Three beakers contain clear, colorless liquids. One beaker contains pure water, another contains salt water, and another contain
s sugar water. How can you tell which beaker is which? (No tasting allowed!)
2 answers:
To differentiate the three solutions in a beaker, the electrode circuit test and direct current source and the heating process are used
<h3>Further explanation</h3>Electric current in an electrolyte solution is caused by the ions that move between the electrodes with one another. So these ions are the conductor of electricity.
Electrical conductivity can be interpreted as the ability of a conductor in this case an electrolyte solution to move an electric charge
Electrical conductivity indicates an easy measure of whether or not a solution conducts an electric current.
Based on the electrical conductivity, electrolytes can be grouped into strong electrolytes and weak electrolytes
Liquid substances can be grouped based on their electrical conductivity, namely electrolyte and non-electrolyte solutions.
The sign of the solution is an electrolyte can be used a test equipment consisting of a series of electrodes and a direct current source. If the light is on, the solution is an electrolyte solution
Some substances in the solid state cannot conduct electricity but in a liquid / solution state can conduct electricity.
examples of strong electrolyte solutions: HBr, NaCl
Example of a weak electrolyte solution: CH₃COOH
Examples of non-electrolyte solutions:
Sugar Solution (C₁₂H₂₂O₁₁), Ethanol (C₂H₅OH), Urea (CO(NH₂)₂)
Of the three beaker water which is an electrolyte solution is a salt solution (NaCl), while water and sugar are not an electrolyte solution, so that when tested in a series of electrodes and direct current sources ,they cannot turn on the lights
Furthermore, to distinguish between water and sugar solution, the heating process can be carried out and the boiling point measured with a thermometer.
The boiling point of the sugar solution will be greater than water because there are sugar solutes
<h3>Learn more</h3>colligative properties
Raoult's law
The vapor pressure of benzene
The freezing point of a solution
Keywords: Boiling Point, electrolyte solution
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Answer:
The electrochemical equivalent of copper, Cu, is 3.29015544 × 10⁻⁷ g/C
Explanation:
The given parameters are;
The element for which the electrochemical equivalent is sought = Copper
The atomic mass of copper = 63.5
The electrochemical equivalent, 'Z', of an element or a substance is the mass, 'm', of the element or substance deposited by one coulomb of electricity, which is equivalent to a 1 ampere current flowing for a period of 1 second
Mathematically, we have;
m = Z·I·t = Z·Q
We have;
Cu²⁺ (aq) + 2·e⁻ → Cu
Therefore, one mole of Cu, is deposited by 2 moles of electrons
The charge carried one mole of electrons = 1 Faraday = 96500 C
∴ The charge carried two moles of electrons, Q = 2 × 96500 C = 193,000 C
Given that the mass of an atom of Cu = 63.5 a.m.u., the mass of one mole of Cu, m = 63.5 g
∴ Z = 3.29015544 × 10⁻⁴ g/C = 3.29015544 × 10⁻⁷ g/C
The electrochemical equivalent of copper, Cu, is Z = 3.29015544 × 10⁻⁷ g/C