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What is the pH of a 0.5 M HF solution?
-log(0.5 M HF) = 0.3 pH
What is the effect of adding NaF to a aqueous HF solution-a pH increases b h30 increases c hf increases?
the pH increases
What determine the strength of acid?
For normal acids, pH is most accurate. For hydrofluoric acid, pH is NOT a good indicator--a 1-percent HF solution has a lower pH than a 50-percent solution does, and a 10-percent HF solution has the highest pH of all. The range is from 3.1 (for a 1-percent solution) to 4.5 (for a 10-percent solution). HF is considered a weak acid--not all the HF molecules dissociate when the HF gas is put into water--but it's the most corrosive acid around.
What is the pH level of 0.0005 M HF solution?
pH = -log[H+] = -log(0.0005) = 3.3
PH value of hydrofloric acid?
pH values depend on the concentration of acidsolutionfor eg.0.02 M HF has pH=2.47
What is the pH of a 0.5 M HF solution?
-log(0.5 M HF) = 0.3 pH
What is the effect of adding NaF to a aqueous HF solution-a pH increases b h30 increases c hf increases?
the pH increases
What determine the strength of acid?
For normal acids, pH is most accurate. For hydrofluoric acid, pH is NOT a good indicator--a 1-percent HF solution has a lower pH than a 50-percent solution does, and a 10-percent HF solution has the highest pH of all. The range is from 3.1 (for a 1-percent solution) to 4.5 (for a 10-percent solution). HF is considered a weak acid--not all the HF molecules dissociate when the HF gas is put into water--but it's the most corrosive acid around.
What is the pH level of 0.0005 M HF solution?
pH = -log[H+] = -log(0.0005) = 3.3
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?
apexvs answer 1.0 x 10-4
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
At equilibrium a solution of hf has a pH of 4.1 if hf equals 1.4 x 10-4 and f equals 6.0 x 10-5 what is the value of ka for hf at this temperature?
apexvs answer 3.4 x 10-5
What is the pH of 0.89 M NaF?
First recognize that NaF is the salt of a strong base (NaOH) and a weak acid (HF), so the pH will be alkaline. Next, look at the hydrolysis of NaF: NaF + H2O ---> NaOH + HF, or looking at it another way.... F^- + H2O ---> HF + OH- and here F^- acts as a base, so we need the Kb for NaF and that will be the inverse of the Ka for HF. The Ka for HF is 6.6x10^-4, so Kb = 1x10^-14/6.6x10^-4 = 1.5x10^-11. Now, Kb = [HF][OH-]/[F-] = (x)(x)/(0.89) = 1.5x10^-11 x^2 = 1.3x10^-11 x = 3.6x10^-6 = [OH-] pOH = -log 3.6x10^-6 = 5.44 pH = 8.6 (note the pH is alkaline, as expected)
At equilibrium a solution of hf has a pH of 5.4 if hf 1.2 x 10-6 and f- 3.5 x 10-6 what is the value of ka for hf at this temperature?
copied-in question and answer
Why is KSCN neutral while NaF is basic despite the fact that HSCN is a weaker acid than HF?
HSCN is not a weaker acid than HF. The Ka for HSCN is approximately 1.2x10^-1 and that for HF is approximately 7x10^-4, making HSCN considerably stronger than HF. In fact, a solution of KSCN would have a pH very slightly above 7.0, but close to neutral because it is almost a strong acid. A solution of NaF will have a pH that is basic because it is the salt of a strong base and a weak acid.
A solution of HF has a pH of 5.5 What is the pOH of this solution?
pH + pOH = 145.3 + pOH = 14pOH = 14 - 5.3pOH = 8.7
