The solubility of ammonium chloride in water at various temperatures is given below :Temperature: 10°C 20°C 40°C 60°C 80°CSolubility : 24g 37g 41g 55g 66gWhat mass of ammonium chloride would be needed to make a saturated solution of ammonium chloride in fifty grams of water at 40°C?
Solubility at 40°C = 41 gm
Solubility = Solid dissolved in 100 grams of water in a solution.
So, the mass of ammonium chloride, required to make a saturated solution of ammonium chloride, in 50 gm of water at 40°C
= 41\2g
= 20.5 gm
Related Articles
- Name the process you would use to separate ammonium chloride from a mixture of sodium chloride and ammonium chloride.
- 21.5 g of sodium chloride dissolves in 60 g of water at 25° C. Calculate the solubility of sodium chloride in water at that temperature.
- 9.72 g of potassium chloride dissolves in 30 g of water at 70°C. Calculate the solubility of potassium chloride at that temperature.
- With the help of a labelled diagram, describe the method of separating ammonium chloride from a mixture of ammonium chloride and common salt. Mention the difference in the properties of ammonium chloride and sodium chloride which has made this separation possible.
- Pragya tested the solubility of three different substances at different temperatures and collected the data as given below(results are given in the following table, as grams of substance dissolved in 100grams of water to form a saturated solution).(a) What mass of potassium nitrate would be needed to produce a saturated solution of potassium nitrate in 50 grams of water at 313K?(b) Pragya makes a saturated solution of potassium chloride in water at 353K and leaves the solution to cool at room temperature. What would she observe as the solution cools? Explain.(c) Find the solubility of each salt at 293K. Which salt has the highest solubility at this temperature?(d) What is the effect of change of temperature on the solubility of a salt?"
- Write the chemical formula of ammonium chloride. Explain why an aqueous solution of ammonium chloride is acidic in nature? Illustrate your answer with the help of a chemical equation.
- One of the following does not undergo sublimation. This one is :(a) iodine (b) sodium chloride(c) ammonium chloride (d) camphor
- To make a saturated solution, 36 g of sodium chloride is dissolved in 100 g of water at 293 K. Find its concentration at this temperature.
- Suggest separation technique(s) one would need to employ to separate the following mixtures.(a) Mercury and water(b) Potassium chloride and ammonium chloride(c) Common salt, water and sand(d) Kerosene oil, water and salt
- (a) What is sublimation? Name two substances (other than ammonium chloride) which undergo sublimation.(b) Draw a labeled diagram of the experimental set-up to demonstrate the sublimation of ammonium chloride.
- Name one property which is shown by ammonium chloride but not by sodium chloride.
- (a) Differentiate between a saturated and an unsaturated solution. How will you test whether a given solution is saturated or not?(b) How would you prepare a saturated solution of sodium chloride in water at 25°C ? What will happen if this solution is cooled to 10°C?
- A student takes a mixture of sand and ammonium chloride in a china dish and heats it under a funnel fitted with a plug over a flame. He would observe that :(1) solid sand gets deposited on the lower cooler parts of the funnel while solid ammonium chloride remains in the china dish.(2) sand and ammonium chloride get deposited on hotter parts of the funnel.(3) ammonium chloride gets deposited on the cooler parts of the funnel and sand remains in the china dish.(4) sand collects on cooler parts of the funnel while ammonium chloride melts in the china dish.
- Which of the following compounds are ionic and which are covalent?Urea, Cane sugar, Hydrogen chloride, Sodium chloride, Ammonium chloride, Carbon tetrachloride, Ammonia, alcohol, Magnesium chloride.
- Describe the method of separating a mixture containing common salt, sand and ammonium chloride.
Kickstart Your Career
Get certified by completing the course
Get Started