**(I)** 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)

= \( 1.5\times 10^{-7} M\)

**(II)** pH ofblack 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= 4.2

Since, pH = –log [H^{+}]

4.2 = –log [H^{+}]

log[H^{+}] = –4.2

[H^{+}] = anitlog(–4.2)

=\( 6.31\times 10^{-5} M\)

**(IV)** pH of lemon juice= 2.2

Since, pH = –log [H^{+}]

2.2 = –log [H^{+}]

log[H^{+}] = –2.2

[H^{+}] = anitlog(–2.2)

= \( 6.31\times 10^{-3} M\)

**(V) **pH of egg white= 7.8

Since, pH = –log [H^{+}]

7.8 = –log [H^{+}]

log[H^{+}] = –7.8

[H^{+}] = anitlog(–7.8)

= \( 1.58\times 10^{-8} M\)

Answered by Pragya Singh | 11 months agoThe concentration of sulphide ion in 0.1M HCl solution saturated with hydrogen sulphide is 1.0 × 10^{–19} M. If 10 mL of this is added to 5 mL of 0.04M solution of the following: FeSO_{4}, MnCl_{2}, ZnCl_{2} and CdCl_{2} . in which of these solutions precipitation will take place?

What is the minimum volume of water required to dissolve 1g of calcium sulphate at 298 K? (For calcium sulphate, K_{sp} is 9.1 × 10^{–6}).

What is the maximum concentration of equimolar solutions of ferrous sulphate and sodium sulphide so that when mixed in equal volumes, there is no precipitation of iron sulphide? (For iron sulphide, Ksp = 6.3 × 10^{–18}).

The ionization constant of benzoic acid is 6.46 × 10^{–5} and Ksp for silver benzoate is 2.5 × 10^{–13}. How many times is silver benzoate more soluble in a buffer of pH 3.19 compared to its solubility in pure water?

Equal volumes of 0.002 M solutions of sodium iodate and cupric chlorate are mixed together. Will it lead to precipitation of copper iodate? (For cupric iodate K_{sp} = 7.4 × 10^{–8} ).