Answer:
The intermolecular forces between CO3^2- and H2O molecules are;
1) London dispersion forces
2) ion-dipole interaction
3) hydrogen bonding
Explanation:
Intermolecular forces are forces of attraction that exits between molecules. These forces are weaker in comparison to the intramolecular forces, such as the covalent or ionic bonds between atoms in a molecule.
Considering CO3^2- and H2O, we must remember that hydrogen bonds occur whenever hydrogen is bonded to a highly electronegative atom such as oxygen. The carbonate ion is a hydrogen bond acceptor.
Also, the London dispersion forces are present in all molecules and is the first intermolecular interaction in molecular substance. Lastly, ion-dipole interactions exists between water and the carbonate ion.
Answer:
Explanation: There are 2 moles of C6H12O6 in 300 g C6H12O6 , rounded to one significant figure.
When you calculate the first two numbers in 493×10
We consider the given reaction H2SO4 + 2 NaOH -> Na2SO4 + 2H2O as applies to an acid-base titration.
moles NaOH = c · V = 0.2767 mmol/mL · 25.34 mL = 7.011578 mmol
moles H2SO4 = 7.011578 mmol NaOH · 1 mmol H2SO4 / 2 mmol NaOH
= 3.505789 mmol
Hence
[H2SO4]= n/V = 3.505789 mmol / 39.54 mL = 0.08866 M
The answer to this question is [H2SO4] = 0.08866 M
