Chemistry: An Atoms-Focused Approach
14th Edition
ISBN: 9780393912340
Author: Thomas R. Gilbert, Rein V. Kirss, Natalie Foster
Publisher: W. W. Norton & Company
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HClO is a weak acid (Ka = 4.0 × 10–8) and so the salt NaClO acts as a weak base. What is the pH of a solution that is 0.054 M in NaClO at 25 °C?
Household bleach is prepared by dissolving chlorine in water.
Cl2 (g) + H2O « H+ (aq) + Cl- (aq) + HOCl
Ka for HOCl is 3.2 x10-8 . How much chlorine must be dissolved in one liter of water so that the pH of the solution is 1.19?
Caproic acid HC6H11O2 is found in coconut oil and is used in making artificial flavors. A solution is made by dissolving 0.450mol of caproic acid in enough water to make 2.0L of solution. The solution has [H+] 1.7 x 10-3 M. what is Ka for caproic acid?
Phenol, once known as carbolic acid, HC6H5O, is a weak acid. It was one of the first antiseptics used by Lister. Its Ka is 1.1 x 10-10. A solution of phenol is prepared by dissolving 14.5g of phenol in enough water to make 892mL of solution. For this solution, calculate the pH
HC3H5O3, is found in sour milk. What is the pH of 0.30M lactic acid?
Ka=1.4 ' 10-4
Formic acid, HCOOH, has Ka= 1.8 x 10–4. Calculate the molar concentration of H3O+ in 0.15 M HCOOH and the pH of solution.
Chapter 15 Solutions
Chemistry: An Atoms-Focused Approach
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- What are the major species in solution after NaHSO4 is dissolved in water? What happens to the pH of the solution as more NaHSO4 is added? Why? Would the results vary if baking soda (NaHCO3) were used instead?arrow_forwardFor conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)arrow_forwardWeak base B has a pKb of 6.78 and weak acid HA has a pKa of 5.12. a Which is the stronger base, B or A? b Which is the stronger acid, HA or BH+? c Consider the following reaction: B(aq)+HA(aq)BH+(aq)+A(aq) Based on the information about the acid/base strengths for the species in this reaction, is this reaction favored to proceed more to the right or more to the left? Why? d An aqueous solution is made in which the concentration of weak base B is one half the concentration of its acidic salt, BHCl, where BH+ is the conjugate weak add of B. Calculate the pH of the solution. e An aqueous solution is made in which the concentration of weak acid HA twice the concentration of the sodium salt of the weak acid, NaA. Calculate the pH of the solution. f Assume the conjugate pairs B/BH+ and HA/A are capable of being used as color-based end point indicators in acidbase titrations, where B is the base form indicator and BH is the acid form indicator, and HA is the acid form indicator and A is the base form indicator. Select the indicator pair that would be best to use in each of the following titrations: (1) Titration of a strong acid with a strong base. (i) B/BH+ (ii) HA/A (2) Titration of a weak base with a strong acid. (i) B/BH+ (ii) HA/Aarrow_forward
- What are the equilibrium concentrations of acetic acid, the acetate ion, and H3O+ for a 0.10 M solution of acetic acid (K2 = 1.8 105)? What is the pH of the solution?arrow_forwardThe active ingredient of bleach such as Clorox is sodium hypochlorite (NaClO). Its conjugate acid, hypochlorous acid (HClO), has a Ka of 3.0 × 10–8. (a)The undiluted bleach contains roughly 1 M NaClO. Calculate the pH of 1 M NaClO solution. (b)Some applications require extremely diluted bleach solution, such as swimming pools. Suppose the solution in (a) is diluted by 10,000 -fold. Calculate the pH of the diluted solution, and demonstrate that you can still neglect the autoionization of water in your calculation. (c)Suppose the solution in (a) is diluted by 1million-fold, briefly explain how your approach will be different. Write the equation with [H3O+] as the unknown, but you do not need to solve it.arrow_forwardThe active ingredient of bleach such as Clorox is sodium hypochlorite (NaClO). Its conjugate acid, hypochlorous acid (HClO), has a Ka of 3.0 × 10–8. (a) The undiluted bleach contains roughly 1 M NaClO.Calculate the pH of 1 M NaClO solution. (b) Some applications require extremely diluted bleach solution, such as swimming pools. Suppose the solution in (a) is diluted by 10,000-fold. Calculate the pH of the diluted solution, and demonstrate that you can still neglect the autoionization of water in your calculation. (c) Suppose the solution in (a) is diluted by 1 million-fold, briefly explain how your approach willbe different. Write the equation with [H3O+] as the unknown, but you do not need to solve it.arrow_forward
- Propionic 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_forwardd. During the fermentation of wine, a buffer system consisting of tartaric acid and potassium hydrogen tartrate is created as the result of a biochemical reaction. Assuming that at some point in the process, the concentrations of the two components are approximately equal, determine the pH of the wine. The pKa of tartaric acid is 2.96.arrow_forward1. The ionization constant (Kb) of trimethylamine ((CH)3)3N) is 7.40 x 10–5. If 5.911 grams of trimethylamine is dissolved in 50.0 mL of water, what are the equilibrium concentration of all species present? 2. A buildup of a certain monoprotic acid in the muscle tissues can cause pain during extreme physical activities. A 0.0288 M solution of this acid is found to have a pH of 2.345. Based on the table below, what most likely is the identity of this unknown acid?arrow_forward
- Benzoic acid, HC7H5O2, and its salts are used as food preservatives. Ka for benzoic acid is 6,3 x 10–5. A solution of sodium benzoate, NaC7H5O2, in water has a concentration of 0,015 mol.dm–3. What is the pH of this solution?arrow_forwardMagnesium trisilicate, Mg2Si3O8·H2O in medicine is an antacid. Explain theuse of magnesium silicate as an antacid to reduce acidity in the stomach. Give theequation of reaction. For titration of 5 ml of gastric juice, 10 ml of a 0.15 Msodium hydroxide solution were used. Does the patient need to takeMg2Si3O8·H2O (The concentration of hydrochloric acid in the stomach of a healthy person is constant and amounts to 160 mmol/L)?arrow_forwardWhat is the equilibrium constant, K, for the reaction between HCN (Ka = 6.2 x 10⁻¹⁰) and OH⁻ at 25 °C?arrow_forward
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