Sulfuric acid (H2SO4) and sodium hydroxide (NaOH) undergo a neutralization reaction, represented by the following balanced chemical equation: H2SO4 + 2NaOH > 2H2O + Na2SO4 A lab analyst performed an experiment to determine the exact concentration of a sulfuric acid sample. In his experiment, he prepared 1M NaOH solution and aimed to determine how many mL of this solution will be needed to completely react with the sulfuric acid sample. He obtained the following data: 30 mL of 1M NaOH was consumed in the experiment.  Other details:  MW of NaOh: 39.997 g/mol  MW of Sulfuric Acid: 98.079 g/mol    Questions: (1)  How many moles of NaOh was consumed in the reaction? (2) Calculate how many grams of H2SO4 must have been present in the sample that has completely reacted with NaOH. Assume complete stoichiometric reaction.

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