Chemistry & Chemical Reactivity
9th Edition
ISBN: 9781133949640
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
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Chapter 20.7, Problem 1Q
Interpretation Introduction
Interpretation: It should be defined for the concentration of various hydroxide a ta certain
Concept Introduction: Alkalinity of a water supply is its capacity to accept hydronium ions.
This factor is important to known when assessing water quality, methods of water treatment, and the biology of natural water because the amount of biomass that can be produced depends on the alkalinity.’
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Rank the compounds in each of the following groups in order of increasing acidity or basicity, as indicated, and explain the order you assign.
(a) acidity: HCl, HBr, HI
(b) basicity: H2O, OH−, H−, Cl−
(c) basicity: Mg(OH)2, Si(OH)4, HClO4
(d) acidity: HF, H2O, NH3, CH4
Please calculate the [H+] in the following solution at 298 K:
a) 0.1 mol·dm-3 NaOH;b) 0.1 mol·dm-3 HCN ( 25ºC). (HCN is a monoprotic acid and Ka= 4.9×10^-10 at 25ºC.) c) A mixture of 0.1 mol·dm-3 CH3COOH and 0.1 mol·dm-3 CH3COONa at 25ºC.(CH3COOH is a monoprotic acid and its Ka=1.8×10^-5 at 25ºC.)
(a) Acid rain is no threat to lakes in areas where the rock is limestone (calcium carbonate), which can neutralize the acid. Wherethe rock is granite, however, no neutralization occurs. How does limestone neutralize acid? (b) Acidic water can be treated withbasic substances to increase the pH, although such a procedure is usually only a temporary cure. Calculate the minimum mass oflime, CaO, needed to adjust the pH of a small lake (V = 4 x 109 L) from 5.0 to 6.5. Why might more lime be needed?
Chapter 20 Solutions
Chemistry & Chemical Reactivity
Ch. 20.1 - Prob. 1RCCh. 20.1 - Prob. 2RCCh. 20.2 - Prob. 1RCCh. 20.2 - Prob. 2RCCh. 20.3 - Prob. 1RCCh. 20.3 - Prob. 2RCCh. 20.3 - Prob. 3RCCh. 20.4 - Prob. 1RCCh. 20.4 - Prob. 2RCCh. 20.4 - 3. Which of the following is a renewable energy...
Ch. 20.5 - Prob. 1RCCh. 20.5 - Prob. 2RCCh. 20.6 - Prob. 1QCh. 20.6 - Prob. 1RCCh. 20.7 - Prob. 1QCh. 20.7 - Prob. 2QCh. 20 - In the discussion on the composition of air,...Ch. 20 - Prob. 2PSCh. 20 - Prob. 3PSCh. 20 - Dinitrogen monoxide, N2O (commonly called nitrous...Ch. 20 - Prob. 5PSCh. 20 - Prob. 6PSCh. 20 - Prob. 9PSCh. 20 - Although there are a number of...Ch. 20 - Prob. 12PSCh. 20 - Prob. 13PSCh. 20 - Prob. 14PSCh. 20 - Prob. 15PSCh. 20 - Prob. 17PSCh. 20 - The enthalpy of combustion of isooctane (C8H18),...Ch. 20 - Energy consumption in the United States amounts to...Ch. 20 - Prob. 20PSCh. 20 - Prob. 23PSCh. 20 - Prob. 25PSCh. 20 - Prob. 28PSCh. 20 - In methane hydrate the methane molecule is trapped...Ch. 20 - Prob. 30PSCh. 20 - Prob. 31PSCh. 20 - Prob. 32PSCh. 20 - Prob. 33PSCh. 20 - Prob. 34PSCh. 20 - Prob. 35GQCh. 20 - Prob. 36GQCh. 20 - Prob. 37GQCh. 20 - Prob. 38GQCh. 20 - Prob. 40GQCh. 20 - Prob. 41ILCh. 20 - Prob. 42ILCh. 20 - Define the terms renewable and nonrenewable as...Ch. 20 - Prob. 44SCQCh. 20 - Prob. 45SCQCh. 20 - Prob. 46SCQCh. 20 - Prob. 47SCQCh. 20 - What is the likelihood that hydrogen (H2) will...Ch. 20 - Prob. 49SCQCh. 20 - Which sulfur compounds are atmospheric pollutants?...
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- Acids You make a solution by dissolving 0.0010 mol of HCl in enough water to make 1.0 L of solution. a Write the chemical equation for the reaction of HCl(aq) and water. b Without performing calculations, give a rough estimate of the pH of the HCl solution. Justify your answer. c Calculate the H3O+ concentration and the pH of the solution. d Is there any concentration of the base OH present in this solution of HCl(aq)? If so, where did it come from? e If you increase the OH concentration of the solution by adding NaOH, does the H3O+ concentration change? If you think it does, explain why this change occurs and whether the H3O+ concentration increases or decreases. f If you were to measure the pH of 10 drops of the original HCl solution, would you expect it to be different from the pH of the entire sample? Explain. g Explain how two different volumes of your original HCl solution can have the same pH yet contain different moles of H3O+. h If 1.0 L of pure water were added to the HCl solution, would this have any impact on the pH? Explain.arrow_forwardWrite the chemical equation and the expression for the equilibrium constant, and calculate Kb for the reaction of each of the following ions as a base. (a) sulfate ion (b) citrate ionarrow_forwardThe pH of a 0.10-M solution of propanoic acid, CH3CH2COOH, a weak organic acid, is measured at equilibrium and found to be 2.93 at 25 °C. Calculate the Ka of propanoic acid.arrow_forward
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- What is the concentration of hydroxide ion in a 0.060 M aqueous solution of methylamine. CH3NH2? What is the pH?arrow_forwardTile pH of a solution of household ammonia, a 0.950 M solution of NH3 is 11.612. Determine Kb for NH3 from these data.arrow_forwardWrite the Lewis structures of the reactants and product of each of the following equations, and identify the Lewis acid and the Lewis base in each: (a) CS2+SHHCS3 (b) BF3+FBF4 (c) I+SnI2SnI3 (d) Al(OH)3+OHAl(OH)4 (e) F+SO3SFO3arrow_forward
- The probe of the pH meter shown here is sitting in a beakerthat contains a clear liquid. (a) You are told the liquid ispure water, a solution of HCl(aq), or a solution of KOH(aq).Which one is it? (b) If the liquid is one of the solutions,what is its molarity? (c) Why is the temperature given onthe pH meter?arrow_forward(a) Describe what happens when each of the following molecules is separately dissolved in water and illustrate with an equation in each case: ethanoic acid (CH3COOH) ammonia (NH3) (b) Identify the conjugate acids and bases in the substances mentioned in question 7(a) above. (c) Explain the difference between: (i) a strong acid and weak acid and (ii) a strong base and a weak basearrow_forwardPropionic acid, HC3H5O2, has Ka= 1.34 x 10–5. (a) What is the molar concentration of H3O+ in 0.15 M HC3H5O2 and the pH of the solution? (b) What is the Kb value for the propionate ion, C3H5O2–? (c) Calculate the pH of 0.15 M solution of sodium propionate, NaC3H5O2. (d) Calculate the pH of solution that contains 0.12 M HC3H5O2 and 0.25 M NaC3H5O2.arrow_forward
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