the experiment is a sequence of Chemical Reactions. Procedure part A preparation fo copper (II) Hydroxide-get a solution of copper(II)nitrate. measure 25ml of solution. to blue solution add 2mL of concertarted NaOH while stirring. Let mixture settle and use litmus paper to test acidity. add addition 10 drop portions of 6M NaOH while stirring until basic. Add 30 mL of water to beaker stir well and allow misture to settle. pour off major part of clear, colorless liquid into a beaker. Save precipitate and residual liquid for part B. Part B-Add dilute (3M) H2SO4 with constant stirring to beaker containing supsension of Cu(OH)2. save color solution of CuSO4 for part C. Part C-add 6M NaOH with constant stirring to colored solution from B until a small amount of blue is visable. Add about 10mL of Na3PO4 solution stirring thoroughly. test with litmus paper. Part D-Add 15mL of 6M HCl to solution from part C. When precipitate is gone filter solution using long stemmed glass funnel and filter paper. Wash filter paper with 20 drops of de-ionized water through filter into beaker containing CuCl2 solution. Part E-to solution CuCl2 add 4 or 5 pieces of magnsium turning and keep them submerged with tip of stirring rod. Add minumum possible quality of concentrated (12M) HCl, to destro excess magnesium. Allow copper to settle. Discard major part of liquid and wash solid copper dust 4 times with 15mL portions of de-ionized water. drain as much water as possible leaving behind copper. place beaker on hot plate and heat until completely dry. after cooled weigh to nearest .001g and record mass. transfer all dried copper onto weighing paper.

Mass of beaker with copper=57.758g
Mass of copper=.243g
.157M X.025L=.003925mols
.003925molsX (1 molCu/i mol Cu(NO3)2) X (63.55g Cu/1 mol Cu)=.25
.243/.25=97.2 % yield

Here is a step-by-step breakdown of the procedure for the experiment:

Part A - Preparation of Copper (II) Hydroxide:
1. Start with a solution of copper(II) nitrate.
2. Measure 25 mL of the copper(II) nitrate solution.
3. Add 2 mL of concentrated NaOH slowly to the blue solution while stirring.
4. Allow the mixture to settle and test the acidity using litmus paper.
5. Add 10 drop portions of 6M NaOH while stirring until the solution becomes basic.
6. Add 30 mL of water to the beaker, stir well, and allow the mixture to settle.
7. Pour off the major part of the clear, colorless liquid into a separate beaker. Save the precipitate and residual liquid for Part B.

Part B - Formation of Copper (II) Sulfate:
1. Add diluted (3M) H2SO4 to the beaker containing the suspension of Cu(OH)2, while constantly stirring.
2. Save the resulting colored solution of CuSO4 for Part C.

Part C - Formation of Copper (II) Phosphate:
1. Add 6M NaOH to the colored solution from Part B, while constantly stirring until a small amount of blue color is visible.
2. Add about 10 mL of Na3PO4 solution and stir thoroughly.
3. Test the solution with litmus paper.

Part D - Precipitation and Filtration:
1. Add 15 mL of 6M HCl to the solution from Part C.
2. When the precipitate disappears, filter the solution using a long-stemmed glass funnel and filter paper.
3. Wash the filter paper with 20 drops of de-ionized water through the filter into a beaker containing CuCl2 solution.

Part E - Drying and Weighing of Copper:
1. To the CuCl2 solution, add 4 or 5 pieces of magnesium turnings and keep them submerged with the tip of a stirring rod.
2. Add the minimum possible quantity of concentrated (12M) HCl to destroy any excess magnesium.
3. Allow the copper to settle.
4. Discard the major part of the liquid and wash the solid copper dust 4 times with 15 mL portions of de-ionized water.
5. Drain as much water as possible, leaving behind the copper.
6. Place the beaker containing the copper on a hot plate and heat until completely dry.
7. After cooling, weigh the dried copper to the nearest 0.001g and record the mass.
8. Transfer all the dried copper onto a weighing paper.

Calculation:
1. Mass of beaker with copper = 57.758g
2. Mass of copper = 0.243g
3. Calculate the moles of copper: 0.157M x 0.025L = 0.003925 moles
4. Determine the theoretical yield of copper:
- 0.003925 moles x (1 mol Cu / 1 mol Cu(NO3)2) x (63.55g Cu / 1 mol Cu) = 0.25g
5. Calculate the percent yield:
- (0.243g / 0.25g) x 100% = 97.2% yield

In the given experiment, you are preparing copper(II) hydroxide and determining the yield of copper obtained. Let's break down the procedure and calculations step by step:

Part A:
1. Get a solution of copper(II) nitrate.
2. Measure 25 mL of the solution.
3. Add 2 mL of concentrated NaOH to the blue solution while stirring.
4. Let the mixture settle and use litmus paper to test the acidity.
5. Add 10 drop portions of 6M NaOH while stirring until it becomes basic.
6. Add 30 mL of water to the beaker, stir well, and allow the mixture to settle.
7. Pour off the major part of the clear colorless liquid into another beaker.
8. Save the precipitate (copper(II) hydroxide) and the residual liquid for Part B.

Part B:
1. Add dilute (3M) H2SO4 with constant stirring to the beaker containing the suspension of copper(II) hydroxide.
2. Save the resulting colored solution of CuSO4 for Part C.

Part C:
1. Add 6M NaOH with constant stirring to the colored solution from Part B until a small amount of blue color is visible.
2. Add about 10 mL of Na3PO4 solution and stir thoroughly.
3. Test the resulting solution with litmus paper.

Part D:
1. Add 15 mL of 6M HCl to the solution from Part C.
2. When the precipitate (copper phosphate) dissolves, filter the solution using a long-stemmed glass funnel and filter paper.
3. Wash the filter paper with 20 drops of de-ionized water through the filter into a beaker containing CuCl2 solution.

Part E:
1. To the CuCl2 solution, add 4 or 5 pieces of magnesium turning and keep them submerged with the tip of a stirring rod.
2. Add the minimum possible amount of concentrated (12M) HCl to destroy excess magnesium.
3. Allow the copper to settle.
4. Discard the major part of the liquid and wash the solid copper dust 4 times with 15 mL portions of de-ionized water.
5. Drain as much water as possible, leaving behind the copper.
6. Place the beaker on a hot plate and heat until the copper is completely dry.
7. After cooling, weigh the copper to the nearest 0.001 g and record the mass.

Calculations:
1. Mass of beaker with copper = 57.758 g
2. Mass of copper = 0.243 g

To determine the yield of copper:
1. Calculate the moles of Cu(NO3)2 using the concentration and volume:
0.157 M x 0.025 L = 0.003925 moles
2. Convert moles of Cu(NO3)2 to moles of Cu using the molar ratio:
0.003925 moles x (1 mol Cu/1 mol Cu(NO3)2) = 0.003925 moles Cu
3. Convert moles of Cu to grams of Cu using the molar mass:
0.003925 moles Cu x (63.55 g Cu/1 mol Cu) = 0.24990 g Cu
4. Calculate the percent yield of copper:
(Actual mass of copper obtained / Theoretical mass of copper) x 100%
0.243 g / 0.24990 g x 100% = 97.2% yield

Therefore, the percent yield of copper obtained in the experiment is 97.2%.