5.0 mL of H2SO4 solution was titrated with 0.20 M NaOH standard solution. The volume of NaOH needed to reach the equivalent point was 9.5 mL.
1. In this titration setup, what is the titrant? and what is the analyte?
2. What is the number of mole of H2SO4 in the 5.0 mL solution?
3. What is the molarity of H2SO4 solution?
4. What is the mass (g) of H2SO4 in the 5.0 mL solution?
5. What is the mass of sulfur in the 5.0 mL solution?
2NaOH + H2SO4 ==>Na2SO4 + 2H2O
1. The NaOH is the titrant; H2SO4 is the analyte.
2. mols NaOH = M x L
mols H2SO4 = 1/2 mols NaOH (Look at the coefficients in the balanced equation.)
3. M H2SO4 = mols H2SO4/L H2SO4
4. g H2SO4 = mols H2SO4 x molar mass H2SO4
5. mass S = mass H2SO4 x (atomic mass S/molar mass H2SO4) = ?
1. In this titration setup, the titrant is the 0.20 M NaOH standard solution, which is being slowly added to the H2SO4 solution. The analyte is the H2SO4 solution being analyzed.
To determine the titrating agent and the substance being analyzed, you should look at the reaction taking place during the titration. In this case, it is a neutralization reaction between NaOH and H2SO4.
2. To calculate the number of moles of H2SO4 in the 5.0 mL solution, you need to use the stoichiometry of the neutralization reaction. The balanced equation for the reaction is:
2 NaOH + H2SO4 -> Na2SO4 + 2 H2O
According to the balanced equation, 2 moles of NaOH react with 1 mole of H2SO4. Since the volume of NaOH used is 9.5 mL and its concentration is 0.20 M, you can calculate the number of moles of NaOH used:
Moles of NaOH = Volume (in L) x Concentration (in mol/L)
= 9.5 mL * (1 L / 1000 mL) * 0.20 mol/L
Now, using the stoichiometry of the reaction, you know that 2 moles of NaOH react with 1 mole of H2SO4. Therefore, the number of moles of H2SO4 in the 5.0 mL solution is half of the number of moles of NaOH used.
3. To determine the molarity of the H2SO4 solution, you need to know the number of moles of H2SO4 and the volume of the H2SO4 solution used.
Molarity (M) = Moles of solute / Volume of solution (in L)
In this case, the molarity of H2SO4 will be calculated using the number of moles of H2SO4 from question 2 and the volume of H2SO4 solution used, which is given as 5.0 mL:
Molarity of H2SO4 = (Number of moles of H2SO4) / (Volume of H2SO4 solution in L)
4. To calculate the mass of H2SO4 in the 5.0 mL solution, we need to convert the number of moles of H2SO4 obtained in question 2 into grams using the molar mass of H2SO4.
The molar mass of H2SO4 is obtained from the periodic table by adding up the atomic masses of each element in the compound. In this case:
Molar mass of H2SO4 = (2 * atomic mass of Hydrogen) + atomic mass of Sulfur + (4 * atomic mass of Oxygen)
Once you have the molar mass, you can calculate the mass of H2SO4 using the formula:
Mass of H2SO4 = (Number of moles of H2SO4) x (Molar mass of H2SO4)
5. Finding the mass of sulfur in the 5.0 mL solution requires determining the number of moles of sulfur in H2SO4 and then converting this to grams.
In H2SO4, there is 1 mole of sulfur per mole of H2SO4, according to the balanced equation. Therefore, the moles of sulfur will be equal to the moles of H2SO4 in the solution.
To find the mass of sulfur, you multiply the moles of sulfur by the molar mass of sulfur, which can be obtained from the periodic table. The formula is:
Mass of sulfur = (Number of moles of sulfur) x (Molar mass of sulfur)