I need help with my homework **Report Sheet for Density and Mass Calculations****Procedure A:**- **Weight of Water needed (show calculations):** *(Space for calculations)*- **Weight of Salt needed (show calculations):** *(Space for calculations)*- **Weight of beaker:** - 78.31 g- **Weight of beaker & 10.0 ml of salt solution:** - 88.29 g- **Weight of 10.0 ml salt solution:** *(Calculations needed here)*- **Density of 10% salt solution:** *(Space for density calculation)*- **Reference Value:** - 1.07 g/ml- **% Error (show calculations):** *(Space for error calculations)***Procedure B:**- **Mass of CuSO₄·5H₂O needed (show calculations):** *(Space for calculations)*This report sheet is used to record the weight measurements and calculate the density and percent error of a 10% salt solution as well as determine the mass needed for a chemical experiment involving copper(II) sulfate pentahydrate (CuSO₄·5H₂O). Please fill in the calculations and observations in the spaces provided for a complete analysis. **Solutions Online Lab Instructions****PROCEDURE A: Preparation of 50 g of a 10.0% salt solution.**1. Calculate the amount of salt and water needed.2. Weigh the calculated amount of salt onto a weighing paper to protect the balance pan.3. Weigh the calculated amount of water in a beaker.4. Add the weighed amount of salt and stir until the salt dissolves.5. Pipet 10.0 ml of the salt solution into another weighed beaker and determine the weight of the salt solution.6. Determine the density of your salt solution. (Density = mass/volume)7. Find the reference value of a 10% salt solution and calculate the percentage error.**PROCEDURE B: Preparation of 50.0 ml of 1.0 M CuSO₄.**1. Calculate the amount of CuSO₄ needed to make 50.0 ml of a 1.00 M solution. CuSO₄•5H₂O molecular weight = 250 g/mole.2. Tare a small beaker. Do not remove it from the balance.3. Slowly pour CuSO₄ into the beaker until it reads the correct weight.4. Dissolve the weighed CuSO₄ in 25-30 ml of distilled water.5. Transfer to a volumetric flask through a funnel. *If you spill any, you must start again.*6. Rinse the funnel into the flask with a stream of distilled water.7. Add distilled water to the mark. Add the last few drops carefully with a dropper.8. Use this standard solution to prepare more dilute solutions of CuSO₄ in procedure C.**PROCEDURE C: Preparation of more dilute solutions of CuSO₄**1. Calculate the size of the aliquot needed to prepare 50.0 ml of 0.50 M CuSO₄ solution from your standard solution.2. Pour a small amount of your standard solution into a small beaker and pipet the calculated aliquot from the beaker to a clean 50 ml volumetric flask. Dilute to volume.3. Stopper the flask, invert and swirl.4. Repeat the above steps to prepare 0.25 M and 0.10 M CuSO₄ solutions.5. Measure the absorbance of all four solutions that you have prepared.**PRO

Mass of salt present in 100 g of salt solution = 10 g Mass of salt present in 1 g of salt solution = 0.1 g Mass of salt present in 50 g of salt solution = 5 g Mass of solution = 50 g Mass of solvent = Mass of solution – mass of solute Mass of solvent = 50 – 5 = 45 g Weight of salt needed = 5 g Weight of water needed = 45 gWeight of beaker = 78.31 g Weight of beaker + weight of 10 ml salt solution = 88.29 g Weight of 10 ml salt solution = 88.29 – 78.31 = 9.98 g Density of salt solution is obtained by dividing the mass of salt solution by volume of salt solution. The density of salt solution as calculated in the salt solution experiment is equal to 9.98/10 = 0.998 g/ml. The reference/actual value is 1.07 g/ml The percentage error can be calculated as follows: Percent error = Reference value - Calculated valueReference value × 100= 1.07 - 0.9981.07 × 100= 0.0721.07 × 100= 6.73%