Ca(OCl)2 + 2NaCl + 2H2SO4 <=> 2Cl2 + CaSO4 + NaSO4 + 2H2O

[We have to prepare 12 ml of 0.050 M Cl2 (Chlorine water) ]
[We are given "solid Ca(OCl)2" , "0.20 M NaCl" and "0.50 M H2SO4" and "D-I water"]

What is the required quantity of Ca(OCl)2, NaCl and H2SO4 and volume of D-I water to be used??

I tried it myself but I'm not sure it is the right steps...please check

1st - I used 0.050 mol/1 L x .012 L to get .00060 mol Cl2

2nd - To get the Ca(OCl)2 grams I used the 1:2 ratio and figured that there is .00030 mol Ca(OCl)2. I multiplied it with 142.98 g molar mass and got ".043 grams Ca(OCl)2"

3rd - I used the 2:2 ratio and think that there is .00060 NaCl. I multiplied it with 1L/.20 mol and got ".0030 L NaCl"

4th - I used the 2:2 ratio again and used .00060 H2SO4. I multiplied 1L/.50 mol and got ".0012 L H2SO4"

5th - Knowing this I wrote that we needed 7.8 ml to create the 12ml Chlorine solution.

I would modify your procedure.

I agree that you want 0.00060 (don't forget the final 0) mol Cl2.
Note that 1/2 of the 2 Cl2 comes from Ca(OCl)2 and the other half of the 2Cl2 comes from the 2NaCl.
0.00030 x molar mass Ca(OCl)2 = about 43 mg.
For NaCl, 0.0030 mol Cl2/2 = mols NaCl and you can go from there.
For H2SO4 you want twice the mols Ca(OCl)2 or 0.0006 so I think that part is ok, too.

I think everything is good, but the equation is not balanced, Check Na (Sodium).

To determine the quantity of Ca(OCl)2, NaCl, H2SO4, and volume of D-I water needed to prepare 12 ml of 0.050 M Cl2 (chlorine water), we need to use the balanced chemical equation you provided.

The balanced chemical equation is:
Ca(OCl)2 + 2NaCl + 2H2SO4 → 2Cl2 + CaSO4 + NaSO4 + 2H2O

From the equation, we can see that the molar ratio between Ca(OCl)2 and Cl2 is 1:2. This means that for every 1 mole of Ca(OCl)2, we will produce 2 moles of Cl2.

Step 1: Calculate the moles of Cl2 needed:
We know that the desired final volume of Cl2 is 12 ml, and the desired concentration is 0.050 M. So, we can convert the volume to liters:
12 ml = 12/1000 L = 0.012 L

Now, use the formula C = n/V to calculate the moles of Cl2:
0.050 M = n/0.012 L

Rearranging the equation, we find:
n = 0.050 M × 0.012 L = 0.0006 moles

Since the molar ratio between Ca(OCl)2 and Cl2 is 1:2, we need twice as many moles of Cl2 as Ca(OCl)2. Therefore, we need 0.0006 moles of Ca(OCl)2.

Step 2: Calculate the required quantity of Ca(OCl)2:
From the molar mass of Ca(OCl)2 (110.98 g/mol), we can calculate the mass of Ca(OCl)2 in grams:
Mass = Moles × Molar mass = 0.0006 moles × 110.98 g/mol

Step 3: Calculate the required quantity of NaCl and H2SO4:
According to the balanced chemical equation, the molar ratio between NaCl and Cl2 is 2:2, and the molar ratio between H2SO4 and Cl2 is 2:2. This means that we need an equal number of moles for NaCl and H2SO4 as Cl2.

Step 4: Calculate the volume of D-I water:
To calculate the volume of D-I water required, subtract the volume of the other components (Ca(OCl)2, NaCl, and H2SO4) from the total desired volume of Cl2 (12 ml).

Remember to thoroughly mix the solutions to achieve the desired concentration and volume.

Note: It is important to handle the chemicals safely and follow appropriate lab procedures while performing this experiment.