Select the solution below that is the most acidic.     [H3O+] = 1.0 × 10–14 M     [H3O+] = 1.0 × 10–6 M     [OH–] = 1.0 × 10–5 M     [OH–] = 1.0 × 10–12 M     [H3O+] = 1.0 × 10–10 M

Each value represents a different aqueous solution at 25 °C. Classify each solution as acidic, basic, or neutral. POH = 13.92 Acidic pH = 12.53 [OH-] = 6.1 × 10-⁹ Basic [H+] = 9.2 x 10-5 pH = 3.20 Answer Bank [OH-] = 7.6 x 10-5 POH Neutral [H+] = 4.61 = 1.0 × 10-7 POH = 7.00 [H+] = 5.7 x 10-11

Question 1 of 11 Complete the balanced chemical reaction for the following weak base with a strong acid. In this case, write the resulting acid and base as its own species in the reaction. NH:(aq) + HCI(aд). |4- n2+ 3+ | 4+ 1 2 3 4 7 8 9. O2 03 04 O5 O6 07 (s) (g) (aq) H20 H3O* OH CI Reset • æ H20 Delete 3.

5. Complete the table for the following strong acids and strong bases solutions. 0.070 M HCI [H*] [OH-] pH pOH acidic/basic/neutral 0.0010 M NaOH [H*] [OH-] pH рон acidic/basic/neutral 2.0 M HNO3 [H*] [OH-] pH pOH acidic/basic/neutral 0.00030 М Са(ОН)2 [H*] [OH-] pH РОН acidic/basic/neutral

Consider the following data on some weak acids and weak bases: acid base K. K, name formula name formula HNO2 4.5 x 10 4 -4 nitrous acid methylamine CH3NH2 |4.4 × 10 hypochlorous acid HCIO 8. 3.0 x 10 ammonia NH3 5 1.8 × 10 Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. solution pH 0.1 M NaCIO choose one 0.1 M KNO3 choose one 0.1 M KNO2 choose one 0.1 M NH4Br choose one

Each value represents a different aqueous solution at 25 °C. Classify each solution as acidic, basic, or neutral. [H+] Acidic = 6.8 × 10-11 [H+] = 1.0 x 10-7 pOH = 1.15 он- pOH = 13.54 pH = 5.65 Basic Answer Bank = 1.2 x 10-5 [OH-] = 3.4 x 10-13 pOH = 7.00 [H+] = 4.1 x 10-3 pH = 9.84 Neutral

Complete the table for each weak acid.

In addition to your recorded pH called make a table showing the corresponding [H3O+]values. Also identify whether 0.1M HCI or 0.1M acetic acid gas a higher [H3O+] and explain why. 1a) pH of 0.1M HCI: 1 pH 1b) pH of 0.1 acetic acid: 3 pH 2a) pH of diluted solution: 2.1 pH 2b) pH of diluted solution: 4.2 pH

Which of the following two acids has the stronger conjugate base? Formic acid, Ka = 1.80 x 10–4                           Hypochlorous acid, Ka = 3.0 x 10–8 Formic acid, because it has a smaller Ka Formic acid, because it has a larger Ka The strength of the conjugate base cannot be obtained from the information given. Hypochlorous acid, because it has a smaller Ka Hypochlorous acid, because it has a larger Ka

Which of the following will produce the strongest conjugate base?        H2O                                                        HCN (Ka = 6.2 x 10-10)      HCl (Ka > 1)                                                 HF (Ka = 7.2 x 10-4)