Advertisements
Advertisements
प्रश्न
50 ml of 0.05 M HNO3 is added to 50 ml of 0.025 M KOH. Calculate the pH of the resultant solution.
उत्तर
Number of moles of HNO3 = 0.05 × 50 × 10−3
= 2.5 × 10−3
Number of moles of KOH = 0.025 × 50 × 10−3
= 1.25 × 10−3
Number of moles of HNO3 after mixing
= 2.5 × 10−3 – 1.25 × 10−3
= 1.25 × 10−3
∴ Concentration of HNO3 = `("Number of moles of HNO"_3)/("Volume is litre")`
After mixing, total volume = 100 ml = 100 × 10−3 L
∴ [H+] = `(1.25 xx 10^-3 "moles")/(100 xx 10^-3 "L")`
= 1.25 × 10−2 moles L−1
pH = –log [H+]
pH = –log (1.25 × 10−2)
= 2 – 0.0969
= 1.9031
APPEARS IN
संबंधित प्रश्न
Calculate the pH of the following solution:
1mL of 13.6 M HCl is diluted with water to give 1 litre of solution.
The degree of ionization of a 0.1M bromoacetic acid solution is 0.132. Calculate the pH of the solution and the pKa of bromoacetic acid.
The pH of 0.005M codeine (C18H21NO3) solution is 9.95. Calculate its ionization constant and pKb.
Among the following, the CORRECT increasing order of acidity:
What is the pH of the resulting solution when equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed?
The concentration of hydroxide ion in a water sample is found to be 2.5 × 10−6 M. Identify the nature of the solution.
If pKb for CN− at 25°C is 4.7, the pH of 0.5 M aqueous NaCN solution is ______.
Derive relationship between pH and pOH.
Define pH.
Define the following term:
pH
