Which of the following equations describes the ionization of a weak acid? (1) HCIO3(aq) + H₂O()→ H3O+ (aq) + ClO3(aq) (2) H₂PO4 (aq) + H₂O(aq) - HPO4 (aq) +H30*(aq) (3) HNO2(aq) + OH(aq) → H₂O(n) + NO₂ (aq) (4) HSO4 (aq) + H₂O(H₂SO4(aq) + OH(aq)
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- Citric acid, C6H8O7 (aq), is sued to add a sour taste to foods and soft drinks. It is prepared in a solution with a concentration of 0.52 mol/L, and has a pH of 1.72.Calculate the acid-dissociation constant, Ka for citric acid. Start with the dissociation equation of the acid and an ICE table.1. Standard acids are commonly standardized using sodium carbonate, while standard bases are standardized by potassium hydrogen phthalate. Select one: True False 2. Which of the following is not used as a standard acid because it could oxidize the visual indicators? a. Perchloric acid b. Sulfuric acid c. Nitric acid d. Hydrochloric acidWhich of the following is a representation of the ion product of water? H2O(ℓ)+H2O(ℓ)⇌H3O+(aq)+OH−(aq)H2O(ℓ)+H2O(ℓ)⇌H3O+(aq)+OH-(aq) Kw=[H+][OH−][H2O]Kw=[H+][OH-][H2O] Kw=[H+][OH−][H2O]2Kw=[H+][OH-][H2O]2 Kw=[H2O]2Kw=[H2O]2 Kw=[H+][OH−]Kw=[H+][OH-] Kw=[H+][H2O]
- An aqueous solution of HNO3 has pH 4. What is the pOH of the solution? Answer 1Choose...neutral1x10^-31x10^-4base10Acid1x10^-141x10^-10 The solution is Answer 2Choose...neutral1x10^-31x10^-4base10Acid1x10^-141x10^-10 What is the Hydroxide ion concentration of the solution Answer 3Choose...neutral1x10^-31x10^-4base10Acid1x10^-141x10^-10 What is the Hydrogen ion concentration of the solution Answer 4Choose...neutral1x10^-31x10^-4base10Acid1x10^-141x10^-10Indicate whether following reactions is a strong, weak, or nonelectrolyte represented in the following equations: 1) C6H12O6(s) (in H2O) --> C6H12O6(aq) 2) MgCl2(s) (in H2O) --> Mg2+(aq) + 2Cl-(aq)QUESTION 17 Which of the following chemical reactions corresponds to the base dissociation constant, Kb, for ammonia? NH4+(aq) + H2O (ℓ) ⇌ NH3 (aq) + H3O+(aq) NH3 (aq) + OH−(aq) ⇌ NH2−(aq) + H2O (ℓ) NH3 (aq) + H2O (ℓ) ⇌ NH4+(aq) + OH−(aq) NH3 (aq) + H3O+(aq) ⇌ NH4+(aq) + H2O (ℓ) NH4+(aq) + OH−(aq) ⇌ NH3 (aq) + H2O (ℓ)
- The unknown acid H2X can be neutralized completely by hydroxide ions according to the following equation: H2X(aq) + OH-→ X-2 + H2O. The ion formed as a product, X-2, was shown to have n electrons, where n is even, and has 12 as a factor. What is element X? Propose an IUPAC name for H2X. To completely neutralize a sample of H2X, 35.6 of 0.175 M OH- solution was required, what was the mass of the H2X sample used?10. Indicate whether following reactions is a strong, weak, or nonelectrolyte represented in the following equations: a. K2SO4(s) (in H2O)2K+(aq) + SO42-(aq)b. NH4OH(aq) (in H2O)NH4+ (aq) + OH- (aq) c. C6H12O6(s) (in H2O)C6H12O6(aq)d. MgCl2(s) (in H2O)Mg2+(aq) + 2Cl-(aq)Like all equilibrium constants, the value of Kw depends on temperature. At body temperature (37 °C), Kw = 2.4 * 10-14. What are the [H3O+] and pH of pure water at body temperature?
- The dissociation of 0.15 M phosphoric acid is given by:H3PO4(aq) + H2O(l) ⇄ H2PO4^-(aq) + H3O^+(aq) Ka = 7.1 x 10-3 (at 25°C) H2PO4^-(aq) + H2O(l) ⇄ HPO4^2-(aq) + H3O^+(aq) Ka = 6.3 x 10-8 (at 25°C) HPO4^2-(aq) + H2O(l) ⇄ PO4^3-(aq) + H3O^+(aq) Ka = 6.3 x 10-8 (at 25°C) A. Classify the species, H3PO4, H2PO4-, HPO4^2-, PO4^3-, as acid, base, or ampholyte.B. Applying the systematic method in solving acid-base equilibria problems, calculate the pH of the following:a. 0.050 M H3PO4 b. 0.050 M NaH2PO4 c. 0.050 M Na2HPO4d. 0.050 M Na3PO4The dissociation of 0.15 M phosphoric acid is given by: H3PO4(aq) + H2O(l) ⇄ H2PO4^-(aq) + H3O^+(aq) Ka = 7.1 x 10-3 (at 25°C) H2PO4^-(aq) + H2O(l) ⇄ HPO4^2-(aq) + H3O^+(aq) Ka = 6.3 x 10-8 (at 25°C) HPO4^2-(aq) + H2O(l) ⇄ PO4^3-(aq) + H3O^+(aq) Ka = 6.3 x 10-8 (at 25°C) B. Applying the systematic method in solving acid-base equilibria problems, calculate the pH of the following: a. 0.050 M H3PO4 b. 0.050 M NaH2PO4 c. 0.050 M Na2HPO4 d. 0.050 M Na3PO4The dissociation of 0.15 M phosphoric acid is given by:H3PO4(aq) + H2O(l) ⇄ H2PO4-(aq) + H3O+(aq)Ka = 7.1 x 10-3 (at 25oC) H2PO4-(aq) + H2O(l) ⇄ HPO42-(aq) + H3O+(aq)Ka = 6.3 x 10-8 (at 25oC) HPO42-(aq) + H2O(l) ⇄ PO43-(aq) + H3O+(aq)Ka = 4.5 x 10-13 (at 25oC)Use the systematic method (Mass-Balance Equations, Charge-Balance Equations, or Proton-Balance Equations) to calculate the pH of the following:a. 0.050 M NaH2PO4b. 0.050 M Na2HPO4c. 0.050 M Na3PO4