The density of a solution of 3.69g KBr in 21.70g H2O is 1.11g/mL. What is the molarity of KBr in the solution.
4 answers
See your other post above.
0.2M
Mass of solution
= 3.69g + 21.70g
=25.39 g
Volume of solution
= 25.39g / 1.11g/mL
=22.9 mL
= 0.0229 L
Moles KCl
= 3.69 g / 74.5513g/mol
= 0.0494961 mol
Molarity of KCl
= 0.0494961 mol / 0.0229L
= 2.1614 mol/L
= 3.69g + 21.70g
=25.39 g
Volume of solution
= 25.39g / 1.11g/mL
=22.9 mL
= 0.0229 L
Moles KCl
= 3.69 g / 74.5513g/mol
= 0.0494961 mol
Molarity of KCl
= 0.0494961 mol / 0.0229L
= 2.1614 mol/L
Now just do that for KBr instead of KCl i.e change the molecular weight in step 3
0 answers