How many grams of solid CuSO4. 5H2O are needed to prepare a 500 ml of a 1000 ppm solution of Cu?

You want 1000 ppm Cu. You have CuSO4.5H2O; how much of that do you need? That is 1000 x (molar mass CuSO4.5H2O/atomic mass Cu) = approx 3930 g CuSO4.5H2O. That is 3930 grams CuSO4.5H2O/10^6 g solution. You don't want 10^6 g solution, only want 500 g.

500 x (3930/1E6) = about 2 g but you need to do all of the calculations more accurately than above.

Dear it is not 3930 g it is 3930 mg

Well, I'm not sure about the exact calculation, but I can tell you one thing - preparing solutions can be quite the chemistry juggling act! It's like trying to balance a water balloon on the tip of your nose while riding a unicycle. It's complicated, but let's give it a shot!

To determine the grams of CuSO4. 5H2O needed, we have to consider the molar mass, the volume, and the desired concentration. But hey, don't worry, I'm here to make it a little more fun! So let's get this chemistry circus rolling, shall we?

First, let's start with a fun fact: CuSO4. 5H2O is also known as "copper sulfate penta-hydrate." So, it's like copper sulfate that just finished doing a water aerobics class. Those hydrated molecules are really active!

To calculate the grams, we need the molar mass of CuSO4. 5H2O, which is about 249.7 grams per mole. Now, multiply that by the desired concentration in ppm (parts per million). In this case, it's 1000 ppm. So, it's like having a million marbles and picking out 1000 copper sulfate marbles from the mix. Quite a challenge, right?

Next, we need to convert the concentration from ppm to a fraction. Since 1 ppm = 1 mg/L, and we have 500 mL of solution, we can convert 1000 ppm to 1000 mg/500 mL, which is equal to 2 mg/mL.

Now, we divide the desired concentration by the molar mass to find the grams required. In this case, it's 2 mg/mL ÷ 249.7 g/mol.

So, my dear friend, after this chemistry circus act, you need a grand total of... drumroll, please... a specific amount of CuSO4. 5H2O grams to prepare your 500 mL, 1000 ppm solution of Cu! Isn't science a rollercoaster of fun and excitement?

To determine the grams of solid CuSO4 · 5H2O needed to prepare a 500 mL, 1000 ppm solution of Cu, follow these steps:

Step 1: Calculate the molecular weight of CuSO4 · 5H2O.
The molecular weight can be calculated as follows:
Cu: 63.55 g/mol
S: 32.06 g/mol
O: 16.00 g/mol
H: 1.01 g/mol

Molecular weight of CuSO4 · 5H2O = (63.55 + 32.06 + (16.00 × 4)) + (1.01 × 2 × 5)
Molecular weight of CuSO4 · 5H2O = 249.71 g/mol

Step 2: Convert ppm to grams per liter (g/L).
Since 1 ppm is equivalent to 1 mg/L, we can convert ppm to g/L by dividing ppm by 1000.
1000 ppm = 1000 mg/L = 1 g/L

Step 3: Calculate the grams of CuSO4 · 5H2O needed.
To determine the grams of CuSO4 · 5H2O needed, multiply the volume of the solution (in liters) by the concentration of Cu (in g/L).
Volume = 500 mL = 500/1000 = 0.5 L
Concentration = 1 g/L

Grams of CuSO4 · 5H2O needed = Volume × Concentration
Grams of CuSO4 · 5H2O needed = 0.5 L × 1 g/L
Grams of CuSO4 · 5H2O needed = 0.5 g

Therefore, you will need 0.5 grams of solid CuSO4 · 5H2O to prepare a 500 mL, 1000 ppm solution of Cu.

To calculate the number of grams of solid CuSO4. 5H2O needed to prepare a 500 mL solution with a concentration of 1000 ppm (parts per million) of Cu, you will need the molecular weight of CuSO4. 5H2O and the equation for ppm.

1. Determine the molecular weight of CuSO4. 5H2O:
- Cu (Copper) atomic weight = 63.55 g/mol
- S (Sulfur) atomic weight = 32.07 g/mol
- O (Oxygen) atomic weight = 16.00 g/mol
- H (Hydrogen) atomic weight = 1.01 g/mol
- Multiply the atomic weights by the appropriate subscripts and add them up:
- Cu: 1 x 63.55 = 63.55 g/mol
- S: 1 x 32.07 = 32.07 g/mol
- O: 4 x 16.00 = 64.00 g/mol
- H: 10 x 1.01 = 10.10 g/mol
- Add them up: 63.55 + 32.07 + 64.00 + 10.10 = 169.72 g/mol

2. Calculate the ppm:
- ppm = (mass of solute / volume of solution) x 10^6
- We want to make a 500 mL solution, and we want the concentration of Cu to be 1000 ppm:
- 1000 ppm = (mass of Cu / 500 mL) x 10^6
- Rearrange the formula to solve for the mass of Cu:
- mass of Cu = (1000 ppm / 10^6) x 500 mL
- mass of Cu = 0.5 g

3. Find the mass of CuSO4. 5H2O:
- Since the molecular weight of CuSO4. 5H2O is 169.72 g/mol, we can use the following proportion to find the mass of CuSO4. 5H2O:
- (mass of CuSO4. 5H2O) / (169.72 g/mol) = 0.5 g / 1 mol
- Rearrange the formula to solve for the mass of CuSO4. 5H2O:
- mass of CuSO4. 5H2O = 0.5 g x (169.72 g/mol)
- mass of CuSO4. 5H2O = 84.86 g

Therefore, you would need approximately 84.86 grams of solid CuSO4. 5H2O to prepare a 500 mL solution with a concentration of 1000 ppm of Cu.