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Concept explainers
(a)
Interpretation:
To give Lewis structure of conjugate base of
Concept introduction:
• Lewis structures are the diagrams that show the bonding between the atoms of the molecules and existing lone pairs of electrons.
• Bonding electrons are those electrons which are shared between the atoms resulting in the formation of bond.
• Non-bonding electrons are the valence electrons of the atom which are not shared with another atom.
(b)
Interpretation:
To give Lewis structure of conjugate base of
Concept introduction:
• Lewis structures are the diagrams that show the bonding between the atoms of the molecules and existing lone pairs of electrons.
• Bonding electrons are those electrons which are shared between the atoms resulting in the formation of bond.
• Non-bonding electrons are the valence electrons of the atom which are not shared with another atom.
(c)
Interpretation:
To give Lewis structure of conjugate base of
Concept introduction:
• Lewis structures are the diagrams that show the bonding between the atoms of the molecules and existing lone pairs of electrons.
• Bonding electrons are those electrons which are shared between the atoms resulting in the formation of bond.
• Non-bonding electrons are the valence electrons of the atom which are not shared with another atom.
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Chapter 21 Solutions
CHEMISTRY:PRIN.+REACTIONS-OWLV2 ACCESS
- The pH of a solution is 2.45. What is the molar concentration of hydronium ions in the solution? The answer should be to the proper number of significant digits.arrow_forwardFor the following acid-base reaction, (1) predict the products, showing both reactants and products complete Lewis structures and arrows showing electron flow; (2) label each structure with the lowing: Bronsted acid, Bronsted base, conjugate acid, conjugate base; (3) give a brief definition of a ronsted acid and Bronsted base; (4) predict the direction of the equilibrium and justify your answer. HC0OH + CH3 Nta PRん106Y pkb = 3.36arrow_forwardB). Is solution, acidic, neutral or basic?arrow_forward
- The following two reactions involve proton transfer. In each reaction, identify the acid and the base. Identify the conjugate base of the acid, and the conjugate acid of the base. Draw Lewis electron dot diagrams for each molecule, and describe the rear- rangement of bonding in the reaction as nonbonding electron pairs become cova- lently shared pairs and vice versa. (a) H¿O(€) + NH (aq) → H;0* (aq) + NH3(aq) (b) CH;CH;OH(aq) + NH7 (aq) → CH;CH;O¯(aq) + NH3(aq)arrow_forwardThe molecule (CH3)2N-PF2 has two atoms that can act as Lewis bases. With boron compounds, BH3 attachesto phosphorus, while BF3 attaches to nitrogen. Give your reasoningarrow_forwardExplain how ammonia can function both as a Brønsted base and as a Lewis base.arrow_forward
- The pH of 0.40 M HF(aq) is 1.93. Calculate how the pH changes when 0.356 g of sodium fluoride is added to 50.0 mL of the solution. Assume that the volume change is small and can be neglectedarrow_forwardWrite the formula for the conjugate base of each of the following acids: (a) CH,CICOOH, (b) HIO4, (c) H,PO4, (d) H,PO, (e) HPO, (f) H,SO,, (g) HSO,, (h) HIO3, (i) HSO,, (j) NH, (k) H,S, (1) HS, (m) HCIO. A58arrow_forwardWrite the formula of the conjugate base of CH3CO2Harrow_forward
- Chemists working with fluorine and its compounds some- times find it helpful to think in terms of acid-base reac- tions in which the fluoride ion (F¯) is donated and ассеpted. (a) Would the acid in this system be the fluoride donor or fluoride acceptor? (b) Identify the acid and base in each of these reactions: CIF;O2 + BF; CIF,O, · BF, -- TiF, + 2 KF – K2[TiF,]arrow_forwardPhosphoric acid, H3PO4(aq),H3PO4(aq), is a triprotic acid, meaning that one molecule of the acid has three acidic protons. Estimate the pH and the concentrations of all species in a 0.150 M phosphoric acid solution. pKa1= 2.16 pKa2= 7.21 pKa3= 12.32 [H3PO4]= ? M [H2PO−4]= ? M [HPO2−4]= ? M [PO3−4]= ? M [H+]= ? M [OH−]= ? M pH=arrow_forwardComplete the balanced chemical reaction for the following weak base with a strong acid. In this case, write the resulting acid and base as its own species in the reaction. CH:NH2(aq) + HCIO:(aq)- |3- 2- 4- 2+ |3+ 4+ 1 2 3 4 5 6 7 8 O2 O3 D4 Os |1 6. 10 (s) (1) (g) (aq) + H2O H3O+ H CI OH- C Reset x H2O Deletearrow_forward
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