Question

what is the pH of a 0.100M soln of H2SO4? Given Ka1=
1.70x10-2, Ka2=6.20x10-8

answer is not 1.39.

Answer #1

Using the data you are providing, the pH should be really low, Ka2 is too far from Ka1 to contribute to the pH.

Initial | 0.1 | 0 | 0 | |

change | -X | +X | +X | |

equilibrium | 0.1-X | X | X |

this yields:

X=0.0336

[H+]=0.0336

pH=-log0.0336=1.47

Calculate the pH of 0.15 M H2SO4(aq) at 25◦C, given that Ka1 is
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Ka2=6.00x10^-8

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Please show work thanks

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Please write out steps if possible so that I can understand,
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Given that the stepwise dissociation constants for phosphoric
acid are:
Ka1 = 7.5×10-3; Ka2 =
6.2×10-8; Ka3 = 4.8×10-13
To prepare 1.20 L of a buffer solution having an ionic strength
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Answer to 3 sig figs.
a) (mass) of Na2HPO4(anhydrous) and
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