Hi!
For a strong acid-weak base titration what's an example of a titrant, analyte, appropriate indicator, pH at neutralization, and a typical graph of the titration?
Help is much appreciated
Thank you so much
The question sounds like you want us to do your work for you but I'll help with some short answer stuff.
A. We can't draw diagrams on these boards so forget the graph.
B. Strong acid example is HCl.
C. Weak base example is NH3.
D. The titrant is what is added from the buret.
E. The analyte is what is being titrated/determined.
F. The indicator usually is something like methyl red or methyl orange but it depends a little upon the concentrations of the acid and base.
G. The pH at the equivalence point is about 5.0 or so.
Hi there!
In a strong acid-weak base titration, the following are some examples:
1. Titrant: Sodium hydroxide (NaOH) solution. Since it is a strong base, it will act as the titrant and be added to the analyte.
2. Analyte: Acetic acid (CH3COOH) solution. It is a weak acid and will react with the titrant.
3. Appropriate indicator: Phenolphthalein is commonly used as an indicator in this type of titration. It turns pink at a pH of around 8.2-10, which is in the alkaline range.
4. pH at neutralization: In a strong acid-weak base titration, the pH at neutralization is slightly acidic, usually around 7-8, due to the presence of the weak acid's conjugate base.
5. Typical graph: The graph of a strong acid-weak base titration usually consists of two parts. Initially, the pH of the solution remains relatively constant as the titrant is slowly added. This is followed by a steep increase in pH as the equivalence point is approached. After the equivalence point, the pH increases more slowly again.
I hope this helps! Let me know if you have any more questions.
Hi there! In a strong acid-weak base titration, you are essentially adding a strong acid (known as the titrant) to a solution containing a weak base (known as the analyte) to determine its concentration. Let's break down each component you asked for:
1. Titrant: An example of a titrant for a strong acid-weak base titration could be hydrochloric acid (HCl). It is a strong acid that will react completely with the weak base analyte.
2. Analyte: An example of an analyte for this titration could be ammonia (NH3). Ammonia is a weak base that will react with the hydrochloric acid.
3. Indicator: An appropriate indicator for this titration would be phenolphthalein. Phenolphthalein is commonly used for acid-base titrations and changes color in the pH range of 8.2 to 10, which corresponds to the endpoint of the titration. It starts colorless in acidic solutions and turns pink as the pH reaches the neutral range.
4. pH at neutralization: The neutralization point of the titration is also the endpoint, which occurs when the stoichiometric ratio of the acid and base has been reached. Since hydrochloric acid is a strong acid and ammonia is a weak base, the pH at neutralization will be acidic, typically around pH 4-6.
5. Typical graph: A typical graph of the titration would involve plotting the volume of the titrant (hydrochloric acid) added on the x-axis and the pH of the solution on the y-axis. It would show an initial gradual increase in pH as the titrant is added until reaching the equivalence point, where it rapidly increases in pH due to excess strong acid. The endpoint is often indicated by a sudden and sharp change in pH value.
I hope this helps! Let me know if you have any further questions.