I need help with this in order to correctly complete my other related problems.
Thank you so much in advance =)
Arrange the following 0.1 M solutions in order of increasing pH and state why you placed each solution in that position: NaCH3COO, HCl, HCN, NaOH, NH3, NaCN, KNO3, H2SO4, NH4Cl, H2SO3, NaHCO3, Na3PO4 and CH3COOH.
In order of increasing pH:
I'm not about to do your homework for you but here is HOW you do it.
All of the materials are salts, bases, or acids.
The long way, but sure way, is to calculate the pH of the solns.
For strong acids such as HCl, the ionization is 100%, and pH = -log(HCl)
For strong bases, such as NaOH, pOH = -log(OH^-) and use pH + pOH = pKw = 14 to convert to pH.
For weak acids are bases, go through an ICE chart; for example, HAc for acetic acid. ........HAc ==> H^+ + Ac^-
initial.......0.1.....0......0
change.......-x........x......x
equil......0.1-x.......x......x
Substitute into the Ka expression, solve for x and convert to pH.
For weak bases, such as NH3, use tahe same process but x = OH^-; convert to pOH then to H.
For salts, the pH is determined by the hydrolysis of the salt. For sodium acetate or NaAc (a basic salt), this is
..............Ac^- + HOH ==> HAc + OH^-
initial.......0.1............0......0
change........-x.............x......x
equil......0.1-x.............x......x
Kb for Ac^- = (Kw/Ka for HAc) = (HAc)(OH^-)/(Ac^-). Substitute and solve for x = (OH^-), convert to pOH and pH.
Acidic salts do the same kind of thing; i.e., NH4^+ + H2O ==>H3O^+ + NH3
Ka for NH4^+ = (Kw/Kb for NH3) = (NH3)(H3O^+)/(NH4^+), solve for x = (H3O^+) and convert to pH.
When you have done each you can arrange them in increasing order of pH.
After you have finished and know the exact order you may wish to think about the results and come up with a shorter way to solve these kinds of problems.
To arrange the solutions in order of increasing pH, we need to understand how pH is related to the nature of the solutions. pH is a measure of the acidity or basicity of a solution and its value ranges from 0 to 14.
Acidic solutions have pH values less than 7, while basic solutions have pH values greater than 7. A neutral solution has a pH of 7.
To determine the pH, we need to consider the nature of the substances present in each solution and their ability to interact with water to produce acidic or basic ions.
1. HCl: Hydrochloric acid is a strong acid that dissociates completely in water to produce hydrogen ions (H+). Hence, it will have the lowest pH value among the provided solutions.
2. H2SO4: Sulfuric acid is also a strong acid and dissociates completely to produce hydrogen ions. Therefore, it will have a lower pH than most other solutions.
3. H2SO3: Sulfurous acid is a weak acid and partially dissociates in water to produce hydrogen ions. It will have a slightly higher pH than HCl and H2SO4 but still acidic.
4. CH3COOH: Acetic acid is a weak acid as well and partially dissociates to produce hydrogen ions. It will have a higher pH compared to the above three acids.
5. NaCN: Sodium cyanide is a basic salt. When dissolved in water, it will produce hydroxide ions (OH-) which makes it basic.
6. NaHCO3: Sodium bicarbonate is also a basic salt. It can react with water to produce hydroxide ions, making it basic.
7. Na3PO4: Sodium phosphate is a basic salt that produces hydroxide ions in water.
8. NaOH: Sodium hydroxide is a strong base that dissociates completely in water to form hydroxide ions. It will have the highest pH among all the provided solutions.
9. NaCH3COO: Sodium acetate is a weak base and partially ionizes in water to produce hydroxide ions. It will have a slightly lower pH compared to NaOH but still basic.
10. NH3: Ammonia is a weak base and when dissolved in water, it reacts with water molecules to produce hydroxide ions, making it slightly basic.
11. KNO3: Potassium nitrate is a neutral salt and does not affect the pH of the solution significantly.
12. NH4Cl: Ammonium chloride is an acidic salt and when dissolved in water, it can release hydrogen ions, making it slightly acidic.
Therefore, the solutions arranged in increasing order of pH are:
HCl, H2SO4, H2SO3, CH3COOH, NH4Cl, KNO3, NaCN, NaCH3COO, NH3, NaHCO3, Na3PO4, NaOH