if you change the indicator of standardization Hcl with Na2co3 methyl red methyl orange titration corset not why?
Why shouldn't you change the indicator from HCl to Na2CO3 in a methyl red and methyl orange titration? Well, it might lead to some interesting results. You see, HCl and Na2CO3 are like two very different characters in a chemistry circus. HCl is a strong acid, while Na2CO3 is a weak base. It's like replacing a lion with a clown in the circus ring!
Methyl red and methyl orange are indicators that change color depending on the pH of the solution. They love to perform their color-changing act when there's an acid-base reaction happening. So, if you introduce Na2CO3 as a base instead of HCl, it would confuse the poor indicators. They won't know whether to show red, orange, or maybe even purple. It's like asking a clown to juggle with lions - chaos is bound to ensue!
In short, stick to HCl for this particular titration, and let the indicators have a chemical comedy show they're familiar with.
If you are asking why you cannot change the indicator used in the standardization process of Hydrochloric Acid (HCl) with Sodium Carbonate (Na2CO3), Methyl Red, or Methyl Orange for titration, there are a few reasons:
1. Indicator Selection: The choice of indicator depends on the specific acid-base reaction being carried out. HCl is a strong acid, while Na2CO3 is a weak base. Methyl Red and Methyl Orange are suitable indicators for different acid-base reactions, but they may not provide accurate or reliable results when used in the standardization process of HCl with Na2CO3.
2. pH Range: Methyl Red and Methyl Orange have specific pH ranges over which they change color. Methyl Red typically changes color at pH 4.4-6.2, while Methyl Orange changes color at pH 3.1-4.4. These pH ranges might not be suitable for the HCl and Na2CO3 titration, as the equivalence point might occur at a different pH.
3. Color Changes: The color changes exhibited by Methyl Red and Methyl Orange might not be distinctive or easily distinguishable during the titration of HCl with Na2CO3. This can lead to difficulties in determining the endpoint accurately, compromising the accuracy of the titration.
4. Standardization Method: The standardization of HCl with Na2CO3 usually involves the use of a primary standard such as sodium carbonate, potassium hydrogen phthalate (KHP), or oxalic acid. These primary standards are selected because of their known purity and stable chemical properties. They are not interchangeable with other substances or indicators without affecting the accuracy of the standardization process.
It is important to select the appropriate indicator based on the specific acid-base reaction and pH range involved in the titration to ensure accurate and reliable results.
To understand why the indicator used in the standardization process of HCl cannot be changed with Na2CO3, methyl red, or methyl orange for titration purposes, we need to consider the properties and behavior of these substances.
During the standardization of an acid solution like HCl, a primary standard substance is used as a reference. This primary standard should have specific characteristics, including high purity, stability, and a known molar mass. Sodium carbonate (Na2CO3) does not meet these criteria for being a primary standard. It has a tendency to absorb moisture from the air, leading to changes in its molecular weight, which would affect the accuracy of the standardization.
Furthermore, methyl red and methyl orange are commonly used as acid-base indicators for titrations. These indicators undergo color changes at specific pH ranges, which helps determine the endpoint of a titration. However, their use is limited to acid-base reactions, and they are not appropriate for the standardization process of HCl in the presence of Na2CO3.
To effectively standardize HCl, it is recommended to use a primary standard substance, such as potassium hydrogen phthalate (KHP), which meets the requirements mentioned earlier.