Concept explainers
Practice Problem ATTEMPT
Identify and label the species in each reaction:
(a)
(b)
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Chemistry
- s practice Identify Brensted-Lowery Acids and bases and their Conjugates (a) C,H;N (aq) + H,O (I) 2 CH,NH* (aq) + OH (aq) (b) HNO, (aq) + H,O () → NO, (aq) + H,O* (aq) Created with Darrow_forwardA) Which of the following reactions show how HSeO3- acts as a Bronsted-Lowry acid? (Select all that apply.) a) HSeO3-(aq) + CN-(aq) → SeO32-(aq) + HCN(aq) b) HSeO3-(aq) + Li+(aq) → LiHSeO3(s) c) HSeO3-(aq) + H3O+(aq) → H2SeO3(aq) + H2O d) HSeO3-(aq) + H2SO4(aq) → H2SeO3(aq) + HSO4-(aq) e) HSeO3-(aq) + OH-(aq) → SeO32-(aq) + H2O B) Which of the following reactions show how HSeO3- acts as a Bronsted-Lowry base? (Select all that apply.) a) HSeO3-(aq) + CN-(aq) → SeO32-(aq) + HCN(aq) b) HSeO3-(aq) + Li+(aq) → LiHSeO3(s) c) HSeO3-(aq) + H3O+(aq) → H2SeO3(aq) + H2O d) HSeO3-(aq) + H2SO4(aq) → H2SeO3(aq) + HSO4-(aq) e) HSeO3-(aq) + OH-(aq) → SeO32-(aq) + H2Oarrow_forwardH. C. 5.7 x 10-10 -11 1.5 x 10- H. | C. 7.9 х 10-12 Br [HB*][OH B(aq) + H20(1)2 HB†(aq) + OH (aq) [B] The table above provides the chemical structures for weak bases and their ionization constants, K. Based on the data, which of the following provides the best reason for the trend in base strengths? A The number of hydrogen atoms The number of resonance structures The different electronegativities of H, I, and Br The different molar masses HO=Uarrow_forward
- 10. What is the value of [OH-] in a 0.015 MCHCOOH solution? Ka= 1.8 x 10-5 (a) 1.9 x 10-11 M(b) 2.0 x 10-6 M(c) 1.0 x 10-9 M (d) 5.0 x 10-8 M(e) 5.0 x 10-7 Marrow_forwardthis reaction takes place in a (aq) solution HNO2(aq)+NO3-(aq) =?= HNO3(aq)+NO2-(aq) the net reaction proceed from: A) The reaction will not happen B) Left -> Right C) Right -> Leftarrow_forwardThe equilibrium for the reaction between (CH3)2NH(CH3)2NH, a weak base, and water is represented by the equation below. The table shows the pHpH of three solutions of (CH3)2NH(aq)(CH3)2NH(aq) at 25°C25°C. (CH3)2NH(aq)+H2O(l)⇄(CH3)2NH2+(aq)+OH-(aq)Kb=5.4×10−4at25°C(CH3)2NH(aq)+H2O(l)⇄(CH3)2NH2+(aq)+OH−(aq)Kb=5.4×10−4at25°C [(CH3)2NH][(CH3)2NH] pH at25°CpH at25°C 0.050 11.69 0.10 11.85 0.20 12.01 Based on the information given, which of the following is true? a.Solutions with a higher concentration of (CH3)2NH(CH3)2NH have a higher pOHpOH because to reach equilibrium a smaller amount of the conjugate acid (CH3)2NH2+(CH3)2NH2+ is produced. b.Solutions with a higher concentration of (CH3)2NH(CH3)2NH have a higher pOHpOH because to reach equilibrium more OH−OH− is produced. c.Solutions with a higher concentration of (CH3)2NH(CH3)2NH have a higher pHpH because to reach equilibrium a smaller amount of the conjugate acid (CH3)2NH2+(CH3)2NH2+…arrow_forward
- (1) Write a net ionic equation for the reaction between H3PO4(aq) and NO₂ (aq) that shows H3PO4(aq) behaving as a Bronsted-Lowry acid. BL acid + BL base Submit Answer Retry E (2) Decide which would be favored at equilibrium for this reaction, reactants or products? ✓ BL base reactants products + BL acidarrow_forwardProblem #2arrow_forwardCan someone solve part B and then explain why its the right answer. I'm confused on how to solve b.arrow_forward
- Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning