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saul85 [17]
4 years ago
6

What are three uses for copper sulfate?

Chemistry
1 answer:
timofeeve [1]4 years ago
6 0

Answer:

- The metal industry uses large quantities of copper sulphate as an electrolyte in copper refining, for copper coating steel wire prior to wire drawing and in various copper plating processes .

- The mining industry employs it as an activator in the concentration by froth flotation of lead, zinc, cobalt and gold ores .

- The paint industry uses it in anti-fouling paints and it plays a part in the colouring of glass.

Explanation:

Hello,

In this case, since copper sulphate also known as blue stone, blue vitriol is more commonly found in a pentahydrated cupric sulphate due to its stability. In fact it is often the starting raw material for the production of other varied copper-based salts. Henceforth, you will find three applications.

- The metal industry uses large quantities of copper sulfate as an electrolyte in copper refining, for copper coating steel wire prior to wire drawing and in various copper plating processes .

- The mining industry employs it as an activator in the concentration by froth flotation of lead, zinc, cobalt and gold ores .

- The paint industry uses it in anti-fouling paints and it plays a part in the colouring of glass.

Best regards.

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(part 1 of 3) Copper reacts with silver nitrate through a single replacement. If 1.29 g of silver are produced from the reaction
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Answer:

See explanation.

Explanation:

Hello there!

In this case, according to the described chemical reaction, we first write the corresponding equation to obtain:

Cu+2AgNO_3\rightarrow 2Ag+Cu(NO_3)_2

Thus, we proceed as follows:

Part 1 of 3: here, since the molar mass of silver and copper (II) nitrate are 107.87 and 187.55 g/mol respectively, and the mole ratio of the former to the latter is 2:1, we can set up the following stoichiometric expression:

m_{Cu(NO_3)_2}=1.29gAg*\frac{1molAg}{107.87gAg}*\frac{1molCu(NO_3)_2}{2molAg}*\frac{187.55gCu(NO_3)_2}{1molCu(NO_3)_2}   \\\\m_{Cu(NO_3)_2}=1.12gCu(NO_3)_2

Part 2 of 3: here, the molar mass of copper is 63.55 g/mol and the mole ratio of silver to copper is 2:1, the mass of the former that was used to start the reaction was:

m_{Cu}=1.29gAg*\frac{1molAg}{107.87gAg}*\frac{1molCu}{2molAg}*\frac{63.55gCu)_2}{1molCu}   \\\\m_{Cu}=0.380gCu

Part 3 of 3: here, the molar mass of silver nitrate is 169.87 g/mol and their mole ratio 2:2, thus, the mass of initial silver nitrate is:

m_{AgNO_3}=1.29gAg*\frac{1molAg}{107.87gAg}*\frac{2molAgNO_3}{2molAg}*\frac{169.87gAgNO_3}{1molAgNO_3}   \\\\m_{AgNO_3}=2.03gAgNO_3

Best regards!

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