A solution has a pOH = 8.54. Its pH is a) -0.93 v) 2.92 c) 7.00 d) 5.46 A soluti

Question

A solution has a pOH = 8.54. Its pH is a) -0.93 v) 2.92 c) 7.00 d) 5.46 A solution has a pH of 5.00. In this solution, [OH] must be a) 1.0 times 10^-9 M b) 1.0 times 10^-7 M c) greater than 1.0 times 10^-5 M d) 1.0 times 10^-5 M A solubility product constant expression for equilibrium in a saturated aqueous solution of iron(III) phosphate is a) K_sp = [Fe^2+][PO_4^3-]^2 c) K_sp = [Fe_2^3+] [PO_4^-] c) K_sp = [Fe^3+] [PO_4^3-] d) K_sp = [Fe^3-] [PO_4^3+] Which of the following dissociates entirely into metal ions and hydroxide in solution? a) a strong acid b) a strong base c) a weak acid b) a strong base

Explanation / Answer

5) Answer pH = 5.46

Given pOH = 8.54

we know that pH + pOH = 14

so pH + 8.54 = 14

pH = 14 - 8.54

6) Answer [OH-] = 1.0 * 10-9 M

Given pH = 5.00

pH + pOH = 14

5 + pOH = 14

pOH = 9

-log ([OH-]) = 9

[OH-] = 1.0 * 10-9 M

7) Answer is b) Ksp = [ Fe3+][PO43-]

iron III phosphate is FePO4 it will diassociate as Fe3+ and PO43- so Ksp will be the above

8) strong base

ex: NaOH (aq) ----> Na+ ( aq) + OH- (aq)

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