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introductory chemistry atoms first

Introductory Chemistry Atoms First 5th Edition Steve Russo And Michael Silver - Solutions

After considering the following diagram, write an equilibrium reaction for what each acid does in water, and then state if the equilibrium lies to the left, in the middle, or goes to completion (all the way to the right) Add 1 mol HCI HO gas Dissolves to give 1 mol HCI Strongly acidic solution 1
An ionic compound with the formula NaX (X– is an unknown anion) is dissolved in water, and the resulting solution is basic. Is HX a strong acid or a weak acid? Explain.
In Chapter 12, you learned that when metal ions dissolve in water they become solvated (hydrated), meaning they form ion–dipole attractions to many water molecules (often six). For example, Na+(aq) really looks like this in water:Fe3+ (aq) ions also do this, but unlike Na+(aq) ions, they also
Lithium hydride (LiH) is a source of hydride ion, shown below.As you can see, the hydride ion has a negative charge (it is an anion) and a lone pair of electrons. When thrown into water, the hydride ion makes the water strongly basic. Write a reaction that shows how the hydride ion reacts with
Consider a mercury manometer, shown belowWhen the trapped gas pushes the mercury level down in the right tube, it causes the mercury to climb to a greater height in the left tube. It will always be true that the amount the mercury column goes down on the right is exactly the same as the increase in
Suppose you come across the following labeled bottle:(a) What would the pH of this solution be?(b) Would you consider this solution to be strongly acidic?(c) Is there any hydroxide ion in this solution? If so, what is its concentration?(d) Would a 10 M solution of acetic acid be more acidic, less
When Fe3+ ions dissolve in water, they immediately form [Fe(OH2)6]3+ aqueous ions in which six molecules of water bind to the iron via six Fe–O bonds. However, this is not all that happens. The solution also becomes acidic. Interestingly, Fe2+ ions also form similar [Fe(OH2)6]2+ ions, but the
A quantity often used to characterize the acidity of an acid is its pKa. The pKa of an acid is equal to –log(Ka). Knowing this, what can you say about acid #1 whose pKa = 2, and acid #2 whose pKa = 6? Which is more acidic and by how much?
Glycine is the simplest of amino acids and is shown below.Notice that it has a weak COOH end similar to acetic acid. Like acetic acid, this end is weakly acidic. It also has an NH2 end similar to NH3. Like NH3, this end is weakly basic. Although not technically a buffer, when glycine is added to
Complete the following sentence: “The lower the pKa, the (stronger/weaker) ______ the acid.” How does this parallel pH?
Actually, once in water, the amino acid glycine (see problem above) exists as a zwitterion, as shown below. A zwitterion is an overall electrically neutral species that nevertheless has a + and – charge in it.Now, the NH3+ end is weakly acidic and the COO– end is weakly basic. Does this mean
Determine the ammonia concentration of an aqueous solution that has a pH of 11.50. The equation for the dissociation of NH3 (K₂ = 1.8 x 10°) is NH3(aq) + H₂O(1) = NH₂ (aq) + OH (aq). +
What is the pH of a solution prepared by mixing 100.00 mL of 0.020 M H2SO4 with 50.00 mL of 0.100 M NaOH? Assume that the volumes are additive.
HZ is a weak acid. An aqueous solution of HZ is prepared by dissolving 0.020 mol of HZ in sufficient water to yield 1.0 L of solution. The pH of the solution was 4.93 at 25.0 °C. What is the Ka of HZ?
How many milliliters of 0.015 M NaOH are needed to neutralize 50.0 mL of 0.010 M HNO3(aq)? Draw a beaker and show all species present after the neutralization. Be sure to include several water molecules in your drawing.
A solution is formed by mixing 50.0 mL of 0.015 M NaOH(aq) with 50.0 mL of 0.010 M HNO3(aq).(a) Is the solution acidic or basic?(b) Draw a beaker and show all species present in the solution.(c) What is the pH of the solution?
A 0.0035 M aqueous solution of a particular compound has pH = 4.76. What kind of compound is this? (Circle one choice in each column.) Briefly explain your answer Strong Weak Acid Base
For a given solute in water, the energy changes are ΔEsolute separation = 835 kJ, ΔEsolvent separation = 98 kJ, and ΔEsolvation = -805 kJ. Will this solute dissolve in water? Explain your answer, both numerically and in terms of the three-step model for a solute’s dissolving in a solvent.
What is the vapor pressure of chloroform at 61.7°C?
To prepare 500.0 mL of a 2.0 M solution, you would:(a) Dissolve 2 moles of solute in enough solvent to give 500.0 mL of solution.(b) Dissolve 1.0 mole of solute in enough solvent to give 500.0 mL of solution.(c) Dissolve 1.0 mole of solute in 500.0 mL of solvent.(d) Dissolve 2.0 moles of solute in
Suppose we want to dissolve a gaseous solute in water. Would you expect ΔEsolute separation to be larger for the gaseous solute or for a solid ionic solute? Explain.
How many moles of dissolved solute particles (molecules or ions) are present in each beaker in the above diagram?
If you have 500. mL of a 2.0 M solution and you add enough solvent to dilute it to a total new volume of 2.0 L, its new concentration will be:(a) 4.0 M.(b) 1.0 M.(c) 0.50 M.(d) 0.25 M.
The more negative ΔEsolvation is, the more likely a solute will dissolve. Explain.
Suppose you put detergent in a dry-cleaning machine that uses carbon tetrachloride. Assuming micelle-type structures form,(a) Draw the micelle-type structures that would form and explain your diagram.(b) Explain what kind of dirt these structures would be good at removing.
When a solute is added to a solvent:(a) The vapor pressure of the solvent increases.(b) The vapor pressure of the solvent decreases.(c) The solvent’s boiling point and freezing point increase.(d) The solvent’s boiling point and freezing point decrease.
Suppose you want to dissolve some MgCl2 in water.(a) How do we know that magnesium cations have a +2 charge?(b) ΔEsolute separation for MgCl2 is much more positive than ΔEsolute separation for NaCl. Explain what this means and why it might be so.(c) MgCl2 is more soluble in water than NaCl.
How many grams of potassium chloride, KCl, will it take to prepare a saturated solution in 500.0 mL of boiling water? (The solubility of KCl at 100 °C is 56.7 g/100.0 g water; assume the density of water is 1.000 g/mL.)
How many grams of sucrose will it take to saturate 1 ton of water at 20.0°C? (1 ton = 2000 lb; 1 lb = 453.6 g)
What mass of solid NaCl do you need to prepare 400.0 mL of a 2.00 M NaCl solution from scratch? How much water do you add to the NaCl? ??? g How much NaCl in grams? 400 mL Water- 400 ml. How much water?
You have 1 L of a 3.00 M stock solution of NaCl and need to prepare 400.0 mL of a 2.00 M solution. Describe how you would do it. 3.00 M NaCl- 400 ml. How much stock solution (in milliliters)? Water- 400 ml. How much water?
A solution is prepared by dissolving 25.0 g of sucrose in 175.0 g of water. Characterize its concentration by the appropriate percent composition.
Gasohol is a solution of gasoline and ethanol. Every liter of gasohol contains 90.0 mL of ethanol dissolved in gasoline. Characterize the solute concentration by the appropriate percent composition.
Suppose you have 65.0 g of the solution from Practice Problem 12.19. How many grams of sucrose do you have?Data from Problem 12.19A solution is prepared by dissolving 25.0 g of sucrose in 175.0 g of water. Characterize its concentration by the appropriate percent composition.
How many moles of CaF2 are there in 25.0 mL of 0.350 M CaF2(aq)?
What volume of 0.350 M CaF2 solution is required to obtain 0.00875 mole of CaF2?
How many moles of glucose are there in 255.0 mL of a 0.998 M solution of glucose?
What volume of 0.350 M BaCl2 solution is required to obtain 0.500 mole of BaCl2?
What volume of 0.350 M BaCl2 solution is required to obtain 0.500 mole of Cl–(aq)?
How would you prepare 9.70 g of PbCl2(s) from a 0.100 M solution of Pb(NO3)2 and a 0.200 M solution of CaCl2?
Suppose you did as required in Practice Problem 12.27 but, because of poor filtering technique, isolated only 8.24 g of PbCl2. What is the percent yield for your synthesis?Data from Problem 12.27How would you prepare 9.70 g of PbCl2(s) from a 0.100 M solution of Pb(NO3)2 and a 0.200 M solution of
How would you prepare 20.0 g of iron(III) hydroxide from a 0.250 M solution of Fe(NO3)3 and a 0.150 M solution of Ba(OH)2? How much product would you have isolated if your percent yield were 67.5%?
A 30.00-mL volume of aqueous sulfuric acid, H2SO4, is titrated using 0.200 M NaOH and an indicator that turns color only after all the sulfuric acid protons have reacted with OH– ions. The solution turns color when 48.32 mL of base has been added. What is the molar concentration of the sulfuric
A 50.00-mL volume of aqueous phosphoric acid, H3PO4, is titrated using 0.100 M NaOH and an indicator that turns color only after all the phosphoric acid protons have reacted with OH– ions. The solution turns color when 38.60 mL of base has been added. What is the molar concentration of the
A 1.65-g sample of an acid that has one acidic proton per molecule is dissolved in water to give 25.00 mL of solution. It takes 27.48 mL of 1.000 M NaOH to neutralize the acid.(a) What is the molar concentration of the acid?(b) What is the molar mass of the acid?(c) The empirical formula of the
Automotive antifreeze is essentially the compound ethylene glycol, C2H6O2, molar mass 62.07 g/mol. Suppose you fill your car radiator with 6.00 L of water and then add 4.00 kg of ethylene glycol. At what temperature will this mixture freeze? (The density of water is 1.00 g/mL.)
A white powder is analyzed via combustion analysis. Results indicate its empirical formula is CH2O. To determine its molecular formula, a chemist dissolves 117.5 g into 1.175 kg of water, and the resulting solution freezes at –1.03°C. What is the molecular formula?
A solution is prepared at sea level (external pressure = 1 atm) by dissolving 100.0 g of calcium nitrate in 450.0 g of water. At what temperature will this solution have a vapor pressure of 760 mm Hg?
A student dissolves 45.0 g of an unknown solid in 225.0 g of cyclohexane. It is known to dissolve without dissociating. She cools the solution and finds that the temperature remains at 2.70 °C while the solution changes phase from liquid to solid. What is the molar mass of the solid?
Suppose you mixed a small amount of table sugar with a large amount of flour and then spent hours grinding the mixture to a very fine powder. Is this mixture a solution? Explain.
Both a soft drink and the atmosphere we breathe are properly called solutions. For each, state why this is true, and also state the solvent for each.
Suppose there is a dust storm due to the winds blowing dry soil into the air. Would a sample of this dusty atmosphere be a mixture? Would it be a solution? Explain.
Vinegar is a common household solution that we consume. What is the solvent and what is the solute in vinegar?
Classify the following as solutions or heterogeneous mixtures:(a) 14 karat gold (prepared by mixing 10 parts molten copper with 14 parts molten gold and then allowing the substance to cool until it solidifies)(b) Filtered ocean water(c) A piece of wood(d) Your exhaled breath(e) A bottle of salad
Suppose you had a 50:50 homogeneous mixture of oxygen gas in helium gas. Which would you call the solvent and which would you call the solute?
Is there anything wrong with the following diagram? Explain your answer. Η. H
A solution of table salt and table sugar in water is allowed to evaporate, leaving behind the two solid solutes. Is what remains a solution or a heterogeneous mixture? Explain your answer.
What evidence is there in your everyday experience to indicate that intermolecular attractive forces must exist between water molecules?
If there were no attractive forces between water molecules, what phase or phases of water would you expect to be prevalent at room temperature? Explain your answer.
In what way is melting a piece of NaCl similar to dissolving it in water?
Why does it take such a high temperature to melt NaCl but a much lower temperature to dissolve it in water?
When an ionic substance such as NaCl dissolves, the crystal lattice has to break apart to release the individual ions into the solution. Does this part of the dissolving process absorb energy or release energy? Explain your answer.
In dissolving any solute, room must be made in the solvent to accommodate solute particles. Does making this room absorb energy or release energy? Explain why.
Consider the process known as hydration during aqueous solution formation.(a) What is hydration?(b) Does it release or absorb energy? Explain.
Anhydrous calcium sulfate [CaSO4]; anhydrous means without any water in its lattice, will absorb water (will hydrate) to give calcium sulfate hydrate. The water molecules end up in “holes” or spaces in the ionic lattice. This process releases a considerable amount of energy in the form of
List the three steps that occur as NaCl dissolves in water, and illustrate each with a diagram.
Solid sucrose consists of individual sucrose molecules fixed in a lattice. The molecules are hydrogen-bonded to one another via OH groups. Knowing this, comment on which takes more energy—breaking up an NaCl lattice or breaking up a sucrose lattice. Justify your answer.
When NaCl dissolves, what helps keep the dissolved Na+ and Cl– ions from coming back together and reforming the lattice, precipitating the solid?
Some alcohols are quite soluble in water. For example, isopropyl alcohol, shown below, is sold as an aqueous solution we call rubbing alcohol. Show how a water molecule would be attracted to isopropyl alcohol, and name the strongest intermolecular force involved. Would you call this interaction
What is the name of the attractive force between dissolved Na+ ions and water molecules? Diagram this force, showing how a water molecule would approach an Na+ ion. Do the same for a Cl– ion.
Why is the amount of energy associated with the solvation step of the dissolving process so critical to whether or not a solute will dissolve?
Consider an ionic solid dissolving in a liquid. Suppose the energy released as solute–solvent interactions take place is substantially less than the energy required to break up the lattice and to make room in the solvent. Would the solid be very soluble in this liquid? Explain your answer fully.
Consider dissolving an ionic salt in roomtemperature water.(a) Some salts dissolve in water to yield a much warmed solution. How is this possible?(b) Some salts dissolve in water to yield a cold solution. How is this possible?
When solid sodium hydroxide NaOH(s) pellets are dissolved in water, the water can get extremely hot and almost boil to give NaOH(aq) solution. What is the source of this heat?
Suppose the hydration energy for an ionic compound is much less than the energy required to pull apart the lattice. Is such a compound likely to be soluble or insoluble in water? Explain your answer.
Sodium chloride is very soluble in water but insoluble in liquid hexane, C6H14. Why is this so?
Even though NaCl does not dissolve in hexane, C6H14, if we imagine the dissolving process for this system, there is one step that would take less energy than the corresponding step for NaCl dissolving in water. Which step is it? Why would it require less energy?
Which has the greater hydration energy, AlCl3 or NaCl? Explain your answer.
In theory, it is possible for one ionic compound to have a greater hydration energy than another and still be the less soluble of the two. What would have to be true for this to be so?
What is meant by the rule of thumb “like dissolves like”?
Consider the following diagram and answer the questions that follow:(a) Why does solute separation require energy?(b) Why does solvent separation require energy?(c) Why does solvation release energy?(d) On the basis of this diagram, would you expect the solute to be soluble or insoluble in the
What do we mean by the total energy change ΔEtotal for the dissolving process, and why is it important to know about this energy change?
When we write (aq) for a dissolved ion, such as Na+(aq), exactly what does it mean? Answer both in words and with a diagram.
Suppose you have two ionic compounds, A and B. The only significant difference between them is that the ionic bonds that hold the lattice together in compound A are stronger than those in compound B. Which compound would you expect to be more soluble in water? Explain your answer.
When a gaseous solute dissolves in water, which step in the dissolving process is essentially skipped? Explain why.
These three substances are all liquids at room temperature:Which do you expect to be least soluble in water? Most soluble in water? Explain your answers fully Cl HEH Η H CH₂Cl CI Cl B Cl CC14 Cl H 1000 H H H CH₂OH
When a liquid solute dissolves in water, there is still a solute-separation step that absorbs energy, but the step doesn’t require breaking up a crystal lattice as for a typical solid solute. What happens in this step with a liquid solute, and why does the step absorb energy?
Oil is insoluble in water. Which step in the threestep process for dissolving is responsible for this? Explain why this step is the problem.
The natural tendency for systems is to decrease in energy. What is the natural tendency for entropy?
What is the reason for your answer to the previous problem? Make sure your answer uses the word probable.
When you release a drop of blue food dye into a beaker of water, the drop eventually dissolves to give a homogeneous light-blue solution. No matter how long you wait, the dye molecules will never regroup to form the original drop. Why not?
In terms of total energy change, when is entropy an important factor in determining whether or not a solute dissolves in a solvent? When is it not an important factor?
True or false? Whenever something spontaneously dissolves in water, the entropy has increased. Justify your answer.
Certainly if NaCl dissolved in liquid hexane, C6H14, the entropy associated with the Na+ and Cl– ions would increase. Nevertheless, NaCl does not dissolve in hexane. Why not?
If the natural tendency of systems is more towards states of increased probability, then what do you predict for the ultimate fate of the universe?
How does increasing temperature affect the solubility in water (a) Of most solids (b) Of gases?
What effect does increasing pressure have on the solubility of gaseous solutes? Explain your answer.
How is the medical condition known as the bends related to solubility?
Examine the bottom graph on page 462 showing solubility in water as a function of temperature. What is the trend for most of the ionic substances shown?Data from Graph page 462 Solubility, g/100.0 g of water 140 120 100 80 60 40 20 NH₂NO3 10 Glucose NaNO3 NHẠC CH₂CO₂Na Ce₂(SO4)3, 20 30 40
One ionic compound in the bottom graph on page 462 shows almost no temperature dependence, and one clearly violates the general trend. Identify these two ionic compounds.Data from Graph page 462 Solubility, g/100.0 g of

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