If a 1.40 g sample of ammonium chloride is placed in 25.0 mL of N-methylformamide at 25 °C, the sample will:A.fully dissolve to form an unsaturated solution, because the amount of the sample will not exceed its solubility limit.B.fully dissolve to form a saturated solution, because the amount of the sample will exactly reach its solubility limit.C.partially dissolve to form a saturated solution, because the amount of the sample will exceed its solubility limit.D.not dissolve at all, because the sample is completely insoluble in the solvent.

Which of the following modifications to the experimental procedure to prepare the solutions will most likely increase the amount of ammonium chloride that dissolves in the amide solvents in Table 1? (Note: The dissolution of ammonium chloride is endothermic.)A.Decreasing the pH of the solutionB.Decreasing the pOH of the solutionC.Adding a small amount of ammonium bromide saltD.Cooling the solution as the ammonium chloride is added

Compared to the solubility of the ammonium chloride in pure formamide, what effect would dissolving KCl into the formamide have on the solubility of ammonium chloride in the solvent?A.The solubility of the ammonium chloride would increase.B.The solubility of the ammonium chloride would be unchanged.C.The solubility of the ammonium chloride would decrease.D.The effect of the added KCl salt cannot be determined without more information.

Determine whether it is possible to dissolve more solute in the solution when it has a concentration of 5 spoons/litre. a) Yes, because the solution is unsaturatedb) Yes, because the solution is saturatedc) No, because the solution is unsaturatedd) No, because the solution is saturatede) I'm not sure

If the solubility of ammonium chloride dissolved in N,N-dimethylformamide is expressed in parts per million (ppm), what is the numerical value?

Which of the following cannot be separated by sublimation?AIodine and NaClBNaphthalene and SandCIodine and Ammonium chlorideDCamphor and Sodium chloride