Answer: 19.4 mL Ba(OH)2
Explanation:
H2(g) + Cl2(g) --> 2HCl(aq) (make sure this equation is balanced first)
At STP, 1 mol gas = 22.4 L gas. Use this conversion factor to convert the 100. mL of Cl2 to moles.
0.100 L Cl2 • (1 mol / 22.4 L) = 0.00446 mol Cl2
Use the mole ratio of 2 mol HCl for every 1 mol Cl2 to find moles of HCl produced.
0.00446 mol Cl2 • (2 mol HCl / 1 mol Cl2) = 0.00892 mol HCl
HCl is a strong acid and Ba(OH)2 is a strong base so both will completely ionize to release H+ and OH- respectively. You need 0.00892 mol OH- to neutralize all of the HCl. Note that one mole of Ba(OH)2 contains 2 moles of OH-.
0.00892 mol OH- • (1 mol Ba(OH)2 / 2 mol OH-) • (1 L Ba(OH)2 / 0.230 M Ba(OH)2) = 0.0194 L = 19.4 mL Ba(OH)2
Total in pot=28 L
400 mL in each bowl
16 bowls filled
1000mL=1L
16 bowls(400mL/1 bowl)=6400mL
6400mL(1L/1000mL)=6.4L
28L-6.4L=21.6 L
Answer:
5.51mol/L
Explanation:
Number of moles = 1.35moles
Volume of the solution = 245mL = 245*10^-3L = 0.245L
Molarity of a solution is the defined as the number of moles of a solute dissolved in 1L of the solution.
1.35 moles = 0.245L
X moles = 1L
X = (1.35 * 1) / 0.245
X = 5.51mol/L
The molarity of the solution is 5.51mol/L
Answer: dipole-induced-dipole interactions
When a polar molecule results to a redistribution of the charges in a nonpolar molecule, the molecules in the mixture could be possibly experiencing a dipole-induced-dipole interactions. This means, that such interaction greatly lies on the existence of a polar molecule.
