The pH of a solution containing CH3COOH (acetic acid) is typically around 2.4 to 2.9.
The pH of a solution containing 6M HCl is 0.
The pH of a solution containing NaCl is neutral, around 7.
The pH of a solution containing NaH2PO4 is around 4.5.
The pH of a solution containing 0.1 M of HC2H3O2 is around 2.88.
The pH of a solution containing 5 acetic acid is approximately 2.9.
The pH of a solution containing 6M HCl is 0.
The pH of a solution containing NaCl is neutral, around 7.
The pH of a solution containing NaH2PO4 is around 4.5.
The pH of a solution containing 0.1 M of HC2H3O2 is around 2.88.
The pH of a solution containing 5 acetic acid is approximately 2.9.
At equal concentrations, the pH of HCl solution will be lower than that of CH3COOH solution due to HCl being a stronger acid than CH3COOH. This is because HCl fully dissociates in water to produce more H+ ions compared to the partial dissociation of CH3COOH.
The pH of a solution containing H2S would be acidic, as H2S is a weak acid. The exact pH value would depend on the concentration of H2S in the solution.
The pH of a solution containing NaCl dissolved in water is neutral, around 7.
The pH of a solution containing hydrofluoric acid (HF) is typically around 3.2.
Given that the pH of a 0.12 M solution of acetic acid (CH3COOH) is 3.0, you can calculate the concentration of H+ ions in the solution using the formula pH = -log[H+]. Once you have the concentration of H+ ions, you can use it to calculate the concentration of CH3COO- ions using the ionization constant expression for acetic acid (CH3COOH) and then determine the Ka value.
Adding NaCH3CO2 to a CH3COOH solution will cause a shift in equilibrium toward the formation of more CH3COO-. Since CH3COO- is the conjugate base of CH3COOH, the solution will become more basic and the pH will increase.
The difference in pH values for the two solutions is due to their chemical properties. NaCl is a neutral salt, so its solution will have a pH around 7. CH3COOH is a weak acid, so its solution will have a pH less than 7 due to the presence of hydrogen ions resulting from the partial dissociation of the acid.