Calculate the concentration of HC6H6O6- in an aqueous solution of 0.0851 M ascorbic acid, H2C6H6O6 (aq).
I do not know how to start this
problem. Can you please explain how to solve it?
The first step is to calculate the molar mass of ascorbic acid, H2C6H6O6. This can be done by adding up the atomic masses of each element in the compound:
2 x 12.011 (for the two hydrogen atoms) + 6 x 12.011 (for the six carbon atoms) + 6 x 15.999 (for the six oxygen atoms) = 176.086 g/mol
Next, you need to calculate the number of moles of ascorbic acid in the solution. This can be done by dividing the given concentration (0.0851 M) by the molar mass of ascorbic acid (176.086 g/mol):
0.0851 M / 176.086 g/mol = 0.0048 moles of ascorbic acid
Finally, you can calculate the concentration of HC6H6O6- in the solution. This can be done by multiplying the number of moles of ascorbic acid (0.0048 moles) by the number of moles of HC6H6O6- produced when one mole of ascorbic acid is oxidized (2 moles):
0.0048 moles x 2 moles = 0.0096 M HC6H6O6-
To calculate the concentration of HC6H6O6- in an aqueous solution of ascorbic acid, we first need to understand the chemical equation and the dissociation of ascorbic acid in water.
The chemical equation for the dissociation of ascorbic acid is:
H2C6H6O6 (aq) ⇌ H+ (aq) + C6H6O6- (aq)
From this equation, we can see that one molecule of ascorbic acid (H2C6H6O6) dissociates to produce one hydrogen ion (H+) and one ascorbate ion (C6H6O6-).
Furthermore, ascorbic acid is a weak acid, so it does not fully dissociate in water. To calculate the concentration of HC6H6O6- in the solution, we need to consider the dissociation constant (Ka) of ascorbic acid. The dissociation constant is a measure of the extent to which the acid dissociates in water.
The dissociation constant (Ka) for ascorbic acid is 7.96 x 10^-5.
Now, let's calculate the concentration of HC6H6O6- in the solution:
Step 1: Write the expression for the dissociation of ascorbic acid:
Ka = [H+][C6H6O6-] / [H2C6H6O6]
Step 2: Substitute the given values and the Ka value into the equation:
7.96 x 10^-5 = [H+][C6H6O6-] / 0.0851
Step 3: Rearrange the equation to solve for [C6H6O6-]:
[C6H6O6-] = (7.96 x 10^-5) * 0.0851 / [H+]
Step 4: Assume that the solution is neutral, so the concentration of H+ is equal to the concentration of OH-:
[H+] = [OH-]
Step 5: Assume that the concentration of [H+] is equal to x:
[H+] = x
Step 6: Calculate the concentration of [C6H6O6-]:
[C6H6O6-] = (7.96 x 10^-5) * 0.0851 / x
Now, you can solve for [C6H6O6-] by substituting the value of [H+] into the equation.
Note: The concentration of HC6H6O6- will be very small because ascorbic acid is a weak acid that only partially dissociates in water.
To start, let's break down the chemical formula of ascorbic acid to understand its structure and charge. Ascorbic acid is written as H2C6H6O6, indicating that it contains 2 hydrogen (H) atoms, 6 carbon (C) atoms, and 6 oxygen (O) atoms. The subscript "6" indicates that there are 6 hydroxyl groups in ascorbic acid.
In an aqueous solution, ascorbic acid (H2C6H6O6) will donate one of its hydrogen ions (H+) to the surrounding water molecules, resulting in the formation of a hydrogen ion (H+) and an ascorbate ion (C6H6O6-).
To calculate the concentration of HC6H6O6- in the solution, we first have to determine the concentration of ascorbic acid (H2C6H6O6).
Given that the concentration of ascorbic acid, H2C6H6O6 (aq), is 0.0851 M, this means that there are 0.0851 moles of H2C6H6O6 in 1 liter of the solution.
Since each mole of ascorbic acid yields one mole of ascorbate ions (HC6H6O6-), the concentration of HC6H6O6- can be calculated as follows:
Concentration of HC6H6O6- = Concentration of H2C6H6O6 (aq) = 0.0851 M
Therefore, the concentration of HC6H6O6- in the given solution is 0.0851 M.