What is the concentration of the solution prepared from combining 26.5

millilitres of six molar H2SO4 with 95 millilitres of water.

Assume volumes are additive.

Now when I look at this problems there's a couple of clues that are telling me

what kind of problem this is.

It's asking about a concentration.

And it only talks about one particular substance, this H2SO4,

and that we're adding more water.

So we're adding water to a solution or adding more solvent.

This indicates that we're dealing with a dilution problem.

So when I have a dilution problem I can use the equation C1V1 equals C2V2.

Now, I'm given my initial concentration of 6 molar and

my initial volume of 26.5 millilitres.

And I don't actually have to change that to liters as long as my volume units for

both V1 and V2 are the same.

Now, it's asking for the concentration of the final solution, so C2s are unknown.

And the key here is that, for

the volume is that we have to look at this as 95.0 plus 26.5 millilitres.

Notice that it doesn't tell us that 95 millilitres is the final volume.

It's saying we're combining the 26.5 and the 95 millilitres of water.

So that means my total final volume will be the sum of those two values.

When I do the math, what I end up with C2 equals 1.3 molar,

remember I have millilitres both here and here.

My units here molarity, so my units of C2 are also going to be in units of molarity.