-log(0.5 M HF)
= 0.3 pH
The pH of a 0.0005 M HF (hydrofluoric acid) solution can be calculated using the formula: pH = -log[H+]. First, determine the concentration of H+ ions produced by HF dissociation and then calculate the negative logarithm of that concentration to find the pH.
A 1.0 M solution of HF will dissociate partially in water to form H+ and F- ions. HF is a weak acid, so it will not fully dissociate like a strong acid would. The solution will be slightly acidic due to the presence of the H+ ions.
pH values depend on the concentration of acidsolutionfor eg.0.02 M HF has pH=2.47
To find the Ka of HF at this temperature, you can use the formula pH = pKa + log([A-]/[HA]). Since HF is a weak acid, [A-] is equal to [H+], so you can substitute [H+] for [A-] in the formula. Rearrange the formula to solve for pKa. Then convert pKa to Ka using the relationship: Ka = 10^(-pKa).
The pH of a solution containing 0.1 M of HC2H3O2 is around 2.88.
The pH of a 0.0005 M HF (hydrofluoric acid) solution can be calculated using the formula: pH = -log[H+]. First, determine the concentration of H+ ions produced by HF dissociation and then calculate the negative logarithm of that concentration to find the pH.
An 0.010 M HF solution gives pH = 2.6, so 0.0022 molesare present in 0.22 L
A 1.0 M solution of HF will dissociate partially in water to form H+ and F- ions. HF is a weak acid, so it will not fully dissociate like a strong acid would. The solution will be slightly acidic due to the presence of the H+ ions.
pH values depend on the concentration of acidsolutionfor eg.0.02 M HF has pH=2.47
To find the Ka of HF at this temperature, you can use the formula pH = pKa + log([A-]/[HA]). Since HF is a weak acid, [A-] is equal to [H+], so you can substitute [H+] for [A-] in the formula. Rearrange the formula to solve for pKa. Then convert pKa to Ka using the relationship: Ka = 10^(-pKa).
The pH of a solution containing 0.1 M of HC2H3O2 is around 2.88.
its PH is 3
The answer is 7,5g.
The pH of a solution can be calculated using the formula: pH = -log[OH-]. Therefore, for a solution with [OH-] concentration of 10-12 M, the pH would be 12.
The approximate pH of a 1 M solution of Na2CO3 is around 11-12, making it basic.
For example, to obtain a solution with the pH=7,00 mix: 756 mL 0,1 M solution of Na2HPO4 with 244 mL of 0,1 M HCl solution.
A 1.0 M aqueous solution has a pH of 11.6