Table 1: Concentrations of [H3O*] and [OH-] when various amounts hydrochloric acid (HCl, strong acid) or hypochlorous acid (HOCI, weak acid) are dissolved in water to make 1.00 L of solution at 25 Moles of acid added 0.00 0.30 mol HC1 0.75 mol HC1 1.00 mol HCI 0.30 mol HOCI 0.75 mol HOCI 1.00 mol HOCI -1- [H30¹] (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 HCI 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?

Table 1: Concentrations of [H3O*] and [OH-] when various amounts hydrochloric acid (HCl, strong acid) or hypochlorous acid (HOCI, weak acid) are dissolved in water to make 1.00 L of solution at 25 Moles of acid added 0.00 0.30 mol HC1 0.75 mol HC1 1.00 mol HCI 0.30 mol HOCI 0.75 mol HOCI 1.00 mol HOCI -1- [H30¹] (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 HCI 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?

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

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

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

Chapter16: Acids And Bases

Section: Chapter Questions

Problem 2STP

See similar textbooks

Similar questions

According to the Arrhenius theory of acids and bases, how do you recognize an acid and a base?
A Liquid HF undergoes an autoionization reaction: 2HFH2F++F (a) Is KF an acid or a base in this solvent? (b) Perchloric acid, HCIO4, is a strong acid in liquid HF. Write the chemical equation for the ionization reaction. (c) Ammonia is a strong base in this solvent. Write the chemical equation for the ionization reaction. (d) Write the net ionic equation for the neutralization of perchloric acid with ammonia in this solvent.
Classify the solutions represented in Exercises 9.28 and 9.30 as acidic, basic, or neutral.
In Arrhenius acidbase theory, what ion is responsible for the properties of a. acidic solutions b. basic solutions
A base is a substance that dissociates in water into one or more ______ ions and one or more ________. a.hydrogen . . . anions b.hydrogen . . . cations c.hydroxide . . . anions d.hydroxide . . . cations
(a) What is the pH of a 0.105 M HCl solution? (b) What is the hydronium ion concentration in a solution with a pH of 2.56? Is the solution acidic or basic? (c) A solution has a pH of 9.67. What is the hydronium ion concentration in the solution? Is the solution acidic or basic? (d) A 10.0-mL sample of 2.56 M HCl is diluted with water to 250. mL What is the pH of the dilute solution?
For which of the following solutions must we consider the ionization of water when calculating the pH or pOH? (a) 3108M HNO3. (b) 0.10 g HCl in 1.0 L of solution. (c) 0.00080 g NaOH in 0.50 L of solution. (d) 1107M Ca(OH)2. (e) 0.0245 M KNO3
Students are often surprised to learn that organic acids, such as acetic acid, contain OH groups. Actually, all oxyacids contain hydroxyl groups. Sulfuric acid, usually written as H2SO4, has the structural formula SO2(OH)2, where S is the central atom. Identify the acids whose structural formulas are shown below. Why do they behave as acids, while NaOH and KOH are bases? a. SO(OH)2 b. ClO2(OH) c. HPO(OH)2
What is the pH of a solution obtained by mixing 235 mL of NaOH with a pH of 11.57 and 316 mL of Sr(OH)2 with a pH of 12.09? Assume that volumes are additive.