If a chemist titrates 300.0ml of h2so4 with a 3.0m solution of naoh and requires only 3.4ml of the base to reach endpoint, what is the concentration of the sulfuric acid

The balanced equation for the acid-base reaction is as follows;
2NaOH + H₂SO₄ --> Na₂SO₄ + 2H₂O
stoichiometry of NaOH to H₂SO₄ is 2:1
this means that for complete neutralisation 2 mol of NaOH reacts with 1 mol H₂SO₄
number of NaOH moles reacted = 3.0 M /1000 x 3.4 = 0.0102 mol
Number of H₂SO₄ moles reacted = 0.0102 /2 = 0.0051 mol
Number of H₂SO₄ moles in 300.0 mL - 0.0051 mol
therefore in 1 L solution -0.0051/300 x 1000= 0.017 mol
concentration is number of moles in 1 L solution
Concentration of H₂SO₄ is 0.017 M 

Less stable  hope this

Hbr dissociates to form h+ and br-ca(oh)2 dissociates to form ca2+ and 2oh-the h+ and oh- react to form waterassuming the reactants are dissolved in water, the net reaction is h+ + oh- —> h2oif you’re asked to show all components of the reaction, the complete reaction is 2hbr + ca(oh)2 —> cabr2 + 2h2o