Acid-Base Titrations
These are fill in the blank and I really am not sure what the answers are
1. Indicators change color over a range that is called its ---?
2. The common indicator ---? is very useful in studying neutralizations that involve strong acids and weak bases.
3. Indicators tend mostly to be in the form that has the general formula ---? in highly basic solutions.
4. Indicators tend mostly to be in the form that has the general formula ---? in highly acidic solutions.
There is a lot of material to be discussed here. See this site to swim through all of this.
https://www.chemguide.co.uk/physical/acidbaseeqia/indicators.html
1. Indicators change color over a range that is called its "transition interval."
2. The common indicator "phenolphthalein" is very useful in studying neutralizations that involve strong acids and weak bases.
3. Indicators tend mostly to be in the form that has the general formula "In-" in highly basic solutions.
4. Indicators tend mostly to be in the form that has the general formula "HIn" in highly acidic solutions.
1. Indicators change color over a range that is called its pH range.
To determine the answer to this question, you can refer to the characteristics of indicators in acid-base titrations. Indicators are substances that undergo a color change at a specific pH value. The range of pH over which the indicator changes color is called its pH range. To find the pH range of a specific indicator, you can consult reference books or do some research online.
2. The common indicator phenolphthalein is very useful in studying neutralizations that involve strong acids and weak bases.
To determine the answer to this question, you can recall the properties of phenolphthalein and its use in acid-base titrations. Phenolphthalein is a commonly used indicator that changes color in the pH range of approximately 8.2-10.0. It is particularly useful in studying neutralizations that involve strong acids and weak bases because its color change occurs in the pH range where the equivalence point of the titration is typically observed in such reactions.
3. Indicators tend mostly to be in the form that has the general formula In^- in highly basic solutions.
To determine the answer to this question, you need to understand the behavior of indicators in highly basic solutions. In highly basic solutions, indicators tend to exist in their conjugate base form (In^-), which is often colored. This is because the basic environment causes the indicator molecule to accept a proton (H+) and be converted to its conjugate base form. To confirm this information for a specific indicator, you can consult reference materials or research the properties of that indicator.
4. Indicators tend mostly to be in the form that has the general formula HIn in highly acidic solutions.
To determine the answer to this question, you need to understand how indicators behave in highly acidic solutions. In highly acidic solutions, indicators tend to exist in their acidic form (HIn), which is often differently colored than their conjugate base form. This is because the acidic environment causes the indicator molecule to donate a proton (H+) and be converted to its acidic form. To confirm this information for a specific indicator, you can consult reference materials or research the properties of that indicator.