The following video is the synthesis of Copper (II) Hydroxide. Copper(II) hydroxide has been known since copper smelting began around 5000 BC although the alchemists were probably the first to manufacture it by mixing solutions of lye (sodium or potassium hydroxide) and blue vitriol (copper(II) sulfate).

Copper(II) hydroxide is the hydroxide of copper with the chemical formula of Cu(OH)₂. It is a pale greenish blue or bluish green solid. It contains copper in its +2 oxidation state. It also contains hydroxide ions.
Formula: Cu(OH)2
Molar mass: 97.561 g/mol
Melting point: 176°F (80°C)
Density: 3.37 g/cm³

The chemical reaction is stated below:

CuSO4 + Li(OH)2 → Cu(OH)2 + LiCL ,

Copper sulfate is mixed with lithium hydroxide to form copper hydroxide and lithium chloride. The chemical reaction occurs instantaneously as soon as the ions are introduced to each other.

CuSO4 + Li(OH)2 → Cu(OH)2 + LiCl,

Copper sulfate (CuSO4), Copper(II) sulfate, also known as cupric sulfate, or copper sulphate, is the inorganic compound with the chemical formula CuSO₄ₓ, where x can range from 0 to 5. The pentahydrate is the most common form.
Molar mass: 159.609 g/mol
Formula: CuSO4
IUPAC ID: Copper(II) sulfate
Melting point: 230°F (110°C)
Boiling point: 482°F (250°C)
Soluble in: Water

Lithium hydroxide (LiOH), Lithium hydroxide is an inorganic compound with the formula LiOH. It is a white hygroscopic crystalline material.
Formula: LiOH
Molar mass: 23.95 g/mol
Specific heat capacity (C): 2.071 J/g K
Basicity (pKb): −0.04(LiOH(aq) = Li+ + OH–)

Lithium Chloride (LiCl), Lithium chloride is a chemical compound with the formula LiCl. The salt is a typical ionic compound, although the small size of the Li+ ion gives rise to properties not seen for other alkali metal chlorides, such as extraordinary solubility in polar solvents (83.05 g/100 mL of water at 20 °C) and its hygroscopic properties.
Molar mass: 42.394 g/mol
Solubility in formic acid: 26.6 g/100 g (18 °C); 27.5 g/100 g (25 °C)
Solubility in liquid ammonia: 0.54 g/100 g (-34 °C); 3.02 g/100 g (25 °C)
Solubility in acetone: 1.2 g/100 g (20 °C); 0.83 g/100 g (25 °C); 0.61 g/100 g (50 °C)
Specific heat capacity (C): 48.03 J/mol·K
Structure and properties: Refractive index (n), Dielectric constant (εr), etc

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