:ӧ :ӧ :ö || :ӧ || NCH3 d. Ӧ: a. b. CH ÖCH, Nн, CH3 ö:

In a coordinate covalent bond: One of the shared electrons comes from one each of the two atoms in the bond One of the atoms in the bond provides both the electrons Neither of the atoms acts as an acid The electron sharing is the same as in a covalent bond Neither atom acts as an electron donor

Table 1: Concentrations of [H3O*] and [OH-] when various amounts hydrochloric acid (HCl, strong acid) or hypochlorous acid (HOC1, weak acid) are dissolved in water to make 1.00 L of solution at 25 Moles of acid added 0.00 0.30 mol HCI 0.75 mol HCI 1.00 mol HCI 0.30 mol HOCI 0.75 mol HOCI 1.00 mol HOCI - 1 - [H3O+] (M) 1.0 x 10-7 0.30 0.75 1.00 9.3 x 10-5 1.5 x 10-4 1.7 x 10-4 [OH-] (M) 1.0 x 10-7 3.3 x 10-¹4 1.3 x 10-14 1.0 x 10-¹4 1.1 x 10-10 6.8 x 10-11 5.9 x 10-11 1. For the strong acid, HCl, in model 1, why are there no HCl molecules present in the beaker? 2. For the weak acid in model 1, why are there mostly HA molecules present in the beaker? 3. From Table 1, what happens to [H3O*] as the number of moles of HOCI increases? 4. From Table 1, how are each of the entries for [OH-] related to the corresponding entries for [H3O+]? 5. If you hadn't been told that HOCI is a weak acid, how could you deduce that from Table 1?

Which one of the following is characteristic of a base? O turns blue litmus red O produces HyO' in water O has a slippery, soapy fee O has a sour taste O is insoluble in water Question 2 Ammonia is a weak base because O it completely ionizes in aqueous solution it forms a dilute solution O it is only slightly soluble in water O it ionizes only slightly in water O it is a good acceptor of protons