[DA ㅂ ㅂ Question 2 Answer all parts i) The acid dissociation constants for H₂S, Kai and Ka2 have values of 9.1*108 and 1.2*10-13, respectively. Show that the mole fraction for H₂S is given by: αH2S = [H+1² [H+1²+Kai [H+]+Kai Kaz 2 H <
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- Complete the following table, which lists information about the measured acid dissociation constants of three unknown weak acids. Note: be sure each number you put in the table has the correct number of significant digits. acid B C Ka M 0 7.28 x 10 pK 1.17 11.3 0 relative strength (Choose one) ✓ (Choose one) ✓ (Choose one) ✓ O *10 X ?Calculate the concentration (M) of the anion Z2- for a 0.100 M solution of H2Z given the acid ionization constants for the acids below. Report your answer to the tenths place using scientific notation and do not include units. (ie. 1.1e+9, 1.1e-9) H2Z(aq) Ka = 7.8 x 10-2 HZ-(aq) Ka = 7.0 x 10-9What is the equilibrium-constant expression of the basic dissociation of NaNO2? Kb = [OH-]/([HNO2] [NO2]) Kb = ([HNO2] [NO2])/[OH-] Kb = ([HNO2] [OH-])/[NO2] Kb = ([NO2] [OH-])/[HNO2]
- NaHSO3 is a salt, which ionized completely to give HSO3- ion. the following equations show that this ion can act either as an acid or as a base. HSO3- + H2O(l) <=> H3O+ + SO3-2 K1 = ? HSO3- + H2O(l) <=> H2SO3 + OH- K2 = ? (a) Knowing that for H2SO3:Ka1=1.4x10-2, Ka2 = 6.5x10-8, find K1 and K2. (b)Predict which reaction of the two is more important based on their K values. (c) What is the pH of 0.10 M NaHSO3Malic acid is a weak diprotic organic acid with Ka1 = 4.0 × 10-4 and Ka2 = 9.0 × 10-5.a Letting the symbol H2A represent malic acid, write the chemical equations that represent Ka1 and Ka2 . Write the chemical equation that represents Ka1 × Ka2. b Qualitatively describe the relative concentrations of H2A, HA-, A2-, and H3 O+ in a solution that is about one molar in malic acid.c Calculate the pH of a 0.0175 M malic acid solution and the equilibriumconcentration of [H2 A].d What is the A2- concentrationin in solutions b and c?4.74 = For HC1O2 /KC102, pKa = 1.96; for HC10/KCIO, pKa = 7.54; and, for NH; MISSED THIS? Read Section 18.3 (Pages 799 - 802) . pKa 14.00 – pKb The following table shows the values of ionization 14.00 – 4.754 constants for a number of acids and bases at 25 9.25 °C: So, HC1O/KCIO is the best choice to create a buffer with pH = 7.30 because HC | Formula Ka value that is closest to 7.30. |НС2 Н3О2 | 1.8х 10 3 -5 HC1O2 1.1 × 10-2 NH3 1.76 x 10-5 Part B HC1O 2.9 x 10-8 For the best system, calculate the ratio of the masses of the buffer components required to ma Express your answer to two significant figures. m(KC1O) = 41.62 m(HC10) Submit Previous Answers Request Answer * Incorrect; Try Again; 3 attempts remaining
- What is the concentration of H3O+ in a solution that is 0.0600 M Hypochlorous acid (HClO)? What is the pH? To solve this problem: Write the acid dissociation equilibrium for HClO Set up an ICE chart ( with x = the concentration of H3O+ at equilibrium) Write the expression for Ka. Fill this in with the concentrations of H3O+, ClO- and HClO at equilibrium, in terms of x. Decide if x can be neglected. You may neglect x if the initial concentration of the HClO is greater than 100 times the Ka. You will need the value of Ka. Look it up on the chart (p 4 of packet) Solve for x Find the pH The pH of a 0.0200 M solution of an unknown acid is 2.56. What is the Ka of this acid? To solve this problem: Write the acid dissociation equilibrium for the generic aicd “HA” Set up an ICE chart ( with x = the concentration of H3O+ at equilibrium) Write the expression for Ka. Fill this in with the concentrations of H3O+, A- and HA at equilibrium, in terms of x. What is x? Can you find it…HC H 36 46 15:11 29.0 ןו:5ר הה" HB/s Assignment 2.pdf 1. Identify the acids and bases in the following reactions: (a) CH3OH + H - CH,OH2 (b) CH3OH + NH2- - CH30- + NH3 Žnca +o (c) + ZnClz H3C HyC H 2. Rank the following substances in order of increasing acidity: H H C0H он H CH3CH. CH3CCH,CCH, CHyCOH Pentane-2,4-dione (pK, = 9) Phenol (pk, = 9.9) Acetone Acetic acid (pk,- 19.3) (pk, = 4.76) 3. List the following carboxylic acids in order from strongest acid to weakest acid: CH,CH;CH;COOH K,-1.52 x 10- CICH CH;CH;COOH K,-2.96 x 10 CH,CH;CHCOOH CH,CHCH;COOH ČI K1.39 10 K-8.9x 10 4. For the following compound, a. draw its conjugate acid. h. draw its conjugate base. H,NCH,COOH 5. List the following compounds in order from strongest acid to weakest acid: CH CH,COOH CH,OH CHCIOH 6. Which of the following are likely to act as Lewis acids and which as Lewis bases? Which might act both ways? (a) CH3CH,OH (b) (CH3)2NH (e) H3C+ (c) MgBrz (D (CHahP (d) (CH3)B IIIIn which of the following aqueous solutions does the weak acid exhibit the highest percentage ionization? 0.01M HC3H5O2(Ka=1.3x10-5) 0.01M HOCI (Ka= 3.5x10-8) 0.01M H2SO3(Ka= 1.4x10-2) 0.01M HC2H3O2(Ka=1.8x10-5) 0.01M H3BO3(Ka= 5.4x10-10)
- Predicting the qualitative acid-base properties of salts 3/5 Consider the following data on some weak acids and weak bases: acid base K. K, name formula name formula hypochlorous acid HCIO 8- ethylamine C,H;NH, 6.4 × 10 -4 3.0 x 10 10 hydrocyanic acid HCN 4.9 x 10 methylamine CH;NH, 4.4 ×10 Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. solution pH 0.1 M KCI choose one v 0.1 M CH3NH3CI choose one v 0.1 M NACN choose one v 0.1 M C2H5NH3Br choose one vWhat is the acid dissociation constant (Ka) expression for the following reaction? CH3COOH+H2O=CH3COO-+H3OThe pH of a 1.0 M solution of pentanoic acid (HC;H,O2) is measured to be 2.42. Calculate the acid dissociation constant K, of pentanoic acid. Be sure your answer has the correct number of significant digits. K = 0