Na2CO3 + 2HCl ==> 2NaCl + H2O + CO2
1. What is the concentration of hydrochloric acid in moldm3?
Don't know and can't calculate it without knowing how much HCl was used in the titration.
2.The mass of concentration of sodium trioxocarbonate iv solution?
You had 0.1 molar Na2CO3. One mole has a mass of 1 mol which is approximately 106 grams. So you have 0.1 x 106 = ? grams Na2CO3 in the solution. But you used only 25 cc of that solution so you had moles = M x L = 0.1M x 0.025 L = moles Na2CO3. grams = moles x molar mass = ?
3. The mass of H+ formed from 1dm3 of the acid?
Don't know since we don't know the molarity of the HCl.
4. The mass of salt formed in the solution during titration?
Assuming you have enough HCl to use all of the Na2CO3 then you will have moles Na2CO3 x 2 = moles NaCl and mols NaCl x molar mass NaCl = grams NaCl.
Post your work if you get stuck. And remember to let me know the source of that funny (and incorrect) name for Na2CO3.
25.0cm³ portions of 0.100mol in 1000cm³ solution of sodium trioxocarbonate(iv) were titrated against hydrochloric acid solution
What is the concentration of hydrochloric acid in moldm3?
The mass of concentration of sodium trioxocarbonate iv solution?
The mass of H+ formed from 1dm3 of the acid?
The mass of salt formed in the solution during titration?
1 answer
1 answer