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1.0 M solution of a strong acid, HA

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Are the following statements about a 1.0 M solution of a strong acid, HA, true or false?
[A-] › [H+]: True/False
The pH is 0.00: True/False
[H+] = 1.0 M: True/False
[HA] = 1.0 M: True/False
From the given solubility data given, calculate the value of Ksp for the following compounds.
SrF2; 7.3 x 10-2 g/L
Ag3PO4; 6.7 x 10-3 g/L

Please provide step by step explanation. Thanks!

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Solution Summary

The expert examines a 1.0M solution of a strong acid HA. The solubility is calculated.

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a) Are the following statements about a 1.0 M solution of a strong acid, HA, true or false?
[A-] › [H+]: True/False:
False, When HA dissociates, it will form equal amounts of H+ and A_

b) The pH is 0.00: True/False
pH = -log[H+] = -log1 = 0
True
c) [H+] = 1.0 M: True/False
True. Since strong acids completely dissociates, concentration of H+ = 1M

d) [HA] = 1.0 M: True/False
It is false. Since strong acid dissociates, there won't be any undissociated [HA] when dissolved in water.

From the given solubility data given, calculate the value ...

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