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introductory chemistry atoms first

Questions and Answers of Introductory Chemistry Atoms First

The pH of a solution is 4.(a) What is the H3O+ concentration?(b) What is the OH– concentration?(c) Is this solution acidic or basic?
The pH of a solution is 8.(a) What is the H3O+ concentration?(b) What is the OH– concentration?(c) Is this solution acidic or basic?
The pH of a solution is –1. What are the H3O+ and OH– concentrations? Is the solution acidic or basic?
Two students each dissolve 1 mole of acid in enough water to get 1 L of solution. Student A uses acetic acid, and student B uses hydrochloric acid. Do the solutions have the same pH? If not, which
Aniline, C6H5NH2, is a weak base, with a lone pair of electrons on the nitrogen atom.(a) According to Brønsted and Lowry, what must aniline do to act as a base?(b) Why can aniline act as a base?(c)
Can a weak acid and its conjugate base ever have the same charge? Explain.
Knowing that aniline (Problem 15.158) is a weak base, is its conjugate acid a weak acid or a strong acid?Problem 15.158Aniline, C6H5NH2, is a weak base, with a lone pair of electrons on the nitrogen
Nitric acid, HNO3, is a very strong acid. Solutions of sodium nitrate, NaNO3, contain lots of nitrate ions. Would you expect such a solution to be acidic, basic, or neutral? Explain.
Why is the conjugate base of a weak acid like acetic acid often referred to as a salt of the acid?
If Cl– is the conjugate base of HCl, why isn’t an aqueous solution of NaCl acidic?
What do we mean when we say that a solution has buffering ability?
Does pure liquid water have any buffering ability? Explain.
What is the general recipe for making a buffer? Explain the function of each ingredient.
Name one biological system in which control of pH (buffering ability) is important, and name the buffer that is in control.
Can a buffer resist pH changes for any added amount of strong acid or base? Explain.
Does a mixture of carbonic acid, H2CO3, a weak acid, and sodium bicarbonate, NaHCO3, in water constitute a buffer? If no, explain why. If yes, explain why and use chemical equations to show what
When a strong acid is added to a buffer, the pH changes a little bit.(a) Does the pH increase or decrease?(b) Why does the pH change at all? Why doesn’t the buffer hold the pH constant?
One way to make an acetic acid buffer is to mix substantial amounts of acetic acid and its salt, sodium acetate, in water. Another way to make the same buffer is to add a substantial amount of acetic
How would you make a buffer based on ammonia?
How would you make a buffer based on hypochlorous acid?
It is possible to make two completely different buffers using the dihydrogen phosphate ion, H2PO4–.(a) In one buffer, H2PO4– serves as the weak acid. What is the conjugate weak base?(b) Write the
Suppose 2.0 moles of sodium acetate, NaO2CCH3, are dissolved in some water and then 1.0 L of a 1.0 M HCl solution is added.(a) Write the chemical reaction that occurs.(b) After the reaction, what are
A buffer works by replacing added strong acid with weak acid. Explain how.
A buffer works by replacing added strong base with weak base. Explain how.
How does a buffer “kill” added strong base?
How does a buffer “kill” added strong acid?
Write the equations that show how a hypochlorous acid buffer defends against added strong acid and base.
Pyridine, C5H5N, is a weak base.(a) Write the chemical equation for the reaction between pyridine and water.(b) List all species present in an aqueous solution of pyridine in order of concentration,
Perchloric acid, HClO4, is a strong acid.(a) Write the chemical equation for the reaction between perchloric acid and water.(b) List all species present in an aqueous solution of perchloric acid in
In each of the following pairs, which is the stronger acid?(a) HPO42– and H2PO4–(b) H2O and H3O+(c) HCN (Keq = 6.2 × 10–10) and HCO2H (Keq = 1.8 × 10–4)(d) HI and HF
Write equilibria similar to Reaction 15.9 that show how CO32– and CH3COO– ions produce small amounts of OH– ions in aqueous solution. H H+ + H H H H Proton donor (acid) Proton acceptor (base)
How many moles of Ba(OH)2 would it take to neutralize 0.1 mole of hydrochloric acid?
According to the pH scale:(a) The higher the pH, the more acidic is the solution.(b) The H3O+ concentration = pH.(c) The H3O+ concentration = 10pH.(d) The lower the pH, the more acidic is the
Carbonic acid, H2CO3, is a weak acid. Carbonate ion, CO32–, is a weak base. A student claims that these are conjugates of each other. Is she right or wrong? Explain.
Draw three beakers as shown in WorkPatch 15.3, but change the labels to make them reflect the reaction mentioned in Practice Problem 15.9. Then list all species present in each beaker.Data from
In Reaction 15.7, water is shown acting as a base. How is water behaving in the following reaction?Explain your answer.Reaction 15.7 NH₂ + H₂O → NH3 + OH
(a) How does a weak acid in a buffer eliminate added OH– ions? To what does it convert these ions? What happens to the weak acid?(b) How does a weak base in a buffer eliminate added H3O+ ions? To
Imagine a buffer made by combining an aqueous solution of the weak acid HF with its sodium salt, NaF.(a) Write the reaction responsible for replacing any added strong base (OH–) by a weak base.(b)
Aniline, C6H7N, is a molecular compound that is a weak base. The molecule has a lone pair of electrons on the N atom.(a) Why can aniline act as a base?(b) Write the equilibrium expression that shows
For (a) Which of the two reactions you wrote in Practice Problem 15.15 has an equilibrium that lies farther to the right? Explain how you know.(b) Based on your answer to part (a), do you think an
In the presence of water, the bicarbonate ion, HCO3–, can be either a Brønsted–Lowry acid or a Brønsted–Lowry base. Write both equilibrium equations.
In the example we worked above, the concentration of H3O+ was 2.56 M and that of OH– was 3.91 × 10–15 M. Suppose you must multiply these values together but are forbidden to use a calculator or
The OH– concentration of an aqueous solution is 0.000 155 M.(a) Is the solution acidic or basic? Explain how you know.(b) What is the molar H3O+ concentration?
Suppose 1.00 mole of HCl is dissolved in enough water to give 500.0 mL of solution.(a) What is the H3O+ concentration? ( When 1 mole of HCl dissociates, we get 1 mole of H3O+ ions because the acid is
Suppose 0.0100 mole of Ba(OH)2 is dissolved in enough water to give 500.0 mL of solution.(a) What is the OH– concentration?(b) What is the H3O+ concentration?
What is the base-10 logarithm of 0.0010?
What is the logarithm of 10,000?
Suppose you have a bottle of acetic acid and a bottle of sodium acetate, CH3CO2Na, and you add some of each to the same beaker of water. Consult Tables 15.5 and 15.6 to help you answer the following
In the reactionwhich reactant is the Brønsted–Lowry acid and which is the Brønsted–Lowry base? NH3 + PH₂ →NH₂ + PH₂+
What would you dissolve in water along with the weak acid HF in order to prepare a buffered solution?
Rewrite the reaction of Practice Problem 15.11 using dot diagrams, and use an arrow to show the proton transfer.Data from Practice Problem 15.11In the reactionwhich reactant is the Brønsted–Lowry
What is the logarithm of 10? The logarithm of 101 is the same. Why?
What is the logarithm of 0.01? The logarithm of 10–2 is the same. Why?
Do not use a calculator for the following problems.What is the base-10 logarithm of 103?
Do not use a calculator for the following problems.What is the logarithm of 1.0 × 10–11 and of 10–11?
Do not use a calculator for the following problems.What is the negative logarithm, –log, of 10–7?
Which solution is less acidic, solution A with pH 2 or solution B with pH 6, and by how much?
Basic solution A has pH = 9. Basic solution B is ten times more basic than A. What is the pH of solution B?
Consider a solution ten times more acidic than the most acidic solution in Table 15.4.(a) What is the pH of this solution?(b) What is the molar concentration of H3O+ in this solution? Table 15.4 The
Write a chemical equation for the reaction between each pair of reactants, using single or double arrows as appropriate:(a) HNO3 and OH–(b) HF and OH–(c) NH3 and H2O(d) HCO3– and H2O
If 100 mL of an aqueous solution of nitric acid contains 0.030 mole of HNO3, what is the pH of the solution?
Complete the table: Type of electrolyte (strong, weak or Substance Name nonelectrolyte) NaCl HNO3 Mg(NO3)2 HF NaF NH4Cl Type of acid/base (strong or weak) - Reaction (s) in water (1) ¤ e ¤ ¤ e d e
A 0.20 M aqueous solution of monoprotic acid HX has a pH of 2.14.(a) Is HX a strong acid or a weak acid?(b) Calculate Keq for the reaction of HX with water.
Without calculating pH values, list these solutions in order of acidity, from lowest pH to highest pH:(a) 0.10 M LiNO3(b) 0.10 M NaF(c) 0.10 M KOH(d) 0.10 M HCN(e) 0.10 M HNO3(f) 0.20 M HCl
How many moles of nitric acid do you need to prepare 200 mL of an aqueous solution that has a pH of 2.0?
Other than water, what would you expect to find in the highest concentration in an aqueous solution of Ca(OH)2? Explain.
Write a chemical equation for the reaction between each pair of reactants, using single or double arrows as appropriate:(a) HCO3– and OH–(b) HCl and F–(c) H2CO3 and OH–(d) HCN and H2O
Other than water, what would you expect to find in the highest concentration in an aqueous solution of KOH? Explain.
What is the pH of these aqueous solutions?(a) 1.0 M HCl,(b) 0.1 M HCl,(c) 0.001 M HCl,(d) 1.0 × 10–5 M HCl,(e) 1.10 × 10–7 M HCl
How many moles of Ca(OH)2 would it take to completely neutralize 0.4 mole of phosphoric acid, H3PO4?
If 2.00 L of an aqueous solution of sodium hydroxide contains 20.0 g of NaOH, what is the pH of the solution?
Sulfuric acid, H2SO4, is a diprotic acid with dissociation equilibrium constants of Keq > 1.0 × 103 and Keq = 1.2 × 10–2. Write the two dissociation equilibrium equations, and match the proper
What is the pH of a 0.010 M aqueous solution of NaOH?
How many grams of NaOH do you need to prepare 1.0 L of an aqueous solution that has a pH of 11?
Which acid and base react to give an aqueous solution of K2SO4? Write a balanced equation for this neutralization reaction.
Rewrite this acid–base reaction in dot-diagram form, and then use an arrow to show the proton being transferred and label the Brønsted–Lowry acid and base: + F+ NH₂ → HF + NH3
The molar concentration of concentrated hydrochloric acid is 12.1 M. What are the pH and OH– ion molar concentration?
Indicate whether each compound is an electrolyte or a nonelectrolyte in water:(a) N2 (b) NH4ClO4(c) HI (d) CH3CH2CH3 (propane)(e) Li3PO4 (f) AgNO3(g) CCl4
Rearrange the acids in this chart so that they are listed with the weakest acid first and the strongest last: Name Hypochlorous acid Nitrous acid Hydrocyanic acid Formic
What is wrong with this question: How many grams of NaOH must be added to pure water to give a solution having a pH of 4.20?
Hydrazine, H2NNH2, is a weak base that can accept two protons. Draw a dot diagram for hydrazine and write equations showing how this compound accepts protons from water in two steps.
Acrylic acid, C2H3COOH, is a weak monoprotic acid. Write a balanced equation for the reaction that occurs when 25.0 mL of 0.200 M KOH is added to 50.0 mL of 0.200 M C2H3COOH. Besides water, what
How many grams of LiOH are there in 750 mL of an aqueous LiOH solution having an H3O+ concentration of 2.30 × 10–13 M?
Citric acid, H3C6H5O7, is a weak triprotic acid. Write equations for the three equilibrium reactions that occur during the stepwise dissociation of citric acid in water.
Using dot diagrams, write a reaction showing how the phenoxide ion, C6H5O–,can act as a weak base in water. Η. H C C. Ο: CIH H C C. Η Ἡ
What is the molar hydroxide ion concentration in a solution that is 1000 times more acidic than a solution that has a pH of 9.20?
For each acid–base pair, write a balanced equation for the neutralization reaction:(a) Lithium hydroxide and hydroiodic acid(b) Acetic acid and sodium hydroxide(c) Hydrobromic acid and calcium
Which acid and base react to give an aqueous solution of magnesium nitrate? Write a balanced equation for the neutralization reaction.
Is a solution that contains 0.10 M HBr and 0.10 M NaBr a buffered solution? Why or why not?
Formic acid, HCHO2, has a Keq of 1.8 × 10–4, and propionic acid, HC3H5O2, has a Keq of 1.3 × 10–5. Which has a higher pH, a 1 M solution of formic acid or a 1 M solution of propionic acid?
How many grams of HCl gas are dissolved in 7.50 L of an aqueous HCl solution that has a pH of 2.40?
Classify each substance as strong electrolyte, weak electrolyte, or nonelectrolyte:(a) CH3COOH (b) KCH3COO (c) H2SO4(d) CH2Cl2 (e) NH3(f) H3PO4 (g) ZnSO4
HClO4 is a strong acid, and HClO2 is a weak acid. If you had a 1.0 M solution of NaClO4 and a 1.0 M solution of NaClO2, which would have the higher pH? Explain.
If you dissolve 0.250 g of Ba(OH)2 in 3.00 L of water, what is the pH of the solution?
An aqueous solution containing CN– ions turns litmus blue. Write an equation showing how CN– makes water basic.
How many moles of HI are there in 2.75 L of an aqueous HI solution having an OH– concentration of 8.20 × 10–12 M?
You mix 500 mL of 1.00 M NaOCl with 500 mL of 0.500 M HNO3. Write an equation for the reaction that occurs. Besides water, what species are in the solution after reaction? Is this solution a buffer?
Rewrite this acid–base reaction in dot-diagram form, and then use an arrow to show the proton being transferred and label the Brønsted–Lowry acid and base: HS + HOCI H₂S + OCI
If 0.378 g of HBr dissolved in enough water to make 1.25 L of solution, what is the H3O+ concentration? What is the OH– concentration?
What is the OH– concentration of a solution that has a pH of 9.66? Is this solution acidic or basic?

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