Classify the solute represented in each of the following equations as a strong, weak, or nonelectrolyte: a. K 2 S O 4 ( a q ) → H 2 O 2 K + ( a q ) + S O 4 2 − ( a q ) K_2SO_4\left(aq\right)\xrightarrow{H_2O}2K^{+}\left(aq\right)+SO_4^{2-}\left(aq\right)

Hey, everyone, we're asked to identify the solute in the following as strong, weak or non electrolyte when placed in water. And our equation here states that we have rubidium carbonate in its solid state then dissociates into our rubidium ion and our carbonate ion. So first, let's go ahead and talk about these terms that were provided to us in our question stem, starting with a strong electrolyte. We've learned that a strong electrolyte are solutes that completely dissociates. And this happens once it is placed in a solvent. In this case, water. Next, looking at weak electrolytes, these are solutes that partially dissociate when placed in a solvent. And lastly looking at our non electrolytes, these are molecular or covalent or non ionic compounds and these do not dissociate into ions. Now, let's go ahead and take a look at our chemical equation right here. So we see that we have rubidium carbonate and we know that rubidium carbonate is an ionic compound and per our solubility rules, salts containing group, one elements are always soluble in our water. So, since rubidium carbonate is an ionic compound, and rubidium is a group, one element, this means that it will completely dissociate. And we can also tell that this completely dissociates since we have our arrow sign right here, telling us that it completely dissociates. So to answer this question, our solute rubidium carbonate is considered a strong electrolyte. Now, I hope this made sense and let us know if you have any questions.

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9. Solutions

Electrolytes (Simplified)

GOB Chemistry

9. Solutions

Electrolytes (Simplified)

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2:24 minutes

Problem 13a

Textbook Question

Classify the solute represented in each of the following equations as a strong, weak, or nonelectrolyte:
a. $K_{2} S O_{4} (a q) \overset{H_{2} O}{\to} 2 K^{+} (a q) + S O_{4}^{2 -} (a q)$

Verified step by step guidance

Step 1: Understand the concept of electrolytes. Electrolytes are substances that dissolve in water to produce ions, allowing the solution to conduct electricity. Strong electrolytes dissociate completely into ions, weak electrolytes partially dissociate, and nonelectrolytes do not dissociate at all.

Step 2: Analyze the given chemical equation: K₂SO₄(s) →H₂O 2K⁺(aq) + SO₄²⁻(aq). This equation shows that potassium sulfate (K₂SO₄) dissociates completely in water to form two potassium ions (K⁺) and one sulfate ion (SO₄²⁻).

Step 3: Recognize that complete dissociation into ions is a characteristic of a strong electrolyte. Since K₂SO₄ dissociates fully into its constituent ions, it is classified as a strong electrolyte.

Step 4: Recall that strong electrolytes include most soluble ionic compounds, such as salts, strong acids, and strong bases. Potassium sulfate is a soluble ionic compound, further supporting its classification as a strong electrolyte.

Step 5: Conclude that the solute K₂SO₄ in the given equation is a strong electrolyte because it dissociates completely into ions in water, enabling the solution to conduct electricity effectively.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Electrolytes

Electrolytes are substances that dissociate into ions when dissolved in water, allowing the solution to conduct electricity. They are classified into strong electrolytes, which completely dissociate into ions, weak electrolytes, which partially dissociate, and nonelectrolytes, which do not dissociate at all. Understanding this classification is essential for analyzing the behavior of solutes in aqueous solutions.

Strong Electrolytes

Strong electrolytes are compounds that fully dissociate into their constituent ions in solution. Examples include soluble salts like potassium sulfate (K₂SO₄), which dissociates completely into 2K⁺ and SO₄²⁻ ions. This complete dissociation results in high conductivity in the solution, making it crucial to identify strong electrolytes when classifying solutes.

Weak Electrolytes

Weak electrolytes are substances that only partially dissociate into ions in solution, resulting in a mixture of ionized and non-ionized molecules. Common examples include acetic acid and ammonia. The degree of dissociation is important for understanding the conductivity and chemical behavior of solutions, particularly in contrast to strong electrolytes.

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