D=_K[H*] [H*]+ k, D= Kk [H*]+k₂ When would you use one of the equations over the other? Does it have to do with if you are dealing with an acid or a base?

D=_K[H] [H]+ k, D= Kk [H*]+k₂ When would you use one of the equations over the other? Does it have to do with if you are dealing with an acid or a base?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

D=
K[H*]
[H*]+k₂
D=
Kk₂
[H*]+k₂
When would you use one of the equations
over the other? Does it have to do with if
you are dealing with an acid or a base?

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Can you please help me thankyou
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?