how many grams of nacl are required to neutralize 100 ml of 1M h2so4???
To determine the number of grams of NaCl required to neutralize 100 mL of 1M H2SO4, we need to follow these steps:
Step 1: Understand the reaction equation:
First, let's write the balanced chemical equation for the neutralization reaction between H2SO4 and NaCl:
H2SO4 + 2NaCl → Na2SO4 + 2HCl
Step 2: Determine the molar ratio:
Looking at the balanced equation, we can see that for every 1 mole of H2SO4, we need 2 moles of NaCl. This ratio comes from the coefficients in the balanced equation.
Step 3: Calculate the moles of H2SO4:
Since we know the concentration of H2SO4 and the volume used, we can calculate the number of moles of H2SO4.
Moles of H2SO4 = Concentration (M) × Volume (L)
To convert the volume from milliliters (mL) to liters (L), divide by 1000.
Moles of H2SO4 = 1 M × 100 mL ÷ 1000 = 0.1 moles
Step 4: Calculate the moles of NaCl:
Using the molar ratio from step 2, we can determine the moles of NaCl required.
Moles of NaCl = Moles of H2SO4 × (2 moles NaCl / 1 mole H2SO4)
Moles of NaCl = 0.1 moles × (2 moles / 1 mole) = 0.2 moles
Step 5: Calculate the grams of NaCl:
Finally, we need to convert the moles of NaCl to grams using the molar mass of NaCl, which is approximately 58.5 g/mol.
Grams of NaCl = Moles of NaCl × Molar Mass of NaCl
Grams of NaCl = 0.2 moles × 58.5 g/mol = 11.7 grams
Therefore, approximately 11.7 grams of NaCl are required to neutralize 100 mL of 1M H2SO4.
To determine the number of grams of NaCl required to neutralize 100 mL of 1M H2SO4 solution, we first need to calculate the number of moles of H2SO4 present.
Step 1: Calculate the number of moles of H2SO4.
The concentration of the H2SO4 solution is given as 1M, which means there is 1 mole of H2SO4 per liter (1000 mL) of solution.
Given that the volume of the solution is 100 mL (0.1 L), the number of moles of H2SO4 can be calculated as follows:
Moles of H2SO4 = concentration (M) x volume (L)
= 1M x 0.1 L
= 0.1 moles
Step 2: Determine the stoichiometry of the reaction.
The balanced equation for the reaction between NaCl and H2SO4 is:
2NaCl + H2SO4 → Na2SO4 + 2HCl
From the equation, we can see that 2 moles of NaCl react with 1 mole of H2SO4.
Step 3: Calculate the number of moles of NaCl required.
Since the stoichiometry ratio between NaCl and H2SO4 is 2:1, the number of moles of NaCl required is half the number of moles of H2SO4:
Moles of NaCl required = 0.1 moles H2SO4 / 2
= 0.05 moles NaCl
Step 4: Calculate the mass of NaCl required.
To calculate the mass of NaCl required, we need to multiply the number of moles of NaCl by its molar mass.
The molar mass of NaCl is 58.44 g/mol (22.99 g/mol for Na + 35.45 g/mol for Cl).
Mass of NaCl required = Moles of NaCl required x Molar mass of NaCl
= 0.05 moles x 58.44 g/mol
= 2.922 g
Therefore, approximately 2.922 grams of NaCl are required to neutralize 100 mL of 1M H2SO4.