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chemistry a molecular approach
Chemistry A Molecular Approach 5th Edition Nivaldo Tro - Solutions
A mixture of Na2CO3 and NaHCO3 has a mass of 82.2 g. It is dissolved in 1.00 L of water, and the pH is found to be 9.95.Find the mass of NaHCO3 in the mixture.
A mixture of NaCN and NaHSO4 consists of a total of 0.60 mol.When the mixture is dissolved in 1.0 L of water and comes to equilibrium, the pH is found to be 9.9. Find the amount of NaCN in the mixture.
Without doing any calculations, determine which solution in each pair is more acidic.a. 0.0100 M in HCl and 0.0100 M in KOHb. 0.0100 M in HF and 0.0100 M in KBrc. 0.0100 M in NH4Cl and 0.0100 M in CH3NH3Brd. 0.100 M in NaCN and 0.100 M in CaCl2
Without doing any calculations, determine which solution in each pair is more basic.a. 0.100 M in NaClO and 0.100 M in NaFb. 0.0100 M in KCl and 0.0100 M in KClO2c. 0.0100 M in HNO3 and 0.0100 M in NaOHd. 0.0100 M in NH4Cl and 0.0100 M in HCN
Rank the acids in order of increasing acid strength. CH3COOH CH₂CICOOH CHCI₂COOH CCl₂COOH
Without using a calculator, determine the pH and pOH of each solution. Rank the solutions from most acidic to most basic. a. 1.0 x 10-2 M HCI c. 1.0 x 10-2 M NaOH b. 1.0 x 10-4 M HCI d. 1.0 x 10M NaOH
Have each group member make two flashcards with an acid or base on one side and its conjugate on the other side. Check each other’s cards and quiz each other until each group member is proficient at identifying conjugate pairs.
Answer the following questions in a complete sentence or two:a. How do you know if an acid is strong or weak?b. How do you calculate the pH of a strong acid solution?c. How do you calculate the pH of a weak acid solution?d. If you know the Ka of an acid, how do you determine the Kb of its conjugate
Sulfur dioxide is a common preservative in wine; it prevents oxidation and bacterial growth. When SO2 is added to wine, it reacts with water to form an equilibrium system with the bisulfite ion:In this equilibrium system, SO2 is called “molecular SO2”; in its HSO3– form, it is called “free
Solve the following problem, taking turns in your group to explain how to do the next step: What is the pH when 5.3 g of sodium acetate, NaC2H3O2, is dissolved in 100.0 mL of water?(The Ka of acetic acid, HC2H3O2, is 1.8 * 10-5.)
Define each of the following with complete sentences, and provide an example chemical equation: an Arrhenius acid, a Brønsted–Lowry base, and a Lewis acid.
In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base. (a) H₂SO4(aq) + H₂O(1) (b) HCO3(aq) + H₂O(1) HSO4 (aq) + H3O+ (aq) H₂CO3(aq) + OH(aq)
Which property is not associated with an acid?(a) Dissolves metals (b) Turns blue litmus red (c) Has a bitter taste
Identify the conjugate base in the reaction shown here: HCIO₂(aq) + H₂O(aq) — H3O+ (aq) + ClO₂ (aq)
What causes heartburn? What are some possible ways to alleviate heartburn?
Calculate [OH–] at 25 °C for each solution and determine if the solution is acidic, basic, or neutral. (a) [H3O¹] = 7.5 x 10-5 M (b) [H3O+] = 1.5 × 10-⁹ M (c) [H3O¹] = 1.0 x 10-7 M
Which pair is not a conjugate acid–base pair?(a) (CH3)3N; (CH3)3NH+(b) H2SO4; H2SO3 (c) HNO2; NO2–
Which pair is a Brønsted–Lowry conjugate acid–base pair? a) NH3; NH4+ c) HCl; HBr b) H3O+; OH™ d) CIO4; CIO3
What are the general physical and chemical properties of acids? Of bases?
Calculate the pH of each solution at 25 °C and indicate whether the solution is acidic or basic. (a) [H3O+] 1.8 x 10-4 M = (b) [OH-] = 1.3 x 10-2 M
Consider the three generic weak acids HA, HB, and HC. The images shown here represent the ionization of each acid at room temperature. Which acid has the largest Ka? (a) HA (b) HB (c) HC
Consider the given acid ionization constants. Identify the strongest conjugate base. Acid HNO₂(aq) HCHO₂(aq) HCIO(aq) HCN(aq) a) NO₂ (aq) c) CIO (aq) Ka 4.6 x 10-4 1.8 x 10-4 2.9 X 10 8 4.9 × 10-10 b) CHO, (aq) d) CN (aq)
What is a carboxylic acid? Give an example.
Consider these two acids and their Ka values:Which acid is stronger? (a) HF (b) HCIO K₂ = 6.8 x 10-4 K₂ = 2.9 x 10-8 a
What is the OH– concentration in an aqueous solution at 25 °C in which [H3O+] = 1.9 * 10-9 M ? a) 1.9 x 10 M c) 5.3 x 106 M b) 5.3 x 10-6 M d) 1.9 x 10-23 M
What is the Arrhenius definition of an acid? Of a base?
Find the [H3O+] of a 0.100 M HCN solution.
The H3O+ concentrations of three solutions at room temperature are as follows. Which solution is acidic? (a) [H3O¹] = 1 x 10³ M (c) [H3O¹] 1 x 10⁹ M (b) [H3O¹] = 1 x 10 M
What is a hydronium ion? Does H+ exist in solution by itself?
An HNO3(aq) solution has a pH of 1.75. What is the molar concentration of the HNO3(aq) solution?a) 1.75 M b) 5.6 * 10-13 Mc) 56 M d) 0.018 M
Find the pH of a 0.200 M HNO2 solution.
As the pH of a solution increases (gets higher), what happens to the acidity of the solution?(a) The acidity increases. (b) The acidity decreases.(c) The acidity remains constant.
What is the Brønsted–Lowry definition of an acid? Of a base?
Find the pH of a 0.350 M aqueous benzoic acid solution. For benzoic acid, Ka = 6.5 * 10-5.a) 4.64 b) 4.19c) 2.32 d) 11.68
The initial concentration and Ka of several weak acid (HA) solutions are listed. For which solution is the x is small approximation least likely to work in finding the pH?(a) Initial [HA] = 0.100 M; Ka = 1.0 * 10-5(b) Initial [HA] = 1.00 M; Ka = 1.0 * 10-6(c) Initial [HA] = 0.0100 M; Ka = 1.0 *
Why is there more than one definition of acid–base behavior?Which definition is the right one?
Find the pH of a 0.155 M HClO2(aq) solution. For HClO2, Ka = 0.011.a) 0.92 b) 1.44c) 1.39 d) 0.69
A 0.100 M weak acid (HA) solution has a pH of 4.25. Find Ka for the acid.
Which solution is most acidic (that is, which one has the lowest pH)?(a) 0.10 M HCl(b) 0.10 M HF(c) 0.20 M HF
Describe amphoteric behavior and give an example.
Calculate the percent ionization of 1.45 M aqueous acetic acid solution. For acetic acid, Ka = 1.8 * 10-5.a) 0.35% b) 0.0018%c) 0.29% d) 0.0051%
Find the percent ionization of a 2.5 M HNO2 solution.
Which weak acid solution has the greatest percent ionization?(a) 0.100 M HC2H3O2(b) 0.500 M HC2H3O2(c) 0.0100 M HC2H3O2
What is a conjugate acid–base pair? Provide an example.
Consider two aqueous solutions of nitrous acid (HNO2).Solution A has a concentration of [HNO2] = 0.55 M and solution B has a concentration of [HNO2] = 1.25 M.Which statement about the two solutions is true?a) Solution A has the higher percent ionization and the higher pH.b) Solution B has the
Find the pH of a mixture that is 0.300 M in HF and 0.100 M in HClO.
Which solution is most acidic (that is, has the lowest pH)?(a) 1.0 M HCl(b) 2.0 M HF(c) A solution that is 1.0 M in HF and 1.0 M in HClO
Find the [OH–] in a 0.200 M solution of ethylamine (C2H5NH2). For ethylamine, Kb = 5.6 * 10-4.a) 11.52 M b) 2.48 Mc) 0.033 M d) 0.011 M
Determine the OH– concentration and pH in each solution.(a) 0.225 M KOH(b) 0.0015 M Sr(OH)2
Which anion acts as a weak base?(a) Cl-(b) Br-(c) F-
Which ion forms a basic solution when dissolved in water? a) Br b) NO3- c) HSO4 2- d) SO3²-
What are diprotic and triprotic acids? List an example of each.
Find the [OH–] and pH of a 0.100 M NH3 solution.
Which ionic compound forms an acidic solution when dissolved in water?(a) NH4Br (b) KCl (c) NaHCO3
Which compound forms an acidic solution when dissolved in water? a) NH4Cl b) NaCl c) KNO₂ d) Ca(NO3)2
Define the acid ionization constant and explain its significance.
Which of the protons shown in red is more acidic? H-C-0-H (a) H H-C-0-H H (b)
Write an equation for the autoionization of water and an expression for the ion product constant for water (Kw). What is the value of Kw at 25 °C?
Find the pH of 0.175 M NaCN solution. For HCN, Ka = 4.9 * 10-10.a) 5.03 b) 11.28 c) 2.31 d) 8.97
Find the pH of a 0.100 M NaCHO2 solution. The salt completely dissociates into Na+(aq) and CHO2–(aq), and the Na+ ion has no acid or base properties.
What is the concentration of X2- in a 0.150 M solution of the diprotic acid H2X? For H2X, Ka1 = 4.5 * 10-6 and Ka2 = 1.2 * 10-11. a) 9.9 x 10-8 M c) 8.2 x 10 4M b) 2.0 x 10 9 M d) 1.2 x 10-11 M
What happens to the [OH–] of a solution when the [H3O+] is increased? Decreased?
Classify each cation as a weak acid or pH-neutral.(a) C5H5NH+ (b) Ca2+ (c) Cr3+
Which acid has the largest Ka: HClO2(aq), HBrO2(aq), or HIO2(aq)? a) HClOz(aq) b) HBrO₂ (aq) c) HIO₂(aq) d) All three acids have the same Ka.
Define pH. What pH range is considered acidic? Basic? Neutral?
Determine if the solution formed by each salt is acidic, basic, or neutral.(a) SrCl2 (b) AlBr3 (c) CH3NH3NO3(d) NaCHO2 (e) NH4F
Define pOH. What pOH range is considered acidic? Basic? Neutral?
Find the pH of a 0.100 M ascorbic acid (H2C6H6O6) solution.
In most solutions containing a strong or weak acid, the autoionization of water can be neglected when calculating [H3O+]. Explain why this statement is valid.
Find the pH of a 0.0100 M sulfuric acid (H2SO4) solution.
When calculating [H3O+] for weak acid solutions, we can often use the x is small approximation. Explain the nature of this approximation and why it is valid.
Find the [C6H6O6 2-] of the 0.100 M ascorbic acid (H2C6H6O6) solution in Example 17.17.Example 17.17Find the pH of a 0.100 M ascorbic acid (H2C6H6O6) solution.
What is the percent ionization of an acid? Explain what happens to the percent ionization of a weak acid as a function of the concentration of the weak acid solution.
In calculating [H3O+] for a mixture of a strong acid and weak acid, the weak acid can often be neglected. Explain why this statement is valid.Write a generic equation showing how a weak base ionizes water.
Write a generic equation showing how a weak base ionizes water.
How can you determine if an anion will act as a weak base?Write a generic equation showing the reaction by which an anion, A–, acts as a weak base.
What is the relationship between the acid ionization constant for a weak acid (Ka) and the base ionization constant for its conjugate base (Kb)?
What kinds of cations act as weak acids? List some examples.
When calculating the [H3O+] for a polyprotic acid, the second ionization step can often be neglected. Explain why this statement is valid.
For a weak diprotic acid H2X, what is the relationship between [X2–] and Ka2? Under what conditions does this relationship exist?
For a binary acid, H—Y, which factors affect the relative ease with which the acid ionizes?
Which factors affect the relative acidity of an oxyacid?
What is the Lewis definition of an acid? Of a base?
What is a general characteristic of a Lewis acid? Of a Lewis base?
What is acid rain? What causes it, and where is the problem the greatest?
Identify each substance as an acid or a base and write a chemical equation showing how it is an acid or a base according to the Arrhenius definition. a. HNO3(aq) C. KOH(aq) b. NH4 (aq) d. HC₂H3O2(aq)
What are the main detrimental effects of acid rain? What is being done to address the problem of acid rain?
Identify each substance as an acid or a base and write a chemical equation showing how it is an acid or a base in aqueous solution according to the Arrhenius definition. a. NaOH(aq) C. HBr(aq) b. H₂SO4(aq) d. Sr(OH)₂ (aq)
In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base. a. H₂CO3(aq) + H₂O(1) b. NH3(aq) + H₂O(1) c. HNO3(aq) + H₂O(1) H3O+ (aq) + NO3 (aq) d. C,H,N(aq) + H₂O(1) = C,H,NH+ (aq) + OH (aq) → H30¹(aq) + HCO3 (aq) NH4+
In each reaction, identify the Brønsted–Lowry acid, the Brønsted– Lowry base, the conjugate acid, and the conjugate base. H30¹(aq) + (aq) a. HI(aq) + H₂O(1)→ b. CH3NH₂(aq) + H₂O(1) CH3NH3 (aq) + OH (aq) c. CO32 (aq) + H₂O(1) — HCO3 (aq) + OH (aq) d. HBr(aq) + H₂O(1) → H3O+
Write the formula for the conjugate base of each acid. a. HCI b. H₂SO3 c. HCHO, d. HF
Write the formula for the conjugate acid of each base. a. NH3 b. CIO C. HSO4 2- d. CO3²-
Both H2O and H2PO4– are amphoteric. Write an equation to show how each substance can act as an acid and another equation to show how each can act as a base.
Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (Ka). a. HNO3 b. HCI c. HBr d. H₂SO3
Both HCO3– and HS- are amphoteric. Write an equation to show how each substance can act as an acid and another equation to show how each can act as a base.
Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (Ka). a. HF b. HCHO₂ c. H₂SO4 d. H₂CO3
The three diagrams represent three different solutions of the binary acid HA. Water molecules have been omitted for clarity, and hydronium ions (H3O+) are represented by hydrogen ions (H+). Rank the acids in order of decreasing acid strength. (a) (b) (c)
Pick the stronger base from each pair. a. F™ or Cl b. NO₂ or NO3 c. F or CIO™
A mixture of water and graphite is heated to 600 K. When the system comes to equilibrium, it contains 0.13 mol of H2, 0.13 mol of CO, 0.43 mol of H2O, and some graphite. Some O2 is added to the system, and a spark is applied so that the H2 reacts completely with the O2. Find the amount of CO in the
At 650 K, the reaction MgCO3(s) ⇌ MgO(s) + CO2(g) has Kp = 0.026. A 10.0-L container at 650 K has 1.0 g of MgO(s) and CO2 at P = 0.0260 atm. The container is then compressed to a volume of 0.100 L. Find the mass of MgCO3 that is formed.
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![(a) [H3O+] = 7.5 x 10-5 M (b) [H3O+] = 1.5 10- M (c) [H3O+] = 1.0 x 10-7 M](https://dsd5zvtm8ll6.cloudfront.net/images/question_images/1700/2/1/9/56265574aaa1d2931700219561874.jpg){kind=small}
![(a) [H3O] 1.8 x 10-4 M = (b) [OH] = 1.3 x 10-2 M](https://dsd5zvtm8ll6.cloudfront.net/images/question_images/1700/2/1/9/57765574ab9a13a51700219577008.jpg){kind=small}
![(a) [H3O] = 1 x 10 M (c) [H3O+] 1 x 10 M (b) [H3O] = 1 x 10 M](https://dsd5zvtm8ll6.cloudfront.net/images/question_images/1700/2/2/1/092655750a4f20601700221092547.jpg)
