Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
![**Question:**
What is the solubility of Cr(OH)₃ at a pH of 10.70? (Ksp Cr(OH)₃ is 6.70 × 10⁻³¹)
**Explanation:**
This question involves finding the solubility of chromium(III) hydroxide, Cr(OH)₃, in a solution with a pH of 10.70, given its solubility product constant (Ksp) as 6.70 × 10⁻³¹.
**Approach:**
To solve this, we need to use the solubility product expression for Cr(OH)₃:
\[ \text{Cr(OH)}₃(s) \leftrightarrow \text{Cr}^{3+}(aq) + 3\text{OH}^{-}(aq) \]
The Ksp expression is:
\[ Ksp = [\text{Cr}^{3+}][\text{OH}^-]^3 \]
Knowing the pH allows us to find the concentration of OH⁻ ions since:
\[ \text{pH} + \text{pOH} = 14 \]
\[ \text{pOH} = 14 - 10.70 = 3.30 \]
\[ [\text{OH}^-] = 10^{-\text{pOH}} = 10^{-3.30} \]
Plugging this [OH⁻] value into the Ksp expression will allow us to solve for [Cr³⁺] and thus determine the solubility.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa91f799b-1b33-41a5-8f4e-af83231854b4%2F79532172-0519-4989-8452-c688bf77a75a%2Fozm04j8_processed.png&w=3840&q=75)

The pH of Cr(OH)3 is 10.70.
The Ksp value is .
To find the solubility of Cr(OH)3.
Step by step
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