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0.497ml sample of HClO4 has a pH of 0.2251. If 647ml of distilledwater was added to the HClO4 solution, what would be the new pH ofsolution be?

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Hubert Koch
Hubert KochLv2
29 Sep 2019

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Related questions

You are given an Erlenmeyer flask containing 100.00 mL of 0.185 M B- and a buret containing 0.141 M HClO4. B- is a weak base with Kb of 5.5 x 10-6. Calculate the pH of the solution (to 2 decimal places) after titrating the following volumes of HClO4:

What is the pH after 0.0 mL HClO4 is added?

What volume of HClO4 is added at the equivalence point (to 0.1 mL)?

What is the pH at the equivalence point?

What is the pH after 97.0 mL HClO4 is added?

What is the pH after 196.0 mL HClO4 is added?

1. The reaction below describes the process of silver phosphate dissolution in water. Ag3(PO4)(s) 3Ag+(aq) + PO43-(aq) What would be the effect of adding HClO4 to a saturated solution represented by the equilibrium reaction shown above? (51%) a. The added HClO4 would have no effect b. The added HClO4 would protonate PO43-(aq), causing Ag+(aq) to precipitate c. The added HClO4 would react with Ag+(aq), forming HAg(aq) and causing more Ag3PO4(s) to dissolve d. The added HClO4 would protonate PO43-(aq), causing more Ag3PO4(s) to dissolve

The reaction below describes the process of silver phosphate dissolution in water.

Ag3(PO4) <> 3 Ag+ + PO4 (3-)

What would be the effect of adding HClO4 to a saturated solution represented by the equilibrium reaction shown above?

A) THe added HClO4 would have no effect

B) The added HClO4 would protonate PO4 (3-), causing Ag+ to precipitate

C) The added HClO4 would react with Ag+, forming HAg and causing more Ag3PO4 to dissolve

D) The added HClO4 would protonate PO4(3-) causing more Ag3PO4 to dissolve

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