For neutralization of 10ml 10% sodium carbonate how many 1N H2SO4 is required?
I assume the 10% Na2CO3 is 10% by volume. That means you have 10g Na2CO3/100 mL and you take 10 mL of that; therefore, g Na2CO3 titrated by the H2SO4 =
10g x (10 mL/100 mL) = 1.00 g Na2CO3
Second assumption. You don't say what indicator is used for the titration. If phenolphthalein is used the milliequivalent weight of Na2CO3 is 0.106; if methyl red is used the milliequivalent weight of Na2CO3 is 0.053.
mLH2SO4 x NH2SO4 x mewNa2CO3 = 1.00 grams.
Solve for mL H2SO4.
To find the number of 1N H2SO4 required for neutralizing 10 mL of 10% sodium carbonate solution, we need to follow a step-by-step approach:
Step 1: Calculate the molarity of sodium carbonate solution.
The given solution has a concentration of 10%, which means it contains 10 g of sodium carbonate per 100 mL of solution. We can convert this to grams per liter (g/L) by multiplying the concentration by 10:
10% * 10 g/100 mL * 10 mL/1L = 10 g/L.
Step 2: Convert grams of sodium carbonate to moles.
To convert grams to moles, we need to know the molar mass of sodium carbonate. It consists of three components: sodium (Na) with a molar mass of 22.99 g/mol, carbon (C) with a molar mass of 12.01 g/mol, and oxygen (O) with a molar mass of 16.00 g/mol. Adding these together, we find the molar mass of sodium carbonate to be:
22.99 g/mol + 12.01 g/mol + (16.00 g/mol * 3) = 105.99 g/mol.
Since we have 10 grams of sodium carbonate, we can now calculate the number of moles:
10 g / 105.99 g/mol ≈ 0.094 moles.
Step 3: Determine the stoichiometry of the reaction.
The reaction between sodium carbonate (Na2CO3) and sulfuric acid (H2SO4) can be represented as follows:
Na2CO3 + H2SO4 -> Na2SO4 + CO2 + H2O.
From the balanced equation, we can see that one mole of sodium carbonate reacts with one mole of sulfuric acid. Therefore, 0.094 moles of sodium carbonate will require 0.094 moles of sulfuric acid.
Step 4: Calculate the volume of 1N H2SO4 needed.
A 1N solution contains one equivalent of solute per liter of solution. Since sulfuric acid (H2SO4) is a diprotic acid, one mole of H2SO4 is needed to provide two equivalents of H+ ions. Therefore, to prepare 1N H2SO4, we dissolve one mole of sulfuric acid in one liter of solution.
To neutralize 0.094 moles of sodium carbonate, we need to have the same number of moles of sulfuric acid, which is 0.094 moles. Since 1L of 1N H2SO4 contains 1 mole, the volume needed will be:
0.094 moles / 1 mole/L = 0.094 L = 94 mL.
Hence, to neutralize 10 mL of 10% sodium carbonate, approximately 94 mL of 1N H2SO4 is required.