So sry for the last confusing post, but i will correct it now:
For the 25g NaOH inside 50ml H2O you need:
We need to calculate the molarity of the NaOH solution.
Molarity (M) = (mass of solute in grams) / (molar mass of solute) / (volume of solution in liters)
Molarity = 25 g / (39.997 g/mol) / (50 ml / 1000 ml/L)
Molarity = 0.625 M
Calculate moles of sodium hydroxide: Moles of NaOH = Molarity x Volume (L) = 0.625 M x 0.050 L = 0.03125 moles of NaOH
Calculate moles of sodium carbonate required to replace NaOH: 1 mole of NaOH requires 1.22 moles of Na2CO3.
Moles of Na2CO3 = 1.22 x Moles of NaOH = 1.22 x 0.03125 moles = 0.038125 moles of Na2CO3
Calculate mass of sodium carbonate required:
Mass of Na2CO3 = Moles of Na2CO3 x Molecular mass of Na2CO3 = 0.038125 moles x 105.9888 g/mol = 4.039 g
So, you will need
4.039 g of sodium carbonate to replace the 25 g of sodium hydroxide. You can dissolve this amount of sodium carbonate
in 50 ml of water to achieve a similar concentration as the original NaOH solution.
For the 100g NaOH inside 100ml H2O you need:
Calculate molarity of NaOH solution:
Molarity (M) = (mass of solute in grams) / (molar mass of solute) / (volume of solution in liters)
Molarity = 100 g / (39.997 g/mol) / (100 ml / 1000 ml/L)
Molarity = 2.501 M
Calculate moles of sodium hydroxide:
Moles of NaOH = Molarity x Volume (L) = 2.501 M x 0.100 L = 0.250 moles of NaOH
Calculate moles of sodium carbonate required to replace NaOH:
1 mole of NaOH requires 1.22 moles of Na2CO3.
Moles of Na2CO3 = 1.22 x Moles of NaOH = 1.22 x 0.250 moles = 0.305 moles of Na2CO3
Calculate mass of sodium carbonate required:
Mass of Na2CO3 = Moles of Na2CO3 x Molecular mass of Na2CO3 = 0.305 moles x 105.9888 g/mol = 32.30 g
So, you will need
32.30 g of sodium carbonate to replace the 100 g of sodium hydroxide. You can dissolve this amount of sodium carbonate in
100 ml of water to achieve a similar concentration as the original NaOH solution.
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