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Use Lewis structures to diagram the following reaction in the manner of reaction (16.24)
Identify the Lewis acid and Lewis base.|
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GENERAL CHEMISTRY(LL)-W/MASTERINGCHEM.
- Consider the following acidic equilibrium: H₂CO₃(aq) + H₂O(l) ⇌ HCO₃⁻(aq) + H₃O⁺(aq). If you add NaHCO₃ to this solution, which of the following will occur? A) The reaction quotient will decrease. B) The reaction will shift in the reverse direction. C) The equilibrium constant will increase. D) No changes to the equilibrium positions will take place.arrow_forwardFor each of the following entities • Identify it as a strong or weak acid. • Select the correct arrow to show the changes that occur when the acids are placed in water. • Select the approximate pH for each resulting solution. HCI(aq) is classified as a + acid. The reaction equation with water utilizes which of the following arrows? Choice A Choice B 7 >>7 H2SO3(aq) is classified as a The reaction equation with water would utilize which of the following arrows? Choice A Choice B < 50% H2SO3(aq) + H20(I) • HSO3 (aq) + H30*(aq) The approximate pH of the solution would bearrow_forwardConsider the following chemical equilibrium for the weak base CN in water: CN (aq) + H₂O(1) HCN(aq) + OH(aq). Which of the following statements is correct when more water is evaporated from system? Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a b C d H pH will go up; [OH-]will go up; net amount of OH will go up pH will go down; [OH-] will go up; net amount of OH will go down pH will go down: [OH-] will go down; net amount of OH will go down pH will go up; [OH will go up; net amount of OH will go down X Your answerarrow_forward
- 30. In the reaction HCl(aq) + H₂O(l) ⇒Cl¯(aq)+ H3O+ (aq) does water act as a Brønsted-Lowry acid, a Brønsted-Lowry base, or neither, or both? (A) Neither as an acid nor as a base; water is neutral (B) Both an acid and a base. (C) An acid (D) A base (E) Depends temperaturearrow_forward(a) Using the expression Ka=[H+][A−]/[HA], explain how to determine which solution has the lower pH, 0.10MHF(aq) or 0.10MHC2H3O2(aq). Do not perform any numerical calculations. (b) Which solution has a higher percent ionization of the acid, a 0.10M solution of HC2H3O2(aq) or a 0.010M solution of HC2H3O2(aq) ? Justify your answer including the calculation of percent ionization for each solution.arrow_forwardThe ion HTe− is an amphiprotic species; it can act as either an acid or a base.(a) What is Ka for the acid reaction of HTe− with H2O?(b) What is Kb for the reaction in which HTe− functions as a base in water?(c) Demonstrate whether or not the second ionization of H2Te can be neglected in the calculation of [HTe−] in a 0.10 M solution of H2Te.arrow_forward
- 13.1) a) What is the pH of a 3.6×10-2 M solution of KOH at 25 °C? b) What is the pH of a 3.48×10-2 M solution of the strong acid HClO4? HClO4(aq) + H2O(ℓ) → ClO4-(aq) + H3O+(aq)[HClO4]0 = 3.48×10-2arrow_forwardIn humans, blood pH is maintained within a narrow range:acidosis occurs if the blood pH is below 7.35, and alkalosis oc-curs if the pH is above 7.45. Given that the pKᵥᵥ of blood is 13.63 at 37°C (body temperature), what is the normal range of [H₃O⁺]and of [OH⁻] in blood?arrow_forward(a) Define a Lewis acid and a Lewis base. (b) Define an Arrhenius acid and an Arrhenius base. (c) Identify As2O5 as either a Brønsted-Lowry, a Lewis, or an Arrenius acid or base, and justify your answer to part (c) by writing a balanced chemical equation in showing As2O5 added to water.arrow_forward
- 17.95 A person suffering from anxiety begins breathing rapidly and as a result suffers alkalosis, an increase in blood pH. (a) Using Equation 17.10, explain how rapid breathing can cause the pH of blood to increase. (b) One cure for this problem is breathing in a paper bag. Why does this proce- dure lower blood pH? H*(aq) + HCO, (aq) = H,CO3(aq) = H,O(1) + CO2(g) [17.10]arrow_forwardPhosphoric acid, H, PO, (aq), is a triprotic acid, meaning that one molecule of the acid has pKal pKa2 pKa3 three acidic protons. Estimate the pH and the concentrations of all species in a 0.250 M phosphoric acid solution. 2.16 7.21 12.32 [H, PO,] = M [H*] = M [H,PO,] = M [OH¯] = M * TOOLS x10 [HPO;" ] = 6.2 х10-8 1.34 M pH = [PO] = Marrow_forward(8): Calculate the pH and percent protonation of 0.10 M ammonia NH3 (aq)(use Table 15.9 to find the Kb of this weak base)arrow_forward
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