Question

pH of an aqueous solution having 0.49g of H.SO, in 100 ml of solution is
a) 1
b) 2
c) 3
D) 4​

Answer 1

Explanation:

The first thing to do here is to calculate the number of moles of hydrochloric acid present in that sample. To do that, use the compound's molar mass

0.0040g⋅1 mole HCl36.46g=0.0001097 moles HCl

Now, hydrochloric acid is a strong acid, which means that it dissociates completely in aqueous solution to produce hydronium cations,

H3O+HCl(aq)+H2O(l)→H3O+(aq)Cl+−(aq)

This basically means that every mole of hydrochloric acid dissolved in water will produce 1

mole of hydronium cations.

no. of moles of H3O+=0.0001097 moles

The molarity of the hydronium cations must be calculated for

1 lakh of solution, so do

1L solution

103mL1L⋅

0.0001097 moles H3O+100mL solution=0.001097 moles H3O+

Since that is how many moles of hydronium cations you have in

1 L

of solution, you can say that the concentration of the hydronium cations will be

[H3O+]=0.001097 M

The pH of the solution is calculated by taking the negative log of the concentration of hydronium cations

pH=−log([H3O+])

−−−−−−−−−−−−−−−−−−−−

Plug in your value to find

pH=−log(0.001097)=3.0

−−−

The answer is rounded to one decimal place, the number of sig figs you have for the volume of the solution.

Explanation:

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Answer 2

The correct answer is option D which is 4