The maximum acceptable concentration of fluoride in tap water is 1.5mg/L. Express this concentration in ppm. Then figure what vo

Pure water lacks sufficient ions to conduct electricity. However, when metals like iron, zinc, and copper are present in moist soil, they can instigate electrolysis, which necessitates excess energy due to limited water's self-ionization. Consequently, wet soil can carry current as long as there are positive and negative ions. Water ions travel from the anode (positive side) to the cathode (negative side) to be oxidized and generate electricity.

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Answer:

The molality of the solution is 1.08 m.

Explanation:

First, determine the mass of the solvent.

A 13% solution by mass indicates that 13 grams are found in every 100 grams of solution.

Thus, solution mass = solute mass + solvent mass

100 g = 13 g + solvent mass

Therefore, solvent mass = 100 g - 13 g → 87 g

Next, we calculate the moles of solute (mass / molar mass):

13 g / 138.2 g/mol = 0.094 moles

Finally, to find the molality, which is the moles of solute per 1 kg of solvent (mol/kg), we convert the solvent mass to kg:

87 g. 1 kg / 1000 g = 0.087 kg

Then, molality → 0.094 mol / 0.087 kg = 1.08 m

Answer:

0.133

Explanation:

The reaction that occurs between KIO3 and KI in an acidic medium is described as

IO3⁻ +5I⁻ +6h⁺ → 3I₂ + 3H₂O

I₂ subsequently reacts with sodium thiosulfate

NaS₂O₃  → 2Na⁺ + S₂O₃²⁻

The overall reaction can be summarized as

IO⁻₃ + 6H⁺ + 6S₂O₃³⁻ → I⁻ + 3S₄O₆²⁻ + 3H₂O

The mole of KIO₃

is computed using molarity multiplied by volume

which equals 0.00002mol

One mole of KIO₃ reacts with 6 moles of S₂O₃²⁻

which gives 2x6x10⁻⁵

To find concentration,

= 0.133m

Answer: The correct choice is that they represent different concentration units.

Explanation:

Molarity: Defined as the quantity of solute moles in a liter of solution.

Molarity formula:

Mass percent: Represents the mass of solute relative to the total mass of the solution.

Mass percent formula:

This demonstrates that they are distinct units of concentration.