Describe the preparation of 100 mL of 6.0 M HCL from a concentrated solution that has a specific gravity of 1.18 and is 37% (w/w) HCL
Ans.: (1000mL/1L)(1.18 g/mL)(0.37)(1mol HCl/36.5 g HCl) = 11.96 M
We want to make 100 mL of 6.0 M: 600 mmol HCl required
V x M = V x M 100 mL x 6.0 mmol/mL = V x 11.96 M
V = 50.17 mL Therefore, take 50 mL of the conc. HCl and dilute to exactly 100.0 mL with water.
Good
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Well, well, well! Looks like it's time to mix things up! Here's how you can entertain yourself while preparing that HCL concoction:
1. Put on your lab safety goggles and your favorite clown wig. Safety first, silliness second!
2. Since we have a concentrated HCL with a specific gravity of 1.18, you'll need to calculate the mass of HCL needed for your 100 mL solution. But remember, this concentration is given as % w/w. So, channel your inner comedian and converting the percentage to grams by assuming you have 100 grams of the concentrated solution.
3. Get ready to laugh at some math! Multiply the mass of the solution (100 g) by the percentage of HCL (37%) to get the mass of HCL you have in grams. Then divide this result by the specific gravity (1.18) to find the volume of pure HCL you'll need to make your solution.
4. Now, it's time to clown around with the volume measurements. Grab your favorite 100 mL volumetric flask. It's like a party cup, but more precise!
5. Pour a splash of distilled water into the flask, enough to cover the bottom. Remember, everyone needs a little hydration!
6. Using a funnel, slowly add the calculated volume of pure HCL to the flask. Be careful not to spill any β it's not acidic, it's just "awkwirdic"!
7. Make sure to wash your hands! Safety is important, and we don't want to leave any HCL jokes on your skin!
8. After all the HCL has been added to the flask, carefully fill it up with distilled water until the bottom of the meniscus reaches the mark. Don't worry, the meniscus isn't a circus act, even though it has a funny name!
9. Once you've finished filling the flask, put a firm stopper on it. Just like a clown's hat, it keeps everything in place!
10. Shake the flask gently, but don't juggle with it β we're not in the circus here! This will help mix the solution thoroughly.
Congratulations! You've successfully prepared your 6.0 M HCL solution. Just remember to store it in a safe place, away from kids and clowns who might think it's some sort of exciting drink!
πΆπ»πΆπ = 1.18 Γ103 π πππππππ‘
πΏ πππππππ‘ Γ 37 π π»πΆπ
100 π πππππππ‘ Γ 1 πππ π»πΆπ
36.5 π π»πΆπ = 12 π
The number of moles HCl required is given by
ππ. πππ π»πΆπ = 100 ππ Γ 1 πΏ
1000 ππΏ Γ 6 πππ π»πΆπ
πΏ = 0.600 πππ π»πΆπ
Finally, to obtain the volume of concentrated reagent we write
π½πππππ
Γ πͺπππππ
= π½π
ππ Γ πͺπ
ππ
ππππππ Γ 12 πππ
πΏ = 0.600 πππ π»πΆπ
ππππππ πππππππ‘ = 0.600 πππ π»πΆπ Γ 1 πΏππππππ π‘
12 π ππ π»πΆπ = 0.0500πΏ ππ 50.0 ππΏ
Therefore, dilute 50 mL of the concentrated reagent and complete the solution with 100mL water
To prepare 100 mL of 6.0 M HCl from a concentrated solution that has a specific gravity of 1.18 and is 37% (w/w) HCl, you will need to calculate the volume and concentration of the concentrated solution you will need.
First, let's calculate the mass of the concentrated solution needed:
1. Determine the mass of the 100 mL solution using its specific gravity:
Mass = Volume x Density
Mass = 100 mL x 1.18 g/mL = 118 g
(Note: The specific gravity is the ratio of the density of a substance to the density of a reference substance, usually water in this case)
2. Determine the mass of HCl within the 100 mL solution:
Mass of HCl = Mass of solution x % HCl
Mass of HCl = 118 g x 37% = 43.66 g
Next, let's calculate the volume and concentration of the concentrated HCl solution needed for the desired 6.0 M HCl solution:
3. Calculate the number of moles of HCl needed for the desired solution:
Moles of HCl = Volume of final solution x Molarity of final solution
Moles of HCl = 100 mL x 6.0 mol/L = 0.6 mol
4. Calculate the volume of concentrated HCl solution needed:
Moles of HCl = Volume of concentrated solution x Molarity of concentrated solution
Volume of concentrated solution = Moles of HCl / Molarity of concentrated solution
Volume of concentrated solution = 0.6 mol / (37 g/mol) = 16.22 mL
Finally, to prepare the 100 mL of 6.0 M HCl solution:
- Measure out 16.22 mL of the concentrated HCl solution, using a measuring cylinder or pipette.
- Add the measured amount to a container.
- Then, add distilled water while stirring until the total volume reaches 100 mL.
Note: It is essential to handle and dilute concentrated acids with caution, using appropriate safety measures such as wearing gloves, goggles, and working in a well-ventilated area.