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Practice ProblemATTEMPT
Determine the pH of a 0.25-M solution of pyridinium nitrate
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Chemistry
- 9. What is the pH of a solution whose hydronium ion concentration is 2.5 X 10-8 M? (a) 7.6 (b) 8.0 (c) 2.5 (d) 6.4 (e) 6.0 10. An aqueous solution has a pOH of 9.35, this solution is: (a) Neutral (b) Basic (c) Acidic (d) Impossible - this pOH cannot be reached in an aqueous solution (e) More information is needed. 11. Which is the strongest acid in the provided table below? Acid Acetamide 2-Pyridinamine Alloxanic Acid (a) Acetamide (b) 2-Pyridinamine (c) Alloxanic Acid (d) 4-chlorophenol (e) Quinoxaline pka 0.63 6.82 6.64 4-chlorophenol 9.18 Quinoxaline 0.56 avods rollorarrow_forwardWhich of the following statements are true regarding a 1.0-M solution of a strong acid HA at 25⁰C (Choose all that apply.) (a) [A-] >[H3O+](b) The pH is 0.00(c) [H3O+]=1.0 M(d) [HA]=1.0 Marrow_forwardCalculate the pH and the pOH of each of the following solutions at 25°C for which the substances ionize completely. (Assume K 1.01x 10-14.) (a) 0.215 M HCI pH 4.0 pOH 4.0 (b) 0.0126M NAOH pH 4.0 РОН 4.0 (c) 2.9 M HNO3 pH 4.0 РОН 4.0 (d) 0.0038 M Ca(OH)2 pH 4.0 РОН 4.0 Supporting Materials Periodic Table Constants and I Supplemental Data Factors Additional Materials Section 14.2 80 000 000 DII DD esc F10 F5 F6 F7 F8 F9 F1 F2 F3 F4arrow_forward
- What are the concentrations of H3O+ and OH − in each of the following? (Assume the value of Kw is 1.0 ✕ 10−14.) (a) 3.1 M HBr H3O+ OH − M (b) 0.48 M KOH H3O+ M OH − M (c) 0.055 M Ca(OH)2 H3O+ M OH − M (d) 0.12 M HNO3 H3O+ M OH − Marrow_forwardShow by suitable net ionic equations that each of the following species can act as a Brønsted-Lowry base:(a) HS−(b) PO4 3−(c) NH2 −(d) C2H5OH(e) O2−(f) H2 PO4 −arrow_forwardCalculate the pH of each of the following solutions. (a) 0.109 M HONH, (Ko = 1.1 x 10-3) 4.0 9.34 X (b) 0.109 M HONH3CI 4.0 2.64 (c) pure H₂O 7.00 X (d) a mixture containing 0.109 M HONH₂ and 0.109 M HONH₂CI 4.0 6.20 Xarrow_forward
- 18) What is the pH of a 0.240 M solution of potassium cyanide? Ka (HCN) = 6.2 x 10-10 A) 4.9 B) 9.1 C) 11.3 D) 2.7 E) 9.4arrow_forwardWhich acid is the weakest? (A) HCN (K, = 4.9×10-10) (B) HOCI (K, = 3.5×10 8) (C) HNO2 (K, = 4.5×104) (D) CH;COOH (K, = 1.8×10-5)arrow_forwarda Choose balanced equations showing how the HSO3 ion of sodium hydrogen sulfite, NaHSO3, can be a Brønsted acid. (Select all that apply.) HSO; (aq) + CIo (aq) 2 So,2 (aq) + HC1O(aq) HSO; (aq) + HNO3(aq) 2 H2SO3(aq) + NO3 (aq) HSO; (aq) + HCI(aq) 2 H2 SO3 (aq) + Cl (aq) HSO3 (aq) + OH (aq) 2 So32 (aq) + H20(€) O HSO3 (aq) + Na* (aq) 2 NAHSO3 (s)arrow_forward
- Which is true of acidic solutions? (A) correct answer is not available (B) more OH- ions than H+ ions (C) same amouint of H+ ions and OH- ions (D) more H+ ions than OH- ionsarrow_forwardMethylamine (CH3NH2) has Kb = 4.4 x 10–4. What is the pH of 0.15 M aqueous solution of methylamine? (A) 1.68 (B) 2.09 (C) 11.91 (D) 13.18arrow_forwardOrder the following three solutions from smallest to largest pH:(i) 0.030 M Ba(OH)2 (ii) 0.040 M KOH (iii) pure water.(a) i < ii < iii (b) ii < i < iii (c) iii <i < ii(d) ii < iii < i (e) iii < ii < iarrow_forward
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