what volume of .5 m sulfuric acid is needed to react completely with 10 mL of 2m potassium hydroxide
Write and balance the equation.
moles KOH = M x L.
Use the equation and coefficients to convert moles KOH to moles H2SO4.
Now use M = moles/L to calculate L H2SO4.
in which compound does sulfur have an oxidation number of -2
1. SO2
2. SO3
3. Na2S
4. Na2SO4
To determine the volume of 0.5 M sulfuric acid needed to react completely with 10 mL of 2 M potassium hydroxide, we can use the concept of stoichiometry and balanced chemical equations.
First, let's write the balanced chemical equation for the reaction between sulfuric acid (H2SO4) and potassium hydroxide (KOH):
H2SO4 + 2KOH → K2SO4 + 2H2O
From the equation, we can see that 1 mole of sulfuric acid (H2SO4) reacts with 2 moles of potassium hydroxide (KOH).
Given that the concentration of potassium hydroxide solution is 2 M and the volume is 10 mL, we can calculate the number of moles of KOH using the formula:
moles = concentration × volume
moles of KOH = 2 M × 0.01 L (converting 10 mL to liters) = 0.02 moles
Since the mole ratio between H2SO4 and KOH is 1:2, we need twice as many moles of sulfuric acid as potassium hydroxide. Therefore, we would need 0.04 moles of sulfuric acid.
Now, we can use the concentration to calculate the volume of 0.5 M sulfuric acid needed:
volume = moles / concentration
volume of H2SO4 = 0.04 moles / 0.5 M = 0.08 L or 80 mL
In summary, 80 mL of 0.5 M sulfuric acid is needed to react completely with 10 mL of 2 M potassium hydroxide.