How do you find what molarity of a solution that was made by mixing 100. mL 1.0 M HCl and 150. mL of 2.0 M HCl

Question

solution?

Answer 1

Moles HCl in the first solution =

= 0.100 L x 1.0 M = 0.100

Moles HCl in the second solution =

= 0.150 L x 2.0 M = 0.300

total moles = 0.100 + 0.300 = 0.400

total volume = 0.100 + 0.150 = 0.250 L

M = 0.400 / 0.250 = 1.6 M

Answer 2

Find the total moles of HCl, then divide by the total volume. Assume that the volumes are additive.

M = mol / L

mol = M x L = 1.0 mol/L x 0.100 L = 0.100 mol

mol = M x L = 2.0 mol/L x 0.150 L = 0.300 mol

Total mol = 0.100 + 0.300 = 0.400 mol

Total volume = 100. + 150. mL = 250 mL = 0.250 L

M = mol / L = 0.400 mol / 0.250 L = 1.6 M

Answer 3

100 mL of 1.0M Hcl is 0.1 Moles. 150mL of 2.0M Hcl is 0.3moles. so it's 0.4 in 250ml times by 4 gives 1.6M HCL

Answer 4

Actually

Moles HCl in the first solution =

= 0.100 L x 1.0 M = 0.100

Moles HCl in the second solution =

= 0.150 L x 2.0 M = 0.300

total moles = 0.100 + 0.300 = 0.400

total volume = 0.100 + 0.150 = 0.250 L

M = 0.400 / 0.250 = 1.6 M