what volume of 1.5M NaOH would be required to neutralize 0.65g of pure aspirin?
Here is a solved example stoichiometry problem. Just follow the steps. For solution, remember moles = M x L.
http://www.jiskha.com/science/chemistry/stoichiometry.html
To determine the volume of 1.5M NaOH needed to neutralize 0.65g of pure aspirin, you need to consider the molar ratio between NaOH and aspirin.
1. Find the molar mass of aspirin (C9H8O4):
C - 12.0 g/mol
H - 1.0 g/mol
O - 16.0 g/mol
Molar mass of aspirin = (9 × 12.0 g/mol) + (8 × 1.0 g/mol) + (4 × 16.0 g/mol)
= 180.16 g/mol
2. Determine the number of moles of aspirin based on the given mass:
Number of moles = Mass / Molar mass
= 0.65g / 180.16 g/mol
≈ 0.0036 moles
3. Since the molar ratio between NaOH and aspirin is 1:1, the number of moles of NaOH required will also be 0.0036 moles.
4. Finally, use the concentration of NaOH to calculate the volume needed using the formula:
Volume = Number of moles / Concentration
Given Concentration = 1.5M
Volume = 0.0036 moles / 1.5 moles/L
≈ 0.0024 L or 2.4 mL
Therefore, approximately 2.4 mL of 1.5M NaOH would be required to neutralize 0.65g of pure aspirin.
To determine the volume of 1.5M NaOH required to neutralize 0.65g of pure aspirin, we need to consider the stoichiometry of the reaction between NaOH and aspirin.
First, let's write the balanced chemical equation for the neutralization reaction between NaOH and aspirin (C9H8O4):
C9H8O4 + 1 NaOH → 1 NaC9H7O4 + 1 H2O
From this equation, we can see that 1 mole of NaOH reacts with 1 mole of aspirin to form 1 mole of the sodium salt of aspirin (NaC9H7O4) and 1 mole of water (H2O).
The molar mass of aspirin (C9H8O4) is calculated by adding up the atomic masses:
C = 12.01 g/mol x 9 = 108.09 g/mol
H = 1.01 g/mol x 8 = 8.08 g/mol
O = 16.00 g/mol x 4 = 64.00 g/mol
So, the molar mass of aspirin is 108.09 g/mol + 8.08 g/mol + 64.00 g/mol = 180.17 g/mol.
To find the number of moles of aspirin, we divide the mass (0.65g) by the molar mass (180.17 g/mol):
0.65g / 180.17 g/mol = 0.0036 mol
According to the balanced equation, 1 mole of NaOH reacts with 1 mole of aspirin. Therefore, we need 0.0036 moles of NaOH to neutralize the aspirin.
Now, let's calculate the volume of 1.5M NaOH needed. The concentration of the NaOH solution is given as 1.5M, which means it contains 1.5 moles of NaOH per liter of solution.
Using the equation: moles = concentration x volume, we rearrange the equation to solve for volume:
volume = moles / concentration
volume = 0.0036 mol / 1.5 mol/L = 0.0024 L = 2.4 mL
Therefore, approximately 2.4 mL of 1.5M NaOH would be required to neutralize 0.65g of pure aspirin.