A solution is made initially with 0.450 M HIO₃ (Kc = 0.170). Once the equilibrium below is established, what is the equilibrium concentration of H⁺ ions? HIO₃ (aq) ⇌ H+ (aq) + IO₃⁻ (aq)

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In water, the equilibrium 2H2O(l) ⇄ H3O+(aq) + OH−(aq) Kc = 10-14 determines the concentrations of H3O+(aq) and OH−(aq). If the pH is 9.2, what is the OH− concentration? (H3O+(aq) and H+(aq) are equivalent ways of representing a solvated proton).

Calculate the equilibrium concentration (in M) of PO43− that would be present in a mixture that is originally 0.015 M H3PO4 as well as 0.005 M NaH2PO4, given the following information:     H3PO4(aq)   ↔   H+(aq)   +   H2PO4−(aq)                   Ka1  =  1.5 x 10−5   H2PO4−(aq)   ↔   H+(aq)   +   HPO42−(aq)                 Ka2  =  2.5 x 10−7   HPO42−(aq)   ↔   H+(aq)   +   PO43−(aq)                    Ka3  =  3.5 x 10−9

For the reaction below, Kc = 1.10 × 10⁻⁸. What is the equilibrium concentration of OH⁻ if the reaction begins with 0.610 M HONH₂? HONH₂ (aq) + H₂O (l) ⇌ HONH₃⁺ (aq) + OH⁻ (aq)

HA, a weak acid, also forms the ion HA, in solution. The reaction is HA(aq) + A (aq) = HA, (aq) The weak acid has K, = 8.64 × 10-7 and the reaction has K = 3.80. Calculate the concentrations of A, H*, and HA, in a 1.00 M solution of HA. [A¯] = M [H*] = M [HA,] = M

Zn(II) hydroxide is amphoteric (amphiprotic). Complete and balance the following equations. Include the phases of all species in the chemical equations. Complete and balance a chemical equation showing how an aqueous suspension of this compound reacts to the addition of a strong acid. Zn(OH)2​(s)+2H+(aq)   Complete and balance a chemical equation showing how an aqueous suspension of this compound reacts to the addition of a strong base.   Zn(OH)2​(s)+2OH−(aq)

Given the following reactions: 3C =D K = 8.33 × 104 D = 3A+ 3B K=3.32 × 10-2