02 mol now H2SO4 + 2 NaOH ---> Na2SO4 + 2 H2O so moles of NaOH required = 0.02 mol H2SO4 x ( 2 mol NaOH / 1 mol H2SO4) moles of NaOH required = 0.04 mol now volume of NaOH solution = 0.04 mol / (0.5 mol/L) volume of NaOH solution = 0.08 L volume of NaOH solution = 0.08 L x 1000 ml / 1 L = 80 ml so 80 ml of NaOH is required .

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- 1. what amount of 0.50 mol/L NaOH is required to titrate 10.0 ml of a 2.00 moll/L H2SO4 solution? Solution volume of H2SO4 solution = 10 ml = 0.01 L concentration of H2SO4 solution = 2 mol / L now moles of H2SO4 = 0.01 L x 2 mol / L = 0.02 mol now H2SO4 + 2 NaOH ---> Na2SO4 + 2 H2O so moles of NaOH required = 0.02 mol H2SO4 x ( 2 mol NaOH / 1 mol H2SO4) moles of NaOH required = 0.04 mol now volume of NaOH solution = 0.04 mol / (0.5 mol/L) volume of NaOH solution = 0.08 L volume of NaOH solution = 0.08 L x 1000 ml / 1 L = 80 ml so 80 ml of NaOH is required