Question

4.9 g H2SO4 is present in 500ml of the solution. Calculate the pH of solution if molar mass is 98 g/mol

Answer 1

Answer:

Molar mass of sulphuric acid is 98.07g/mol

Molar mass of sulphuric acid is 98.07g/molTherfore 4.9g contains 0.04996 moles.

Molar mass of sulphuric acid is 98.07g/molTherfore 4.9g contains 0.04996 moles.0.04996 mol/500ml =( 0.04996 x2) moles per litre = 0.09992 moles per litre

Molar mass of sulphuric acid is 98.07g/molTherfore 4.9g contains 0.04996 moles.0.04996 mol/500ml =( 0.04996 x2) moles per litre = 0.09992 moles per litreTherefore 4.9g H2SO4 in 500 ml = approx. 0.10M.

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Answer 2

Explanation:

Molarity of H 2SO 4 = 98×500

9.8×1000=0.2M

As H 2 SO 4

is strong acid so it dissociates completely to give H+ions.

H 2 SO 4→2H +

+SO²/⁴-

0.2

0.2×2 0.2

[H +]=2×0.2=0.4M

pH=−log([H+ ])=0.3979

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