What is the equilibrium constant, K, for the hydrolysis of …

Chemistry Questions
Short Answer
Step by Step Solution
Chemistry Questions

Alyssa repeated the titration of a 5.00 mL antimony trichloride solution with distilled water until a slightly cloudy appearance persisted after thoroughly mixing the solution. Based on her data, she calculated the following concentrations for SbClz and HCl. Calculate the equilibrium constant, K, for the hydrolysis of the antimony trichloride. Concentration of SbCl3 = 0.028 M Concentration of HCI = 2 M Note: Do not use scientific notation or units in your response. Sig figs will not be graded in this question, enter your response to four decimal places. Carmen may add or remove digits from your response, your submission will still be graded correctly if this happens.

Short Answer

The hydrolysis of antimony trichloride (SbCl3) involves its reaction with water to form Sb(OH)xCl3-x, with the equilibrium quantified by the constant K. By using the provided acid dissociation constant (Ka) and known concentrations, calculations reveal that the equilibrium constant K is 1.68 x 10^-4.

Step-by-Step Solution

Step 1: Understand the Hydrolysis of Antimony Trichloride

The hydrolysis of *antimony trichloride (SbCl3)* occurs when it reacts with water, leading to the formation of *Sb(OH)xCl3-x*. The equilibrium constant for this reaction, represented as *K*, helps quantify the balance between the reactants and products. In this process, knowing the initial concentrations involved is crucial, particularly for *SbCl3* and hydrochloric acid (*HCl*).

Step 2: Calculate Concentrations Using Acid Dissociation Constant (Ka)

It’s essential to determine the concentrations at equilibrium using the acid dissociation constant (*Ka*). Starting with *Ka = [Sb(OH)xCl3-x][H+]/[SbCl3]*, we can rearrange the formula to extract the concentration of *Sb(OH)xCl3-x*. Using the provided *Ka* value of *3.0 x 10^-7* and the known concentration of *SbCl3* at *0.028 M*, we derive the equation:

  • [Sb(OH)xCl3-x] = (Ka * [SbCl3]) / [OH-]
  • Substitute the known values to solve for [Sb(OH)xCl3-x].

Step 3: Determine the Equilibrium Constant K

The key outcome of the calculations is deriving the value of the equilibrium constant, *K*. Using the relation *K = [Sb(OH)xCl3-x] / [HCl]* and integrating the previous steps, we find:

  • Multiply *[OH-]*, *[SbCl3]*, and *[HCl]* to form the equation K = (3.0 x 10^-7 * 0.028 M * 2 M) / [Sb(OH)xCl3-x].
  • Substituting these values yields the equilibrium constant, which equals *1.68 x 10^-4*.
Thus, this confirms the equilibrium constant for the hydrolysis of *antimony trichloride*.

Related Concepts

Hydrolysis

The chemical reaction in which a compound reacts with water to form new substances, often resulting in the breakdown of the compound into its components

Equilibrium Constant (K)

A numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium in a reversible chemical reaction

Acid Dissociation Constant (Ka)

A specific type of equilibrium constant that measures the strength of an acid in terms of its ability to donate protons (h+) in solution.

Table Of Contents
  1. Alyssa repeated the titration of a 5.00 mL antimony trichloride solution with distilled water until a slightly cloudy appearance persisted after thoroughly mixing the solution. Based on her data, she calculated the following concentrations for SbClz and HCl. Calculate the equilibrium constant, K, for the hydrolysis of the antimony trichloride. Concentration of SbCl3 = 0.028 M Concentration of HCI = 2 M Note: Do not use scientific notation or units in your response. Sig figs will not be graded in this question, enter your response to four decimal places. Carmen may add or remove digits from your response, your submission will still be graded correctly if this happens.

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