Citric acid (H3C6H5O7) is triprotic acid which reacts with NaOH according to the balanced chemical equation shown below what volume of 0.200m Naoh is required to titrate 7.50ml of lemon juice which is 0.245 m in citric acid?
H3C6H5O7+3NaOH->Na3C6H5aO7+ 3H2O
Citric acid is H3C. I assume you meant 0.245 M and not 0.245 m.
mols H3C = M x L = ?
Convert mols H3C to mols NaOH.
Then M NaOH = mols NaOH/L NaOH. You know mols and M, solve for L
To solve this problem, we need to determine the balanced chemical equation, calculate the number of moles of citric acid in the lemon juice, and then use stoichiometry to find the volume of NaOH solution required.
Let's start step-by-step:
Step 1: Write the balanced chemical equation:
H3C6H5O7 + 3NaOH -> Na3C6H5O7 + 3H2O
Step 2: Calculate the number of moles of citric acid in the lemon juice.
The lemon juice is 0.245 M in citric acid, and we have 7.50 mL of lemon juice. Using the formula:
moles = concentration x volume
moles of H3C6H5O7 = 0.245 mol/L x 0.00750 L
moles of H3C6H5O7 = 0.00184 moles
Step 3: Use stoichiometry to find the volume of NaOH solution required.
From the balanced chemical equation, we can see that for every 1 mole of citric acid (H3C6H5O7), 3 moles of NaOH are required. Therefore, the number of moles of NaOH required is also 0.00184 moles.
Now we can use the formula:
moles = concentration x volume
to find the volume of 0.200 M NaOH solution required.
0.00184 moles = 0.200 mol/L x Volume
Volume = 0.00184 moles / 0.200 mol/L
Volume = 0.0092 L or 9.2 mL
Therefore, 9.2 mL of 0.200 M NaOH solution is required to titrate 7.50 mL of lemon juice.
To determine the volume of 0.200 M NaOH required to titrate 7.50 mL of lemon juice, you can use the concept of stoichiometry and the dilution formula.
1. Determine the number of moles of citric acid in the given volume (7.50 mL) of lemon juice.
- Moles of citric acid = Volume (in L) × Concentration of citric acid
- Convert the volume of lemon juice to liters: 7.50 mL ÷ 1000 mL/L = 0.00750 L
- Moles of citric acid = 0.00750 L × 0.245 M = 0.0018375 moles
2. Use the balanced chemical equation to determine the stoichiometric ratio between citric acid (H3C6H5O7) and NaOH.
- From the equation, the stoichiometric ratio between H3C6H5O7 and NaOH is 1:3.
- This means that for every mole of citric acid, you need three moles of NaOH.
3. Calculate the number of moles of NaOH required to react with the given number of moles of citric acid.
- Moles of NaOH = 3 × Moles of citric acid = 3 × 0.0018375 moles = 0.0055125 moles
4. Use the concentration and moles of NaOH to determine the required volume of 0.200 M NaOH.
- Concentration of NaOH = 0.200 M
- Volume of NaOH = Moles of NaOH ÷ Concentration of NaOH
- Volume of NaOH = 0.0055125 moles ÷ 0.200 M = 0.0275625 L
5. Convert the volume of NaOH from liters to milliliters (mL).
- Volume of NaOH = 0.0275625 L × 1000 mL/L = 27.5625 mL
Therefore, approximately 27.6 mL of 0.200 M NaOH is required to titrate 7.50 mL of lemon juice containing 0.245 M citric acid.