Question
How many mL of 0.5 M sodium hydroxide would it take to react completely with 50 mL of 0.3 M sulfuric acid?
Answers
GPT 3.5
To answer this question, we need to determine the balanced chemical equation for the reaction between sodium hydroxide (NaOH) and sulfuric acid (H2SO4).
The balanced equation is:
2 NaOH + H2SO4 -> Na2SO4 + 2 H2O
From the balanced equation, we can see that for every 2 moles of NaOH, we need 1 mole of H2SO4.
We can use the equation:
moles = concentration × volume (in liters)
to calculate the number of moles of H2SO4:
moles of H2SO4 = 0.3 M × 0.050 L = 0.015 moles
Since the stoichiometry of the reaction is 2:1 (NaOH:H2SO4), we need 2 times the number of moles of NaOH:
moles of NaOH = 2 × moles of H2SO4 = 2 × 0.015 moles = 0.030 moles
Now we can use the equation:
volume (in liters) = moles / concentration
to calculate the volume of 0.5 M NaOH needed:
volume of NaOH = 0.030 moles / 0.500 M = 0.060 L = 60 mL
Therefore, it would take 60 mL of 0.5 M sodium hydroxide to react completely with 50 mL of 0.3 M sulfuric acid.
The balanced equation is:
2 NaOH + H2SO4 -> Na2SO4 + 2 H2O
From the balanced equation, we can see that for every 2 moles of NaOH, we need 1 mole of H2SO4.
We can use the equation:
moles = concentration × volume (in liters)
to calculate the number of moles of H2SO4:
moles of H2SO4 = 0.3 M × 0.050 L = 0.015 moles
Since the stoichiometry of the reaction is 2:1 (NaOH:H2SO4), we need 2 times the number of moles of NaOH:
moles of NaOH = 2 × moles of H2SO4 = 2 × 0.015 moles = 0.030 moles
Now we can use the equation:
volume (in liters) = moles / concentration
to calculate the volume of 0.5 M NaOH needed:
volume of NaOH = 0.030 moles / 0.500 M = 0.060 L = 60 mL
Therefore, it would take 60 mL of 0.5 M sodium hydroxide to react completely with 50 mL of 0.3 M sulfuric acid.