What is the #"molar concentration"# of a mass of #21.9g# mass of #"potassium chloride"# dissolved in #869mL# of solution?

Question

2038 views around the world

You can reuse this answer
Creative Commons License

Answer 1 · 2017-02-03T16:15:45

#"Molarity"# #=# #"Moles of solute"/"Volume of solution"#

And so we just have to plug the given numbers in, knowing that #"potassium chloride"# has a molar mass of #74.55*g*mol^-1#.

#"Molarity"# #=# #((21.9*g)/(74.55*g*mol^-1))/(0.869*L)~=0.3*mol*L^-1#.

Note that #1*mL=10^-3L#; equivalently, #1000*mL-=1.000*L#. What are the concentrations with respect to #K^(+)(aq)# and #Cl^(-)(aq)#?

What is the #"molar concentration"# of a mass of #21.9*g# mass of #"potassium chloride"# dissolved in #869*mL# of solution?