How many mL of 0.200 M NaOH are needed to titrate 20.0 mL of 0.100 M

Here you go man bit.ly/o3fZeG

40 To determine how many mL of 0.200 M NaOH are needed to titrate 20.0 mL of 0.100 M H2SO4, we can use the concept of stoichiometry and the balanced chemical equation for the reaction between NaOH and H2SO4.

The balanced chemical equation for the neutralization reaction between NaOH and H2SO4 is:

2 NaOH + H2SO4 → Na2SO4 + 2 H2O

From the balanced equation, we can see that 2 moles of NaOH react with 1 mole of H2SO4.

First, let's calculate the number of moles of H2SO4 in 20.0 mL of 0.100 M H2SO4 using the formula:

moles = concentration (M) × volume (L)

moles of H2SO4 = 0.100 M × (20.0 mL / 1000 mL/L) = 0.002 moles

Since the mole ratio of NaOH to H2SO4 is 2:1, we can determine the number of moles of NaOH needed:

moles of NaOH = 2 × 0.002 moles = 0.004 moles

Now, let's calculate the volume of 0.200 M NaOH needed to provide 0.004 moles of NaOH using the formula:

volume (L) = moles / concentration (M)

volume (L) = 0.004 moles / 0.200 M = 0.02 L

Finally, convert the volume from liters to milliliters:

volume (mL) = 0.02 L × 1000 mL/L = 20.0 mL

Therefore, 20.0 mL of 0.200 M NaOH are needed to titrate 20.0 mL of 0.100 M H2SO4.

How many mL of 0.200 M NaOH are needed to titrate 20.0 mL of 0.100 M H2SO4?

Here you go man bit.ly/o3fZeG

40

To determine how many mL of 0.200 M NaOH are needed to titrate 20.0 mL of 0.100 M H2SO4, we can use the concept of stoichiometry and the balanced chemical equation for the reaction between NaOH and H2SO4.