Advertisements
Advertisements
Question
The pH of a sample of vinegar is 3.76. Calculate the concentration of hydrogen ion in it.
Solution
Given
pH = 3.76
it is known that
pH = -log[`"H"^(+)`]
`=> log["H"^+] = -"pH"`
`=> ["H"^(+)] = "antilog" (-"pH")`
`= "antilog" (-3.76)`
`= 1.74 xx 10^(-4) "M"`
Hence, the concentration of hydrogen ion in the given sample of vinegar is 1.74 × 10–4M.
APPEARS IN
RELATED QUESTIONS
Assuming complete dissociation, calculate the pH of the following solution:
0.003 M HCl
Calculate the pH of the resultant mixtures: 10 mL of 0.01M H2SO4 + 10 mL of 0.01M Ca(OH)2.
Calculate the pH of the resultant mixtures: 10 mL of 0.1M H2SO4 + 10 mL of 0.1M KOH
Choose the most correct answer:
Which of the following solution will have a pH value equal to 1.0?
Derive the relation pH + pOH = 14.
Calculate the pH and pOH of 0.0001 M HCl solution.
The pH of 0.001 M NaOH(aq) solution will be:
Aqueous solution of ____________ will turn red litmus blue.
pH of a solution is 12. The number H+ ions present in 1 cm3 of this solution is ____________.
An aqueous solution of which of the following will have a pH greater than 7?
What is the pH of 0.01 M solution of ammonium hydroxide which is 10% dissociated?
Which of the following is CORRECT for an aqueous solution of NH4CN?
[Ka of HCN = 4.0 × 10−10, Kb for NH4OH = 1.8 × 10−5]
The least basic hydroxide from the following is:
What is the pH of a 2.6 × 10-8 MH+ ion solution? (log 2.6 = 0.4150)
A buffer solution is prepared in which the concentration of NH3 is 0.30 M and the concentration of \[\ce{NH^+_4}\] is 0.20 M. If the equilibrium constant, Kb tor NH3 equals 1.8 × 10-5, what is the pH of the solution?
The degree of dissociation of 0.1 M monobasic acid is 0.4%. Its dissociation constant is ______.
Define pOH.
Define pH.
Define the following term:
pH
