a) 1.0M HCl solution, 500ml of this solution (from a 6.0M solution) b) 1.0M HC2H3O2 solution, 500.ml of this solution (from a 6.0M solution) c) 1.0M NaOH solution, 250.ml of this solution (from a 2.0ml solution). d) 1.0M NH4OH solution (it is called ammonium hydroxide but the other name is ammonia water solution), 250.ml of this solution (from a 2.0ml solution) |
a) 1.0M HCl solution, 500ml of this solution (from a concentrated, (concen), 12.0M solution) b) 1.0M HC2H3O2 solution, 500.ml of this solution (from a concen 12.0M solution) c) 1.0M NaOH solution, 500.ml of this solution (from a solid NaOH). d) 1.0M NH4OH solution (it is called ammonium hydroxide but the other name is ammonia water solution), 500..ml of this solution (from concen 14.5M solution) e) 2.0M HCl solution, 500mL of this solution from concen 12.0M solution |
2017-2018 AP Chem Extension |
a) To the 1.0 M HCl solution, add a few grains of NaCl, stir/dissolve salt and record new pH. |
b) To the 1.0M HC2H3O2 solution, add a few grains of Sodium acetate ( NaC2H3O2), stir/dissolve and record new pH. c) To the 1.0M NaOH solution, add a few grains of NaCl, stir/dissolve salt and record new pH. d) To the 1.0M NH4OH solution, add a few grains of Ammonium chloride ( NH4Cl ), stir/dissolve and record pH. |
Question for 2018-2018 AP Chem Extension. (Will answer these questions on different sheet of paper) |
1. What would LeChatlier's Principle about adding NaC2H3O2) to a HC2H3O2 solution? What would the new Equilibrium "bucket" look like and do any concentrations change? Do those changes the pH of the new solution compared to the original solution? |
2. Similarly, how would the same thing happen when you added NH4Cl to the NH3 ( i.e. NH4OH solution). |
|
3. Does the same thing happen when added the NaCl to either the HCl solution and/or NaOH solution? Explain? |