How many ml of molar sulfuric acid is to be added to 50.0 ml of 0.250 molar sodium hydroxide solution to neutralize it completely . cannot post reaction sorry ..
The reaction is
H2SO4 + 2NaOH ==> Na2SO4 =+ 2H2O;
BUT you didn't post the molarity of the H2SO4 and that is needed to do the problem.
Sorry it is .300ml
.300 molar
mols NaOH = M x L = ?
Using the coefficients in the balanced equation, convert mols NaOH to mols H2SO4. That should be mols H2SO4 = 1/2 mols H2SO4.
Then M H2SO4 = mols H2SO4/L H2SO4. Solve for L H2SO4 and convert to mL.
To determine the number of milliliters (ml) of molar sulfuric acid required to neutralize 50.0 ml of 0.250 molar sodium hydroxide solution completely, we need to consider the stoichiometry of the balanced equation for the neutralization reaction between sulfuric acid (H2SO4) and sodium hydroxide (NaOH). Unfortunately, since you haven't provided the balanced equation for the reaction, I will explain the general process you can follow to calculate the solution.
Here are the steps you can take to find the answer:
Step 1: Write the balanced equation
Write the balanced equation for the neutralization reaction between sulfuric acid (H2SO4) and sodium hydroxide (NaOH) based on the information you have or the equation you're referring to. The balanced equation will indicate the stoichiometric ratio between the reactants.
Step 2: Determine the stoichiometric ratio
From the balanced equation, determine the stoichiometric ratio between sulfuric acid and sodium hydroxide. This ratio will allow you to determine how many moles of sulfuric acid are required to neutralize one mole of sodium hydroxide.
Step 3: Convert the volume to moles
Use the given concentration of the sodium hydroxide solution (0.250 molar) to convert the given volume (50.0 ml) into moles. To do this, multiply the concentration by the volume in liters (50.0 ml = 0.0500 L).
Number of moles of sodium hydroxide = concentration × volume in liters
Step 4: Determine the required amount of sulfuric acid
Use the stoichiometric ratio obtained in Step 2 to determine the number of moles of sulfuric acid required to neutralize the calculated number of moles of sodium hydroxide.
Step 5: Convert moles to milliliters
Finally, use the concentration of the sulfuric acid solution to convert the calculated moles of sulfuric acid into milliliters. To do this, divide the required moles by the concentration in molar.
Volume (in ml) of sulfuric acid = (moles of sulfuric acid required) / concentration (in molar)
By following these steps, you can calculate the appropriate volume of molar sulfuric acid needed to neutralize the sodium hydroxide solution completely. If you provide the balanced equation for the reaction, I can assist you further with the calculation.