he 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
this is basically my whole experiment hope this helps
OK. This is the experiment. The questions are here and there on the board. If you will copy your above post to a new one and add the questions at the end, I will try and go through it, at least for the first question to get you started. It's so many steps I'm confused before we start. It will help if you also give your take on each question you post so I can see what you are thinking. That way I can prepare a better answer if I know what you don't understand.
Based on the information you provided, it seems like you have conducted a series of reactions to prepare copper (II) hydroxide and eventually obtain copper. Here's a breakdown of the procedure:
Part A: Preparation of Copper (II) Hydroxide
1. Obtain a solution of copper (II) nitrate.
2. Measure 25 mL of the copper (II) nitrate solution.
3. Add 2 mL of concentrated sodium hydroxide (NaOH) to the blue solution while stirring.
4. Allow the mixture to settle and test its 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 and stir well, then allow the mixture to settle.
7. Pour off a major portion of the clear, colorless liquid into another beaker.
8. Save the precipitate and residual liquid for Part B.
Part B: Formation of Copper (II) Sulfate
1. Add dilute (3M) sulfuric acid (H2SO4) to the beaker containing the suspension of Cu(OH)2, while stirring.
2. Save the resulting color solution of copper (II) sulfate for Part C.
Part C: Formation of Copper (II) Phosphate
1. Add 6M NaOH to the colored solution from Part B with constant stirring until a small amount of blue color is visible.
2. Add about 10 mL of sodium phosphate (Na3PO4) solution while stirring thoroughly.
3. Test the resulting mixture with litmus paper.
Part D: Filtration and Washing
1. Add 15 mL of 6M hydrochloric acid (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 the CuCl2 solution.
Part E: Drying and Weighing
1. To the CuCl2 solution, add 4 or 5 pieces of magnesium turnings while keeping them submerged using the tip of a stirring rod.
2. Add the minimum possible quantity of concentrated (12M) HCl to destroy the excess magnesium.
3. Allow the copper to settle, then discard the major part of the liquid.
4. Wash the solid copper dust four times with 15 mL portions of de-ionized water.
5. Drain as much water as possible, leaving behind the copper.
6. Place the beaker with the copper on a hot plate and heat it until completely dry.
7. After the beaker has cooled, weigh it to the nearest 0.001g and record the mass.
8. Transfer all the dried copper onto weighing paper.
Based on the calculations provided at the end, you determined the mass of the copper obtained and calculated the percent yield, which was 97.2%.
Note: It's important to make sure you follow all necessary safety precautions while conducting chemical experiments and handling chemicals.