Advertisements
Advertisements
Question
Calculate the pH of 0.04 M HNO3 solution.
Advertisements
Solution
Concentration of HNO3 = 0.04 M
[H3O+] = 0.04 mol dm−3
pH = –log [H3O+]
= –log (0.04)
= –log (4 × 10−2)
= 2 – log4
= 2 – 0.6021
= 1.3979
= 1.40
APPEARS IN
RELATED QUESTIONS
The concentration of hydrogen ion in a sample of soft drink is 3.8 × 10–3 M. what is its pH?
If 0.561 g of KOH is dissolved in water to give 200 mL of solution at 298 K. Calculate the concentrations of potassium, hydrogen and hydroxyl ions. What is its pH?
The pH of 0.1M solution of cyanic acid (HCNO) is 2.34. Calculate the ionization constant of the acid and its degree of ionization in the solution.
Choose the most correct answer :
Blood in the human body is highly buffered at a pH of ________.
Select the INCORRECT relation.
In which of the following solvents is silver chloride most soluble?
Define pOH.
Define pH.
Derive relationship between pH and pOH.
Define pH.
