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What is the pH level of 0.0005 M HF solution?
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.
What is true about a solution of 1.0 M HF?
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 value of hydrofloric acid?
pH values depend on the concentration of acidsolutionfor eg.0.02 M HF has pH=2.47
At a certain temperature a 0.25 M solution of HF has a pH of 2.3 What is the Ka of HF at this temperature?
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).
What is the pH of a solution containing 0.1 M of HC2H3O2?
The pH of a solution containing 0.1 M of HC2H3O2 is around 2.88.
What is the pH level of 0.0005 M HF solution?
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.
How many moles of HF Ka6.8104 must be present in 0.220dm3 to form a solution with a pH of 2.60?
An 0.010 M HF solution gives pH = 2.6, so 0.0022 molesare present in 0.22 L
What is true about a solution of 1.0 M HF?
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 value of hydrofloric acid?
pH values depend on the concentration of acidsolutionfor eg.0.02 M HF has pH=2.47
At a certain temperature a 0.25 M solution of HF has a pH of 2.3 What is the Ka of HF at this temperature?
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).
What is the pH of a solution containing 0.1 M of HC2H3O2?
The pH of a solution containing 0.1 M of HC2H3O2 is around 2.88.
What is the pH of a 0.001 M of HCl solution?
its PH is 3
How many grams of HF are needed to make 0.50L of a 0.750 M solution?
The answer is 7,5g.
What would be the pH of a solution with a hydroxide ion OH- concentration of 10-12 M?
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.
What is the approximate pH of a 1 M solution of Na2CO3?
The approximate pH of a 1 M solution of Na2CO3 is around 11-12, making it basic.
What is the pH of Na2HPO4?
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.
What is ammonia's pH value?
A 1.0 M aqueous solution has a pH of 11.6
