At equilibrium, what is the hydrogen-ion concentration if the acid dissociation constant is 0.000 001 and the acid concentration is 0.01M?
can you help me step by step and explain?
...........HA --> H^+ + A^-
I.........0.01....0......0
C..........-x.....x......x
E........0.01-x...x......x
Ka = 1E-6 = (H^+)(A^-)/(HA)
Substitute the E line into Ka expression and solve for x = (H^+).
acid(aq)>>H+ ??
keq=[H+)[??]/(.01-x)
1E-6=x^2/(.01-x)
x^2+xE-6-1E-8=0
x= (-E-6+-(1E-12 +4E-8)/2
x= you work it out, about
= -.5E-6+1E-4 about .000095
Certainly! Let's solve this step by step.
Step 1: Write the expression for the acid dissociation constant (Ka).
Ka = [H+][A-]/[HA]
Step 2: Identify the given values:
Ka = 0.000001 (given)
[HA] = 0.01 M (given)
Step 3: Assume that the concentration of [H+] at equilibrium is x M.
Step 4: Write the equilibrium expression using the assumption from Step 3:
Ka = [H+][A-]/[HA]
0.000001 = x * [A-] / 0.01
Step 5: Since the acid is monoprotic, [A-] = [H+] (because the dissociation gives one H+ and one A-).
Step 6: Substitute [A-] with x in Step 4:
0.000001 = x * x / 0.01
Step 7: Simplify the equation from Step 6:
0.000001 = x^2 / 0.01
Step 8: Multiply both sides of the equation by 0.01 to isolate the x^2 term:
0.00000001 = x^2
Step 9: Take the square root of both sides to solve for x:
x = sqrt(0.00000001)
Step 10: Calculate x:
x = 0.0001
So, at equilibrium, the hydrogen-ion concentration ([H+]) is 0.0001 M.
I hope this explanation was helpful! Let me know if you have any further questions.
Yes, I can help you step by step and explain how to find the hydrogen-ion concentration at equilibrium.
Step 1: Write down the acid dissociation equation.
In this case, the acid dissociation equation can be written as follows:
HA ↔ H+ + A-
Step 2: Set up the expression for the acid dissociation constant (Ka).
The acid dissociation constant (Ka) is defined as the ratio of the concentration of the products (H+ and A-) to the concentration of the acid (HA) at equilibrium. The expression for Ka is given by:
Ka = [H+][A-] / [HA]
Step 3: Substitute the known values into the expression for Ka.
In this case, the acid concentration (HA) is given as 0.01M, and the acid dissociation constant (Ka) is given as 0.000001. Substituting these values in, the equation becomes:
0.000001 = [H+][A-] / 0.01
Step 4: Solve for [H+].
To find the hydrogen-ion concentration ([H+]), we need to isolate it in the equation. Rearrange the equation by multiplying both sides by 0.01:
0.000001 * 0.01 = [H+][A-]
0.00000001 = [H+][A-]
Step 5: Assume that at equilibrium, [H+] = [A-].
This is based on the principle of neutralization. Therefore, we can assume that [H+] is equal to [A-]. Let's denote this as x.
Step 6: Substitute the assumed value into the equation.
The equation becomes:
0.00000001 = x * x
Step 7: Solve for x.
To find the value of x, we need to take the square root of both sides:
√(0.00000001) = x
x ≈ 0.0001
Step 8: Calculate the hydrogen-ion concentration at equilibrium.
Since [H+] = [A-], the hydrogen-ion concentration at equilibrium is approximately 0.0001M.
So, at equilibrium, the hydrogen-ion concentration is approximately 0.0001M.