Principles of Modern Chemistry
8th Edition
ISBN: 9781305079113
Author: David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher: Cengage Learning
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Chapter 15, Problem 88AP
Interpretation Introduction
Interpretation:
The solution is prepared from 0.23 mol of HF and 0.57 mol of HClO which is dissolved in 3.60 L of water. The pH of stronger acid and equilibrium concentration of HF, F-, HCO and ClO- should be determined.
Concept Introduction:
pH is used to determine the concentration of solution.
The ratio of mole to the volume of solution is known as concentration.
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Calculate the pH of a solution that is prepared by dissolving 0.23 mol of hydrofluoric acid (HF) and 0.57 mol of hypochlorous acid (HClO) in water and diluting to 3.60 L. Also, calculate the equilibrium concentrations of HF, F-,HClO, and ClO2. (Hint: The pH will be determined by the stronger acid of this pair.)
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Chapter 15 Solutions
Principles of Modern Chemistry
Ch. 15 - Vitamin C is ascorbic acid (HC6H7O6), for which Ka...Ch. 15 - Suppose a 0.100 M solution of each of the...Ch. 15 - Sulfanilic acid (NH2C6H4SO3H) is used in...Ch. 15 - Phthalic acid ( H2C8H4O4, abbreviated H2Ph ) is a...Ch. 15 - Prob. 88APCh. 15 - Prob. 94APCh. 15 - Prob. 100APCh. 15 - Prob. 102AP
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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_forwardCalculate the pH of a 0.10 molar solution of sodium formatearrow_forwardThe Kb of pyridine, C5H5N, is 1.7 x 10−9. Calculate the pH of a 0.124 M solution of pyridinium bromide, C5H5NH+Br−.arrow_forward
- calculate the pH of a 0.10 M perchloric ,HCIO4, solution.arrow_forwardDetermine the pH of each solution and classify it as acidic,basic, or neutral.(a) pOH = 8.5(b) pOH = 4.2(c) pOH = 1.7(d) pOH = 7.0arrow_forwardBacteria in the human mouth release enzymes to break up sucrose, and thenpolymerize glucose to form a bacterial plaque. When this glucose is digested, it formslactic acid, which causes tooth decay. Tooth enamel is made of calcium phosphate.Lactic acid has a Ka 1.38x10 -4 and ionizes into lactate and H3O+ ions. Assuming aninitial lactic acid concentration of 0.10 mol/L on your tooth, determine the pH(assume a 1:1:1 mole ratio) and the percent ionization. Should people be concernedwith plaque buildup? Justify your answer.arrow_forward
- Suppose that, instead of using NaOH, a base such as Ba(OH)2 had been used. What changes in the calculations would then have to be made to determine the molar concentrations of the base?arrow_forwardCalculate the pH of a 0.25 mol/L solution of magnesium hydroxidearrow_forwardCalculate the pH of a solution in which [OH−]=7.1×10−3M.arrow_forward
- Define pH in words. The strong acid HClaq has a pH value of 1, use the following equation for a strong acid: HClaq à H+aq + Cl-aq and convert the following expression to deduce the hydrogen ion concentration: pH = -log10 [H+] (ii) Use the above expression to deduce the pH of HCl (aq) given the concentration of the acid to be 4.5 mol/dm3arrow_forwardCalculate the pH of the weak acid, lactic acid (HC3H5O3), if the concentration is 0.10 mol/L and the Ka value is 1.4 x 10-4arrow_forwardCalculate the pH of 0.10 M (COOH)2 (aq), oxalic acid. Ka1 = 5.9 × 10–2 ; Ka2 = 6.4 × 10–5.arrow_forward
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