Question: You mix 100.0 mL of 0.

> Calculate how many grams of solute and solvent are needed to prepare the following solutions. a. 525 g of 3.91% iron(III) chloride solution b. 225 g of 11.9% sucrose solution c. 1.45 kg of 12.5% sodium chloride solution d. 635 g of 15.1% potassium nit

> Write the equilibrium expression for each of the following reactions. a. NO2( g) + ClNO( g) ⇌ ClNO2( g) + NO( g) b. Br2( g) + 5F2( g) ⇌ 2BrF5( g) c. 4NH3( g) + 6NO( g) ⇌ 5N2( g) + 6H2O( g)

> Write the equilibrium expression for each of the following reactions. a. N2( g) + 3Cl2( g) ⇌ 2NCl3( g) b. H2( g) + I2( g) ⇌ 2HI( g) c. N2( g) + 2H2( g) ⇌ N2H4( g)

> Write the equilibrium expression for each of the following reactions. a. C2H6( g) + Cl2( g) ⇌ C2H5Cl(s) + HCl( g) b. 4NH3( g) + 5O2( g) ⇌ 4NO( g) + 6H2O( g) c. PCl5( g) ⇌ PCl3( g) + Cl2( g)

> Consider the following exothermic reaction at equilibrium: N2(g)+ 3H2(g) ⇌ 2NH3(g) Predict how the following changes affect the number of moles of each component of the system after equilibrium is reestablished by completing the tabl

> For the following endothermic reaction at equilibrium: 2SO3(g) ⇌ 2SO2(g) + O2(g) which of the following changes will increase the value of K? a. increasing the temperature b. decreasing the temperature c. removing SO3( g) (constant T) d. decreasi

> For the reaction: H2(g) + F2(g) ⇌ 2HF(g) K = 2.1 * 10-3 at a certain temperature. At equilibrium, [H2] = [F2] = 0.083 M. What is the concentration of HF under these conditions?

> The reaction H2(g) + I2(g) ⇌ 2HI(g) has Kp = 45.9 at 763 K. A particular equilibrium mixture at 763 K contains HI at a pressure of 4.94 atm and H2 at a pressure of 0.628 atm. Calculate the equilibrium pressure of I2( g) in this mixture.

> For the reaction: 3O2(g) ⇌ 2O3(g) K = 1.8 * 10-7 at a certain temperature. If at equilibrium [O2] = 0.062 M, calculate the equilibrium O3 concentration.

> Suppose that for a hypothetical reaction: A2(g) + 2B(g) ⇌ 2AB(g) It is determined that at a certain temperature the equilibrium concentrations are: [A2] = 0.0090, [B] = 0.940, and [AB] = 5.3 * 10-4. Calculate the numerical value of K for the reaction.

> At a particular temperature, a 3.50-L flask contains 1.16 moles of NH3, 2.40 moles of H2, and 1.14 moles of N2 in equilibrium. Calculate the value of K for the reaction 3H2(g) + N2(g) ⇌ 2NH3(g)

> What does it mean to say that an acid is strong in aqueous solution? What does this reveal about the ability of the acid’s anion to attract protons?

> For the reaction 2CO2( g) ⇌ 2CO( g) + O2( g) an analysis of an equilibrium mixture is performed. At a particular temperature, it is found that [CO] = 0.11 M, [O2] = 0.055 M, and [CO2] = 1.4 M. Calculate K for the reaction.

> Ammonia, a very important industrial chemical, is produced by the direct combination of the elements under carefully controlled conditions. N2(g) + 3H2(g) ⇌ 2NH3(g) Suppose, in an experiment, that the reaction mixture is analyzed after equilibrium is re

> When a reaction system has reached chemical equilibrium, the concentrations of the reactants and products no longer change with time. Why does the amount of product no longer increase, even though large concentrations of the reactants may still be pres e

> What are the catalysts in living cells called? Why are these biological catalysts necessary?

> What does the activation energy for a reaction represent? How is the activation energy related to whether a collision between molecules is successful?

> For the reaction N2( g) + 3H2( g) 2NH3( g), list the types of bonds that must be broken and the type of bonds that must form for the chemical reaction to take place.

> Mercuric sulfide, HgS, is one of the least soluble salts known, with Ksp = 1.6 * 10-54 at 25 °C. Calculate the solubility of HgS in moles per liter and in grams per liter.

> Approximately 9.0 * 10-4 g of silver chloride, AgCl(s), dissolves per liter of water at 10 °C. Calculate Ksp for AgCl(s) at this temperature.

> As you learned in Chapter 7, most metal hydroxides are sparingly soluble in water. Write balanced chemical equations describing the dissolving of the following metal hydroxides in water. Write the expression for Ksp for each process. a. Cu(OH)2(s) b. C

> The equilibrium constant for the reaction 2NOCl(g) ⇌ 2NO(g) + Cl2(g) has the value 9.2 * 10-6 at a particular temperature. The system is analyzed at equilibrium, and it is found that the concentrations of NOCl( g) and NO( g) are 0.44 M and 1.5 * 10-3 M

> Calculate the percent by mass of solute in each of the following solutions. a. 6.11 mg of calcium chloride dissolved in 5.25 g of water b. 6.11 mg of calcium chloride dissolved in 52.5 g of water c. 6.11 g of calcium chloride dissolved in 52.5 g of wa

> For the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) K = 1.3 * 10-2 at a given temperature. If the system at equilibrium is analyzed and the concentrations of both N2 and H2 are found to be 0.10 M, what is the concentration of NH3 in the system?

> For the process CO(g) + H2O(g) ⇌ CO2(g) + H2(g) it is found that the equilibrium concentrations at a particular temperature are [H2] = 1.4 M, [CO2] = 1.3 M, [CO] = 0.71 M, and [H2O] = 0.66 M. Calculate the equilibrium constant K for the reaction under

> The reaction PCl3(l) + Cl2(g) ⇌ PCl5(s) liberates 124 kJ of energy per mole of PCl3 reacted. Will an increase in temperature shift the equilibrium position toward products or toward reactants?

> Suppose the reaction system 2NO(g) + O2(g) ⇌ 2NO2(g) has already reached equilibrium. Predict the effect of each of the following changes on the position of the equilibrium. Tell whether the equilibrium will shift to the right, will shift to the left, o

> Write the equilibrium expression for each of the following heterogeneous equilibria. a. P4(s) + 5O2( g) ⇌ P4O10(s) b. CO2( g) + 2NaOH(s) ⇌ Na2CO3(s) + H2O( g) c. NH4NO3(s) ⇌ N2O( g) + 2H2O( g)

> Write the equilibrium expression for each of the following heterogeneous equilibria. a. 4Al(s) + 3O2( g) ⇌ 2Al2O3(s) b. NH3( g) + HCl( g) ⇌ NH4Cl(s) c. 2Mg(s) + O2( g) ⇌ 2MgO(s)

> Calculate the pH corresponding to each of the pOH values listed, and indicate whether each solution is acidic, basic, or neutral. a. pOH = 4.32 b. pOH = 8.90 c. pOH = 1.81 d. pOH = 13.1

> Of the following combinations, which would act as buffered solutions? a. HClO2 and KClO2 b. H2S and Na2S c. HCOOH and NaHCO d. HClO and HClO4

> In each of the following chemical equations, identify the conjugate acid–base pairs. a. HF(aq) + H2O(l) ⇌ F-(aq) 1 H3O+(aq) b. CN-(aq) + H2O(l) ⇌ HCN(aq) + OH-(aq) c. HCO3-(aq) + H2O(l) ⇌ H2CO3(aq) + OH-(aq)

> A(n) solution contains a conjugate acid–base pair and through this is able to resist changes in its pH.

> Calculate the percent by mass of solute in each of the following solutions. a. 2.14 g of potassium chloride dissolved in 12.5 g of water b. 2.14 g of potassium chloride dissolved in 25.0 g of water c. 2.14 g of potassium chloride dissolved in 37.5 g o

> A 0.20 M HCl solution contains M hydrogen ion and M chloride ion concentrations.

> A solution with pH = 9 has a (higher/lower) hydrogen ion concentration than a solution with pOH = 9.

> The number of in the logarithm of a number is equal to the number of significant figures in the number.

> Because of , even pure water contains measurable quantities of H+ and OH-.

> Draw the structure of the carboxyl group, -COOH. Show how a molecule containing the carboxyl group behaves as an acid when dissolved in water.

> Acetate ion, C2H3O2-, has a stronger affinity for protons than does water. Therefore, when dissolved in water, acetate ion behaves as a(n) .

> When organic compounds containing sulfur are burned, sulfur dioxide is produced. The amount of SO2 formed can be determined by the reaction with hydrogen peroxide: H2O2(aq) + SO2(g) H2SO4(aq) The resulting sulfuric acid is then

> A 50.00-mL sample of aqueous Ca(OH)2 requires 34.66 mL of a 0.944 M nitric acid for neutralization. Calculate the concentration (molarity) of the original solution of calcium hydroxide.

> A 450.0-mL sample of a 0.257 M solution of silver nitrate is mixed with 400.0 mL of 0.200 M calcium chloride. What is the concentration of Cl- in solution after the reaction is complete?

> A 500.0-mL sample of 0.200 M sodium phosphate is mixed with 400.0 mL of 0.289 M barium chloride. What is the mass of the solid produced?

> There is only one value of the equilibrium constant for a particular system at a particular temperature, but there are an infinite number of equilibrium positions. Explain.

> What volume of 0.100 M NaOH is required to precipitate all of the nickel(II) ions from 150.0 mL of a 0.249 M solution of Ni(NO3)2?

> A solution is prepared by dissolving 0.6706 g of oxalic acid (H2C2O4) in enough water to make 100.0 mL of solution. A 10.00-mL aliquot (portion) of this solution is then diluted to a final volume of 250.0 mL. What is the final molarity of the oxalic acid

> Consider the following generic reaction: 2A2B( g) ⇌ 2A2( g) + B2( g) Some molecules of A2B are placed in a 1.0-L container. As time passes, several snapshots of the reaction mixture are taken as illustrated below. Which illustration i

> Consider the reaction between 0.156 L of 0.105 M magnesium nitrate and 0.166 L of 0.106 M potassium hydroxide. a. What mass of precipitate will form? b. What is the concentration of nitrate ions left in solution after the reaction is complete?

> Explain why the development of a vapor pressure above a liquid in a closed container represents an equilibrium. What are the opposing processes? How do we recognize when the system has reached a state of equilibrium?

> How many milliliters of 0.105 M NaOH are required to neutralize exactly 14.2 mL of 0.141 M H3PO4?

> Teeth and bones are composed, to a first approximation, of calcium phosphate, Ca3(PO4)2(s). The Ksp for this salt is 1.3 * 10-32 at 25 °C. Calculate the concentration of calcium ion in a saturated solution of Ca3(PO4)2.

> As you know from Chapter 7, most metal carbonate salts are sparingly soluble in water. Below are listed several metal carbonates along with their solubility products, Ksp. For each salt, write the equation showing the ionization of the salt in water, and

> For each of the following solutions, the mass of solute taken is indicated, as well as the total volume of solution prepared. Calculate the normality of each solution. a. 15.0 g of HCl; 500. mL b. 49.0 g of H2SO4; 250. mL c. 10.0 g of H3PO4; 100. mL

> In general terms, what does the equilibrium constant for a reaction represent? What is the algebraic form of the equilibrium constant for a typical reaction? What do square brackets indicate when we write an equilibrium constant?

> What volume of 0.250 M HCl is required to neutralize each of the following solutions? a. 25.0 mL of 0.103 M sodium hydroxide, NaOH b. 50.0 mL of 0.00501 M calcium hydroxide, Ca(OH)2 c. 20.0 mL of 0.226 M ammonia, NH3 d. 15.0 mL of 0.0991 M potassium

> Suppose K = 4.5 * 10-3 at a certain temperature for the reaction PCl5(g) ⇌ PCl3(g) + Cl2(g) If it is found that the concentration of PCl5 is twice the concentration of PCl3, what must be the concentration of Cl2 under these conditions?

> For a given reaction at a given temperature, the special ratio of products to reactants defined by the equilibrium constant is always equal to the same number. Explain why this is true, no matter what initial concentrations of reactants (or products) may

> An aqueous solution of ammonium sulfide is mixed with an aqueous solution of iron(III) chloride. a. Write a balanced molecular equation, complete ionic equation, and net ionic equation for the two solutions mixed above. Include all phases. b. If 50.0 m

> Consider the following reaction at some temperature: H2O( g) + CO( g) ⇌ H2( g) + CO2( g) K = 2.0 Some molecules of H2O and CO are placed in a 1.0-L container as shown below. When equilibrium is reached, how many molecules

> Consider the reaction between 1.0 L of 3.0 M AgNO3(aq) and 1.0 L of 1.0 M CuCl2(aq), according to the equation: 2AgNO3(aq) + CuCl2(aq) ( 2AgCl(s) + Cu(NO3)2(aq) Which of the following will increase the amount of AgCl(s) produced? a. Adding another 1.0

> The solubility product of iron(III) hydroxide is very small: Ksp = 4 * 10-38 at 25 °C. A classical method of analysis for unknown samples containing iron is to add NaOH or NH3. This precipitates Fe(OH)3, which can then be filtered and weighed. To demonst

> Calculate the new molarity when 150. mL of water is added to each of the following solutions. a. 125 mL of 0.200 M HBr b. 155 mL of 0.250 M Ca(C2H3O2)2 c. 0.500 L of 0.250 M H3PO4 d. 15 mL of 18.0 M H2SO4

> Mercury(I) chloride, Hg2Cl2, was formerly administered orally as a purgative. Although we usually think of mercury compounds as highly toxic, the Ksp of mercury(I) chloride is small enough (1.3 * 10-18) that the amount of mercury that dissolves and enter

> Calculate the number of moles of each ion present in each of the following solutions. a. 1.25 L of 0.250 M Na3PO4 solution b. 3.5 mL of 6.0 M H2SO4 solution c. 25 mL of 0.15 M AlCl3 solution d. 1.50 L of 1.25 M BaCl2 solution

> Consider an initial mixture of N2 and H2 gases that can be represented as follows: The gases react to form ammonia gas (NH3) as represented by the following concentration profile: a. Label each plot on the graph as N2, H2, or NH3, and explain your answ

> Suppose a reaction has the equilibrium constant K = 4.5 * 10-6 at a particular temperature. If an experiment is set up with this reaction, will there be large relative concentrations of products present at equilibrium? Is this reaction useful as a means

> How many moles and how many grams of the indicated solute does each of the following solutions contain? a. 4.25 L of 0.105 M KCl solution b. 15.1 mL of 0.225 M NaNO3 solution c. 25 mL of 3.0 M HCl d. 100. mL of 0.505 M H2SO4

> Lead(II) chloride, PbCl2(s), dissolves in water to the extent of approximately 3.6 * 10-2 M at 20 °C. Calculate Ksp for PbCl2(s), and calculate its solubility in grams per liter.

> When 200.0 mL of 0.10 M Zn(NO3)2 is mixed with 100.0 mL of 0.10 M KOH, a precipitate forms. a. How many moles of precipitate can form in this reaction? b. Calculate the concentration of Zn2+ ions in the final solution after precipitate formation is com

> Magnesium fluoride dissolves in water to the extent of 8.0 * 10-2 g/L at 25 °C. Calculate the solubility of MgF2(s) in moles per liter, and calculate Ksp for MgF2 at 25 °C.

> You are given 1.00 gram of each of five substances. In which of the substances will there be the greatest number of potassium ions when dissolved in water? a. potassium chloride b. potassium chlorate c. potassium phosphate d. potassium nitrate e. po

> For each of the following solutions, the mass of the solute is given, followed by the total volume of solution prepared. Calculate the molarity. a. 5.0 g of BaCl2; 2.5 L b. 3.5 g of KBr; 75 mL c. 21.5 g of Na2CO3; 175 mL d. 55 g of CaCl2; 1.2 L

> Approximately 0.14 g of nickel(II) hydroxide, Ni(OH)2(s), dissolves per liter of water at 20 °C. Calculate Ksp for Ni(OH)2(s) at this temperature.

> Chromium(III) hydroxide dissolves in water only to the extent of 8.21 * 10-5 M at 25 °C. Calculate Ksp for Cr(OH)3 at this temperature.

> Approximately 1.5 * 10-3 g of iron(II) hydroxide, Fe(OH)2(s), dissolves per liter of water at 18 °C. Calculate Ksp for Fe(OH)2(s) at this temperature.

> What does it mean to say that a state of chemical or physical equilibrium is dynamic?

> The three common silver halides (AgCl, AgBr, and AgI) are all sparingly soluble salts. Given the values for Ksp for these salts below, calculate the concentration of silver ion, in mol/L, in a saturated solution of each salt. Silver Halide……….Ksp AgCl……

> Consider 0.25 M solutions of the following salts: NaCl, RbOCl, KI, Ba(ClO4)2, and NH4NO3. For each salt, indicate whether the solution is acidic, basic, or neutral.

> Write the formulas for three combinations of weak acid and salt that would act as buffered solutions. For each of your combinations, write chemical equations showing how the components of the buffered solution would consume added acid and base.

> Calculate the hydrogen ion concentration, in moles per liter, for solutions with each of the following pH or pOH values. a. pH = 5.41 b. pOH = 12.04 c. pH = 11.91 d. pOH = 3.89

> A 15.0% (by mass) NaCl solution is available. Determine what mass of the solution should be taken to obtain the following quantities of NaCl. a. 10.0 g b. 25.0 g c. 100.0 g d. 1.00 lb

> Calculate the hydrogen ion concentration and the pH of each of the following solutions of strong acids. a. 1.4 * 10-3 M HClO4 b. 3.0 * 10-5 M HCl c. 5.0 * 10-2 M HNO3 d. 0.0010 M HCl

> Calculate the hydrogen ion concentration, in moles per liter, for solutions with each of the following pH or pOH values. a. pOH = 0.90 b. pH = 0.90 c. pOH = 10.3 d. pH = 5.33

> You mix 225.0 mL of a 2.5 M HCl solution with 150.0 mL of a 0.75 M HCl solution. What is the molarity of the final solution?

> Calculate [OH-] in each of the following solutions, and indicate whether the solution is acidic, basic, or neutral. a. [H+] = 4.21 * 10-7 M b. [H+] = 0.00035 M c. [H+] = 0.00000010 M d. [H+] = 9.9 * 10-6 M

> For each hydrogen or hydroxide ion concentration listed, calculate the concentration of the complementary ion and the pH and pOH of the solution. a. [H+] = 5.72 * 10-4 M b. [OH-] = 8.91 * 10-5 M c. [H+] = 2.87 * 10-12 M d. [OH-] = 7.22 * 10-8 M

> How do chemists recognize a system that has reached a state of chemical equilibrium? When writing chemical equations, how do we indicate reactions that come to a state of chemical equilibrium?

> What are some physical properties that historically led chemists to classify various substances as acids and bases?

> A financial institution has the following portfolio of over-the-counter options on sterling: A traded option is available with a delta of 0.6, a gamma of 1.5, and a vega of 0.8. (a) What position in the traded option and in sterling would make the port

> A portfolio manager has maintained an actively managed portfolio with a beta of 0.2. During the last year, the risk-free rate was 5% and major equity indices performed very badly, providing returns of about −30%. The portfolio manager produced a return o

> A bank estimates that its profit next year is normally distributed with a mean of 0.8% of assets and the standard deviation of 2% of assets. How much equity (as a percentage of assets) does the company need to be (a) 99% sure that it will have a positiv

> Explain the moral hazard problems with deposit insurance. How can they be overcome?

> Consider a one-year European call option on a stock when the stock price is $30, the strike price is $30, the risk-free rate is 5%, and the volatility is 25% per annum. Use the RMFI software to calculate the price, delta, gamma, vega, theta, and rho of t

> Suppose that one investment has a mean return of 8% and a standard deviation of return of 14%. Another investment has a mean return of 12% and a standard deviation of return of 20%. The correlation between the returns is 0.3. Produce a chart similar to F

> Suppose that a one-day 97.5% VaR is estimated as $13 million from 2,000 observations. The one-day changes are approximately normal with mean zero and standard deviation $6 million. Estimate a 99% confidence interval for the VaR estimate.

> Suppose that each of two investments has a 4% chance of a loss of $10 million, a 2% chance of a loss of $1 million, and a 94% chance of a profit of $1 million. They are independent of each other. (a) What is the VaR for one of the investments when the co

> With the benefit of hindsight, we can say that Kodak was in the “imaging and moment-sharing business.” What business are banks in?

> Look at the data in Table 28.1. Is Lending Club good at assessing risk? Is there a reasonable trade-off between risk and return for lenders? What risks are lenders taking?

> What is meant by a bubble? Consider whether the increase in the price of bitcoin in 2017 is a bubble.