Unit 3 -Acid base equilibria |Science

Unit 3 -Acid base equilibria |Science

CHEMISTRY 1220 – UNIT 3 ISSUES SET 3b

3b-1 For each of the following solutions, compute the [OH-] from the [H3O+] and classify the solution as acidic or basic.
(a) [H3O+] = 7.310-7
(b) [H3O+] = 2.310-10
3b-2 For each of the following solutions, calculate the [H3O+] from the [OH-] and classify the solution as acidic or basic.
(a) [OH-] = 7.310-7
(b) [OH-] = 3.710-6
3b-3 Compute the pH to the correct number of significant figures for the following solutions.
(a) [H3O+] = 2.010-5
(b) [H3O+] = 3.5610-9
(c) [OH-] = 410-3
(d) [OH-] = 110-6
3b-4 Compute the [H3O+] concentration associated with each of the following pH values.
(a) 2.43
(b) 3.430

(c) 7.4
3b-5 A solution has a pH of 4.500. What will be the pH of this solution if the hydronium ion concentration is;

(a) doubled
(b) quadrupled
(c) increased by a factor of 10
(d) increased by a factor of 1000
3b-6 Calculate the pH for each of the following solutions of a strong acid or base.
(a) 0.0063 M HNO3
(b) 0.2 M HCl
(c) 0.000021 M Ba(OH)2
(d) 0.000232 M NaOH
3b-7 Compute the following for a 0.015 M HNO3 solution.
(a) [H3O+]
(b) pH
(c) [OH-]

(d) pOH
3b-8 A solution of HCl has a pH of 3.32. What is the molarity of the solution?
3b-9 A 1.00 L aqueous solution contains 5.80 grams of sodium hydroxide. What is the pH of the solution at 25oC?
3b-10 The volume of an adult’s stomach ranges from 50 mL when empty to 1 L when full. If its volume is 450 mL and its contents have a pH of 2.0;
(a) How many moles of H+ does it contain?
(b) Assuming all the H+ comes from HCl, how many grams of sodium bicarbonate will totally neutralize the stomach acid?

CHEMISTRY 1220 – UNIT 3 ISSUES SET 3c

3c-1 Prepare the acid ionization constant expression for each of the following acids
(a) HF – hydrofluoric acid
(b) HC6H7O6 – ascorbic acid
3c-2 Calculate the acid ionization constant for the acid HA based on each of the following sets of data.
(a) 0.0100 M HA solution which gives [H+] = 0.0025
(b) 0.0200 M HA solution which gives [A-] = 0.0050
(c) 0.1000 M HA solution that is 12.0% ionized
3c-3 The pH of a 0.250 M HF solution is 2.036. Calculate the:
(a) Ka for HF
(b) percent ionization of HF in solution
3c-4 For a 0.30 M HClO solution (hypochlorous acid), calculate the pH and the concentrations of all species present (H3O+, ClO-, HClO, and OH-). Ka = 3.510-8 at 25oC for HClO.
3c-5 For a 0.0036 M HC9H7O4 solution (acetylsalicylic acid; active ingredient in aspirin), calculate the solution pH. Ka = 3.310-4 at 25oC for HC9H7O4.
3c-6 A 0.200 M solution of a weak acid is 9.4 percent ionized. What is the Ka for the acid?
3c-7 A sample of vinegar has a pH of 2.90. Assuming that he vinegar, HC2H3O2, contains only acetic acid, Ka = 1.810-5, calculate the concentration of acetic acid (undissociated) in the vinegar.
3c-8 Calculate the concentrations of all species present in a 0.10 M solution of the diprotic acid H2C6H6O6 (ascorbic acid, vitamin C). At 25oC the ionization constants are K1 = 7.910-5 and K2 = 1.610-12.
3c-9 Citric acid, present in citrus fruits, is a triprotic acid. Calculate the pH of a 0.050 M solution of citric acid.
K1 = 7.410-4, K2 = 1.710-5, K3 = 4.010-7

CHEMISTRY 1220 – UNIT 3 ISSUES  SET 3d

3d-1 Prepare the base ionization constant expression for each of the following bases.
(a) NH3 (ammonia)
(b) CH3NH2 (methylamine)
(c) CHO2- (formate ion)
3d-2 The painkiller morphine (C17H19NO3) is a weak base with Kb = 1.610-6 at 25oC. Calculate the pH in a 0.0075 M morphine solution.
3d-3 What is the chemical formula of the salt produced from each of the following complete acid-base neutralizations?
(a) HNO3 and NaOH
(b) HCN and KOH
(c) HC2H3O2 and Ca(OH)2
3d-4 Classify each of the following salts in terms of its “neutralization parent.” (strong acid-strong base, weak acid weak base, etc).
(a) NaCl

(b) KCN
(c) NH4Cl
(d) LiC2H3O2
(e) NH4F
3d-5 For each salt in 3d-4, identify the ion (or ions) that will undergo hydrolysis in aqueous solution.
3d-6 For each salt in 3d-4, predict whether the aqueous solution will be acidic, basic, or neutral.
3d-7 Write an equation for the hydrolysis of each of the following ions in an aqueous solution.
(a) F-
(b) NH4+
(c) C2H3O2-
3d-8 organize  the following 0.1 M aqueous solutions in order of increasing pH: KOH, HC2H3O2, NaC2H3O2, HBr, and Ca(NO3)2.
3d-9 Given that Ka(HF) = 6.8×10-4, Ka(HCN) = 4.9×10-10, and Kb(NH3) = 1.8×10-5, predict whether each of the following 0.1 M aqueous salt solutions is acidic, basic, or neutral.
(a) NaF
(b) NH4F
(c) NaCN
(d) NH4CN
3d-10 Given that Ka(H3PO4) = 6.9×10-3, Ka(H2PO4-) = 6.2×10-8, and Ka(HPO42-) = 4.8×10-13, predict whether each of the following 0.1 M aqueous salt solutions is acidic, basic, neutral.
(a) Na3PO4
(b) Na2HPO4
(c) NaH2PO4
3d-11 Complete  the pH of a 0.20 M NH4Cl solution; Kb(NH3) = 1.8×10-5.
3d-12 Calculate the pH of a 0.20 M NaNO2 solution; Ka(HNO2) = 4.5×10-4.

CHEMISTRY 1220 – UNIT 3 ISSUES  SET 3e

3e-1 organize the compounds in each of the following series in order of increasing acid strength:

(a) H2S, H2Se, H2O
(b) HClO, HClO2, HClO3, HBrO, HIO

3e-2 Based on composition and structure, select the stronger BASE in each of the following pairs:

(a) NO2-, NO3

(b) PO43-, AsO43

(c) HCO3-, CO32

(d) H2SeO4, H2SO4

3e-3 Indicate whether each of the following statements is true or false. For those that are false, correct the statement so that it is true.

(a) In general, the acidity of binary acids increases from left to right in a given row of the periodic table.
(b) In a series of acids that have the same central atom, acid strength increases with the number of hydrogen atoms.
(c) Hydrotelluric acid, H2Te, is a stronger acid than H2S because Te has a greater electronegativity than S.

3e-4 Classify the following substances as either a Lewis acid or Lewis base.

(a) CO2
(b) BCl3
(c) I-
(d) H2O
(e) H+(f) OH-

3e-5 Identify the Lewis acid and Lewis base among the reactants in each of the following reactions.

(a) Cr3+ + 6H2O ÿ Cr(H2O)63+
(b) SnCl4 + 2Cl- ÿ SnCl62-
(c) Fe(ClO4)3(s) + 6H2O(l) ÿ Fe(H2O)63+(aq) + 3ClO4-(aq)
(d) CN-(aq) + H2O(l) ÿ HCN(aq) + OH-(aq)

3e-6 Predict which member of each pair produces the more acidic aqueous solution.

(a) K+, Cu2+
(b) Fe2+, Fe3+
(c) Al3+, Ga3+
(d) CuCl, Cu(NO3)2
(e) H2S, HS-

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