Which is more concentrated, a solution (1) prepared by dissolving 21.0 g of naf (0.500 mol) in enough water to make 500 ml of solution or a solution (2) prepared by dissolving 10.5 g (0.250 mol) of naf in enough water to make 100 ml of solution?

Answer:

A solution (2) prepared by dissolving 10.5 g (0.250 mol) of naf in enough water to make 100 ml of solution is more concentrated.

Explanation:

Calculate the molarity of Solution 1

                      M = (moles)× 1000/ V (ml)

                      M =  (0.500) × 1000/500 = 1 M

Calculate the molarity of Solution 2

                     M = (moles)× 1000/ V (ml)

                     M =  (0.250) × 1000/100 = 2.5 M

Result:

As the molarity of Solution two is greater than solution 1. so Solution 2 is more concentrated

Answer:

A solution (2) prepared by dissolving 10.5 g (0.250 mol) of naf in enough water to make 100 ml of solution is more concentrated.

Explanation:

Calculate the molarity of Solution 1

                      M = (moles)× 1000/ V (ml)

                      M =  (0.500) × 1000/500 = 1 M

Calculate the molarity of Solution 2

                     M = (moles)× 1000/ V (ml)

                     M =  (0.250) × 1000/100 = 2.5 M

Result:

As the molarity of Solution two is greater than solution 1. so Solution 2 is more concentrated

Iam not sure butch i thinnk it is ab

Spontaneity tell us the direction of the reaction, but not how fast it goes. gibbs free energy brings together enthalpy, entropy and temperature in one easy formula. g = h - ts. and, finally the sign of delta g is always negative for a spontaneous reaction.