A 0.0100 L sample of H2SO4 was titrated with 0.150 M NaOH. It took 23.3 mL of Na

Question

A 0.0100 L sample of H2SO4 was titrated with 0.150 M NaOH. It took 23.3 mL of NaOH from the buret--that's 0.0233 L--to reach the titration endpoint. 1) Balance the chemical equation for this titration by placing coefficients in the spaces below. (If you need to learn or review how to balance equations, visit this link for a tutorial or see section 3.7 in your Chang Chemistry textbook.) ____ H2SO4(aq) + ____ NaOH(aq) ?? ____ H2O(l) + ____ Na2SO4(aq) 2) Based on the coefficients of the equation that you just balanced, how many moles of NaOH would be consumed by one mole of H2SO4? 3) How many moles of NaOH are contained in the 0.0233 L volume of 0.150 M NaOH that is delivered from the buret? 4) How many moles of H2SO4 must be present to react completely with the NaOH delivered from the buret? 5) What is the molarity (M) of the H2SO4 solution titrated? Hint: Molarity refers to the number of moles of H2SO4 per liter, i.e., mol divided by L. Use the number of moles (question #4 above) along with the actual volume of H2SO4 titrated, 0.0100 L.

Explanation / Answer

always must start with abalanced equation:

2NaOH+H2SO4? Na2SO4 + 2 H2O

Each mole of H2SO4 consumes 2 moles of NaOH.

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