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Practice ProblemATTEMPT
Determine the pH of a 0.25-M solution of pyridinium nitrate
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Chemistry
- Which 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_forwardWhat 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_forward
- Calculate 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_forward18) 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_forward
- a 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_forwardWhich 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_forward
- Order 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_forwardWhich one of the following correctly shows the weak acid equilibrium for trichloroacetic acid, CCI,COOH? A) CCI,COOH (aq)= CC,Co (aq) + ОН (аq) в) ССІ СООН (аq) + н.о () — CC,COOH, (aq) + OH (aq) С) CI СООH (aq) + Н,О (1) CCI,CoO (aq) + H,0* (aq) D) CCI,COOH (aq) + H,O (1) = CC,CO(OH), (aq) + H* (aq)arrow_forwardPlease help: A) Write the acidic equilibrium equation for HC₆H₅CO₂ B) The concentration of hydroxide ion in an aqueous solution at 25°C is 5.7 × 10⁻⁴ M. What is the concentration of the hydronium ion? C) The concentration of the hydronium ion in an aqueous solution at 25 °C is 0.0025 M. What is the concentration of the hydroxide ion? D) The OH⁻ concentration in an aqueous solution at 25 °C is 8.3 × 10⁻³. What is [H⁺]? Thank you!!arrow_forward
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