MC Practice F2 Solubility Equilibrium, Ksp Name
|
|
- Juliet O’Connor’
- 6 years ago
- Views:
Transcription
1 MC Pratie F Solubility Equilibrium, Ksp Name This is pratie - Do NOT heat yourself of finding out what you are apable of doing. Be sure you follow the testing onditions outlined below. DO NOT USE A CALCULATOR. You may use ONLY the periodi table and formula sheets. Try to finish at a rate of about 1.5 min per question. Time yourself. It is important that you pratie working for speed. Please mail me if you think you find any issues or typos. 1. Temperature is often given with Ksp values beause a. the solubility of solids always inreases with inreasing temperature. b. the solubility of solids varies with temperature hanges.. solubility hanges with temperature but Ksp values do not. d. Ksp varies with temperature even though onentrations do not. e. the number of ions varies with the kind of salt that is dissolving. 5. Determine the solubility of lead(ii) fluoride, Ksp , in a M lead(ii) nitrate solution. a M b M.! d. e.! M M M. The Ksp expression for silver phosphate is a.! K sp [Ag + [PO 4 b.! K sp [Ag + [PO 4. d.! K sp [Ag + [PO 4 e.!. The solubility of nikel(ii) hydroxide, Ksp , is about a. b.!.! d.! e.! K sp [Ag + [PO 4 K sp [Ag+ [PO 4 [Ag PO ( )() ( )(4) 6. The solubility of silver sulfide is M. Determine the Ksp of this salt. a b. [ [ [ ) [ d. [ [ e. [ ) [ Equal volumes of M KCl and M AgNO are mixed. the Ksp for silver hloride is As these two solutions are ombined, a. a preipitate of AgCl forms. b. there is no preipitate formed.. NaCl will preipitate. d. AgNO will preipitate. e. the [Na + will beome 0.00 M 4. What is the molar solubility in water of PbI? (The Ksp for PbI is ) a M b M. (1.6) ½ 10 8 M d. (1.6) ⅓ 10 8 M e. 10 M 8. The solubility of metal(ii) sulfide, Ksp , is about a. b.!.! d.! e.!
2 Pratie MC Unit F Solubility Equilibrium Ksp (page of ) 9. Calulate the ph of a saturated metal hydroxide, XOH, whose Ksp a. 4.0 b d. 8.0 e Magnesium hydroxide, Mg(OH), has a Ksp The solubility of Mg(OH) will be the lowest in 1.0 L of whih of the following? a M HCl b M NaOH M MgCl d. pure HO 10. Calulate the Ksp of a saturated metal hydroxide, X(OH), solution whose ph a b d e On the basis of the Ksp values listed below, what is the order of least soluble to most soluble for these ompounds? AgBr, Ksp AgCO, Ksp AgCl, Ksp a. AgBr < AgCO <AgCl b. AgBr <AgCl < AgCO. AgCl < AgCO <AgBr d. AgCO < AgBr <AgCl Use the following information to answer the next questions 150 ml of saturated SrF solution is present in a 50 ml beaker at room temperature. The molar solubility of SrF at 5ºC is 1 10 M 14. What are the onentrations of Sr + and F in the beaker? a. [Sr M, [F M b. [Sr M, [F.0 10 M. [Sr M, [F M d. [Sr M, [F.0 10 M 15. If some of the solution evaporates overnight, whih of the following will our? a. The mass of the solid and onentration of the ions will stay the same. b. The mass of the solid and onentration of the ions will stay the inrease.. The mass of the solid will derease, and onentration of the ions will stay the same. d. The mass of the solid will inrease, and onentration of the ions will stay the same. 1. On the basis of the solubilities (in mol/l) listed below, what is the orret order of dereasing Ksp values (largest first). AgBr AgCN AgSCN a. AgBr > AgCN > AgSCN b. AgCN > AgBr > AgSCN. AgCN > AgSCN > AgBr d. AgSCN > AgBr > AgCN 16. How ould the onentration of Sr + ions in solution be dereased? a. Adding some NaF(s) to the beaker. b. Adding some Sr(NO)(s) to the beaker.. By heating the solution in the beaker. d. By adding a small amount of water to the beaker, but not dissolving all of the solid.
3 Pratie MC Unit F more pratie General Equilbrium Kp and K (page of ) 17. HI(g) + Cl(g) HCl(g) + I(g) + energy A gaseous reation ours and omes to equilibrium as shown above. Whih of the following hanges to the system will serve to inrease the number of moles of I present at equilibrium? a. Inreasing the volume at onstant temperature. b. Dereasing the volume at onstant temperature.. Adding a mole of inert gas at onstant volume. d. Inreasing the temperature at onstant volume. e. Dereasing the temperature at onstant volume. 0. An evauated 1.00-liter vessel is injeted with 1. moles of sulfur trioxide gas, SO. The vessel is then heated to a high temperature where the SO partially deomposes to form the produts SO and O in the reation shown below: SO(g) SO(g) + O(g) The temperature is kept onstant, and the amount of SO in the vessel at equilibrium is 0.40 mol. What is the value of K at this temperature? a b d. 1.0 e In the reation shown below, 0.0 mole of Br and 0.0 moles of I are plaed in an evauated 1.00 liter vessel and allowed to reah equilibrium. What is the value of K if the vessel ontains 0.40 moles of IBr at equilibrium? a. 1.0 b d. 16 e. 40 I(g) + Br(g) IBr(g) 19. Whih is the orret set up to determine K for the reation below? 4CuO(s) + CH4(g) CO(g) + 4Cu(s) + HO(g) a.! [CO [Cu 4 [H O [CuO 4 [CH 4! b. [CuO 4 [CH 4 [CO [Cu 4 [H O. [CO [H O [CH 4 d.! [CO [H O [CuO 4 [CH 4 e.! [CO [Cu 4 [H O [CuO 4 [CH 4 1. A sample of solid potassium nitrate is plaed in water. The solid potassium nitrate omes to equilibrium with its dissolved ions by the endothermi proess shown below. KNO(s) + energy K + (aq) + NO (aq) Whih of the following hanges to the system would inrease the onentration of K + ions at equilibrium? a. The volume of the solution is inreased. b. The volume of the solution is dereased.. Additional solid KNO is added to the solution. d. The temperature of the solution is inreased. e. The temperature of the solution is dereased. A.00-liter reation vessel is filled with arbon monoxide gas, CO, and hlorine gas, Cl. The mixture is heated to 670 K and allowed to reah equilibrium aording to the balaned equation shown below: CO(g) + Cl(g) COCl(g) At equilibrium, the mixture ontains 0. moles CO, 0.5 moles Cl, and 1.5 moles COCl. What is K at this temperature? a. 0.0 b. 1. d. 10 e. 0
4 Pratie MC Unit F Ksp and Kp and K (page 4 of 4). The reation below is allowed to ome to equilibrium at room temperature. At equilibrium, the partial pressure of HO is 96 mm Hg, ClO is 15 mm Hg, and HOCl is 0 mm Hg. What is the value of Kp at this temperature? a. b d e HO(g) + ClO(g) HOCl(g) 4. At 7 K, the reation shown below has an equilibrium onstant, K COCl(g) CO(g) + Cl(g) After plaing a mixture of gases in the reation vessel, the onentrations were measured to be [COCl M, [CO M, and [Cl M. Whih statement below aurately desribes the reation? a. The reation is at equilibrium b. The reation is not at equilibrium, and it is proeeding to the left. The reation is not at equilibrium, and it is proeeding to the right d. The reation quotient is equal to K e. The reation quotient is less than K 5. In the reation W + X Y + Z, all substanes are gases. The reation is initiated by adding equal number of moles of W and of X. When equilibrium is reahed, a. [Y [Z b. [X [Y. [W [X d. [X > [W e. [W + [X [Y + [Z 6. Consider the reations below, both at the same temperature: Rx I X Y K 1 x 10 8 Rx II Z Y K 1 x 10 5 a. I is times faster than II. b. I is 1000 times faster than II.. II is times faster than I. d. II is 1000 times faster than I. e. The size of K and the time required to reah equilibrium are not diretly related. 7. The reation H(g) + N(g) NH(g) is exothermi. Inreasing the temperature of this equilibrium system auses a. an inrease in [NH b. an inrease in [N. a derease in [H d. an inrease in K e. a derease in pressure at onstant volume 8. Consider N(g) + O(g) NO(g). The reation was initiated by adding 15.0 moles of NO to a 1.0-L flask. At equilibrium,.0 moles of oxygen are present in the 1.0-L flask. The value of K must be a. 0. b d. 9.0 e At a ertain temperature, the synthesis of ammonia gas from nitrogen and hydrogen gases, shown below, has a value for K of If [H [N 0.10 M and [NH 0.0 M N + H NH a. the reation would shift toward the ammonia b. the reation would shift toward the N and the H. the system is at equilibrium, therefore no shifting will our d. the reation will shift toward a new equilibrium position, but the diretion annot be determined from these data e. the equilibrium may shift but it is not possible to alulate Q without knowing the temperature 0. The equilibrium onstant, K, may be used to determine the K of other reations. I. When the equation is reversed the reiproal of the original K beomes the value of K for the new equation. II. When the equation is doubled the square root of the original K beomes the value for the new equation. III. When reations are added, the sum of the equilibrium onstants of eah reation added will the equilibrium onstant of the new equation. Of the above three statements, those whih are always true are a. I only b. II only. III only d. I and III e. I, II, and III
5 Pratie MC Unit F Ksp and Kp and K (page 5 of 5) 1. The equilibrium P4(g) + 6Cl(g) 4PCl(L) is established at 10 o C. The equilibrium onstant expression is a.! K [PCl [P 4 [Cl b.! K [PCl 4 [P 4 [Cl 6.! K [P [Cl 4 6 [PCl 4 1 d.! K [PCl 4 1 e.! K [P 4 [Cl 6. Ammonium hydrogen sulfide will deompose into ammonia gas and hydrogen sulfide gas when heated. Consider the equilibrium system NH4HS(s) NH(g) + HS(g) whih is developed from mole of NH4HS in a 100- L ylinder. At equilibrium the total pressure is found to be atm. Kp will be equal to a b d e. a value impossible to alulate from only these data. At a ertain temperature, it has been determined that K 8.0 for the reation below. If we also determine that the equilibrium mixture ontains 0.80 mole of HO(g), mole of CO(g), and mole of CO(g), in an 8.0-L flask, what must be the number of moles of H(g) at equilibrium? a mole b mole. 6.4 moles d. 8.0 moles e. 64 moles HO(g) + CO(g) CO(g) + H(g) 4. Whih of the following systems at equilibrium are not affeted by a hange in pressure aused by hanging the volume at onstant temperature? a. H(g) + Cl(g) HCl(g) b. H(g) + I(s) HI(g). N(g) + H(g) NH(g) 5. After the equilibrium represented below is established, some pure O(g) is injeted into the reation vessel at onstant temperature. After equilibrium is reestablished, whih of the following has a lower value ompared to its value at the original equilibrium? CO(g) CO(g) + O(g) a. Keq for the reation b. The total pressure in the reation vessel. The amount of CO(g) in the reation vessel d. The amount of O(g) in the reation vessel e. The amount of CO(g) in the reation vessel 6. Whih of the following hanges alone would ause a derease in the value of Keq for the reation represented below? SO(g) + O(g) SO(g) Exothermi a. Dereasing the temperature b. Inreasing the temperature. Dereasing the volume of the reation vessel d. Inreasing the volume of the reation vessel e. Adding a atalyst 7. In whih of the following systems would the number of moles of the substanes present at equilibrium NOT be shifted by a hange in the volume of the system at a onstant temperature? a. SO(g) + O(g) SO(g) b. N(g) + H(g) NH(g). NO(g) + SO(g) SO(g) + NO(g) d. NO4(g) NO(g) e. CO(g) + H(g) CH4(g) + HO(g) 8. For: N(g) + H(g) NH(g) + energy Some N and H are mixed in a ontainer at 00 o C, and the system reahes equilibrium aording to the equation above. Whih of the following auses an inrease in the number of moles of NH present at equilibrium? I. Dereasing the volume of the ontainer II. Raising the temperature III. Adding a mole of Ar gas at onstant volume a. I only b. II only. I and III only d. II and III only e. I, II, and III d. NH(g) N(g) + H(g) e. O(g) O(g)
6 Pratie MC Unit F Ksp and Kp and K ANSWERS (page 6 of 6) 1. b All K values always hange with varying temperature. Whether or not the equilibrium onstant is larger or smaller is a funtion of whether the reation is exothermi or endothermi. If the reation is exothermi K will be smaller value at higher temperatures, and a larger value for lower temperatures. The onverse is also true.. The formula for silver phosphate is AgPO4 whih leads to the reation AgPO4 Ag + + PO4. a The formula for nikel(ii) hydroxide is Ni(OH) whih leads to the reation Ni(OH) Ni + + OH and the resulting solubility expression is Ksp [Ni + [OH. Sine there are OH ions for every Ni + ion upon dissolving, we an identify Ni + as s and OH as s and substitute into the Ksp expression. Thus Ksp (s)(s) and Ksp 4s solve for s s without a alulator, we an t 4 4 really lean this up any further. Sine s onentration of the Ni +, the 1:1 stoihiometry the onentration of the Ni(OH) that atually dissolves, s would be the molar solubility. 4. e This problem is nearly the same as #, however, this time the numbers are simple enough to finish the solve. The formula for lead(ii) iodide is PbI whih leads to the reation PbI Pb + + I and the resulting solubility expression is Ksp [Pb + [I. Sine there are I ions for every Pb + ion upon dissolving, we an identify Pb + as s and I as s and substitute into the Ksp expression. 5. d This problem has a twist ompared to # s and 4 beause instead of dissolving the insoluble salt, lead (II) fluoride in water, it is being dissolved in a solution that already ontains some lead ions, lead(ii) nitrate. We all this type of problem a ommon ion problem, meaning the solution you are dissolving into already has an ion in it that is ommon to the salt that you are trying to dissolve. More information on this in your text on page 681. The formula for lead(ii) fluoride is PbF whih leads to the reation PbF Pb + + F and the resulting Ksp expression is Ksp [Pb + [F. Up till now we have substituted s and s into this equation, and solved for s whih will be the solubility. Sine you are given a onentration of the Pb + ion that is already dissolved in the water (and is muh larger, when onsidering signifiant figures, than any lead ions that would be added to it) whih you an insert diretly into the Ksp expression. Thus Ksp (0.004)[s Solve: 4s Sine s onentration of the Pb +, the 1:1 stoihiometry the onentration of the PbF that atually dissolves, this s would be the molar solubility. (If you needed a gram solubility, you would have to multiply by the molar mass of PbF.) 6. When you are told the solubility of some salt, you are being told the maximum amount of the ompound that dissolves to ahieve a saturated solution. For silver sulfide, AgS, the solubility of , this tells you the onentration of the AgS that dissolves, whih is equal to the sulfide ion that forms, and the silver ion is twie that due to the dissolving reation, AgS Ag + + S thus Ksp [Ag + [S. Substitute Thus Ksp (s)(s) and Ksp 4s solve for s s Sine s onentration of the Pb +, the 1:1 stoihiometry the onentration of the PbI that atually dissolves, this s would be the molar solubility. (If you needed a gram solubility, you would have to multiply by the molar mass of PbI.) K sp b In order to answer this question, you need to alulate Q and ompare it to Ksp. For this ombination, the possible preipitate is AgCl, thus the Ksp reation of interest is AgCl Ag + + Cl and Ksp [Ag + [Cl. The trik in this problem is to remember that when solutions ombine, the onentrations of the ions will be diluted beause there is more volume for the same number of moles. Sine equal volumes are ombined, eah onentration is halved. [Ag + [Cl , or , So Q [ [ whih results in Q or In effet, reation shifts to the right and no preipitate forms when Ksp > Q.
7 ! Pratie MC Unit F Ksp and Kp and K ANSWERS (page 7 of 7) 8. a The formula for metal(ii) sulfide is MS whih leads to the reation MS M + + S and the resulting Ksp expression is Ksp [M + [S and thus Ksp s Change Ksp to to make it easier without a alulator, and then solve for s whih will be the solubility. 9. e The formula for metal hydroxide, XOH leads to the reation XOH X + + OH and the resulting Ksp expression is Ksp [X + [OH and thus Ksp s Solve for s whih will be the solubility, s , and then take the poh log[oh 4, then 14-it to solve for ph b The formula for metal hydroxide is X(OH) whih leads to the reation M(OH) M + + OH and the resulting Ksp expression is Ksp [M + [OH. ph of 9 should be onverted to a poh 5, whih an be unlogged to [OH Due to the stoihiometry of the reation above, the [M Now insert the values bak into the Ksp formula. Ksp [ [ b It is tempting to just look at the Ksp and assume that the smallest Ksp means the lowest solubility, however, you must onsider the amount of ions that the salt dissoiates into. Sine the AgCO salt has ions, Ksp 4s, whereas for the other two salts, the Ksp s. Thus for AgBr s ~ , for AgCl s ~ , but for 4s , thus 10 1 ~ d There is no need to make this problem any harder than neessary. Sine all three salts are ion salts, alulating the Ksp will be a simple squaring of the solubility. Thus the dereasing order of the Ksp values will be in the same order as the solubility values. 1. b HCl will reat with the OH ion, lowering the OH, ausing a shift to the right resulting in greater solubility, thus not the answer. This problem requires you to pik out the substane with a ommon ion, and both NaOH and MgCl will satisfy that riteria. So there is a twist. Remember the solubility an be determined by solving for s from the equilibrium expression. K sp Mg + OH. For the introdution of 0.1 M MgCl, you an simply substitute the onentration of [Mg + into the equilibrium expression, and the equation to solve for s would look like this! Divide by 0.1 for, 0.1 s , onvert to , then divide by 4, to get ~ and square root to solve for s ~ For the introdution of 0.1 M Mg(OH), you an simply substitute the onentration of [OH into the equilibrium expression, and the equation to solve for s would look like this Square 0.1, then divide Ksp by s , and solve for s It should now be obvious that the squared effet of the onentration of the ommon ion [OH auses the NaOH to have the greater effet on solubility. 14. b Remember that solubility desribes the amount of the hemial that does dissolve. Sine SrF dissolves and dissoiates aording to the following equation, SrF Sr + + F the onentration of Sr + will be the same as the solubilty, and the onentration of F will be the solubility. 15. d When evaporation ours, only water will evaporate, the salt will stay in the solution. Sine there an NOT be a greater onentration in solution, that the saturation quantity, preipitation will have to our to maintain the saturation onentrations. 16. a Addition of NaF(s) provides the ommon ion [F,whih will serve to ause the equilibrium to shift left, thus reduing the [Sr +. Addition of Sr(NO)(s) would also ause a shift to the left, but the addition of the [Sr + ions will inrease [Sr +, and while the [F will shift below the original [F, the [Sr + will never be able to redue below the original [Sr + onentration before the addition of Sr(NO)(s). 17. e Changing the volume will NOT ause any shift in the equilibrium position sine Q will not hange due to the fat that the stoihiometry of the gas moleules is the same on both sides of the equation. Just as adding an inert gas will not Choies would all ause no shift. Choie d would ause a shift to the left. Thus e is the orret hoie.
8 ! Pratie MC Unit F Ksp and Kp and K ANSWERS (page 8 of 8) 18. d This is a lassi RICE box and then solve for K. It is true that the math of the K alulation is not so simple, yet the answers are quite spread, so approximations make it possible. So, noting that the ontainer is 1.0 L, plug in the known info in the problem (in blue) then alulate the rest of the items with stoihiometry.! [0.4M K to do the easy math revise this! you an [0.4 [0.1M [0.1M [0.1[0.1 whih will then lean up to! 0.16 whih is 16, hoose d 1 10 R I(g) + Br(g) IBr(g) I 0. M 0. M 0 C 0. M 0. M +0. M E 0.1 M 0.1 M 0.4 M 19. In this problem, it is important to remember that solids (nor liquids) should be inluded in the solubility expression. 0. e This is a lassi RICE box and then solve for K. So, noting that the ontainer is 1.0 L, plug in the known info in the problem (in bold) then alulate the rest of the items with stoihiometry. [0.8M [0.4M [0.8M [0.4M [0.4M [0.8M [0.8M [M [0.8M 1.6 [0.4M R SO(g) SO(g) + O(g) I 1. M 0 0 C 0.8 M +0.8 M +0.4 M E 0.4 M 0.8 M 0.4 M 1. d Inreasing the temperature of an endothermi proess will ause a shift toward produts, thus ausing more ions to go into solution.. e For this problem there is no reason to do a rie box sine you were given the equilibrium mole values. It is important to note that the ontainer is.0 L. I plugged in the moles and the volume diretly into the equilibrium expression for the equation CO(g) + Cl(g) COCl(g) K Yikes, the math looks to be a mess, and you don t have a [COCl [ 1.5 K [CO[Cl [ 0. [0.5 alulator, so look for fators that are easy to anel and end up with 0. d Again, for this problem there is no reason to do a rie box sine you were given the equilibrium pressure values. I plugged in the moles and the volume diretly into the equilibrium expression for the equation HO(g) + ClO(g) HOCl(g)! [HOCl This time the math isn t so bad.! [0 K whih approximates to! [400 drop some zeros [H O[ClO [15[96 [15[~ 00 and all it! [4 K whih is! whih is something just smaller than 1/10th or hoie d [4 [15[~ [45 4. b For this problem, you must plug into the equilibrium expression and solve for! Q [ [ you an do some [.5 10 estimating sine you probably will be omparing orders of magnitude. I anelled out the.5 and.5 to get Q [ [ Remember that 10 in the denominator is 10 in the numerator, thus [1 10 Q ( )( )(1 10 ) whih is Ksp < Q ( ) given in the problem, thus the equilibrium will shift left to redue the value of Q. 5. d Starting with only W and X, Y ould never be equal to Z due to the :1 stoihiometry. We do not have enough information to know where the equilibrium position will land, so we annot ompare X to Z. W ould not be equal to X beause of starting with equal quantities of them, and the :1 ratio between them, thus we an tell that X will be greater than W beause W reats x the rate of X. Choie e is ertainly not what equilibrium means. 6. e rate laws and rate k onstants gives us info about speed. Keq tells us nothing about speed of reation, only where the position ends up. 7. b Sine we know from the reation is exothermi, think of energy on the right side. Raising the temp of the system, and the reation will shift to use some of this inoming heat, that s left.
9 Pratie MC Unit F Ksp and Kp and K ANSWERS (page 9 of 9) 8. d It is a 1.0 L flask, so moles are equal to molarity. This is easy math ompared to those others.! 9. b Plug in values to solve for! [0. whih is! [0.04 Q Q whih is! Q [4 10 whih is 400 whih is greater than [0.1[0.1 [0.1[.001 [ the K given in the problem and thus the shift will be left. (Note: If you have trouble multiplying or squaring deimals, turn 0.0 into 10 1 whih is might be easier to ope with.) 0. a Only I is true. For II when the stoihiometry of a reation is hanged, the equilibrium onstant of the original equation should be raised to the power of the stoihiometry hange. For III, when reations are added, the produt of the equilibrium onstants of eah reation added will the equilibrium onstant of the new equation. 1. e Note that PCl in this problem is a liquid, so it should not be inluded in the equilibrium expression.. In this problem, take note that the reatant is a solid. The produt gases ome only from the solid reatant, thus the two produts must be present in equal quantities, this allows the total equilibrium pressure to be ut in half to get eah gases partial pressure, 0. atm for eah gas. Then you an square the partial pressures to solve for Kp. (0.)(0.). Plug into the K expression and solve for [H 8 [0.01[H, thus [H 0.8 and multiply by 8.0 L to get 6.4 moles. [0.01[ a You are looking for a reation in whih the number of moles of gases are the same on both sides. [9 [[ 5. e If oxygen is injeted at equilibrium, stress has been applied and the system must shift to restore equilibrium. Thus a shift toward reatants will our, whih will redue the quantity of arbon monoxide. 6. b Sine we know that the reation is exothermi, think of energy on the right side. Raising the temperature of the system, and the reation will shift to use some of this inoming heat, that s left, thus reduing the value of K, sine K is onstant only for one partiular temperature. 7. You are looking for a reation in whih the number of moles of gases are the same on both sides. (Note there was a typo in the original version of the test in hoie a 8. a Dereasing the volume of the ontainer will inrease the partial pressure of all the gases and ause the equilibrium to shift toward the produts where there are less gas moleules. Raising the temp would ause a shift left, and adding argon would have no effet on partial pressures (even though the total pressure is inreased), and thus would reate no shift at all.
Solubility Equilibrium, Ksp and more Name
MC Practice F.2 (Ch 15 & 17.4-6) This is practice - Do NOT cheat yourself of finding out what you are capable of doing. Be sure you follow the testing conditions outlined below. DO NOT USE A CALCULATOR.
More informationGeneral Equilibrium. What happens to cause a reaction to come to equilibrium?
General Equilibrium Chemial Equilibrium Most hemial reations that are enountered are reversible. In other words, they go fairly easily in either the forward or reverse diretions. The thing to remember
More informationChapter 14. The Concept of Equilibrium and the Equilibrium Constant. We have for the most part depicted reactions as going one way.
Chapter 14 The Conept of Equilibrium and the Equilibrium Constant In hapter 1 we dealt with Physial Equilibrium Physial Changes HO 2 (l) HO 2 (g) In hapter 14 we will learn about Chemial Equilibrium. We
More informationChapter 15: Chemical Equilibrium
Chapter 5: Chemial Equilibrium ahoot!. At eq, the rate of the forward reation is the rate of the reverse reation. equal to, slower than, faster than, the reverse of. Selet the statement that BEST desribes
More information2 How far? Equilibrium Answers
How far? Equilibrium Answers ratie: pages 37 39 1 Answer is D. Only a hange in temperature harges the value of the equilibrium onstant. Answer is D. [B] /[A] so [B] [A] or [B] [A] 1/ 3 Answer is B. Amounts
More informationSample Teaching Sequence (Hong Kong Secondary 4 6 Chemistry)
Revised (1 Sept 009 Sample Teahing Suene (Hong Kong Seondary 4 6 Chemistry Topi: Chemial Equilibrium Teahing Suene Content 1.1 Reversible reations Examples of reversible reation; forward reation; reverse
More informationAnswer: Easiest way to determine equilibrium concentrations is to set up a table as follows: 2 SO 2 + O 2 2 SO 3 initial conc change
Problem #1 6 mol of SO and 4 mol of O are plaed into a 1 L flask at temperature, T. The equilibrium onentration of SO is found to be 4 mol/l. Determine K. SO (g) + O (g) SO (g) K = [SO ] / [SO ] [O ] Answer:
More informationChapter 15 Chemical Equilibrium
Chapter 5 Chemial Equilibrium 5. The Conept of Equilibrium Figure: 3. from Chemistry by MMurray & Fey Figure 3.(a) NO 4( g) NO( g) olorless brown we start with reatant, N O 4, so the solution is olorless
More informationTest bank chapter (14)
Test bank hater (14) Choose the most orret answer 1. Whih is the orret equilibrium onstant exression for the following reation? Fe 2 O 3 (s) + 3H 2 (g) 2Fe(s) + 3H 2 O(g) a) K = [Fe 2 O 3 ] [H 2 ] 3 /[Fe]
More informationChapter 15 Equilibrium. Reversible Reactions & Equilibrium. Reversible Reactions & Equilibrium. Reversible Reactions & Equilibrium 5/27/2014
Amount of reatant/produt 5/7/01 quilibrium in Chemial Reations Lets look bak at our hypothetial reation from the kinetis hapter. A + B C Chapter 15 quilibrium [A] Why doesn t the onentration of A ever
More informationChapter 15 Equilibrium. Reversible Reactions & Equilibrium. Reversible Reactions & Equilibrium. Reversible Reactions & Equilibrium 2/3/2014
Amount of reatant/produt //01 quilibrium in Chemial Reations Lets look bak at our hypothetial reation from the kinetis hapter. A + B C Chapter 15 quilibrium [A] Why doesn t the onentration of A ever go
More informationPractice Test F.1 (pg 1 of 7) Unit F - General Equilibrium Kp and Kc Name Per
Practice Test F. (pg of 7) Unit F - General Equilibrium Kp and Kc Name Per This is practice - Do NOT cheat yourself of finding out what you are capable of doing. Be sure you follow the testing conditions
More informationREVIEW QUESTIONS Chapter 15
hemistry 10 ANSWER EY REVIEW QUESTIONS hapter 15 1. A mixture of 0.10 mol of NO, 0.050 mol of H and 0.10 mol of HO is plaed in a 1.0-L flask and allowed to reah equilibrium as shown below: NO (g) + H (g)
More informationWrite equilibrium law expressions from balanced chemical equations for heterogeneous and homogeneous systems. Include: mass action expression.
Equilibrium 1 UNIT 3: EQUILIBRIUM OUTCOMES All important vocabulary is in Italics and bold. Relate the concept of equilibrium to physical and chemical systems. Include: conditions necessary to achieve
More informationName period AP Unit 8: equilibrium
Name period AP Unit 8: equilibrium 1. What is equilibrium? Rate of the forward reaction equals the rate of the reverse reaction 2. How can you tell when equilibrium has been reached? The concentrations
More informationChapter 13, Chemical Equilibrium
Chapter 13, Chemial Equilibrium You may have gotten the impression that when 2 reatants mix, the ensuing rxn goes to ompletion. In other words, reatants are onverted ompletely to produts. We will now learn
More informationCHAPTER 16. Basic Concepts. Basic Concepts. The Equilibrium Constant. Reaction Quotient & Equilibrium Constant. Chemical Equilibrium
Proerties of an Equilibrium System CHAPTER 6 Chemial Equilibrium Equilibrium systems are DYNAMIC (in onstant motion) REVERSIBLE an be aroahed from either diretion Pink to blue Co(H O) 6 Cl ---> > Co(H
More informationEquilibrium HW Holt May 2017
Equilibrium HW Holt May 2017 Answer Key p. 595 (PP 1-3, SR 1-10), p. 604 (SR 1-6); p. 616 (PP 1&2); p. 618 (PP 1&2); p. 620 (PP 1&2, SR 1-7) pp. 622-624 (2-11, 14-16, 27, 29, 32, 33, 34, 37, 39, 40 (review
More informationChapter 17. Additional Aspects of Equilibrium
Chapter 17. Additional Aspects of Equilibrium Sample Exercise 17.1 (p. 726) What is the ph of a 0.30 M solution of acetic acid? Be sure to use a RICE table, even though you may not need it. (2.63) What
More information2. Failure to submit this paper in its entirety at the end of the examination may result in disqualification.
Memorial University of Newfoundland St. John s, Newfoundland and Labrador Chemistry 101 Intersession 007 Midterm Exam May 8 th, 007 Time: 0 Minutes Name: MUN #: Dr. Peter Warburton READ THE FOLLOWING CAREFULLY!
More informationChapter 19. Solubility and Simultaneous Equilibria p
Chapter 19 Solubility and Simultaneous Equilibria p. 832 857 Solubility Product ) The product of molar concentrations of the constituent ions, each raised ot the power of its stoichiometric coefficients
More information8. A piece of Mg(s) ribbon is held in a Bunsen burner flame and begins to burn according to the equation: 2Mg(s) + O2 (g) 2MgO(s).
1. Which event must always occur for a chemical reaction to take place? A) formation of a precipitate B) formation of a gas C) effective collisions between reacting particles D) addition of a catalyst
More informationCalculating equilibrium constants
Equilibrium Work Book Writing Equilibrium Constants Expressions 1. Write the equilibrium law (mass action expression) for each of the following reactions: a. SO 2 (g) + NO 2 (g) SO 3 (g) + NO(g) b. 2 C(s)
More informationSOLVED QUESTIONS 1 / 2. in a closed container at equilibrium. What would be the effect of addition of CaCO 3 on the equilibrium concentration of CO 2?
SOLVED QUESTIONS Multile Choie Questions. and are the veloity onstants of forward and bakward reations. The equilibrium onstant k of the reation is (A) (B) (C) (D). Whih of the following reations will
More informationName Chem 6 Section #
Equilibrium Constant and its Meaning 1. Write the expressions for K eq for the following reactions. a) CH 4 (g) + 2 H 2 S(g) CS 2 (g) + 4 H 2 (g) b) 2 N 2 O 5 (g) 4 NO 2 (g) + O 2 (g) c) 3 O 2 (g) 2 O
More informationUnit 3: Chemical Equilibrium Chemistry Write balanced chemical equations for each of the following. Pay close attention to the physical states!
Practice Questions Section. The Equilibrium Constant 1. Write balanced chemical equations for each of the following. Pay close attention to the physical states! Also - you must include the charge when
More informationA great video concept approach to each Big Idea may be found on BOZEMANSCIENCE at
Big Idea 6: Chemical Equilibrium Problem Set: / 25 pts DUE: Fri. 4/10 Big Idea 6: AP Chemistry is a rigorous course that requires students to use their analytical and problem solving skills as they apply
More informationChemical Equilibrium. A state of no net change in reactant & product concentrations. There is a lot of activity at the molecular level.
Chemical Equilibrium A state of no net change in reactant & product concentrations. BUT There is a lot of activity at the molecular level. 1 Kinetics Equilibrium For an elementary step in the mechanism:
More informationKinetics & Equilibrium. Le Châtelier's Principle. reaction rates. + Packet 9: Daily Assignment Sheet '19 Name: Per
Daily Assignment Sheet '19 Name: Per (check them off as you complete them) Due Date Assignment Thur 2/21 Do clock reaction lab Fri 2/22 Do Not Write In That Box Below Mon 2/25 Do WS 9.1 Tue 2/26 Do WS
More informationJanuary 03, Ch 13 SB equilibrium.notebook
Ch 13: Chemical Equilibrium exists when 2 opposing reactions occur simultaneously at the same rate (dynamic rather than static) Forward rate = reverse rate https://www.youtube.com/watch?v=wld_imyqagq The
More informationChemistry 40S Chemical Equilibrium (This unit has been adapted from
Chemistry 40S Chemical Equilibrium (This unit has been adapted from https://bblearn.merlin.mb.ca) Name: 1 2 Lesson 1: Defining Equilibrium Goals: Describe physical and chemical equilibrium. Describe the
More informationPart II SECTION I : One or more options correct Type
[1] JEE Advaned 2013/ Paper -2 Part II SECTION I : One or more options orret Type This setion ontains 8 multiple hoie questions. Eah question has four hoies (A), (B), (C) and (D), out of whih ONE or MORE
More informationFinal Exam: know your section, bring your ID!
Chapter 15: Equilibrium Part 1 Read: BLB 15.1 3 HW: BLB 15:13,14, 21 Supplemental 15:1 4 Know: Chemial Equilibrium Catalysts Equilibrium Constant Equilibrium onstant expression Homogeneous/Heterogeneous
More informationAP Chapter 14: Chemical Equilibrium & Ksp
AP Chapter 14: Chemical Equilibrium & Ksp Warm-Ups (Show your work for credit) Name Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. AP Chapter 14: Chemical Equilibrium & Ksp 2 Warm-Ups
More informationChemical Equilibrium
Chemical Equilibrium THE NATURE OF CHEMICAL EQUILIBRIUM Reversible Reactions In theory, every reaction can continue in two directions, forward and reverse Reversible reaction! chemical reaction in which
More informationEquilibrium Simulation
Equilibrium Simulation Imagine the two large beakers (2000 ml) are actually the same space...we have just separated them to help us keep track of reactants and products. Imagine the size of the transfer
More informationNotation 2, 8, 1 2, 8, 2 2, 8
Page 90 Atomi struture 2 1 a Contains 3 protons (1); and 4 neutrons (1) Page 90 Eletroni struture 2 a 2, 8 Type of reation Ionisation Nulear fission Nulear fusion Change in mass of nuleus Stays the same
More informationModule 4 Lesson 2 Exercises Answer Key squared square root
Module Lesson Eerises Answer Key 1. The volume is 1 L so onentrations an be done by inspetion. Just substitute values and solve for K [ CO][ HO] K CO H (0.8)(0.8) (0.55) (0.55) K 0.659. [CH ][HS] K [H
More information"No matter what costume you wear, when you start eating Halloween candy, you will be a goblin. - Unknown
CHEMISTRY 101 Hour Exam II October 31, 2017 Andino/McCarren Name Signature Section "No matter what costume you wear, when you start eating Halloween candy, you will be a goblin. - Unknown This exam contains
More information1. Forming a Precipitate 2. Solubility Product Constant (One Source of Ions)
Chemistry 12 Solubility Equilibrium II Name: Date: Block: 1. Forming a Precipitate 2. Solubility Product Constant (One Source of Ions) Forming a Precipitate Example: A solution may contain the ions Ca
More informationUnit 3: Solubility Equilibrium
Unit 3: Chem 11 Review Preparation for Chem 11 Review Preparation for It is expected that the student understands the concept of: 1. Strong electrolytes, 2. Weak electrolytes and 3. Nonelectrolytes. CHEM
More informationModified Dr. Cheng-Yu Lai
Ch16 Aqueous Ionic Equilibrium Solubility and Complex Ion Equilibria Lead (II) iodide precipitates when potassium iodide is mixed with lead (II) nitrate Modified Dr. Cheng-Yu Lai Solubility-product constant
More information2. What mass of an aqueous 22.9% sodium chloride solution contains 99.5 g of water?
CHEM 1412 MIDTERM EXAM (100 pts total) ANSWER KEY Student s Name PART A (20 multiple choice questions, 3 pts each): 1. The solubility of a gas in a liquid can always be increased by: a) decreasing the
More informationCh 17 Solubility Equilibria. Brown & LeMay
Ch 17 Solubility Equilibria Brown & LeMay When a typical ionic solid is dissolved in water that dissolved material can be assumed to be present as separate hydrated anions & cations. For example: CaF 2
More informationb. There is no net change in the composition (as long as temperature is constant).
CHAPTER THIRTEEN Questions 9. a. The rates of the forward and reverse reactions are equal at equilibrium. b. There is no net change in the composition (as long as temperature is constant). 10. False. Equilibrium
More informationUnit 3: Solubility Equilibrium
Unit 3: Chem 11 Review Preparation for Chem 11 Review Preparation for It is expected that the student understands the concept of: 1. Strong electrolytes, 2. Weak electrolytes and 3. Nonelectrolytes. CHEM
More informationAP Questions: Thermodynamics
AP Questions: Thermodynamics 1970 Consider the first ionization of sulfurous acid: H2SO3(aq) H + (aq) + HSO3 - (aq) Certain related thermodynamic data are provided below: H2SO3(aq) H + (aq) HSO3 - (aq)
More informationCHEMICAL EQUILIBRIUM. Chapter 15
Chapter 15 P a g e 1 CHEMICAL EQUILIBRIUM Examples of Dynamic Equilibrium Vapor above a liquid is in equilibrium with the liquid phase. rate of evaporation = rate of condensation Saturated solutions rate
More informationSolubility Equilibrium
2016 Ksp note.notebook Solubility Equilibrium Learning Goals: to understand what happens when a compound dissolves in water to calculate the extent of dissolution...the molar solubility to calculate the
More informationM = Molarity = mol solute L solution. PV = nrt % yield = actual yield x 100 theoretical yield. PM=dRT where d=density, M=molar mass
Solubility Rules: 1. Most nitrate salts are soluble. 2. Most salts of alkali metals and ammonium cations are soluble. 3. Most chloride, bromide and iodide salts are soluble. Exceptions: salts containing
More informationCHM 1046 FINAL REVIEW
CHM 1046 FINAL REVIEW Prepared & Presented By: Marian Ayoub PART II Chapter Description 14 Chemical Equilibrium 15 Acids and Bases 16 Acid-Base Equilibrium 17 Solubility and Complex-Ion Equilibrium 19
More informationCHEMISTRY 202 Hour Exam I. Dr. D. DeCoste T.A.
CHEMISTRY 202 Hour Exam I September 28, 2017 Dr. D. DeCoste Name Signature T.A. This exam contains 23 questions on 10 numbered pages. Check now to make sure you have a complete exam. You have two hours
More informationSolubility & Equilibrium Unit Review
Solubility & Equilibrium Unit Review This review is worth 3 marks of your total test marks. It must be completed on test day. 3 marks will be given to students who have fully completed this review with
More informationName Date Class SECTION 16.1 PROPERTIES OF SOLUTIONS
SOLUTIONS Practice Problems In your notebook, solve the following problems. SECTION 16.1 PROPERTIES OF SOLUTIONS 1. The solubility of CO 2 in water at 1.22 atm is 0.54 g/l. What is the solubility of carbon
More informationCHM 112 Chapter 13 Extra Credit : Chemical Equilibrium Name:
CHM 112 Chapter 13 Extra Credit : Chemical Equilibrium Name: 1. Write the equilibrium expression for following reactions. In each case indicate whether the equilibrium is Homogeneous or Heterogeneous 2
More informationUNIT III: SOLUBILITY EQUILIBRIUM YEAR END REVIEW (Chemistry 12)
I. Multiple Choice UNIT III: SOLUBILITY EQUILIBRIUM YEAR END REVIEW (Chemistry 12) 1) Which one of the following would form an ionic solution when dissolved in water? A. I 2 C. Ca(NO 3 ) 2 B. CH 3 OH D.
More informationSOLUBILITY REVIEW QUESTIONS
Solubility Problem Set 1 SOLUBILITY REVIEW QUESTIONS 1. What is the solubility of calcium sulphate in M, g/l, and g/100 ml? 2. What is the solubility of silver chromate? In a saturated solution of silver
More informationWhat s in a solution? How far does a reaction go? Review (Chapter 4) & Section 13.5
I will try to structure our tour of chemistry in 3150:153 around three Big Questions: 1. What s in a solution? How far does a reaction go?. What factors influence how far a reaction goes and how fast it
More informationEquilibrium 07 M07_CHSL_SB_IBD_9069_U07.indd /07/ :21
07 Equilibrium Essential ideas 7.1 Many reations are reversible. These reations will reah a state of equilibrium when the rates of the forward reation and reverse reation are equal. The position of equilibrium
More informationAqueous Equilibria: Part II- Solubility Product
Aqueous Equilibria: Part II- Solubility Product PSI AP Chemistry Name-------------------------- I Solubility Product, K sp MC #63-103 a) Writing K sp expression b) Solving for K sp c) Solving for (molar)
More informationEquilibrium Test Review
AP Chemistry Equilibrium Test Review Name..... Hour. Directions: Complete the following problems. 1. Consider the reaction system, CoO(s) + H(g) Co(s) + HO(g) The equilibrium constant expression is Note
More information7. A solution has the following concentrations: [Cl - ] = 1.5 x 10-1 M [Br - ] = 5.0 x 10-4 M
Solubility, Ksp Worksheet 1 1. How many milliliters of 0.20 M AlCl 3 solution would be necessary to precipitate all of the Ag + from 45ml of a 0.20 M AgNO 3 solution? AlCl 3(aq) + 3AgNO 3(aq) Al(NO 3)
More informationPRACTICE MULTIPLE CHOICE- Chapters 17&18
PRACTICE MULTIPLE CHOICE- Chapters 17&18 1. What is the solubility product expression for Fe2(CO3)3? A) Ksp = [2Fe 3+ ][3CO3 2 ] B) Ksp = [2Fe 3+ ] 2 [3CO3 2 ] 3 C) Ksp = [Fe 2+ ] 2 [CO3 2 ] 3 D) Ksp =
More informationCHAPTERS 8-12 BOOKLET-3
CHEMISTRY XI CHAPTERS 8-1 BKLET- Contents: Page No. Chapter 8 Chemial Equilibrium 181-199 Chapter 9 Redox Reations 00-19 Chapter 10 s & p Blok Elements part 1 0-49 Chapter 11 s & p Blok Elements part 50-77
More informationReview 7: Solubility Equilibria
Review 7: Solubility Equilibria Objectives: 1. Be able to write dissociation equations for ionic compounds dissolving in water. 2. Given Ksp, be able to determine the solubility of a substance in both
More informationK P VERSUS K C PROPERTIES OF THE EQUILIBRIUM CONSTANT
K P VERSUS K C 1. What are the units of K p and K c for each of the following? a) 2H 2 S(g) 2H 2 (g) + S 2 (g) b) 4NH 3 (g) + 3O 2 (g) 2N 2 (g) + 6H 2 O(g) 2. What are the units of K p and K c for each
More informationChapter 15 Chemical Equilibrium
Equilibrium To be in equilibrium is to be in a state of balance: Chapter 15 Chemical Equilibrium - Static Equilibrium (nothing happens; e.g. a tug of war). - Dynamic Equilibrium (lots of things happen,
More informationCHAPTER 15 PRINCIPLES OF CHEMICAL EQUILIBRIUM
CHAPTER 15 PRINCIPLES OF CHEMICAL EQUILIBRIUM PRACTICE EXAMPLES 1A 1B (E) The reation is as follows: Cu (aq) Sn (aq) Cu (aq) Sn (aq) Therefore, the equilibrium exression is as follows: Cu Sn Cu Sn Rearranging
More informationTest #3 Last Name First Name November 13, atm = 760 mm Hg
Form G Chemistry 1442-001 Name (please print) Test #3 Last Name First Name November 13, 2003 Instructions: 1. This exam consists of 25 questions. 2. No scratch paper is allowed. You may do the work in
More informationChemistry 2202 Stoichiometry Unit Retest Review Guide
Chemistry 2202 Stoichiometry Unit Retest Review Guide Chapter 2: The Mole Pgs. 42 77 You should be able to: 1. Define the term molar mass and calculate the molar mass of any given element or compound.
More informationAnswer Sheet for Sample Problems for Chemistry Level 1 Final Exam 2016 Study Guide
Answer Sheet for Sample Problems for Chemistry Level 1 Final Exam 2016 Study Guide Electrons in Atoms Chapter 5 1. What is the frequency of green light, which has a wavelength of 4.90 x 10-7 m? 8 c 3.00x10
More informationUnit 3 ~ Learning Guide Name:
Unit 3 ~ Learning Guide Name: Instructions: Using a pencil, complete the following notes as you work through the related lessons. Show ALL work as is explained in the lessons. You are required to have
More informationCHEMISTRY 101 Hour Exam II. Dr. D. DeCoste T.A (30 pts.) 16 (15 pts.) 17 (15 pts.) Total (60 pts)
CHEMISTRY 101 Hour Exam II March 15, 2018 Dr. D. DeCoste Name Signature T.A. This exam contains 17 questions on 6 numbered pages. Check now to make sure you have a complete exam. You have one hour and
More informationChapter 8: Applications of Aqueous Equilibria
Chapter 8: Applications of Aqueous Equilibria 8.1 Solutions of Acids or Bases Containing a Common Ion 8.2 Buffered Solutions 8.3 Exact Treatment of Buffered Solutions 8.4 Buffer Capacity 8.5 Titrations
More informationAP Chemistry Chapter 16 Assignment. Part I Multiple Choice
Page 1 of 7 AP Chemistry Chapter 16 Assignment Part I Multiple Choice 1984 47. CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2 O(l) H = 889.1 kj H f H 2 O(l) = 285.8 kj mol 1 H f CO 2 (g) = 393.3 kj mol 1 What is
More informationAP Chemistry 1st Semester Final Review Name:
AP Chemistry 1st Semester Final Review Name: 2015-2016 1. Which of the following contains only sigma (s) bonds? 5. H2O(g) + CO(g) H2(g) + CO2(g) A) CO2 B) C3H6 C) CH3Cl D) N2O3 E) SiO2 2. What is the equilibrium
More informationCHEMICAL EQUILIBRIA: GENERAL CONCEPTS
CHEMICAL EQUILIBRIA: GENERAL CONCEPTS THE NATURE OF THE EQUILIBRIUM STATE: Equilibrium is the state where the concentrations of all reactants and products remain constant with time. (in stoichiometry,
More information1. a. The rates of the forward and reverse reactions are equal at equilibrium.
CHATER THIRTEEN CHEMICAL EQUILIBRIUM For Review 1. a. The rates of the forward and reverse reactions are equal at equilibrium. b. There is no net change in the composition (as long as temperature is constant).
More informationCOPYRIGHTED MATERIAL. Gravimetrics. Key Terms. Key Concepts. Words that can be used as topics in essays: accuracy atomic theory
8684-X Ch02.F 2/9/01 7:49 AM Page 23 Gravimetris Key Terms Words that an be used as topis in essays: auray atomi theory density empirial formula extensive property frational rystallization heterogeneous
More information22. What is the maximum concentration of carbonate ions that will precipitate BaCO 3 but not MgCO 3 from a solution that is 2.
PX312-1718 1. What is the solubility product expression for Th(IO 3 ) 4? A) K sp = [Th 4+ ][4IO 3 ] 4 B) K sp = [Th 4+ ][IO 3 ] C) K sp = [Th][IO 3 ] 4 D) K sp = [Th 4+ ][IO 3 ] 4 E) K sp = [Th 4+ ][IO
More informationCHAPTER 11 Stoichiometry Defining Stoichiometry
CHAPTER 11 Stoichiometry 11.1 Defining Stoichiometry Stoichiometry is the study of quantitative relationships between amounts of reactants used and products formed by a chemical reaction. Stoichiometry
More informationSI session Grue 207A
Chem 105 Wednesday 21 Sept 2011 1. Precipitation and Solubility 2. Solubility Rules 3. Precipitation reaction equations 4. Net ionic equations 5. OWL 6. Acids and bases SI session Grue 207A TR, 12:001:30
More informationThe solvent is the dissolving agent -- i.e., the most abundant component of the solution
SOLUTIONS Definitions A solution is a system in which one or more substances are homogeneously mixed or dissolved in another substance homogeneous mixture -- uniform appearance -- similar properties throughout
More informationChapter 18. Solubility and Complex- Ionic Equilibria
Chapter 18 Solubility and Complex- Ionic Equilibria 1 The common ion effect Le Chatelier Why is AgCl less soluble in sea water than in fresh water? AgCl(s) Ag + + Cl Seawater contains NaCl 2 Problem: The
More informationCHEMISTRY 202 Hour Exam I. Dr. D. DeCoste T.A.
CHEMISTRY 0 Hour Exam I September, 016 Dr. D. DeCoste Name Signature T.A. This exam contains 3 questions on 11 numbered pages. Check now to make sure you have a complete exam. You have two hours to complete
More informationAP CHEMISTRY NOTES 8-1 CHEMICAL EQUILIBRIUM: AN INTRODUCTION
AP CHEMISTRY NOTES 8-1 CHEMICAL EQUILIBRIUM: AN INTRODUCTION Chemical Equilibrium a dynamic state in which the rate of the forward reaction and the rate of the reverse reaction in a system are equal (the
More information"We are what we repeatedly do. Excellence, therefore, is not an act but a habit." --Aristotle--
CHEMISTRY 101 Hour Exam II October 25, 2016 Adams/Huynh Name Signature Section "We are what we repeatedly do. Excellence, therefore, is not an act but a habit." --Aristotle-- This exam contains 17 questions
More informationCh 10 Practice Problems
Ch 10 Practice Problems 1. Which of the following result(s) in an increase in the entropy of the system? I. (See diagram.) II. Br 2(g) Br 2(l) III. NaBr(s) Na + (aq) + Br (aq) IV. O 2(298 K) O 2(373 K)
More informationEquilibrium Reversible Reactions
1 Equilibrium Reversible Reactions Oak Park High School Mrs. Kornelsen Chemistry 40s Intro: Do Blue bottle Reaction demo Or watch online: http://www.dlt.ncssm.edu/core/chapter14- Gas_Phase- Solubility-
More informationReview Questions (Exam II)
Announcements Exam tonight, 7-8:15pm (locations posted on website) Conflict Exam, 5:15-6:30pm (114 Transportation Bldg) No lab this week! Start new material on Thursday (read chapter 10!) Review Questions
More informationChapter 7 - Chemical Reactions
Chapter 7 - Chemical Reactions Evidence of a Chemical Reaction If we could see the atoms and molecules that compose matter, we could easily identify a chemical reaction: Atoms combine with other atoms
More informationJF Physical Chemistry JF CH 1101: Introduction to Physical Chemistry.
JF Physial Chemistry 010-011. JF CH 1101: Introdution to Physial Chemistry. Dr Mike Lyons. Shool of Chemistry Trinity College Dublin. melyons@td.ie A ompendium of past examination questions set on Physial
More informationChapter 4: Stoichiometry of Chemical Reactions. 4.1 Writing and Balancing Chemical Equations
Chapter 4: Stoichiometry of Chemical Reactions 4.1 Writing and Balancing Chemical Equations A chemical equation represents or symbolizes a chemical reaction. o Substances are represents by their chemical
More informationPractice Packet Unit 7: Moles & Stoichiometry
PRACTICE PACKET: Unit 7 Moles & Stoichiometry Regents Chemistry: Practice Packet Unit 7: Moles & Stoichiometry Vocabulary: Lesson 1: Lesson 6: Lesson 2: Lesson 4A: Lesson 4B: Lesson 3: Lesson 5: www.chempride.weebly.com
More informationTYPES OF CHEMICAL REACTIONS
TYPES OF CHEMICAL REACTIONS Precipitation Reactions Compounds Soluble Ionic Compounds 1. Group 1A cations and NH 4 + 2. Nitrates (NO 3 ) Acetates (CH 3 COO ) Chlorates (ClO 3 ) Perchlorates (ClO 4 ) Solubility
More information] after equilibrium has been established?
Chemistry 1 Solubility Equilibrium onster Review 1. A saturated solution forms when a 0. 10 mol of salt is added to 10. L of water. The salt is A. Li S B. CuBr C. Zn( OH) ( ) D. NH CO 4. Consider the following
More information3. Indicate the mass action expression for the following reaction: 2X(g) + Y(g) 3W(g) + V(g) a) [X] 2 [Y][W] 3 [V] [W] 3 [V] [X] 2 [Y] [3W][V] [2X][Y]
1. Which of the following statements concerning equilibrium is not true? a) A system that is disturbed from an equilibrium condition responds in a manner to restore equilibrium. b) Equilibrium in molecular
More informationAP Chemistry Table of Contents: Ksp & Solubility Products Click on the topic to go to that section
Slide 1 / 91 Slide 2 / 91 AP Chemistry Aqueous Equilibria II: Ksp & Solubility Products Table of Contents: K sp & Solubility Products Slide 3 / 91 Click on the topic to go to that section Introduction
More informationPractice Worksheet - Answer Key. Solubility #1 (KEY)
Practice Worksheet - Answer Key Solubility #1 (KEY) 1 Indicate whether the following compounds are ionic or covalent a) NaCl ionic f) Sr(OH) 2 ionic b) CaBr 2 ionic g) MgCO 3 ionic c) SO 2 covalent h)
More informationf) Perchloric acid g) Dihydrogen sulfide i) Barium phosphate j) Copper(II) sulfate pentahydrate
1 2 1. For the following provide the correct name or formula. [8] a) Hg2(NO3)2 b) Mg(C2H3O2)2 c) (NH4)2CO3 d) Ca(OH)2 f) Perchloric acid g) Dihydrogen sulfide i) Barium phosphate j) Copper(II) sulfate
More information