Titration of strong acid with weak base

In summary, the conversation discusses the use of the Henderson-Hasselbalch Equation to solve a problem involving a given equation and an ICE table. The user is unsure if their solution is correct and is seeking feedback. The helper states that the solution is incorrect and suggests showing the work more clearly for better feedback. The helper also mentions that they cannot provide the solution directly due to forum rules.
  • #1
reminiscent
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Please post readable solutions to your problems, not shaky images impossible to read.

Homework Statement


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Homework Equations


Henderson-Hasselbalch Equation

The Attempt at a Solution


GKxObdC.jpg

Sorry for the huge picture, but the number says 0.007558 mol. Is my ICE table correct?
Equation:
7.42 = 6.85 + log((0.007558-x)/x)
(0.007558-x)/x = 3.715
x = 0.00160 mol H+/(0.07483 L + 0.01339 L) = 0.0181 M = [HCl]
It says it is incorrect, though.
 
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  • #2
This one is not difficult, but still requires a couple of equations and several algebraic steps. You do need to show the work more clearly for the helper to be able to give good feedback. I think I figured out the solution, but the Physics Forum rules do not allow the helper to simply furnish the solution.
 

FAQ: Titration of strong acid with weak base

What is titration of strong acid with weak base?

Titration of strong acid with weak base is a laboratory technique used to determine the concentration of an acid by reacting it with a known concentration of a base. This allows for the calculation of the acid's concentration and can also be used to determine the acid's dissociation constant.

How does titration of strong acid with weak base work?

In this titration, a burette is filled with a known concentration of a base and the acid is slowly added to it until the equivalence point is reached. The equivalence point is where the moles of acid and base are equal, and it is determined by using an indicator or a pH meter. The volume of acid used at the equivalence point is used to calculate the acid's concentration.

Why use a strong acid and a weak base in titration?

Using a strong acid and a weak base allows for a more precise determination of the acid's concentration. This is because the pH at the equivalence point will be closer to 7, making it easier to determine the endpoint using an indicator or pH meter.

What are the common indicators used in titration of strong acid with weak base?

The most commonly used indicators in this titration are phenolphthalein and methyl orange. Phenolphthalein changes color at a pH of around 8.3, making it ideal for titrations involving weak bases. Methyl orange changes color at a pH of around 4.4, making it useful for titrations involving strong acids.

What are some sources of error in titration of strong acid with weak base?

Some sources of error in this titration include impurities in the chemicals used, inaccurate measurements of volume, and incomplete neutralization due to the presence of excess acid or base. It is important to perform multiple trials and calculate an average to minimize these errors.

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