Calculate the concentrations of [H₃O⁺] and [OH⁻] in the following solutions

Question

4.5 mol/l HCl (strong acid)

1.6 mol/l H₂SO₄ (strong, only lose the first proton)

0.32 mol/l X(OH)₂ (strong base)

0.012 mol/l X(OH)₂ (strong base)

Answer 1

4.5 mol/l HCl (strong acid)

HCl-->H+ + Cl-

4.5 0 0

0 4.5 4.5

[H+]=4.5

1E-14=[H+][OH-]

1E-14=[4.5][x]

[OH-]=2.22E-15

1.6 mol/l H₂SO₄ (strong, only lose the first proton)

H2SO4-->HSO4^- +H+

1.6 0 0

0 1.6 1.6

[H+]=1.6

1E-14=[1.6][OH-]

[OH-]=6.25E-15

0.32 mol/l X(OH)₂ (strong base)

X(OH)2-->2OH-+X^2+

0.32 0 0

0 0.64 0.32

[OH-]=0.64

1E-14=[H+][0.64]

[H+]=1.56E-14

0.012 mol/l X(OH)₂ (strong base)

X(OH)2-->2OH-+X^2+

0.012 0 0

0 0.024 0.012

[OH-]=0.024

1E-14=[H+][0.024]

[H+]=4.17E-13