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I need help with 2 but 1 tells you other measurements

I need help with 2 but 1 tells you other measurements

Curren'S Math For Meds: Dosages & Sol
Curren'S Math For Meds: Dosages & Sol
11th Edition
ISBN:9781305143531
Author:CURREN
Publisher:CURREN
Chapter9: Parenteral Medication Labels And Dosage Calculation
Section: Chapter Questions
Problem 2.5P
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I need help with 2 but 1 tells you other measurements

Name: Procedure: 1. Begin by measuring out approximately 0.40 g of copper (II) sulfate and dissolve it in 300-400 mL ọf water to make a solution of CuSO4. Note the formula of the solid: if the solid is light blue-green, then it is CUSO4, but if instead the solid is provided as blue crystals then it is actually CuSO4 5H2O; if in doubt, ask your instructor because the molecular weight of the solid will differ. 2. Use the mass of your solid to calculate the volume of 0.20 M NaOH solution required to fully react with the CUSO4. Then add 5 mL to that value and go acquire that volume of NaOH solution (we want to make sure that the copper is the limiting reactant, so use an excess of NaOH). VO Mot 3. Now carefully add the NAOH solution to the beaker containing the CUSO4. You have just caused the precipitation reaction between CUSO4 and NaOH! Stir the mixture gently, then allow the solid to settle. 4. After the precipitate has had some time to settle, inspect the solution. If the solution is still tinted blue then there may be some copper ions that did not react with the NaOH; in that case, allow it to settle and add a few more mL of NaOH until no more precipitate is formed (you want to make sure you precipitate all the copper so it's OK to overdo it with the NaOH). If the solution is clear then you can assume that the reaction is complete and that all the copper has been precipitated.
Transcribed Image Text:Name: Procedure: 1. Begin by measuring out approximately 0.40 g of copper (II) sulfate and dissolve it in 300-400 mL ọf water to make a solution of CuSO4. Note the formula of the solid: if the solid is light blue-green, then it is CUSO4, but if instead the solid is provided as blue crystals then it is actually CuSO4 5H2O; if in doubt, ask your instructor because the molecular weight of the solid will differ. 2. Use the mass of your solid to calculate the volume of 0.20 M NaOH solution required to fully react with the CUSO4. Then add 5 mL to that value and go acquire that volume of NaOH solution (we want to make sure that the copper is the limiting reactant, so use an excess of NaOH). VO Mot 3. Now carefully add the NAOH solution to the beaker containing the CUSO4. You have just caused the precipitation reaction between CUSO4 and NaOH! Stir the mixture gently, then allow the solid to settle. 4. After the precipitate has had some time to settle, inspect the solution. If the solution is still tinted blue then there may be some copper ions that did not react with the NaOH; in that case, allow it to settle and add a few more mL of NaOH until no more precipitate is formed (you want to make sure you precipitate all the copper so it's OK to overdo it with the NaOH). If the solution is clear then you can assume that the reaction is complete and that all the copper has been precipitated.
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