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Question

When equal volumes of pH=4 and pH=6 are mixed together then the pH of the resulting solution will be: [log 5=0.7]


A
4.3
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B
4.7
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C
5
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D
5.3
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Solution

The correct option is D $$4.3$$
pH=4, pH=6
For pH=4, $$[H^{+}] = 10^{-4}M$$
For pH=6, $$[H^{+}] = 10^{-6}M$$
Molarity=$$\cfrac{\text{no. of moles}}{\text{volume}}$$
Let the volume be V.
No. of moles, $$n_{1}=10^{-4} \times V$$
No. of moles, $$n_{2}=10^{-6} \times V$$
Net number of moles after mixing = $$10^{-4}\times V+10^{-6} \times V$$
Net $$[H^{+}]$$ concentration = $$\cfrac{10^{-4} \times V + 10^{-6} \times V}{2V}$$
pH = $$-\log{[H^{+}]}$$
pH = 4.3

Chemistry

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