Concept explainers
Crystals of AgBr can be removed from black-and-white photographic film by reacting the AgBr with sodium thiosulfate.
- a What is the equilibrium constant for this dissolving process?
- b In order to dissolve 2.5 g of AgBr in 1.0 L of solution, how many moles of Na2S2O3 must be added?
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Chapter 17 Solutions
General Chemistry - Standalone book (MindTap Course List)
- An important component of blood is the buffer combination of dihydrogen phosphate ion and the hydrogen phosphate ion. Consider blood with a pH of 7.44. a What is the ratio of [H2PO4] to [HPO42]? b What does the pH become if 25% of the hydrogen phosphate ions are converted to dihydrogen phosphate ion? c What does the pH become if 15% of the dihydrogen phosphate ions are converted to hydrogen phosphate ions?arrow_forwardWrite an equation for each of the following buffering actions. a. the response of a HPO42/PO43 buffer to the addition of OH ions b. the response of a HF/F buffer to the addition of OH ions c. the response of a HCN/CN buffer to the addition of H3O+ ions d. the response of a H3PO4/H2PO4 buffer to the addition of H3O+ ionsarrow_forwardWhat is the pH of a solution that consists of 0.20 M ammonia, NH3, and 0.20 M ammonium chloride, NH4Cl?arrow_forward
- Write 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_forwardIdentify the buffer system(s)the conjugate acidbase pair(s)present in a solution that contains equal molar amounts of the following: a. HF, KC2H3O2, NaC2H3O2, and NaF b. HNO3, NaOH, H3PO4, and NaH2PO4arrow_forwardAn important component of blood is the buffer combination of bicarbonate ion and carbonic acid. Consider blood with a pH of 7.42. a What is the ratio of [H2CO3] to [HCO3]? b What does the pH become if 15% of the bicarbonate ions are converted to carbonic acid? c What does the pH become if 25% of the carbonic acid molecules are converted to bicarbonate ions?arrow_forward
- Malic acid is a weak diprotic organic acid with Ka1 = 4.0 104 and Ka2 = 9.0 105. a Letting the symbol H2A represent malic acid, write the chemical equations that represent Ka1 and Ka2. Write the chemical equation that represents Ka1 Ka2. b Qualitatively describe the relative concentrations of H2A, HA, A2, and H3O+ in a solution that is about one molar in malic acid. c Calculate the pH of a 0.0175 M malic acid solution and the equilibrium concentration of [H2A]. d What is the A2 concentrationin in solutions b and c?arrow_forwardThe pigment cyanidin aglycone is one of the anthocyanin molecules that gives red cabbage (Brassica oleracea var. capitata f. rubra) its characteristic red coloration. Many chemistry students have used this red cabbage indicator to study acid-base chemistry. Estimate tire pH range at which cyanidin agly-cone shows a color change. Anth-H(aq) Anth(aq) + H+ (aq) Ka = 1.3 107arrow_forwardA chemist wanted to determine the concentration of a solution of lactic acid, HC3H5O3. She found that the pH of the solution was 2.60. What was the concentration of the solution? The Kd of lactic acid is 1.4 104.arrow_forward
- Potassium hydrogen phthalate (KHP) concentrations can be determined through titrating samples of KHP (a monoprotic acid) with bases such as NaOH in the presence of an indicator such as phenolphthalein. The indicator is colorless in an acidic solution and turns pink in an alkaline solution. Thus, we can establish an equilibrium for the phenolphthalein with the following reaction. HIn + H2O ⇌ In− + H3O+ If the HIn species is "acid color" or colorless for the phenolphthalein, and the In− species is "base color" or pink for this particular indicator, what color will appear in a flask in which a 0.2993 gram sample of KHP is completely neutralized with an excess of NaOH? The flask will be colorless. The flask will be pink. The flask will be white from KCl precipitation. There is insufficient information to solve this problemarrow_forwardPotassium hydrogen phthalate (KHP) concentrations can be determined through titrating samples of KHP (a monoprotic acid) with bases such as NaOH in the presence of an indicator such as phenolphthalein. The indicator is colorless in an acidic solution and turns pink in an alkaline solution. Thus, we can establish an equilibrium for the phenolphthalein with the following reaction. HIn + H2O ⇌ In− + H3O+ If the HIn species is "acid color" or colorless for the phenolphthalein, and the In− species is "base color" or pink for this particular indicator, what color will appear in a flask in which a 0.2993 gram sample of KHP is completely neutralized with an excess of NaOH? A. The flask will be colourless B. The flask will be pink C. The flask will be white from KCI precipitation D. There is insufficient information to solve this problemarrow_forwardWhat is the equilibrium expression for the following reaction? Zn(s) + 2NaOH(aq) + 2H2O(ℓ) ⇌ Na2Zn(OH)4(aq) + H2(g)arrow_forward
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