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The diagrams show solutions of three different weak acids with formulas
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Chemistry
- Each box represents an acid solution at equilibrium. Squares represent H+ ions, and circles represent the anion. Water molecules are not shown. Which figure represents a strong acid? Which figure is a weak acid?arrow_forwardIn each of the following chemical equations, identify the conjugate acid—base pairs. a. HF(aq)+H2O(l)F-(aq)+H3O+(aq)b. CN(aq)+H2O(l)HCN(aq)+OH(aq) c. HCO3-(aq)+H2O(l)H2CO3(aq)+OH-(aq)arrow_forward1. Which of the following can act as a Lewis acid? (Hint : In each case, draw the Lewis electron dot structure of the molecule or ion. Are there lone pairs of electrons on the central atom? If so, it can be a Lewis base. Does the central atom lack an electron pair? If so, it can behave as a Lewis acid.) PH3 BCl3 H2S HS−arrow_forward
- . Using Fig. 16.3, list the approximate pH value of live “everyday” solutions. How do the familiar properties (such as the sour taste for acids) of these solutions correspond to their indicated pH?arrow_forwardUse Table 14.3 to help order the following acids from strongest to weakest HNO3,H2O,NH4+,C5H5NH+arrow_forwardConsider two separate solutions: one containing a weak acid. HA, and one containing HCl. Assume that you start with 10 molecules of each. a. Draw a molecular-level picture of what each solution looks like. b. Arrange the following from strongest to weakest base: Cl- H2O. A- . Explain.arrow_forward
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