Answer:
The pH of the solution is 1.91
Explanation:
Step 1:
Data obtained from the question. This includes the following:
Mass of HNO3 = 5.41g
Volume of solution = 7L
Molar Mass of HNO3 = 63.02g/mol
pH =?
Step 2:
Determination of the number of mole of HNO3. This is illustrated below:
Mass of HNO3 = 5.41g
Molar Mass of HNO3 = 63.02g/mol
Number of mole HNO3 =?
Number of mole = Mass/Molar Mass
Number of mole of HNO3 = 5.41/63.02
Number of mole of HNO3 = 0.086 mole
Step 3:
Determination of the molarity of HNO3. This is illustrated below:
Mole of HNO3 = 0.086 mole
Volume of solution = 7L
Molarity of HNO3 =.?
Molarity = mole/Volume
Molarity of HNO3 = 0.086/7
Molarity of HNO3 = 0.0123 M
Step 4:
Determination of the hydrogen ion concentration in HNO3. This can be achieved by doing the following:
Dissociation equation of HNO3
HNO3(aq) —> H+ + NO3-
From the above equation,
1 mole of HNO3 produced 1 mole of H+.
Therefore, 0.0123 M of HNO3 will also produce 0.0123 M of H+.
The concentration of H+ is 0.0123 M
Step 5:
Determination of the pH of the solution.
pH = –Log [H+]
[H+] = 0.0123 M
pH = –Log 0.0123
pH = 1.91
