Chemistry, asked by shantanukhodake, 26 days ago

What volume of a 0.5200 M solution of H2SO4 would be needed to titrate 100.00 mL of a 0.1225 M
solution of Sr(OH)2?

Answers

Answered by ramroopbharati
1

Explanation:

23.56mL 0.5200M H2SO4 100.0mL Sr(OH)2 x (0.1225mol/1000mL) x (1mol Sr(OH)2/1mol H2SO4) = 0.01225mol H2SO4 0.01225mol x (1000mL/.5200mol) = 23.56mL H2SO4 Check it: 2 OH- and 2 H+, so 1-to-1 .5200/.1225 = 4.24 4.24 x 23.56 = 100.01

Answered by attitudegirl11
0

Answer:

23.56mL 0.5200M H2SO4 100.0mL Sr(OH)2 x (0.1225mol/1000mL) x (1mol Sr(OH)2/1mol H2SO4) = 0.01225mol H2SO4 0.01225mol x ..

Explanation:

I think it is right answer of ur Question

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