(b) II I III (d) I III II. Higher the electronegativity of the atom attached with oxygen greater the acidity. So order is III II I (c)
|
|
- Paulina Haynes
- 5 years ago
- Views:
Transcription
1 Chemistry: Concepts of Acids and Bases-1 Solved Problems bjective Problem 1: The following acids have been arranged in order of increasing acid strength. Identify the correct order. Cl (I) Br (II) I (III) (a) I II III (b) II I III (c) III II I (d) I III II igher the electronegativity of the atom attached with oxygen greater the acidity. So order is III II I (c) Problem : Among the following compounds, the strongest acid is (a) C C (b) C66 (c) C6 (d) C ydrogen atom attached with oxygen is maximum acidic. (d) Problem : The conjugate acid of P is (a) P (b) P (c) P (d) P Conjugate acid and base differs by one proton hence the conjugate acid of P is P (b) Problem : The anhydride of Cl is (a) Cl (b) Cl (c) Cl7 (d) None Cl has +7 oxidation state in Cl7 and Cl Anhydride is Cl7 (c) Problem 5: The conjugate acid of azide ion is (a) N (b) N (c) N (d) N N + + N (b) Problem 6: P is.. acid (a) Monobasic (b) Dibasic
2 Chemistry: Concepts of Acids and Bases- (c) Tribasic P (d) None Thus two hydrogens are attached with oxygen, therefore P is dibasic acid (b) Problem 7: Which salt undergoes hydrolysis (a) KCl (b) NaN (c) CaS (d) CN Salts of strong acids and strong bases do not hydrolyse. Thus only CN is hydrolysed (d) Problem 8: In the following compounds, the order of acidity is N C N (I) (II) (III) (IV) (a) III > IV > I > II (c) II > I > III > IV (b) I > IV > III > I (d) IV > III > I > II +I effect decreases acidity, I and R effect increases acidity. N group cannot exert R effect from the metal position. (d) Problem 9: Which of the following species is an acid and also a conjugate base of another acid (a) S (b) S (c) (d) + S can donate a proton also can accept a proton. (a) Problem 10: Among the following which is the least basic (a) F (b) I (c) Cl (d) Br I is the strongest acid among the hydro acids of halogen, so I is least acid. Problem 11: Which of the following species cannot be a Bronsted base? (a) (b) C (c) C (d) P. (b)
3 Chemistry: Concepts of Acids and Bases- Problem 1: In Mond s process, C(g) is passed over Ni(s) when volatile complex Ni( C ) escapes. Ni(s) C(g) Ni(C) (g) In this reaction, which one is correct. (a) Ni(s) is a Lewis base and C(g) is a Lewis acid (b) Ni(s) is a Lewis acid and C(g) is a Lewis base (c) Ni(s) as well as C(g) behaves as amphoteric (d) It is not Lewis acid-base reaction. (b) Problem 1: The compound Cl behaves as. in the reaction Cl + F + Cl + F (a) Strong acid (b) Strong base (c) Weak acid (d) Weak base Cl is accepting proton in F medium and acts as weak base. (d) Problem 1: Which of the following statements is true for a 0.1 M solution of a weak acid A? (a) the p is 1.00 (b) the p is less than 1 (c) [ ] [A ] (d) [ ] [A ]. (c) Problem 15: The anhydride of P is (a) P5 (c) P (b) P (d) None P has +5 oxidation numbers in P5 and P (a) Problem 16: The conjugate base of hydrazoic acid is (a) N (b) N (c) N (d) N N (c) N Problem 17: Strongest conjugate base is: (a) C (b) C C
4 Chemistry: Concepts of Acids and Bases- (c) C N (d) (d) Problem 18: Which of the following orders regarding acid strength is correct? (a) C < CC < PhC (b) C > PhC > CC (c) C > CC > PhC (d) CC > C > PhC (b) Problem 19: In the following compounds, the correct order of basicity is N N N N (I) (II) (III) (IV) (a) IV > I > III > II (c) II > I > III > IV (b) III > I > IV > II (d) I > III > II > IV (d) Problem 0: Arrange the following ions in increasing order of acidity. [Na ()6] +, [Al ()6] +,[Mn ()6] +, [Ni ()6] + (I) (II) (III) (IV) (a) I < II < III < IV (b) I < III < IV < II (c) I < III < II < IV (d) II < IV < III < II (b) Subjective Problem 1: Why sulphuric acid is stronger than sulphurous acid? Subphuric acid is stronger than sulphurous since the sulphur atom in sulphuric acid has more coordinated oxygen atoms. S S Sulphurous acid Sulphuric acid Problem : Explain
5 Chemistry: Concepts of Acids and Bases-5 F is a strong base Problem : Problem : Problem 5: Problem 6: Problem 7: F is a conjugate base of acid F. F is a weak acid. Weaker the acid, stronger the conjugate base. In hypophosphorus acid P is in +1 state (P) and in phosphoric acid(p) P is in +5 state but still P is stronger than P. Explain. A consideration of the structures of these acids explains the observed trend. P P The hydrogen atoms bonded directly to phosphorus are not acidic as the P bond is not polar enough due to equal electronegativity of phosphours and hydrogen. Acidity arises due to groups, one in P and three in P. The inductive effect of the single oxygen atom acts in the single bond in P but it is distributed over three bonds in P respectively. So bond in P much easily broken, explaining its higher acidity over P. Compare the acidity between Cl and As. Cl is much stronger than As, conjugate base of it more stabilised than conjugate base of As. pnitro phenol is stronger acid than phenol. Explain Conjugate base of pnitrophenol is more resonance stabilized than conjugate base of phenol (one more canonical from is possible for conjugate base of pnitro phenol). Compare the basic strengths of ortho, meta and para isomers of nitroaniline and predict the decreasing order of basicity. The N group which is a powerful electron withdrawing inductive effect when present at ortho and para positions for the interaction of the unshared pair of the amino nitrogen with the delocalised p-orbital system of the benzene nucleus is then enhanced. The neutral molecule is thus stabilized even further with respect to the cation, resulting in further weakening as a base. Thus the order of basicity of nitroanilines is as m-nc6n p-nc6n o-nc6+n. Which way would the p shift when AlCl is added to pure water? Write a net ionic equation to support your answer. AlCl + Al() Cl
6 Chemistry: Concepts of Acids and Bases-6 As it is clear from the above equation that aqueous solution of AlCl is acidic, so p will shift below 7. Problem 8: Write the formula for the conjugate acids of the following bases: (a) C (b) C (c) C55N (d) N 5. In each case the conjugate acid is formed from the base by the addition of a proton. a) C. This is a species which might form in liquid acetic acid upon addition of a strong acid. C. Note that C can serve as both an acid and a base. (c) b) d) CN 5 5. N. Note that bases, like acids, can be polyfunctional. The second 6 proton is accepted by N, however, only with great difficulty. Problem 9: a) Is a solution of AlCl in water acidic, basic, or neutral? b) Write a net ionic equation to support your answer. Problem 10: Problem 11: a) Acidic b) Al( ) [Al( ) ] or Al( ) [Al( ) ] When a strong acid dissolves in water, there are ions in the solution afterward. When a soluble metal hydroxide dissolves in water, there are ions in solution afterward. Besides the difference in the identity of the ions, what is the basic difference in these processes? The dissolving process causes the formation of the ions in the case of the strong acids; the ions are present from the beginning in the case of the metal hydroxides. The ionization constant of CN is given as The ionization constant of N + is Decide which is the stronger acid, CN or N +. N + is slightly stronger acid (Ka for N + = ). [Larger the value of ionization constant, stronger the acid will be.] Problem 1: Arrange o-nitro, p-nitro, m-nitrophenol in decreasing acid strength p-nitrophenol o-nitrophenol m-nitrophenol The N is electron withdrawing and acid strengthening. Its resonance effect, which occurs only from para and ortho positions, predominates over its inductive effect, which occurs also from the meta position between ortho and para derivative, para derivative is more acidic because increase of ortho the
7 Chemistry: Concepts of Acids and Bases-7 hydrogen of phenolic group is attached through hydrogen bonding with oxygen of N group and hence not possible to remove easily. Problem 1: Which is the stronger base towards a proton N or P and why? Problem 1: Problem 15: Problem 16: Problem 17: Bond energy (N P ) ionisation suggests that N will be stronger base. This is constituent with the relative strengths of the respective conjugate acids: N P. Why pyrole is less basic than pyridine? Pyrole uses lone pair of electron on nitrogen atom in delocalisation hence less electron are available for protonation, hence less basic than pyridine. Arrange according to increasing Lewis acid character, B(nBu), B(tBu) The highly branched tertiary butyl group involve appreciable back strain (Bstrain) when the boron atom changes to pyramidal environment on adduct formation. This destabilizes the adduct. ence the order is B(tBu) < B(nBu) Which of the following oxide is most acidic Ag, V5, C, N5 The oxide with the highest positive oxidation state on the element other than should be most acidic. xidation states of V in V5 and N in N5 are both +5. But the electronegativity of N is higher, making N5 the most acidic oxide. n the basis of -bonding explain that the second ionization constant K for fumaric acid is greater than for maleic acid. We know that -bonding involving acidic has an acid weakening effect and -bonding in conjugate base has an acid strengthening effect. Both dicarboxylic acids have two ionisable hydrogen atoms. Considering second ionization step. C C C C C C C C Fumarate monoanion (no -bonding) Maleate monoanion (-bonding) Since the second ionisable of the Maleate participates in -bonding more energy is needed to remove this because the -bond must be broken. The maleate mono anion is, therefore, the weaker acid.
8 Chemistry: Concepts of Acids and Bases-8 Assignments (New Pattern) SECTIN I Single Choice Questions 1. Consider the complete ionization of S (strong acid) and (C), oxalic acid (weak acid) in liquid N. S N N S (C) N N (C ) Liquid N is called : (a) proton-acceptor (b) leveling solvent (c) both (d) none of these.. ydrated proton cannot be (a) 5 (b) 9 (c) 5 (d) () n.. The strongest base that can exist in aqueous solution is : (a) N (b) Cl (c) (d) F.. Select correct statement: (a) NF is stronger base than N (b) N is stronger base than NF (c) N is always a base and NF an acid (d) N is always an acid and NF a base. 5. Among the following compounds, the strongest acid is (a) C C (b) C66 (d) C (c) C6 6. Amongst the following the most basic compound is (a) Benzyl amine (b) Aniline (c) Acetanilide (d) p nitro aniline 7. What is the decreasing order of strength of bases? (a) C C N > C C > (b) C C > C- C > N >
9 Chemistry: Concepts of Acids and Bases-9 (c) > N > - C C > CC (d) N > C C > > C -C 8. The following acids have been arranged in order of decreasing acid strength. Identify the correct order. Cl (I) Br (II) I (III) (a) I > II > III (b) II > I > III (c) III > II > I (d) I > III > II 9. f the following orders regarding basicity, which one is correct (a) CCN > PhCN > CCN (b) CCN > PhCN > CCN (c) CCN > PhCN < CCN (d) CCN < PhCN < CCN 10. Which among the following is the strongest base (a) aniline (b) N,N dimethyl amine (c) para nitro aniline (d) meta nitro aniline 11. Which of the following pairs represents the strongest acid and strongest base that can exist in water? (a) and (b) N and N (c) Cl and F (d) N and C C 1. Which of the following has been arranged correctly in order of increasing acidic strength? (a) CC NCC NCCC CC (b) CC CC NCCC NCC (c) CC NCCC CC NCC (d) NCC NCCC CC CC 1. Which of the following is arranged in order of increasing proton affinity? (a) S I N F (b) F I N S (c) I F S N (d) N S F I 1. Among the following, which is the strongest acid? (a) Cl () (b) Cl () (c) S() (d) S (). 15. Among the following, which is the most basic towards BMe? (a) MeN (b) EtN (c) (d) S. 16. NCC May behave
10 Chemistry: Concepts of Acids and Bases-10 (a) only as an acid (c) as an acid as well as a base 17. is capable to act as an acid with (a) N (c) C66 (b) only as a base (d) neither as an acid nor as a base (b) S (d) Cl 18. Which of the following species is an acid and also a conjugate base of another acid (a) S (b) S (c) (d) Which of the following has been arranged correctly in order of increasing basic strength? (a) C C N CC (b) C C CC N (c) N C C C C (d) N C C C C 0. Which of the carboxylic acid is the most acidic? (a) Acetic acid (b) Formic acid (c) Benzoic acid (d) Cyclopentane carboxylic acid. 1. The conjugate acid of S8 (a) S8 (b) S (c) S (d) S8. The following acids have been arranged in order of decreasing acid strength. Identify the correct order. Cl (I) Br (II) I (III) (a) I > II > III (b) II > I > III (c) III > II > I (d) I > III > II. Which of the following are amphiprotic in nature? (a) (b) P (c) S (d) F. Among the following compounds, the strongest acid is (a) C C (b) C66 (c) C6 (d) C 5. With reference to protonic acid which of the following statement is correct? (a) P is more basic than N (b) P is less basic than N (c)p is equally basic than N (d) P is amphoteric while N is basic SECTIN II May be more than one choice 1. Which of the following is a hard acid (a) C (b) Br (c) Fe + (d) Cd +. Which of the following statements is/are correct (a) I is a weaker base than F
11 Chemistry: Concepts of Acids and Bases-11 (b) is a stronger base N (c) N is a weaker base than N (d) FC: is a stronger base than ClC:. Which one of following is the strongest acid (a) Cl (b) Cl (c) Cl (d) Cl. The conjugate acid of S7 is (a) S7 (b) S (c)s6 + (d) S 5. Among the following weakest acid is (a) N (b) As (c) Sb (d) P 6. Increasing order of Lewis acid strength AlCl GaCl InCl I II III (a) I II III (c) II I III (b) III II I (d) III I II 7. Which one of following is the strongest acid (a) P (b) P (c) P (d) S 8. What is the decreasing order of strength of bases (a) C C N > C C > (b) C C > C- C > N > (c) > N > - C C > CC (d) N > C C > > C -C 9. Which of the following is a soft base? (a) RS (b) N (c) (d) Cu = 10. Amongst the following the most basic compound is N (a) (b) N N
12 Chemistry: Concepts of Acids and Bases-1 N C (c) (d) N N 11. Which of the following is strongest Lewis acid (a) C (b) F (c) N (d) 1. The conjugate base of + is (a) (b) (c) + (d) None of these 1. Acetic acid is a conjugate base of which acid. (a) CC (b) CCC (c) CC + (d) None 1. Conjugate base of N is (a) N (b) N + (c) N (d) N 15. Which of the following is the soft base? (a) C ion (b) C (c) Ce + (d) Pb Which among the following is the strongest base (a) Be() (b) Mg() (c) Ba() (d) Sr() 17. The conjugate acid of N is (a) N (c) N + (b) N (d) N 18. In the equilibrium CC + F C C + F (a) F is the conjugate acid of CC (b) F is the conjugate base of F (c) CC is the conjugate acid of C C (d) C C is the conjugate base of CC. 19. Which of the following statements is/are correct? (a) Maleic acid is a stronger acid than fumaric acid but maleate monoanion is a weaker acid than fumarate monoanion (b) Maleic acid is a stronger acid than fumaric acid and also maleate monoanion is a stronger acid than fumarate monoanion (c) Maleic acid is a weaker acid than fumaric acid but maleate monoanion is a stronger acid than fumarate monoanion
13 Chemistry: Concepts of Acids and Bases-1 (d) Maleic acid is a weaker acid than Fumaric acid and also maleate monoanion is a weaker acid than fumarate monoanion. 0. Which of the following is the strongest acid (a) N (c) N (b) S (d) All have same strength 1. Which of the following species is an acid and also a conjugate base of another acid (a) S (b) S (c) (d) +. Which of the following orders regarding acid strength is correct? (a) C < CC < PhC (b) C > PhC > CC (c) C > CC > PhC (d) CC > C > PhC. The following equilibrium is established when hydrogen chloride is dissolved in acetic acid. Cl + CC Cl + CC + The set that characteristics the conjugate acid-base pair is (a) (Cl, CC) and (CC + and Cl ) (b) (Cl, CC + ) and (CC, Cl ) (c) (CC +, Cl) and (Cl, CC) (d) (Cl, Cl ) and (CC +, CC). In the following compounds, the order of acidity is N C N (I) (II) (III) (IV) (a) III > IV > I > II (c) II > I > III > IV (b) I > IV > III > II (d) IV > III > I > II 5. f the following orders regarding basicity, which one is correct (a) CCN > PhCN > CCN (b) CCN > PhCN > CCN (c) CCN > PhCN < CCN (d) CCN < PhCN < CCN SECTIN III Comprehension Type Questions Write-up I Acids are the species capable of donating the proton in a reaction while bases are the species capable of accepting the proton in a reaction, i.e., acids are proton donors (protogenic) and bases are proton acceptors (protophilic). 1. The conjugate acid of S 8 is
14 Chemistry: Concepts of Acids and Bases-1 (a) S (b) S 8 (c) S (d) S. The conjugate base of P is (a) P (c) P. Proton donating species is called (a) acid (c) salt (b) (d) P P (b) base (d) none of these Write-up II A base is a substance which can furnish a pair of electrons to form a coordinate bond whereas an acid is a substance which can accept a pair of electrons. A Lewis acid is a substance that acts as an electron acceptor or electrophile while a Lewis base is a substance that acts as an electron donor or nucleophile.. Which of the following is a Lewis acid? (a) N (c) + (b) S (d) AlCl 5. BF is taken as an example of Lewis acid because it behaves (a) electrophile (b) nucleophile (c) neutral molecules (d) free radical 6. Which of the following is a Lewis base? (a) (c) N (b) Cl (d) C SECTIN IV Subjective Questions LEVEL I 1. Which of the following reagents are strong electrolytes? (a) N (b) NCl (c) C (d) NaC, (e) Cl (f) NaCl.. Arrange according to increasing Lewis acid character, SiF, SiCl, SiBr, Sil. Draw an electron dot diagram to illustrate that ammonium hydroxide could not exist as a weak base. Explain the weakly basic properties of a solution of ammonia in water.. The amino acid glycine exists predominantly in the form NCC. Write formulas for (a) the conjugate base and (b) the conjugate acid glycine. 5. Arrange according to increasing Lewis acid character, B(nBu), B(tBu)
15 Chemistry: Concepts of Acids and Bases Identify conjugate acid base pair in the following reactions C C65 Cl + + Cl 7. Write the equation representing self-ionisation of PCl and BrF as non-aqueous solvents. 8. Using the Lewis acid-base concept determine the trend in the acid strengths in the series: a) Cl, Cl, Cl b) P, P, P 9. Rationalize the relative Lewis basicities (Si) < (C); (b) (Si)N < (C)N. 10. Be() exhibits amphoterism. Explain by reactions. LEVEL II 1. Identify the Lewis acid and base in the reaction BrF + F [BrF].. If you mix equal concentration of reactants and products which of the following reactions proceed to the right and which proceed to the left? a) S (aq) N (aq) N (aq) S (aq) b) C (aq) S (aq) S (aq) C (aq). In the acid of the type A, at 5 C [ + ] = 1 10 M. What is [ ]?. ydration of CuS is a Lewis acid-base reaction. Explain. 5. Boric acid B is dissolved in water. ow does it behave? 6. Arrange the following in the order of their basic strength. Justify your answer NN,N,N 7. Account for the trend in acidity [Fe()] [Fe()] [Al()] [g()] n 8. Silver perchlorate, AgCl, is significantly more soluble in benzene than in alkane solvents. Account for this observation in terms of Lews acid-base properties. 9. The common ores of nickel and copper are sulphides. In contrast, aluminium is obtained from the oxide and calcium from the carbonate. Can these observations be explained in terms of hardness? 10. In the traditional scheme of qualitative analysis, a solution of metal ions are oxidized and then aqueous ammonia is added to raise the p. The ions Fe +, Ce +, Al +, Cr +, and V + precipitate as hydroxides. The addition of and Na re-dissolves the aluminum, chromium, and vanadium. Discuss these steps in terms of the acidities of oxides. SECTIN V Miscellaneous Questions
16 Chemistry: Concepts of Acids and Bases Match the following a) BF i) Cationic Bronsted base b) N ii) Cl c) iii) P d) [Al()5] + iv) Ag + e) Monobasic acid v) Bronsted acid f) Soft acid vi) g) ard base vii) Lewis acid h) Neutralisation viii) Amphiprotic. Fill in the blanks a) According to Arrhenius acid-base theory, in neutralization reaction. molecule is formed. b). acid-base theory cannot define that N is a base c) In the reaction, BCl + P ClB:P, the Lewis base is. d) In the reaction, SnCl + Cl SnCl + e, the Lewis acid is. e) The conjugate acid of P is. f) The basicity of phosphorous acid (P) is. Answers to Assignments SECTIN - I 1. (c). (c). (b). (b) 5. (a) 6. (a) 7. (a) 8. (a) 9. (a) 10. (b) 11. (a) 1. (b) 1. (c) 1. (a) 15. (a) 16. (c) 17. (a) 18. (a) 19. (a) 0. (b) 1. (d). (a). (a). (a) 5. (b) SECTIN - II 1. (a), (c). (a), (c), (d). (d). (a) 5. (c) 6. (b) 7. (c) 8. (a) 9. (a) 10. (a) 11. (a) 1. (a) 1. (c) 1. (a) 15. (b) 16. (c) 17. (c) 18. (b) 19. (a) 0. (b) 1. (a). (b). (a). (d) 5. (a) SECTIN - III 1. (a). (b). (a). (d) 5. (a) 6. (a) SECTIN - IV
17 Chemistry: Concepts of Acids and Bases-7 1. (b), (d), (e) and (f). LEVEL I. The order in this case is the reverse of that for BX. -conjugation from the halogen p-orbital to the Si-d orbital is not as intense as in the case of BX and the order of acidity follows the increase in electron withdrawing power of the halogen from I to F. ence the order is SiI < SiBr < SiCl < SiF. N The diagram shows that there is no covalent bonding of the ion to the N ion. Since solutions of ammonia in water do not act as strong bases, this representation must be incorrect. The fact that ammonia acts as a weak base is explained by the equilibrium. N N. (a) NCC (b) N C C 5. The highly branched tertiary butyl group involve appreciable back strain (B-strain) when the boron atom changes to pyramidal environment on adduct formation. This destabilizes the adduct. ence the order is B(tBu) < B(nBu) 6. (Base) (conjugate acid) C(Acid) 6 5 C 6 5 (conjugate base) Cl (acid Cl (conjugate base) (Base) (conjugate acid) 7. PCl PCl PCl, BrF BrF BrF 8. As a general rule, the greater the number of terminal oxygens in the Lewis structure of oxy acid, the greater is its acidity. Thus, in a) Cl Cl Cl three terminal oxygen two terminal oxygen one terminal oxygen b) P P P one bonded to, two bonded to three bonded to All have only one terminal oxygen. Also electronegativity of and P are also approximately same. ence, there is not large difference in the strengths of the acids.
18 Chemistry: Concepts of Acids and Bases-8 9. Nonmetallic elements in period and below can expand their valence shells by delocalization of the or N lone paris (7), so the silyl ether and silyl amine are the weaker Lewis bases in each pair. 10. Be() is an amphoteric hydroxide since it reacts with both acids and bases. Be() (s) Be (aq) ( ) Be() (s) (aq) Be() (aq) 1. The acid BrF adds the base : F. LEVEL II. a) From S is stronger acid than N and N is stronger base than b) S (aq) N (aq) N (aq) S (aq) stronger acid stronger base wea ker acid wea ker base S. Thus, Since proton transfer takes place from stronger acid to stronger base, the reaction proceeds from left to right. C (aq) S (aq) S (aq) C (aq) stronger acid stronger base wea ker acid wea ker base This is reverse of (a), hence, proceeds right to left.. A(aq) ( ) (aq) A (aq) Since, and [ ][ ] K 1 10 at 5 C 1 w [ ] 1 10 M, hence, K 110 [ ] 1 10 M 1 w 1 [ ] 110. ydration of metal ions in solution is in itself a Lewis acid-base reaction. Thus, when CuS dissolves in water, each Cu ion is associated with six water molecules as Cu() 6. In this case, the Cu ion acts as the acid and the molecules as the base. CuS 6 [Cu( ) ]S (aq) acid 6 base 5. Boric acid is an oxoacid weak acid with the following structure? C B It does not ionize in water to produce ion. Its reaction with water is: B() (aq) ( ) B() (aq) (aq) In this Lewis acid-base reaction, boric acid accepts a pair of electrons from the hydroxide ion that is derived from the molecule. 6. N N N N
19 Chemistry: Concepts of Acids and Bases-9 7. The weakest acid is the Fe complex on account of its relatively large radius and low charge. The increase of charge to + increases the acid strength. the greater acidity of Al can be explained by its smaller radius. the anomalous ion in the series is the g complex. This complex reflects the failure of an ionic model, for in this complex there is a large transfer of positive charge to oxygen as a result of covalent bonding. 8. The electrons of benzene, a soft base, are available for complex formation with the empty orbitals of the cation Ag, a soft acid (recall 19). The species [Ag C6 6] is the complex of the acid Ag with electrons of the weak base benzene. 9. We know that and Cu are considerably softer acids than rule accounts for the sorting observed. C are hard bases; S is a soft base. The cations Al or Ni and Ca. ence the hard=hard and soft-soft 10. When the oxidation number is +, all the metal oxides are sufficiently basic to be insoluble in a p 10 solution. Aluminum (III) is amphoteric and redissolves in strong base to give aluminate ions, [Al() ]. Vanadium (III) and chromium (III) are oxidized by to give vanadate ions, [V ], and chromate ions, [Cr ], which are the anions derived from the acidic oxides V 5 and Cr, respectively. SECTIN - V 1. (a vii)l (b v); (c viii); (d i); (e iii); (f iv); (g ii); (h vi). a) Water b) Arrhenius c) P d) SnCl e) P f)
Chapter In each case the conjugate base is obtained by removing a proton from the acid: (a) OH (b) I (c)
Practice Exercises 16.1 Conjugate acid base pairs (a), (c), and (f) (b) The conjugate base of I is I (d) The conjugate base of N 2 is N 2 and the conjugate base of N 4 is N 3 (e) The conjugate acid of
More informationChapter 2: Acids and Bases
hapter 2: Acids and Bases 32 hapter 2: Acids and Bases Problems 2.1 Write each acid- reaction as a proton-transfer reaction. Label which reactant is the acid and which the, as well as which product is
More informationAcid Dissociation Constant
CE 131 Lecture 37 Lewis Acids and Bases Chapter 16: pp. 800-802. Acid Dissociation Constant C 2 3 2 + 2 3 + + C 2 3-2 [ 3 + ][C 2 3-2 ] K = [ 2 ][C 2 3 2 ] [ 3 + ][C 2 3-2 ] K a = K [ 2 ] = [C 2 3 2 ]
More informationHA(aq) H + (aq) + A (aq) We can write an equilibrium constant expression for this dissociation: [ ][ ]
16.6 Weak Acids Weak acids are only partially ionized in aqueous solution. There is a mixture of ions and un-ionized acid in solution. Therefore, weak acids are in equilibrium: Or: HA(aq) + H 2 O(l) H
More informationWeak acids are only partially ionized in aqueous solution: mixture of ions and un-ionized acid in solution.
16.6 Weak Acids Weak acids are only partially ionized in aqueous solution: mixture of ions and un-ionized acid in solution. Therefore, weak acids are in equilibrium: HA(aq) + H 2 O(l) H 3 O + (aq) + A
More informationChapter 16. Acid-Base Equilibria
Chapter 16. Acid-Base Equilibria 16.1 Acids and Bases: A Brief Review Acids taste sour and cause certain dyes to change color. Bases taste bitter and feel soapy. Arrhenius concept of acids and bases: An
More informationChapter 14. Acids and Bases
Chapter 1. Acids and Bases Reactions in aqueous solutions Precipitation reactions Acid-Base reactions xidation-reduction reactions Precipitation reaction : a reaction which results in the formation of
More informationModule 2 Acids and Bases. Lecture 3 Acids and Bases
Module 2 Acids and Bases Lecture 3 Acids and Bases 2.1 Concepts A compound is classified as an acid or a base based on certain properties. At present there are several theories which define the concepts
More informationChapter 14. Acids and Bases
Chapter 14 Acids and Bases Section 14.1 The Nature of Acids and Bases Models of Acids and Bases Arrhenius: Acids produce H + ions in solution, bases produce OH - ions. Brønsted Lowry: Acids are proton
More informationAcid / Base Properties of Salts
Acid / Base Properties of Salts n Soluble ionic salts produce may produce neutral, acidic, or basic solutions depending on the acidbase properties of the individual ions. n Consider the salt sodium nitrate,
More informationLecture 21 Cations, Anions and Hydrolysis in Water:
2P32 Principles of Inorganic Chemistry Dr. M. Pilkington Lecture 21 Cations, Anions and ydrolysis in Water: 1. ydration.energy 2. ydrolysis of metal cations 3. Categories of acidity and observable behavior
More informationCH 4 AP. Reactions in Aqueous Solutions
CH 4 AP Reactions in Aqueous Solutions Water Aqueous means dissolved in H 2 O Moderates the Earth s temperature because of high specific heat H-bonds cause strong cohesive and adhesive properties Polar,
More information(Label the Conjugate Pairs) Water in the last example acted as a Bronsted-Lowry base, and here it is acting as an acid. or
Chapter 16 - Acid-Base Equilibria Arrhenius Definition produce hydrogen ions in aqueous solution. produce hydroxide ions when dissolved in water. Limits to aqueous solutions. Only one kind of base. NH
More informationChapter 3 An Introduction to Organic Reactions: Acids and Bases
There are 4 types of Organic Reactions Chapter 3 An Introduction to Organic Reactions: SUBSTITUTION: ADDITION: X Y + A X A + Y Example Example A B + X Y A B X Y ELIMINATION There are 4 Types of Organic
More informationChapter 14 Acids and Bases
Properties of Acids and Bases Chapter 14 Acids and Bases Svante Arrhenius (1859-1927) First to develop a theory for acids and bases in aqueous solution Arrhenius Acids Compounds which dissolve (dissociate)
More informationChapter 16 Acid-Base Equilibria
Chapter 16 Acid-Base Equilibria Learning goals and key skills: Understand the nature of the hydrated proton, represented as either H + (aq) or H 3 O + (aq) Define and identify Arrhenuis acids and bases.
More informationRequired Reading Material.
JF Chemistry 1101 2010 Introduction to Physical Chemistry: Acid Base and Solution Equilibria. Dr Mike Lyons School of Chemistry melyons@tcd.ie Required Reading Material. Silberberg, Chemistry, 4th edition.
More informationAspects of Bonding & Acid Strength
Aspects of Bonding & Acid Strength CHEM 110/ 2014 Slide 1 of 35 Intramolecular Bonding The bonding between molecules/atoms in the solid state Ionic bonding Covalent bonding Metallic bonding e.g. sodium
More information2. Polar Covalent Bonds: Acids and Bases
2. Polar Covalent Bonds: Acids and Bases Based on McMurry s Organic Chemistry, 6 th edition, Chapter 2 2003 Ronald Kluger Department of Chemistry University of Toronto 2.1 Polar Covalent Bonds: Electronegativity!
More informationChapter 2 Acids and Bases. Arrhenius Acid and Base Theory. Brønsted-Lowry Acid and Base Theory
hapter 2 Acids and Bases A significant amount of chemistry can be described using different theories of acids and bases. We ll consider three different acid-base theories (listed in order of increasing
More informationElements react to attain stable (doublet or octet) electronic configurations of the noble gases.
digitalteachers.co.ug Chemical bonding This chapter teaches the different types and names of bonds that exist in substances that keep their constituent particles together. We will understand how these
More informationTopic-1 Lowry - Bronsted and Lewis theory of acids and bases with examples and applications
Topic-1 Lowry - Bronsted and Lewis theory of acids and bases with examples and applications VERY SHORT ANSWER QUESTIONS 1. What is bronsted acid and base give one example? Strength of bronsted acids and
More informationChapter 4 Chemical Formulas, Reactions, Redox and Solutions
Terms to Know: Solubility Solute Solvent Solution Chapter 4 the amount of substance that dissolves in a given volume of solvent at a given temperature. a substance dissolved in a liquid to form a solution
More informationAcids and Bases. A strong base is a substance that completely ionizes in aqueous solutions to give a cation and a hydroxide ion.
Acid-Base Theories Arrhenius Acids and Bases (1884) Acids and Bases An acid is a substance that, when dissolved in water, increases the concentration of hydrogen ions. A base is a substance that, when
More informationAcids Bases and Salts Acid
Acids Bases and Salts Acid ph less than 7.0 Sour taste Electrolyte Names of Acids Binary acids Contain only 2 elements Begin with hydro; end with ic Ternary acids Ex: H 2 S = hydrosulfuric Contain a polyatomic
More informationAcid/Base Definitions
Acids and Bases Acid/Base Definitions Arrhenius Model Acids produce hydrogen ions in aqueous solutions Bases produce hydroxide ions in aqueous solutions Bronsted-Lowry Model Acids are proton donors Bases
More informationLecture Topics: I. Electrophilic Aromatic Substitution (EAS)
Reactions of Aromatic Compounds Reading: Wade chapter 17, sections 17-1- 17-15 Study Problems: 17-44, 17-46, 17-47, 17-48, 17-51, 17-52, 17-53, 17-59, 17-61 Key Concepts and Skills: Predict and propose
More informationACIDS AND BASES. Note: For most of the acid-base reactions, we will be using the Bronsted-Lowry definitions.
DEFINITIONS: ACIDS AND BASES Arrhenius Definition An acid in aqueous solution produces H + ions. A base in aqueous solution produces OH - ions. Bronsted Lowry Theory An acid is a proton donor A base is
More informationCHAPTER 14 ACIDS AND BASES
CHAPTER 14 ACIDS AND BASES Topics Definition of acids and bases Bronsted-Lowry Concept Dissociation constant of weak acids Acid strength Calculating ph for strong and weak acids and bases Polyprotic acids
More informationWednesday, February 25, Acid and Base Reactions
Acid and Base Reactions Dilute aqueous solution of acetic acid, C3COO Aqueous solution of sodium hydroxide, NaO The role of the ydrogen Ion Cl (aq) Æ + (aq) + Cl - (aq) What does the neutral atom consist
More informationCu 2+ (aq) + 4NH 3(aq) = Cu(NH 3) 4 2+ (aq) I (aq) + I 2(aq) = I 3 (aq) Fe 3+ (aq) + 6H 2O(l) = Fe(H 2O) 6 3+ (aq) Strong acids
There are three definitions for acids and bases we will need to understand. Arrhenius Concept: an acid supplies H + to an aqueous solution. A base supplies OH to an aqueous solution. This is the oldest
More informationand Stereochemistry) PAPER 1: ORGANIC CHEMISTRY- I (Nature of Bonding and Stereochemistry) MODULE 4: Applications of Electronic Effects
Subject Chemistry Paper No and Title Module No and Title Module Tag Paper 1: ORGANIC - I (Nature of Bonding Module 4: Applications of Electronic Effects CHE_P1_M4 PAPER 1: ORGANIC - I (Nature of Bonding
More informationChapter 8 Acid-Base Equilibria
Chapter 8 Acid-Base Equilibria 8-1 Brønsted-Lowry Acids and Bases 8-2 Water and the ph Scale 8-3 The Strengths of Acids and Bases 8-4 Equilibria Involving Weak Acids and Bases 8-5 Buffer Solutions 8-6
More informationChapter 16 Acid-Base Equilibria
Page 1 of 20 Chapter 16 Acid-Base Equilibria 16.1 Acids and Bases: A Brief Review Acids: taste sour and cause certain dyes to change color. Bases: taste bitter and feel soapy. Arrhenius concept o acids
More informationChapter 3 Acids and Bases"
Chapter 3 Acids and Bases BrØnsted-Lowry Acids and Bases A BrØnsted-Lowry acid is a proton donor. A BrØnsted-Lowry base is a proton acceptor. H + = proton Acids and Bases Reactions of BrØnsted-Lowry Acids
More informationChapter 14. Objectives
Section 1 Properties of Acids and Bases Objectives List five general properties of aqueous acids and bases. Name common binary acids and oxyacids, given their chemical formulas. List five acids commonly
More informationAcids and Bases. Acids and Bases
BrØnsted-Lowry A BrØnsted-Lowry acid is a proton donor. A BrØnsted-Lowry base is a proton acceptor. H + = proton BrØnsted-Lowry Some molecules contain both hydrogen atoms and lone pairs and thus, can act
More informationReactions in Aqueous Solutions I: Acids, Bases & Salts
10 Reactions in Aqueous Solutions I: Acids, Bases & Salts CHAPTER GOALS 1. Properties of Aqueous Solutions of Acids and Bases 2. The Arrhenius Theory 3. The Hydronium Ion (Hydrated Hydrogen Ion) 4. The
More informationCHAPTER 18 ACID-BASE EQUILIBRIA
CAPTER 18 ACID-BASE EQUILIBRIA FOLLOW UP PROBLEMS 18.1A Plan: Examine the formulas and classify each as an acid or base. Strong acids are the hydrohalic acids Cl, Br, and I, and oxoacids in which the number
More informationAcids and Bases. CHEM 102 T. Hughbanks. In following equilibrium, will reactants or products be favored? Strong acid (HCl) + Strong base (NaOH)
Acids and Bases According to the Brønsted Lowry theory, all acid base reactions can be written as equilibria involving the acid and base and their conjugates. CEM 102 T. ughbanks All proton transfer reactions
More informationChap 16 Chemical Equilibrium HSU FUYIN
Chap 16 Chemical Equilibrium HSU FUYIN 1 Definitions: Arrhenius & Brønsted Lowry acid and base Arrhenius theory: An acid is a substance that, when dissolved in water, increases the concentration of hydrogen
More informationI. Multiple Choice Questions (Type-I) 1. Which of the following is not an example of redox reaction? Cu + H HCl. BaSO 4
Unit 8 REDX REACTINS REAC I. Multiple Choice Questions (Type-I) 1. Which of the following is not an example of redox reaction? Cu Cu Fe 2 3 + 3C 2Fe + 3C 2 2K + F 2 2KF BaCl 2 S 4 BaS 4 + 2HCl 2. The more
More informationChapter 2 Polar Covalent Bonds; Acids and Bases SAMPLE. Chapter Outline
Chapter 2 Polar Covalent Bonds; Acids and Bases Chapter utline I. Polar covalent bonds (Sections 2.1 2.3). A. Electronegativity (Section 2.1). 1. Although some bonds are totally ionic and some are totally
More informationAssignment 16 A incorrect
Assignment 16 A 1- What is the concentration of hydronium ions in a solution with a hydroxide-ion concentration of 2.31 10 4 M at 25 C? a) 4.33 10 11 M b) 2.31 10 4 M c) 2.31 10 18 M d) 2.31 10 10 M (The
More informationCh 2 Polar Covalent Bonds
h 2 Polar ovalent Bonds Two primary bond types: ovalent (shared e -1 s) and Ionic (transferred e -1 s) Ionic bonds can have covalent character, such as with Na:l. An e -1 pair on l -1 can fill the 3s orbital
More informationChemistry: The Central Science. Chapter 16: Acid-Base Equilibria. 16.1: Acids and Bases: A Brief Review
Chemistry: The Central Science Chapter 16: Acid-Base Equilibria 16.1: Acids and Bases: A Brief Review Acids have a sour taste and cause certain dyes to change color Base have a bitter taste and feel slippery
More informationChapter 16: Acid Base Equilibria Chapter 16 Acid-Base Equilibria Learning Standards & Objectives;
Chapter 16: Acid Base Equilibria Chapter 16 Acid-Base Equilibria Learning Standards & Objectives; Chapter 16 AP16-1,2-01 AP16-1,2-02 AP16-1,2-03 AP16-3,4-01 AP16-3,4-02 AP16-5-01 AP16-6,7-01 AP16-6,7-02
More informationWhat we learn from Chap 17
Acids and Bases hapter 17 What we learn from hap 17 17.2 This chapter concerns the nature and uses of acids and bases. It is the second in our three-chapter h discussion i about equilibrium, and reinforces
More informationPractice Examination #6 A. H :..
Practice Examination #6 Name: Date:. Which kind of bond is formed when two atoms share electrons to form a molecule? A. ionic B. metallic C. electrovalent D. covalent 2. The distance between two adjacent
More information1. Which response contains all the molecules below that violate the octet rule, and no others? SF 4, SiCl 4, H 2Te, AsF 5, BeI 2
Chem 1100 Pre-Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Which response contains all the molecules below that violate the octet rule, and no
More informationProperties of Acids and Bases
Chapter 15 Aqueous Equilibria: Acids and Bases Properties of Acids and Bases Generally, an acid is a compound that releases hydrogen ions, H +, into water. Blue litmus is used to test for acids. Blue litmus
More informationReactions in Aqueous Solutions
Reactions in Aqueous Solutions 1 Chapter 4 General Properties of Aqueous Solutions (4.1) Precipitation Reactions (4.2) Acid-Base Reactions (4.3) Oxidation-Reduction Reactions (4.4) Concentration of Solutions
More informationUnit 8 REDX REACTINS I. Multiple Choice Questions (Type-I) 1. Which of the following is not an example of redox reaction? Cu Cu Fe 3 + 3C Fe + 3C K + F KF BaCl S 4 BaS 4 + HCl. The more positive the value
More informationBonding Mrs. Pugliese. Name March 02, 2011
Bonding Mrs. Pugliese Name March 02, 2011 1. Atoms of which element have the greatest tendency to gain electrons? 1. bromine 3. fluorine 2. chlorine 4. iodine 2. Which polyatomic ion contains the greatest
More informationContents and Concepts
Learning Objectives Chapter 15 Acid Base Concepts Arrhenius Concept of Acids and Base a. Define and according to the Arrhenius concept. Brønsted Lowry Concept of Acids and Bases a. Define and according
More informationCHEM 109A Organic Chemistry
CHEM 109A Organic Chemistry https://labs.chem.ucsb.edu/zakarian/armen/courses.html Chapter 2 Acids and Bases Central to Understanding Organic Chemistry Draw the conjugate acid of each of the following:
More informationChapter 8. Acidity, Basicity and pk a
Chapter 8 Acidity, Basicity and pk a p182 In this reaction water is acting as a base, according to our definition above, by accepting a proton from HCl which in turn is acting as an acid by donating a
More informationChapter 8 Acid-Base Equilibria
Chapter 8 Acid-Base Equilibria 8-1 Brønsted-Lowry Acids and Bases 8-2 Water and the ph Scale 8-3 The Strengths of Acids and Bases 8-4 Equilibria Involving Weak Acids and Bases 8-5 Buffer Solutions 8-6
More informationAcids & Bases. Strong Acids. Weak Acids. Strong Bases. Acetic Acid. Arrhenius Definition: Classic Definition of Acids and Bases.
Arrhenius Definition: Classic Definition of Acids and Bases Acid: A substance that increases the hydrogen ion concetration, [H ], (also thought of as hydronium ion, H O ) when dissolved in water. Acids
More informationName Date Class STUDY GUIDE FOR CONTENT MASTERY. covalent bond molecule sigma bond exothermic pi bond
Covalent Bonding Section 9.1 The Covalent Bond In your textbook, read about the nature of covalent bonds. Use each of the terms below just once to complete the passage. covalent bond molecule sigma bond
More informationLecture 7. Acids. non-metals form anions. metals form cations H+ - Professor Hicks Inorganic Chemistry (CHE152) + anion. molecular compounds
Lecture 7 Professor icks Inorganic Chemistry (CE152) Acids + + anion + - anion substances that release + ions when dissolved Strong acids Cl NO 3 2 SO 4 + Cl - + NO - 3 2 + SO 2-4 hydrochloric acid nitric
More informationChapter 2 Polar Covalent Bonds; Acids and Bases. Chapter Outline
rganic Chemistry 9th Edition McMurry SLUTINS MANUAL Full clear download at: https://testbankreal.com/download/organic-chemistry-9th-edition-mcmurrysolutions-manual/ rganic Chemistry 9th Edition McMurry
More informationInorganic Chemistry with Doc M. Day 9. Acids and Bases Overview
Inorganic Chemistry with Doc M. Day 9. Acids and Bases Overview Topics: 1. Bronsted-Lowry Concept 5. ph of salts 2. Lewis acid and base concepts 6. Hard-soft acid and base theory 3. Oxyacids 7. Non-aqueous
More informationQ.1 Draw structures for all amines of molecular formula C 4 H 11 N. Classify them as primary, secondary or tertiary amines.
1 AMIES Structure ontain the 2 group. lassification primary (1 ) amines secondary (2 ) amines tertiary (3 ) amines quarternary (4 ) ammonium salts + 1 2 3 4 Aliphatic Aromatic methylamine, ethylamine,
More informationChem 1046 Lecture Notes Chapter 17
Chem 1046 Lecture Notes Chapter 17 Updated 01-Oct-2012 The Chemistry of Acids and Bases These Notes are to SUPPLIMENT the Text, They do NOT Replace reading the Text Book Material. Additional material that
More informationChapter 6: Chemical Bonding
Chapter 6: Chemical Bonding Learning Objectives Describe the formation of ions by electron loss/gain to obtain the electronic configuration of a noble gas. Describe the formation of ionic bonds between
More informationChapter 7. Ionic & Covalent Bonds
Chapter 7 Ionic & Covalent Bonds Ionic Compounds Covalent Compounds 7.1 EN difference and bond character >1.7 = ionic 0.4 1.7 = polar covalent 1.7 Electrons not shared at
More informationCHM 130: Final Exam Practice Problems
CHM 130: Final Exam Practice Problems 1. Complete the following table: Isotope Mass number # of protons # of neutrons # of electrons strontium-90 neon-19 iron-55 2. Consider Figures A-F below: A B C D
More informationThe Chemistry of Acids and Bases
The Chemistry of 1 Acids and Bases 2 Acid and Bases 3 Acid and Bases 4 Acid and Bases 5 Strong and Weak Acids/Bases Generally divide acids and bases into STRONG or WEAK ones. STRONG ACID: HNO 3 (aq) +
More informationg. Looking at the equation, one can conclude that H 2 O has accepted a proton from HONH 3 HONH 3
Chapter 14 Acids and Bases I. Bronsted Lowry Acids and Bases a. According to Brønsted- Lowry, an acid is a proton donor and a base is a proton acceptor. Therefore, in an acid- base reaction, a proton (H
More informationTalk n Acids & Bases... Lady Dog! Definitions
Talk n Acids & Bases... Lady Dog! Definitions So far in this course, we have looked at processes in chemistry that deal with, or are best explained by, ionic salts or molecules. Now we will turn our attention
More informationChapter 22 Amines. Nomenclature Amines are classified according to the degree of substitution at nitrogen.
CH. 22 Chapter 22 Amines Amines are very important in biological chemistry. Most of the bases in biological acid-base reactions are amines. They are also very important nucleophiles in biochemical reactions.
More informationChapter 16 Acids and Bases. Chapter 16 Acids and Bases
. Chapter 16 Acids and Bases 1 Some Definitions Arrhenius Acid: Substance that, when dissolved in water, increases the concentration of hydrogen ions. Base: Substance that, when dissolved in water, increases
More informationAqueous Equilibria: Acids and Bases
Slide 1 Chapter 14 Aqueous Equilibria: Acids and Bases Slide 2 Acid Base Concepts 01 Arrhenius Acid: A substance which dissociates to form hydrogen ions (H + ) in solution. HA(aq) H + (aq) + A (aq) Arrhenius
More informationChemistry of period II elements
digitalteachers.co.ug Chemistry of period II elements Period 2 consists of the following elements as shown in table 7.1 below. Table 7.1 Period 2 elements Element: Li Be B C N O F Ne Electron Configuration
More information(A) Composition (B) Decomposition (C) Single replacement (D) Double replacement: Acid-base (E) Combustion
AP Chemistry - Problem Drill 08: Chemical Reactions No. 1 of 10 1. What type is the following reaction: H 2 CO 3 (aq) + Ca(OH) 2 (aq) CaCO 3 (aq) + 2 H 2 O (l)? (A) Composition (B) Decomposition (C) Single
More informationClass XII: Chemistry Chapter 13: Amines Top concepts
Class XII: Chemistry Chapter 13: Amines Top concepts 1. Amines are regarded as derivatives of ammonia in which one, two or all three hydrogen atoms are replaced by alkyl or aryl group 2. Classification
More informationSCHOOL YEAR CH- 13 IONS IN AQUEOUS SOLUTIONS AND COLLIGATIVE PROPERTIES SUBJECT: CHEMISTRY GRADE : 11 TEST A
SCHOOL YEAR 2017-18 NAME: CH- 13 IONS IN AQUEOUS SOLUTIONS AND COLLIGATIVE PROPERTIES SUBJECT: CHEMISTRY GRADE : 11 TEST A Choose the best answer from the options that follow each question. 1. A solute
More information2. Which of the following salts form coloured solutions when dissolved in water? I. Atomic radius II. Melting point III.
1. Which pair of elements reacts most readily? A. Li + Br 2 B. Li + Cl 2 C. K + Br 2 D. K + Cl 2 2. Which of the following salts form coloured solutions when dissolved in water? I. ScCl 3 II. FeCl 3 III.
More informationClassifying Organic Chemical Reactions
Chemical Reactivity Organic chemistry encompasses a very large number of compounds ( many millions ), and our previous discussion and illustrations have focused on their structural characteristics. Now
More informationADVANCED PLACEMENT CHEMISTRY ACIDS, BASES, AND AQUEOUS EQUILIBRIA
ADVANCED PLACEMENT CHEMISTRY ACIDS, BASES, AND AQUEOUS EQUILIBRIA Acids- taste sour Bases(alkali)- taste bitter and feel slippery Arrhenius concept- acids produce hydrogen ions in aqueous solution while
More informationChapter 4 Three Major Classes of Chemical Reactions
Chapter 4 Three Major Classes of Chemical Reactions Solution Stoichiometry Many reactions (biochemical, marine, etc.) take place in solution. We need to be able to express the number of moles of particles
More informationChemistry 304B, Spring 99 Lecture 2 1
Chemistry 04B, Spring 99 Lecture 2 1 Consider Acidity and Basicity Recall carboxylic acids and amines (base). Jones: p 27-8; 149, 291, 822-826, 1086-1090, 958-96, 878-882 General terms: Lewis acid: capable
More informationAP Chemistry Honors Unit Chemistry #4 2 Unit 3. Types of Chemical Reactions & Solution Stoichiometry
HO AP Chemistry Honors Unit Chemistry #4 2 Unit 3 Chapter 4 Zumdahl & Zumdahl Types of Chemical Reactions & Solution Stoichiometry Students should be able to:! Predict to some extent whether a substance
More information1. How many significant digits are there in each of the following measurements? (½ mark each) a) ha b) s. c) d) 0.
SCH 4U_07-08 SCH3U: REVIEW NAME: (TOTAL SCORE = 80) 1. How many significant digits are there in each of the following measurements? (½ mark each) a) 204.45 ha b) 18.23 s c) 380 000 d) 0.00560 g 2. Name
More informationCh.2 Polar Bonds and Their Consequences. 2.1 Polar Covalent Bonds and Electronegativity. polar covalent bonds: electron distribution is unsymmetrical
2.1 Polar ovalent Bonds and Electronegativity polar covalent bonds: electron distribution is unsymmetrical Ionic haracter δ+ δ- + - X Y X Y X Y symmetrical covalent bond polar covalent bond ionic bond
More informationCHEM1902/ N-8 November Consider the following reaction sequences beginning with the carboxylic acid, E.
CEM1902/4 2014--8 ovember 2014 Consider the following reaction sequences beginning with the carboxylic acid, E. 6 ame compounds E and G. E: propionic acid G: methyl propionate Propose structures for compounds
More informationChemistry 51 Chapter 5 OCTET RULE & IONS
OCTET RULE & IONS Most elements, except noble gases, combine to form compounds. Compounds are the result of the formation of chemical bonds between two or more different elements. In the formation of a
More informationChemistry Questions ans Answers BASED ON HIGH ORDER THINKING SKILL (HOTS) UNIT- 13 ORGANIC COMPOUNDS CONTAINING NITROGEN
Chemistry Questions ans Answers BASED N HIGH RDER THINKING SKILL (HTS) UNIT- 13 RGANIC CMPUNDS CNTAINING NITRGEN 1 MARK QUESTINS Q. 1. Why the presence of a base is essential in the ammonolysis of alkyl
More information11/14/10. Properties of Acids! CHAPTER 15 Acids and Bases. Table 18.1
11/14/10 CHAPTER 15 Acids and Bases 15-1 Properties of Acids! Sour taste React with active metals i.e., Al, Zn, Fe, but not Cu, Ag, or Au 2 Al + 6 HCl 2 AlCl3 + 3 H2 corrosive React with carbonates, producing
More informationContents and Concepts
Chapter 16 1 Learning Objectives Acid Base Concepts Arrhenius Concept of Acids and Base a. Define acid and base according to the Arrhenius concept. Brønsted Lowry Concept of Acids and Bases a. Define acid
More informationEquations. M = n/v. M 1 V 1 = M 2 V 2 if the moles are the same n 1 n 2 you can cancel out the n s. ph = -log [H + ] poh = -log [OH - ] ph + poh = 14
Equations M = n/v M 1 V 1 = M 2 V 2 if the moles are the same n 1 n 2 you can cancel out the n s. ph = -log [H + ] poh = -log [OH - ] ph + poh = 14 [H 3 O + ] = 10^-pH [OH - ] = 10^-pOH [H 3 O + ] [OH
More informationCHAPTER 7.0: IONIC EQUILIBRIA
Acids and Bases 1 CHAPTER 7.0: IONIC EQUILIBRIA 7.1: Acids and bases Learning outcomes: At the end of this lesson, students should be able to: Define acid and base according to Arrhenius, Bronsted- Lowry
More informationF.Y.B.Sc BIOTECH TOPIC: ACID BASE
F.Y.B.Sc BIOTECH TOPIC: ACID BASE 2016-17 Q.1) Define the following terms: 1)Electrolyte: A substance which forms a conducting solution when dissolved in water is called an electrolyte. 2) Strong electrolyte:
More informationChapter 16. Acid-Base Equilibria
Chapter 16 Acid-Base Equilibria Arrhenius Definition Acids produce hydrogen ions in aqueous solution. Bases produce hydroxide ions when dissolved in water. Limits to aqueous solutions. Only one kind of
More informationReview for Chapter 4: Structures and Properties of Substances
Review for Chapter 4: Structures and Properties of Substances You are responsible for the following material: 1. Terms: You should be able to write definitions for the following terms. A complete definition
More informationTest Review # 4. Chemistry: Form TR4.11A
Chemistry: Form TR4.11 REVIEW Name Date Period Test Review # 4 Bonding. The electrons of one atom are attracted to the protons of another. When atoms combine, there is a tug of war over the valence electrons.
More informationAll chemical bonding is based on the following relationships of electrostatics: 2. Each period on the periodic table
UNIT VIII ATOMS AND THE PERIODIC TABLE 25 E. Chemical Bonding 1. An ELECTROSTATIC FORCE is All chemical bonding is based on the following relationships of electrostatics: The greater the distance between
More informationChapter 4. The Major Classes of Chemical Reactions 4-1
Chapter 4 The Major Classes of Chemical Reactions 4-1 The Major Classes of Chemical Reactions 4.1 The Role of Water as a Solvent 4.2 Writing Equations for Aqueous Ionic Reactions 4.3 Precipitation Reactions
More information5072 CHEMISTRY (NEW PAPERS WITH SPA) BASIC TECHNIQUES 5067 CHEMISTRY (NEW PAPERS WITH PRACTICAL EXAM) BASIC TECHNIQUES
5072 CHEMISTRY (NEW PAPERS WITH SPA) BASIC TECHNIQUES 5067 CHEMISTRY (NEW PAPERS WITH PRACTICAL EXAM) BASIC TECHNIQUES LEARNING OUTCOMES a) Be able to write formulae of simple compounds b) Be able to write
More information