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E) CI; HCI 36. HCI is a strong acid that completely dissociates in water. 1 M HCI will thus yield 1 M [H] and the pH (pH = -log [H]) will be A) -1 B) 0 C) 1 D) 10 E) 14 37. pka = -log Ka, where K₂ is acid dissociation constant. pK, of a strong acid is thot

E) CI; HCI 36. HCI is a strong acid that completely dissociates in water. 1 M HCI will thus yield 1 M [H] and the pH (pH = -log [H]) will be A) -1 B) 0 C) 1 D) 10 E) 14 37. pka = -log Ka, where K₂ is acid dissociation constant. pK, of a strong acid is thot

Applications and Investigations in Earth Science (9th Edition)
Applications and Investigations in Earth Science (9th Edition)
9th Edition
ISBN:9780134746241
Author:Edward J. Tarbuck, Frederick K. Lutgens, Dennis G. Tasa
Publisher:Edward J. Tarbuck, Frederick K. Lutgens, Dennis G. Tasa
Chapter1: The Study Of Minerals
Section: Chapter Questions
Problem 1LR
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B) HCI; H₂O C) HCI; CI D) OH; H₂O E) CF; HCI 36. HCI is a strong acid that completely dissociates in water. 1 M HCI will thus yield 1 M A) -1 [H] and the pH (pH = -log [H]) will be B) 0 C) 1 D) 10 E) 14 37. pka = -log Ka, where K₁ is acid dissociation constant. pK, of a strong acid is that of a weak acid. 39. A) lower than B) higher than C) equal to D) comparable to E) derived from 38. Increased CO₂ increases the ocean's acidity and results in ocean acidification. Which of the following statement is true about ocean acidification? A) Ocean acidification will dissolve silicate sediments or shells. B) Ocean acidification will decrease H+ concentration in water. C) Ocean acidification will lead to more calcium carbonate precipitation. D) Ocean acidification will dissolve carbonate sediments or shells. E) Ocean acidification has no effect on ocean organisms. is the neutralizing capacity of a solution. A) CEC B) Acidity C) Solubility D) pH E) Total alkalinity 40. When more gypsum (CaSO4) dissolves and adding more Ca²+ to calcite (CaCO3) solution, calcite will become oversaturated and precipitate. This is due to A) incongruent dissolution of calcite B) incongruent dissolution of gypsum C) common ion effect TON D) lower solubility of calcite E) lower solubility of gypsum 10 7 H
Transcribed Image Text:B) HCI; H₂O C) HCI; CI D) OH; H₂O E) CF; HCI 36. HCI is a strong acid that completely dissociates in water. 1 M HCI will thus yield 1 M A) -1 [H] and the pH (pH = -log [H]) will be B) 0 C) 1 D) 10 E) 14 37. pka = -log Ka, where K₁ is acid dissociation constant. pK, of a strong acid is that of a weak acid. 39. A) lower than B) higher than C) equal to D) comparable to E) derived from 38. Increased CO₂ increases the ocean's acidity and results in ocean acidification. Which of the following statement is true about ocean acidification? A) Ocean acidification will dissolve silicate sediments or shells. B) Ocean acidification will decrease H+ concentration in water. C) Ocean acidification will lead to more calcium carbonate precipitation. D) Ocean acidification will dissolve carbonate sediments or shells. E) Ocean acidification has no effect on ocean organisms. is the neutralizing capacity of a solution. A) CEC B) Acidity C) Solubility D) pH E) Total alkalinity 40. When more gypsum (CaSO4) dissolves and adding more Ca²+ to calcite (CaCO3) solution, calcite will become oversaturated and precipitate. This is due to A) incongruent dissolution of calcite B) incongruent dissolution of gypsum C) common ion effect TON D) lower solubility of calcite E) lower solubility of gypsum 10 7 H
C) K = aso? D) K = E) K = 31. A special name for equilibrium constant for minerals is A) constant B) IAP C) solubility a24a50² acaso4(s) aca24 so² acaso4(s) D) solubility product E) saturation index 32. In very dilute solutions, the dissolved components are spread far apart, so interactions among them are very weak and activity coefficient is very close to A) 0 B) 1 C) 10 D) 100 E) 1000 to assess the effects of temperature on solubility of minerals. 33. You can use A) relationship between solubility product and Gibbs free energy change of reaction log K = -A,Gº 2.303RT B) solubility product Ksp C) saturation index (KAP) SI = log D) van't Hoff equation log K₁₂ = log K₁₁ + E) ionic strength 1/2 - 1/2) ▲‚Hº 2.303R T₁ T₂ -1 34. If the ionic strength of a solution is < 0.1 mol L-¹, you will use calculate its ionic strength. A) Debye-Huckel B) Davies C) activity coefficient D) equilibrium E) kinetics 35. In the reaction HCl + OH ⇒ H₂O + Cl, base. A) OH; CI- 6 is the acid and equation to is the conjugate
Transcribed Image Text:C) K = aso? D) K = E) K = 31. A special name for equilibrium constant for minerals is A) constant B) IAP C) solubility a24a50² acaso4(s) aca24 so² acaso4(s) D) solubility product E) saturation index 32. In very dilute solutions, the dissolved components are spread far apart, so interactions among them are very weak and activity coefficient is very close to A) 0 B) 1 C) 10 D) 100 E) 1000 to assess the effects of temperature on solubility of minerals. 33. You can use A) relationship between solubility product and Gibbs free energy change of reaction log K = -A,Gº 2.303RT B) solubility product Ksp C) saturation index (KAP) SI = log D) van't Hoff equation log K₁₂ = log K₁₁ + E) ionic strength 1/2 - 1/2) ▲‚Hº 2.303R T₁ T₂ -1 34. If the ionic strength of a solution is < 0.1 mol L-¹, you will use calculate its ionic strength. A) Debye-Huckel B) Davies C) activity coefficient D) equilibrium E) kinetics 35. In the reaction HCl + OH ⇒ H₂O + Cl, base. A) OH; CI- 6 is the acid and equation to is the conjugate
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