Calculate the volume of the specified titrant required to neutralize 35 ml of .4 M NaOH. Titrant: 0.75 M H2SO4 [2NaOH + H2SO4 „» 2H2O + Na2SO4]
To calculate the volume of the specified titrant required to neutralize 35 ml of 0.4 M NaOH, we can use the concept of stoichiometry.
First, let's write the balanced chemical equation for the reaction between NaOH and H2SO4:
2NaOH + H2SO4 → 2H2O + Na2SO4
From the balanced equation, we can see that the molar ratio between NaOH and H2SO4 is 2:1. This means that for every 2 moles of NaOH, we need 1 mole of H2SO4 to completely neutralize it.
Now, let's calculate the amount of moles of NaOH in 35 ml of 0.4 M NaOH. We can use the formula:
moles = volume (in liters) x concentration
First, convert the volume from milliliters to liters:
35 ml = 35/1000 = 0.035 liters
Now, calculate the moles of NaOH:
moles of NaOH = 0.035 L x 0.4 M = 0.014 moles
Since the molar ratio between NaOH and H2SO4 is 2:1, we need half the amount of moles of H2SO4 to neutralize the NaOH.
moles of H2SO4 = 0.014 moles / 2 = 0.007 moles
Finally, let's calculate the volume of 0.75 M H2SO4 required to contain 0.007 moles of H2SO4. We can rearrange the moles formula:
moles = volume (in liters) x concentration
Rearranging it to solve for volume:
volume = moles / concentration
volume of H2SO4 = 0.007 moles / 0.75 M = 0.00933 liters
Remember to convert liters back to milliliters:
volume of H2SO4 = 0.00933 L x 1000 = 9.33 ml
Therefore, approximately 9.33 ml of 0.75 M H2SO4 is required to neutralize 35 ml of 0.4 M NaOH.
To calculate the volume of the specified titrant required to neutralize 35 ml of 0.4 M NaOH with 0.75 M H2SO4, we need to use the balanced equation:
2NaOH + H2SO4 -> 2H2O + Na2SO4
From the equation, we can see that the stoichiometric ratio between NaOH and H2SO4 is 2:1.
First, let's calculate the number of moles of NaOH in 35 ml of 0.4 M NaOH:
Moles of NaOH = Volume (in liters) × Concentration
= 35 ml × (1 L / 1000 ml) × 0.4 M
= 0.014 moles
Since the stoichiometric ratio is 2:1 (NaOH:H2SO4), we need half the number of moles of H2SO4. Therefore, we require 0.007 moles of H2SO4.
Now, let's calculate the volume of 0.75 M H2SO4 needed to provide 0.007 moles of H2SO4:
Volume (in liters) = Moles ÷ Concentration
= 0.007 moles ÷ 0.75 M
= 0.00933 liters
Finally, convert the volume from liters to milliliters:
Volume (in ml) = Volume (in liters) × 1000
= 0.00933 L × 1000
= 9.33 ml
Therefore, the volume of 0.75 M H2SO4 required to neutralize 35 ml of 0.4 M NaOH is approximately 9.33 ml.