Advertisements
Advertisements
Question
Calculate the pH of the following solution:
0.3 g of NaOH dissolved in water to give 200 mL of solution.
Advertisements
Solution
For 0.3 g of NaOH dissolved in water to give 200 mL of solution:
\[\ce{NaOH -> Na^+_{(aq)} + OH^-_{(aq)}}\]
`["NaOH"] = 0.3 xx 1000/200 = 1.5 "M"`
`["OH"_("aq")^-] = 1.5 "M"`
Then `["H"^+] = 10^(-14)/1.5`
`= 6.66 xx 10^(-13)`
`"pH" = - log(6.66 xx 10^(-13))`
= 12.18
APPEARS IN
RELATED QUESTIONS
It has been found that the pH of a 0.01M solution of an organic acid is 4.15. Calculate the concentration of the anion, the ionization constant of the acid and its pKa.
Assuming complete dissociation, calculate the pH of the following solution:
0.002 M KOH
Calculate the pH of the following solutions:
0.3 g of Ca(OH)2 dissolved in water to give 500 mL of solution.
Calculate the pH of the resultant mixtures: 10 mL of 0.01M H2SO4 + 10 mL of 0.01M Ca(OH)2.
Choose the most correct answer :
For pH > 7 the hydronium ion concentration would be _________.
An aqueous solution of which of the following will have a pH greater than 7?
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 concentration of hydroxide ion in a water sample is found to be 2.5 × 10−6 M. Identify the nature of the solution.
Acidity of \[\ce{BF3}\] can be explained on the basis of which of the following concepts?
Assertion (A): Increasing order of acidity of hydrogen halides is \[\ce{HF < HCl < HBr < HI}\]
Reason (R): While comparing acids formed by the elements belonging to the same group of periodic table, \[\ce{H - A}\] bond strength is a more important factor in determining acidity of an acid than the polar nature of the bond.
What is the pH of a 2.6 × 10-8 MH+ ion solution? (log 2.6 = 0.4150)
The degree of dissociation of 0.1 M monobasic acid is 0.4%. Its dissociation constant is ______.
Define pH.
Derive a relationship between pH and pOH.
Define pOH.
Define pH.
Define pOH.
Derive the relation pH + pOH = 14.
Define the following term:
pH
