Advertisements
Advertisements
प्रश्न
The pH of milk, black coffee, tomato juice, lemon juice and egg white are 6.8, 5.0, 4.2, 2.2 and 7.8 respectively. Calculate corresponding hydrogen ion concentration in each.
Advertisements
उत्तर
The hydrogen ion concentration in the given substances can be calculated by using the given relation:
pH = –log [H+]
(i) pH of milk = 6.8
Since, pH = –log [H+]
6.8 = –log [H+]
log [H+] = –6.8
[H+] = anitlog(–6.8)
`= 1.5 xx 10^(-7) :M"`
(ii) pH of black coffee = 5.0
Since, pH = –log [H+]
5.0 = –log [H+]
log [H+] = –5.0
[H+] = anitlog(–5.0)
= 10-5 M
(iii) pH of tomato juice = 4.2
Since, pH = –log [H+]
4.2 = –log [H+]
log [H+] = –4.2
[H+] = anitlog(–4.2)
`= 6.31 xx 10^(-5)`M
iv) pH of lemon juice = 2.2
Since, pH = –log [H+]
2.2 = –log [H+]
log [H+] = –2.2
[H+] = anitlog(–2.2)
`= 6.31 xx 10^(-3)`M
(v) pH of egg white = 7.8
Since, pH = –log [H+]
7.8 = –log [H+]
log [H+] = –7.8
[H+] = anitlog(–7.8)
`= 1.58 xx 10^(-8)`M
संबंधित प्रश्न
The pH of a sample of vinegar is 3.76. Calculate the concentration of hydrogen ion in it.
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 pOH of 10-8 M of HCl.
Calculate the pH and pOH of 0.0001 M HCl solution.
When CuSO4 solution in water is treated with concentrated HCl it turns _______.
The aqueous solutions of sodium formate, anilinium chloride and potassium cyanide are respectively.
The percentage of pyridine (C5H5N) that forms pyridinium ion (C5H5NH) in a 0.10 M aqueous pyridine solution (Kb for C5H5N = 1.7 × 10−9) is ____________.
The pH of an aqueous solution is Zero. The solution is ____________.
Calculate the pH of 1.5 × 10−3 M solution of Ba(OH)2.
The Ka value for HCN is 10−9. What is the pH of 0.4 M HCN solution?
The aqueous solution of sugar does not conduct electricity. However, when sodium chloride is added to water, it conducts electricity. How will you explain this statement on the basis of ionisation and how is it affected by concentration of sodium chloride?
If pKb for CN− at 25°C is 4.7, the pH of 0.5 M aqueous NaCN solution is ______.
Calculate the pH of a buffer solution containing 0.1 M CH3COOH and 0.05 M CH3COONa. Dissociation constant of CH3COOH is 1.8 × 10-5 at 25°C.
Define pH.
Define pH.
Define pH.
Derive relationship between pH and pOH.
Define pOH.
Define the following term:
pOH
