Copper(II) sulfate carries SC180's Unit 10 solution chemistry report through stock preparation, a fourfold dilution and a precipitation that closes on 0.610 g of Cu(OH)2. Searches like "sc 180 unit 10 assignment example", "sc180 unit 10 sample" and "sc180 unit 10 example" land here.
What a finished SC180 Unit 10 solution chemistry report looks like
A report of four to six pages in three linked parts, each opening with a short calculation block. Part one prepares the stock: 0.2500 L times 0.500 mol/L gives 0.125 mol, and multiplying by 249.68 g/mol for the pentahydrate gives 31.2 g, with a note that the five waters belong in the molar mass. Part two dilutes 25.00 mL of stock to 100.0 mL, using M1V1 equals M2V2 to reach 0.125 M, and explains why a volumetric flask rather than a beaker sets the final volume. Part three mixes 50.00 mL of the diluted solution with excess sodium hydroxide, writes the molecular, complete ionic and net ionic equations, and carries 0.00625 mol of copper ion to 0.610 g of precipitate. Where the section includes a bench step, the recovered mass appears as [mass recovered] beside the prediction.
How a SC180 Unit 10 example is structured
The report usually runs introduction, three calculation sections, discussion and references, with the parts presented in the order the solutions were made. The introduction defines molarity as moles of solute per liter of solution, not per liter of solvent, since that distinction determines how the stock is prepared. Each part states its given values, performs one chained calculation with units, and ends with a sentence giving the result and its precision. The equations section shows sodium and sulfate canceling as spectator ions, leaving copper and hydroxide in the net reaction in a 1:2 ratio. The discussion links the three parts, showing that an error in the stock concentration would carry through the dilution into the predicted mass, and it states the minimum 125 mL of 0.100 M sodium hydroxide required, so the claim of excess base can be verified.
Waters of hydration in the molar mass
The pentahydrate's 249.68 g/mol includes five water molecules, and the report points out that a mass calculated from anhydrous copper(II) sulfate's 159.61 g/mol, then weighed out as pentahydrate, would leave the stock about 36 percent short.
Dilution with the flask named
M1V1 equals M2V2 fixes the concentration, and the report specifies a 100.0 mL volumetric flask filled to the mark, since the equation assumes a final solution volume rather than a volume of added water.
Three equations, one reaction
Molecular, complete ionic and net ionic forms are all written, so spectator sodium and sulfate ions are shown canceling rather than simply disappearing between lines.
Excess base, verified
At least 125 mL of 0.100 M sodium hydroxide is needed to react all 0.00625 mol of copper ion. Stating that figure lets a reader confirm the copper really limits the precipitate.
Prediction beside measurement
The theoretical 0.610 g sits next to a bracketed recovered mass, and the discussion treats losses on the filter paper and incomplete drying as factors pulling in opposite directions.
Where marks go in SC180 Unit 10
Solution reports lose the most on molarity defined per liter of water, which leads to stock made by adding solid to 250 mL of solvent and a concentration that is quietly wrong. Leaving the hydrate's waters out of the molar mass is the second classic loss. Dilutions computed correctly but described as adding 75 mL of water, rather than filling to the mark, draw method comments because volumes are not strictly additive. Net ionic equations that keep spectator ions, or that write copper(II) hydroxide as dissolved ions, cost accuracy credit. Reports that never check whether the base was truly in excess leave the limiting reagent assumed. Predicted masses given to four figures from three-figure data, and discussions that treat the three parts as unrelated exercises, account for most remaining deductions.
Get a SC180 Unit 10 example written to your instructions
Send the SC180 Unit 10 assignment sheet and rubric, listing the solute, target concentrations and reaction the prompt specifies, and whether a bench step is part of it. Linked parts carry every calculation in one chain, with any measured values held open in brackets for your own data. Generally ready in 24-48h, the first custom report is free.
SC180 Unit 10 questions, answered
Why use a volumetric flask instead of adding a measured volume of water?
Molarity is moles per liter of final solution, and dissolving a solid or mixing two liquids does not always produce a volume equal to the sum of the parts. Filling a volumetric flask to its mark guarantees the final volume the calculation assumes. Adding exactly 75 mL of water to 25 mL of stock lands close to 100 mL, but not exactly.
What is the point of the net ionic equation?
It shows the chemistry that actually happens. Sodium and sulfate ions are present before and after mixing, unchanged, so they drop out of the net equation. What remains, copper(II) ions combining with hydroxide ions to form solid Cu(OH)2, is the reaction whose stoichiometry predicts the precipitate. Graders often award separate credit for identifying the spectators correctly.
Does the report need my lab results or just the calculations?
That depends on the section. Some Unit 10 prompts are purely calculation reports; others attach a bench or kit step with a recovered mass. Where measured values are required, they must be your own, and the model shows exactly where they go and how the discussion compares them with the prediction.