Chemistry Practicals Class 10
Testing Solubility and pH of Various Salts in Water
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- Engaging simulations with easy-to-teach instructions
About Simulation
- In this virtual science experiment, you will gain a comprehensive understanding of salt solubility and its relationship to solution acidity or alkalinity, all within a virtual laboratory environment.
- By interacting with the content, you will uncover the fundamental principles underlying solubility phenomena, enriching your understanding of chemical processes.
- You will learn to identify the solubility of various salts in water as you progress through the simulated experiment. This hands-on learning approach allows you to engage with different salt solutions actively, developing your skills in solution analysis and observation.
- Throughout the simulation, you can explore the relationship between solubility and the pH of solutions. By conducting virtual experiments and observing the outcomes, you can grasp how solution acidity or alkalinity influences salt solubility.
- By participating in the simulated experiment, you can gain proficiency in using litmus paper to determine the acidic or basic nature of solutions.
Simulation Details
Description
Solubility:
The maximum amount of a substance that can be dissolved in 100 grams of water at a given temperature is called its solubility in water.
- Water readily dissolves all salts derived from inorganic acids and inorganic bases, such as HCl and NaOH.
- Most salts originating from organic acids and organic bases exhibit water solubility, although some may be insoluble. One specific example is sodium acetate, an organic salt highly soluble in water.
The pH of the solution:
- When salts obtained from strong acids and strong bases combine with water, they form a neutral solution, for example, sodium chloride.
- In contrast, salts formed from a strong base and a weak acid result in a basic solution, as seen in the case of sodium acetate. This salt, originating from the strong base sodium hydroxide and the weak acid acetic acid, turns pH paper blue.
- Salts from a weak base and strong acid yield an acidic solution, as demonstrated by ammonium chloride. Due to ammonium hydroxide’s weaker nature compared to hydrochloric acid, its salts create an acidic solution when combined with water.
For salts of strong acids and strong bases, complete ion dissociation occurs without disrupting the water equilibrium.
Example:
However, salts of a strong acid and weak base (e.g., ammonium chloride) or a weak acid and strong base (e.g., sodium acetate) exhibit incomplete dissociation, disturbing the equilibrium of water. In the former case, the solution has more H+ while the latter has more OH–.
Salts of a strong acid and a strong base are neutral, with a pH value of 7. On the other hand, salts of a strong acid and weak base are acidic, with a pH value of less than 7, and those of a strong base and weak acid are basic, with a pH value of more than 7.
Watch this video to learn more about chemistry.
Requirements for this Science Experiment
- Sodium chloride
- Potassium nitrate
- Aluminium chloride
- Zinc sulphate
- Copper sulphate
- Sodium acetate
- Sodium carbonate
- Sodium bicarbonate
- Distilled water
- Test tubes
- White tile
- Droppers
- pH papers
- pH scale
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