A student reacts 25.0 mL of 0.225 M NaOH with 25.0 mL of 0.147 M H_2SO_4. Write

Question

A student reacts 25.0 mL of 0.225 M NaOH with 25.0 mL of 0.147 M H_2SO_4. Write a balanced chemical equation to show this reaction. Calculate the concentrations of NaOH and H_2SO_4 that remain in solution, as well as the concentration of the salt that is formed during the reaction. A student reacts 45.0 mL of 0.198 M Ba (OH)_2 with 50.0 mL of 0.102 M H_3PO_4. Write a balanced chemical equation to show this reaction. Note that the salt formed in this reaction is a solid. Calculate the concentrations of Ba (OH)_2 and H_3PO_4 that remain in solution, as well as the mass of the salt that is formed during the reaction.

Explanation / Answer

Balanced chemical reaction;

2 NaOH + H2So4 = Na2So4 + 2 H2O

from this reaction 2moles of NaOH and one mole of H2SO4 gives one mole of Na2SO4

moles of NaOH present are=0.225M/1L*25mL=0.005625moles of NaOH

for 0.005625 moles of NaOH 0.005625/2 =0.002813mole H2SO4 required

moles of H2SO4 present are 0.147M/1L*25mL=0.003675moles

so extra H2SO4 is 0.003675-0.002813=0.000862moles

for 2 moles of NaOH and one mole of H2SO4, there will be one mole of Na2SO4

so salt concentration is 0.002813moles

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