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

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

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

Write the conjugate base of each acid in HNO2,  Ka = 4.6 x 10-4; HClO2,  Ka = 1.1 x 10-2; HCN,  Ka = 4.9 x 10-10

Consider the concept of acid strength based upon molecular structure and select the weakest acid. HCIO2 HCIO3 O HBRO2 O HBRO3

Which of the following solutions would have the lowest pH? Assume that they are all 0.10 M in acid at 25°C. The acid is followed by its K, value. Select one: O HNO2, 4.6 x 10-4 O HCIO2, 1.1 x 102 O HCN, 4.9 x 10 10 HF, 3.5 x 104

Fill in the table below for the following solutions if the concentration of hydronium ion is given.Find the pH of each solution given and are they acidic, basic, or neutral? Solution [H3O+] (M) pH Acidic, basic, or neutral? Lemon juice 1.9 x 10-2     Apple cider 5.0 x 10-4     Household cleaner 6.3 x 10-10