Arrange the following 0.10M solutions in order of increasing pH:

a. Nacl
b. NH4CL
C. HCL
D. NaCH3CO2
e. KOH

The pH is determined by the hydrolysis of the salt(for salts) or the reactin with water (as in HCl and KOH). For example,

KOH is a strong base; ie., it ionizes 100% so K^+ = OH^- = 0.1M.
NaC2H3O2 is the salt of a strong base (NaOH) and acetic acid (HC2H3O2) The Na^+ is not hydrolyzed but the acetate ion (C2H3O2^-) is. Etc. Please explain what your trouble is in answering this question so I will know how to explain.
The correct order is
HCl, NH4Cl, NaCl, NaC2H3O2, KOH

Alright, let's see what we've got here! Arrange the following solutions in order of increasing pH:

a. NaCl: Well, salt may make your food taste better, but it won't bring your pH up or down. So, I'll place this one in the middle of the pack.

b. NH4Cl: Ah, the infamous ammonium chloride. This one is going to be a bit on the acidic side, so let's put it near the lower end of the list.

c. HCl: Ah, good old hydrochloric acid. This one is definitely going to bring the pH down, so it gets the acidic crown.

d. NaCH3CO2: Ah, sodium acetate. It's a slightly basic salt, so I'll put it closer to the alkaline end.

e. KOH: The mighty potassium hydroxide. This one is definitely going to give us a boost on the alkaline side, so it takes the top spot.

So, the final order would be:

c. HCl
b. NH4Cl
a. NaCl
d. NaCH3CO2
e. KOH

Hope that brings a smile to your face!

To arrange the solutions in order of increasing pH, we need to consider the chemical properties of each solution. pH is a measure of the acidity or basicity of a solution. A lower pH value indicates higher acidity, while a higher pH value indicates higher basicity.

Let's analyze each solution and determine their pH values:

a. NaCl: NaCl is a neutral salt. It dissociates completely into Na+ and Cl- ions in water but does not have any effect on the pH of the solution. Therefore, the pH of a 0.10M NaCl solution is around 7, which is neutral.

b. NH4Cl: NH4Cl is a salt that is derived from a weak base (NH3) and a strong acid (HCl). The ammonium ion, NH4+, is acidic, while the chloride ion, Cl-, is neutral. When NH4Cl is dissolved in water, NH4+ acts as a weak acid and lowers the pH of the solution. Therefore, the pH of a 0.10M NH4Cl solution is slightly acidic, less than 7.

c. HCl: HCl is a strong acid that completely ionizes in water. It dissociates into H+ and Cl- ions. Since HCl is a strong acid, the concentration of H+ ions in a 0.10M HCl solution is relatively high, resulting in a significantly low pH, less than 7.

d. NaCH3CO2: NaCH3CO2 is a salt that is derived from a weak acid (CH3COOH) and a strong base (NaOH). The acetate ion, CH3COO-, is the conjugate base of a weak acid and is slightly basic. When NaCH3CO2 is dissolved in water, it releases CH3COO- ions that slightly increase the pH of the solution. Therefore, the pH of a 0.10M NaCH3CO2 solution is slightly basic, greater than 7.

e. KOH: KOH is a strong base that completely ionizes in water. It dissociates into K+ and OH- ions. Since KOH is a strong base, the concentration of OH- ions in a 0.10M KOH solution is relatively high, resulting in a significantly high pH, greater than 7.

Based on the analysis, we can arrange the solutions in increasing order of pH as follows:

c. HCl (most acidic)
b. NH4Cl
a. NaCl
d. NaCH3CO2
e. KOH (most basic)

To arrange the given 0.10M solutions in order of increasing pH, we need to consider the nature of the ions present in each solution and the effect they have on the acidity or basicity of the solution. Let's analyze each solution:

a. NaCl:
NaCl is a salt composed of a strong base (NaOH) and a strong acid (HCl). Since both the cation (Na+) and the anion (Cl-) are derived from strong acids or bases, they do not affect the pH when dissolved in water. Therefore, NaCl will have a neutral pH of 7.

b. NH4Cl:
NH4Cl is a salt composed of a weak base (NH3) and a strong acid (HCl). When NH4Cl dissolves in water, it undergoes hydrolysis, where the weak base NH3 accepts a proton (H+) from water, resulting in the formation of NH4OH and HCl. The formation of NH4OH makes the solution slightly acidic, hence NH4Cl solution will have a slightly acidic pH below 7.

c. HCl:
HCl is a strong acid that ionizes completely in water, releasing H+ ions. Since H+ ions increase the concentration of positive hydrogen ions, HCl solution will have a very low pH and is highly acidic.

d. NaCH3CO2:
NaCH3CO2 is a salt composed of a strong base (NaOH) and a weak acid (CH3COOH, also known as acetic acid). Similar to NaCl, the ions Na+ and CH3COO- do not significantly affect the pH in this case. However, the presence of CH3COO- ions, which can accept a proton from water, will cause a slight increase in hydroxide ion concentration. This results in a slightly basic pH above 7.

e. KOH:
KOH is a strong base that ionizes completely in water, releasing OH- ions. The presence of OH- ions increases the concentration of hydroxide ions, resulting in a high pH and a highly basic solution.

Now, let's arrange the 0.10M solutions in order of increasing pH:
1. HCl - highly acidic
2. NH4Cl - slightly acidic
3. NaCl - neutral
4. NaCH3CO2 - slightly basic
5. KOH - highly basic

Therefore, the correct order of increasing pH is: HCl < NH4Cl < NaCl < NaCH3CO2 < KOH.