Is m-nitroaniline soluble in water, 1.0M NaOH, 1.0M HCl?
Here is a link that lists solubility in water as less than 0.1 mg/mL so I would call it insoluble but use the guidelines set up by your instructor as to whether it is soluble or not. Of course it is soluble in HCl (since it is a base) and I wouldn't expect it to be soluble in NaOH if it isn't soluble in water.
http://en.wikipedia.org/wiki/4-Nitroaniline
m-Nitroaniline is not significantly soluble in water, but it can dissolve in certain acidic and basic solutions. Let's analyze its solubility in 1.0M NaOH and 1.0M HCl step by step:
1. m-Nitroaniline in water:
- It has limited solubility in water, meaning that only a small amount will dissolve. The solubility is around 0.2 g/L at room temperature. Therefore, it cannot be considered as soluble in water.
2. m-Nitroaniline in 1.0M NaOH:
- Since NaOH is a strong base, it could potentially react with the acidic nature of m-nitroaniline.
- The amino group (NH2) present in m-nitroaniline can react with the hydroxide ion from NaOH to form a water-soluble sodium salt.
- Therefore, m-nitroaniline is soluble in 1.0M NaOH.
3. m-Nitroaniline in 1.0M HCl:
- HCl is a strong acid, which could potentially protonate the amino group (NH2) of m-nitroaniline.
- Protonation of the amino group will convert m-nitroaniline into a water-soluble salt, making it soluble in 1.0M HCl.
In summary, m-nitroaniline is not soluble in water but is soluble in 1.0M NaOH and 1.0M HCl due to the formation of water-soluble salts.
To determine the solubility of m-nitroaniline in different solutions like water, 1.0M NaOH (sodium hydroxide), and 1.0M HCl (hydrochloric acid), we need to consider the chemical properties of m-nitroaniline and how it interacts with these substances.
m-nitroaniline is a weak base with a nitro group (-NO2) and an amino group (-NH2) attached to a benzene ring. Benzene derivatives are usually not very soluble in water due to the nonpolar nature of the aromatic ring. However, the presence of the amino group can enhance solubility by forming hydrogen bonds with water molecules.
1. Solubility in Water:
To assess the solubility in water, we need to consider the polar and nonpolar characteristics of m-nitroaniline. The hydrophilic (-NH2) amino group interacts with water, which is polar, through hydrogen bonding, increasing the solubility of m-nitroaniline. Thus, m-nitroaniline is soluble in water, but the solubility may be limited due to the nonpolar benzene ring. The exact solubility value would require reference to experimental data or solubility tables.
2. Solubility in 1.0M NaOH:
1.0M NaOH is a strong base with a high pH. In an alkaline solution, the amino group (-NH2) in m-nitroaniline can react with hydroxide ions (OH-) from the NaOH. This results in the formation of an ionic compound called a salt. The salt formed is likely to be soluble in water, but the solubility of this salt in NaOH would require experimental data to confirm. Therefore, m-nitroaniline is expected to be soluble in 1.0M NaOH.
3. Solubility in 1.0M HCl:
1.0M HCl is a strong acid with a low pH. The acidic nature of HCl can protonate the amino group (-NH2) in m-nitroaniline by donating a hydrogen ion (H+). Protonation of the amino group makes m-nitroaniline positively charged, leading to the formation of a salt. This salt is also likely to be soluble in water, but the exact solubility in HCl would require experimental data.
In summary, m-nitroaniline is soluble in water due to the hydrogen bonding between the amino group and water molecules. It is also expected to be soluble in both 1.0M NaOH and 1.0M HCl, as these solutions would likely form soluble salts with m-nitroaniline.