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Practice Exercise 2 For each reaction, use Figure 16.4 to predict whether the equilibrium lies to the left or to the right: (a) HPO,²-(aq) + H,0(1) = (b) NH,(aq) + OH (ag) = NH,(aq) + H,O(1) H,PO, (aq) + OH (aq)

Practice Exercise 2 For each reaction, use Figure 16.4 to predict whether the equilibrium lies to the left or to the right: (a) HPO,²-(aq) + H,0(1) = (b) NH,(aq) + OH (ag) = NH,(aq) + H,O(1) H,PO, (aq) + OH (aq)

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Preview File Edit View Go Tools Window Help Sun Aug 8 5:50 PM bartleby.com (1) Ć Theodore E. Brown, H. Eugene H LeMay, Bruce E. Bursten, Cather... Page 717 of 1,246 – Shared Search Theodore E. Brown, H. Eu... (a) i < ii < iii (b) ii < i< iii (c) iii < i< ii (d) ii < iii < i (e) iii < ii < i Raluise ngh af Acita and lann Practice Exercise 2 For each reaction, use Figure 16.4 to predict whether the equilibrium lies to the left or to the right: (а) НРО (ад) + H0(1) — Н,РО, (ад) + Он (ад) ngeleakelm Cel ope (Ъ) NH, (аq) + он (ад) — NH, (ag) + H,0() 676 16.3 | The Autoionization of Water CON A One of the most important chemical properties of water is its ability to act as either a Brønsted-Lowry acid or a Brønsted-Lowry base. In the presence of an acid, it acts as a proton acceptor; in the presence of a base, it acts as a proton donor. In fact, one water molecule can donate a proton to another water molecule: Ge H Some Theght w E Crigg WIO at l H2O(1) + H2O(1) ОН (ад) + H;O* (aq) asa l e wio ed er r aalo od O ov a A. uriel .l IE + :ö-H :ö-H F ng Se ger + :O: + Н-ӧ—Н IR Pd te Pekes s reton-Trawer H H H. H [16.12] 677 + ind sy Acid Base We call this process the autoionization of water. Because the forward and reverse reactions in Equation 16.12 are extremely rapid, no water molecule remains ionized for long. At room temperature only about two out of every 10' water molecules are ionized at any given instant. Thus, pure water consists almost entirely of H2O molecules and is an extremely poor conductor of electricity. Nevertheless, the autoionization of water is very important, as we will e 16.3 The Autoionization of Water t ren lade E ad hesa p W he ld w e upl . delg M soon see. Th.pa Lig 678 3 AUG 8. étv A P 00 |||
Transcribed Image Text:Preview File Edit View Go Tools Window Help Sun Aug 8 5:50 PM bartleby.com (1) Ć Theodore E. Brown, H. Eugene H LeMay, Bruce E. Bursten, Cather... Page 717 of 1,246 – Shared Search Theodore E. Brown, H. Eu... (a) i < ii < iii (b) ii < i< iii (c) iii < i< ii (d) ii < iii < i (e) iii < ii < i Raluise ngh af Acita and lann Practice Exercise 2 For each reaction, use Figure 16.4 to predict whether the equilibrium lies to the left or to the right: (а) НРО (ад) + H0(1) — Н,РО, (ад) + Он (ад) ngeleakelm Cel ope (Ъ) NH, (аq) + он (ад) — NH, (ag) + H,0() 676 16.3 | The Autoionization of Water CON A One of the most important chemical properties of water is its ability to act as either a Brønsted-Lowry acid or a Brønsted-Lowry base. In the presence of an acid, it acts as a proton acceptor; in the presence of a base, it acts as a proton donor. In fact, one water molecule can donate a proton to another water molecule: Ge H Some Theght w E Crigg WIO at l H2O(1) + H2O(1) ОН (ад) + H;O* (aq) asa l e wio ed er r aalo od O ov a A. uriel .l IE + :ö-H :ö-H F ng Se ger + :O: + Н-ӧ—Н IR Pd te Pekes s reton-Trawer H H H. H [16.12] 677 + ind sy Acid Base We call this process the autoionization of water. Because the forward and reverse reactions in Equation 16.12 are extremely rapid, no water molecule remains ionized for long. At room temperature only about two out of every 10' water molecules are ionized at any given instant. Thus, pure water consists almost entirely of H2O molecules and is an extremely poor conductor of electricity. Nevertheless, the autoionization of water is very important, as we will e 16.3 The Autoionization of Water t ren lade E ad hesa p W he ld w e upl . delg M soon see. Th.pa Lig 678 3 AUG 8. étv A P 00 |||
Preview File Edit View Go Tools Window Help Sun Aug 8 5:50 PM bartleby.com (1) Ć Theodore E. Brown, H. Eugene H LeMay, Bruce E. Bursten, Cather... Page 715 of 1,246 – Shared Search SIroriger a UUSE, irie WEUKET TiS corijuguie uCIA. Tiius, II we KIHOW HoW TeaUIly ali aciu UOliates Theodore E. Brown, H. Eu... protons, we also know something about how readily its conjugate base accepts protons. The inverse relationship between the strengths of acids and their conjugate bases is illustrated in ▼ Figure 16.4. Here we have grouped acids and bases into three broad categories based on their behavior in water: wng lte for hoton er actione u Balui Strenghe of Acie and lane mletesl Cel GO FIGURE l Th ln ope If 02- ions are added to water, what reaction, if any, occurs? ACID BASE HCl Strong acids - Negligible basicity H,SO4 HNO3 H3O* (aq) HSO4 H3PO4 HSO4 NO3 676 H2O 2- SO4 H,PO4 HF F LA ne CH;COOH H2CO3 H,S CH;COO¯ t The L y . ng . ng HCO3 Crigg Weak acids Weak bases g epeo g HS H Thinght НРО- NH3 H,PO4 NH4* HCO3 HPO,?- H,O IM t A WIO at a ALE e ing ger A Tha d e CO2 3- PO4 NA M OU RIod oM a UPl E The . ed ee et r le r IR Pdghe Peen s reeTraer labrn ОН Negligible acidity· Strong bases H2 CH4 H ind CH3 677 A Figure 16.4 Relative strengths of select conjugate acid-base pairs. The two members of each pair are listed opposite each other in the two columns. e ite TH te haleie SECTION 16.2 Brønsted-Lowry Acids and Bases 677 16.3 |The Autoionization of Water L lil rin l 1. A strong acid completely transfers its protons to water, leaving essentially no undis- sociated molecules in solution. (Section 4.3) Its conjugate base has a negligible tendency to accept protons in aqueous solution. (The conjugate base of a strong acid Lig w 3 AUG 8. étv 00 Base strength increasing Acid strength increasing
Transcribed Image Text:Preview File Edit View Go Tools Window Help Sun Aug 8 5:50 PM bartleby.com (1) Ć Theodore E. Brown, H. Eugene H LeMay, Bruce E. Bursten, Cather... Page 715 of 1,246 – Shared Search SIroriger a UUSE, irie WEUKET TiS corijuguie uCIA. Tiius, II we KIHOW HoW TeaUIly ali aciu UOliates Theodore E. Brown, H. Eu... protons, we also know something about how readily its conjugate base accepts protons. The inverse relationship between the strengths of acids and their conjugate bases is illustrated in ▼ Figure 16.4. Here we have grouped acids and bases into three broad categories based on their behavior in water: wng lte for hoton er actione u Balui Strenghe of Acie and lane mletesl Cel GO FIGURE l Th ln ope If 02- ions are added to water, what reaction, if any, occurs? ACID BASE HCl Strong acids - Negligible basicity H,SO4 HNO3 H3O* (aq) HSO4 H3PO4 HSO4 NO3 676 H2O 2- SO4 H,PO4 HF F LA ne CH;COOH H2CO3 H,S CH;COO¯ t The L y . ng . ng HCO3 Crigg Weak acids Weak bases g epeo g HS H Thinght НРО- NH3 H,PO4 NH4* HCO3 HPO,?- H,O IM t A WIO at a ALE e ing ger A Tha d e CO2 3- PO4 NA M OU RIod oM a UPl E The . ed ee et r le r IR Pdghe Peen s reeTraer labrn ОН Negligible acidity· Strong bases H2 CH4 H ind CH3 677 A Figure 16.4 Relative strengths of select conjugate acid-base pairs. The two members of each pair are listed opposite each other in the two columns. e ite TH te haleie SECTION 16.2 Brønsted-Lowry Acids and Bases 677 16.3 |The Autoionization of Water L lil rin l 1. A strong acid completely transfers its protons to water, leaving essentially no undis- sociated molecules in solution. (Section 4.3) Its conjugate base has a negligible tendency to accept protons in aqueous solution. (The conjugate base of a strong acid Lig w 3 AUG 8. étv 00 Base strength increasing Acid strength increasing
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