Question

1. How many grams of calcium chloride (CaCl2) are there in 600.0 mL of an aqueous solution that has a concentration of 0.450 M CaCl2?

2. The conjugate base of HS- is:

3. What mass of calcium chloride, CaCl2, is needed to prepare 3.65 L of a 1.75 M solution?
The molar mass of calcium chloride is 111.0 g/mol.

Answer 1

1. mols CaCl2 = M x L = ?
Then grams = mols x molar mass

2. The base is what's left after the H is gone.

3. How many mols do you need? That's mols = M x L
How many grams is that many mols? That's grams = mols x molar mass = ?

Answer 2

mxl=270
so the answer to 1. is 270?
so the answer to 2. is S2-?
so the answer to 3. is 6.3875?

Answer 3

1. You forgot to change 600 mL to L. The answer is 0.270 mols.
2. is yes
3. I don't get your answer.
M x L = 1.75 x 3.65 = ?
? x molar mass = ? x 111 = approx 710 grams.

Answer 4

1. is incorrect, it is not .270, i have one more chance on my practice sheet to answer this.

2. was good, thanks

Answer 5

You misunderstood on 1.
mols = M x L = 0.600 x 0.450 = 0.270.

Then you omitted the second step which I wrote in my first response which is
grams = mols x molar mass = ?
That will be grams = 0.270 x molar mass CaCl2 = ?

Answer 6

i got 29.9646 from your explaination on 1

Answer 7

is that correct?