Ag2CrO4(s) + 2e- 2Ag(s) + CrO42-(aq) A chemist wishes to determine the concentration of CrO42- electrochemically. A cell is constructed consisting of a saturated calomel electrode (SCE; which has a reduction potential of 0.242 V relative to the SHE) and

29,984 results
  1. Chemistry

    Write a balanced overall reaction from these unbalanced half-reactions. Sn->Sn2+ Ag+->Ag Balanced overall equation I got Sn+2Ag+->Sn+2Ag, but its wrong.

  2. Chemistry

    Heart pacemakers are often powered by lithium-silver chromate “button” batteries. The overall cell reaction is: 2Li(s) + Ag2CrO4(s) --------> Li2CrO4(s) + 2Ag(s) Lithium metal is the reactant at one of the electrodes of the battery. Is it the anode or

  3. chemistry

    Balance the redox reactin in basic. ClO- + Cr(OH)4- --> CrO42- + Cl- H2O + ClO- --> Cl- + 2OH ClO- has a +1 O# and Cl- has a -1 O# how do I balance that. And is what Ive done so far correct? Cr(OH)4- --> CrO42- Im confused on how to balance the oxygen and

  4. Chemistry

    For the following balanced equation: 2 Ag+ (aq) + Cu(s) ---> Cu2+ (aq) + 2 Ag(s) Which letter corresponds to the correct cell notation at standard state conditions? A. Cu2+(aq)/ Cu(s) // Ag(s) / Ag+(aq) B. 2Ag+(aq)/ Cu2+(aq)// 2Ag(s)/ Cu(s) C. Ag+(aq) /

  5. chemistry

    Which of the following is a precipitation reaction? I. 2 Mg (s) + O2 (g) → 2 MgO (s) II. SO3 (g) + 2 H2O (l) → H3O+ (aq) + HSO4- (aq) III. Pb2+ (aq) + CrO42- (aq) → PbCrO4 (s) IV. 2 H2O (g) → 2 H2 (g) + O2 (g) V. Ag+ (aq) + 2 NH3 (aq) →

  6. Chemistry

    What hydroxide concentration is required to (a) Initiate precipitation of Ag2CrO4 from a solution that is 2.12 x 10^-3 M in Ag+? (b) lower the Al^3+ concentration in the foregoing solution to 1.00 x 10^-9

  7. Chemistry

    Complete and balance the equation for this reaction in basic solution? Redox reaction Cr is oxidized to CrO42– and Fe3 is reduced to Fe2...? For a particular redox reaction Cr is oxidized to CrO42– and Fe3 is reduced to Fe2 . Complete and balance the

  8. Chemistry!!

    A chemist wants to prepare a stock solution of H2SO4 so that a sample of 20.00mL will produce a solution with a concentration of .50 M when added to 100.0mL of water. A)what should the molarity of the stock solution be? B)If the chemist wants to prepare

  9. Chemistry

    Balance these reactions using the half-reaction method Sn2+ + IO3- -> Sn4= + I- (acidic solution) CrO2 + ClO- -> CrO42- + Cl- (basic solution)

  10. Chemistry

    A solution containing a mixture of 0.0381 M potassium chromate (K2CrO4) and 0.0769 M sodium oxalate (Na2C2O4) was titrated with a solution of barium chloride (BaCl2) for the purpose of separating CrO42– and C2O42– by precipitation with the Ba2 cation.

  11. Chemistry

    Which equation shows conservation of mass and charge? A.NH4Br → NH3 + Br2 B. 2Mg + Fe3+ → Mg2+ + 3Fe C. H2SO4 + LiOH → Li2SO4 + H2O D. Cu + 2Ag+ → Cu2+ + 2Ag It's either b or d, since they both have two elements with an oxidation number of 0. Which

  12. chemistry

    In a reaction, a chemist is observing the absorbance of CoCl2(aq) as a function of time to determine the rate at which it is being consumed in a reaction. At time t=10 s, the chemist determines that the concentration of CoCl2(aq) is 0.12 M. At time t=20 s,

  13. Chemistry

    A solution containing a mixture of 0.0492 M potassium chromate (K2CrO4) and 0.0565 M sodium oxalate (Na2C2O4) was titrated with a solution of barium chloride (BaCl2) for the purpose of separating CrO42– and C2O42– by precipitation with the Ba2 cation.

  14. chemistry

    A chemist wishes to determine the rate of reaction of zinc with hydrochloric acid. The equation for the reaction is: Zn(s) + 2HCl(aq) ---> H2(g) + ZnCl2(aq) A piece of zinc is dropped into 1.00 L of 0.100 M HCl and the following data were obtained:

  15. Chemistry

    1. A chemist prepares a solution by dissolving 4.603 g of NaNO3 in enough water to make 200 mL of solution. What molar concentration of sodium nitrate should appear on the label? Answer in units of M 2.If the chemist mistakenly makes 225 mL of solution

  16. chemistry

    0.10 M potassium chromate is slowly added to a solution containing 0.50 M AgNO3 and 0.50 M Ba(NO3)2. What is the Ag+ concentration when BaCrO4 just starts to precipitate? The Ksp for Ag2CrO4 and BaCrO4 are 1.1 x 10-12 and 1.2x10^-10 respectively

  17. Chemistry

    Calculate the solubility of Ag2CrO4 in a) 0.05M KClO4 b) 0.005M AgNO3 a) I have figured out: Ag2CrO4=2Ag- + CrO42- Ksp=1.12*10^-12. Ksp=[2Ag]^2*[CrO4] Ksp=(2x)^2(x) = 1.12*10^-12=4x^3= x=2.65*10^-5 (?) b)Ag2CrO4=2Ag- + CrO42- Ksp=1.12*10^-12.

  18. Chemistry

    Balance the following redox (oxidation-reduction) reaction under basic conditions. (Include states-of-matter under the given conditions in your answer. Use the lowest possible whole number coefficients.) CrO42−(aq) + S2O32−(aq) → Cr3+(aq) +

  19. chemistry

    how many liters of gaseous hydrogen bromide at 97 degrees c and 0.953 atm will a chemist need if she wishes to prepare 3.50 L of 1.20 M hydrobromic acid?

  20. Chemistry

    Calculate the mass of solid AgNo3 that can be added to 2.0 L of 0.10M K2CrO4 solution in order to just start precipitation? Here is what I have done so far: 2AgNO3(aq) + K2CrO4(aq) ==> Ag2CrO4(s) + 2KNO3(aq) Ag2CrO4(s) ===> 2Ag^+ CrO4^^2- Ksp =

  21. Chemistry

    in a particular redox reaction, Cr is oxidized to CrO42- and Ag+ is reduced to Ag. Complete and balance the equation for this reaction in acidic solution.

  22. Chemistry

    Solutions of silver nitrate and sodium chromate are mixed. What is the net ionic equation? I got: 2Ag(aq) + CrO4-2(aq) -> Ag2CrO4(s) is that right?

  23. Chemistry

    For the following balanced equation: 2Ag+(aq) + Cu(s)Cu2+ (aq) + 2 Ag(s) Which letter corresponds to the correct cell notation at standard state conditions? A. Cu(s) | Cu2+(aq) || Ag+(aq) | Ag(s) B. Ag+(aq) | Cu2+(aq) || Cu(s) | Ag(s) C. 2Ag+(aq) |

  24. Chemistry

    For the following balanced equation: 2 Ag+ (aq) + Cu(s)--> Cu2+ (aq) + 2 Ag(s) Which letter corresponds to the correct cell notation at standard state conditions? A. Cu(s)/Cu2+(aq)//Ag+(aq)/Ag(s) B. Cu2+(aq)/ Cu(s)// Ag(s)/ Ag+(aq) C. Ag+(aq)/ Cu2+(aq)//

  25. chemistry

    For the following balanced equation: 2 Ag+ (aq) + Cu(s) Cu2+ (aq) + 2 Ag(s) Which letter corresponds to the correct cell notation at standard state conditions? A. Cu(s) Cu2+(aq) Ag+(aq) Ag(s) B. Cu2+(aq) Cu(s) Ag(s) Ag+(aq) C. Ag+(aq) Cu2+(aq) Cu(s) Ag(s)

  26. Chemistry

    A voltaic cell is constructed as follows: Ag(s)|Ag^+,(satd Ag2CrO4)||Ag^+(0.110 M)|Ag(s). What is the value of Ecell? For Ag2CrO4, Ksp=1.1*10^-12.

  27. Chemistry

    Calculate the cell voltage for the following reaction: 2Ag^+ (0.090M) + H2 (1atm) -> 2Ag(s) + 2H^+ (pH=4.0)

  28. Chemistry-Rates of Reaction

    A chemist wishes to determine the rate of reaction of zinc with hydrochloric acid. The equation for the reaction is: Zn(s) + 2HCl(aq) ---> H2(g) + ZnCl2(aq) A piece of zinc is dropped into 1.00 L of 0.100 M HCl and the following data were obtained:

  29. chemistry

    If 0.10 M potassium chromate is slowly added to a solution containing 0.50 M AgNO3 and 0.50 M Ba(NO3)2. What is the Ag+ concentration when BaCrO4 just starts to precipitate? The Ksp for Ag2CrO4 and BaCrO4 are 1.1 x 10-12 and respectively.

  30. chemistry

    In a particular redox reaction, Cr is oxidized to CrO42– and Cu2 is reduced to Cu . Complete and balance the equation for this reaction in acidic solution. Phases are optional. Cr + Cu2+ = CrO42- + Cu+

  31. AP Chem (Thanks!)

    Hey guys! Stuck on some! My maybe answers are written next to the problem (1 problem-5 parts). Thanks for any help: 1. Lead (II) chromate, PbCrO4, is a slightly soluble salt. Write a net ionic equation for the dissolution of solid PbCrO4 in water. My

  32. chemistry

    A sample of silver chromate (Ag2CrO4) has a mass of 29.0 g. (a) How many Ag+ ions are present? (b)What is the mass in grams of one formula unit of silver chromate? (c) How many CrO42- ions are present?

  33. chemistry

    If a solution containing 0.22 M Cl -, Br -, I -, and CrO42- is treated with Ag+, in what order will the anions precipitate?

  34. Chemistry

    Balance the following in basic solution: Al(s) + CrO42¯(aq) → Al(OH)3(s) + Cr(OH)4¯(aq) Can someone please help me do this. I having a hard time, especially determining the charge of Al(OH)3. Thanks to anyone who helps

  35. Chemistry ASAP

    the concentration of Ag+ in a saturated solution of Ag2Cro4 is 1.6x10^-4 M. what is the Ksp value for Ag2Cro4? the solubility of BaCO3(s) in water is 4.0X10^-5 M. Calculate the value of Ksp for BaCO3

  36. chemistry!

    If the chemist mistakenly makes 275 mL of solution instead of the 200 mL, what molar concentration of sodium nitrate will the chemist have actually prepared? Answer in units of M

  37. College Chem 2

    Calculate the solubility Ag2CrO4(s) in a 0.100 M solution of AgNO3 and compare its solubility with Ag2CrO4 solubility in pure water at room temperature. The Ksp for Ag2CrO4 is 9.0 x 10^-12 at room temperature. The Kspfor Ag2CrO4 at room temperature in pure

  38. Chemistry

    When 20.0 mL of 0.100 M AgNO3 are mixed with 80.0 mL of 0.0100 M Na2CrO4, what is the chromate ion concentration (CrO4^2-)? Ksp for Ag2CrO4 = 9.0 x 10^-12. I think it's 1.0 x 10^-9. Am I right?

  39. Chemistry

    The reaction of nitrogen dioxide with fluorine generates nitryl fluoride: 2NO2(g) + F2(g) --> 2NO2F(g) To determine the rate law for this reaction, a chemist performed several initial-rate experiments using different initial concentration, with the details

  40. Chemistry 114

    Write down the Ksp expression for Ag2CrO4. If the solubility of Ag2CrO4 is 0.0216 g/L, calculate the value of Ksp

  41. Chemistry

    An analytical chemist determines that an estuarine water sample contains 1.5 g/L of sulfate ion. What is the concentration in terms of (a) g/L of S (b) molar concentration of sulfate (c) normality (d) parts per million of sulfate

  42. Chemistry

    A chemist prepared a solution by dissolving 52.0 g of hydrated sodium carbonate in water to a total volume of 5.00 dm3. The concentration was determined to be 0.0366 M. Determine the formula of the hydrated sodium carbonate.

  43. Chemistry

    Which of the following redox reactions are spontaneous -- SN2+(aq)+BA(s)->Sn(s)+Ba2+(aq) 2AG+(ag)+2Cl-(aq)->2Ag(s)+C12(g) ZN(s)+F2(g)->2F-(aq)+Zn2+(aq) 2LI(s)+Co2+->(aq)->2Li+(aq)+Co(s) 2I-(aq)+K+(aq)->I2(s)+K(s) I believe it is A, C & E

  44. Chemistry

    What is the Cl concentration just as Ag2CrO4 begins to precipitate when 1.0 M AgNO3 is slowly added to a solution containing 0.015 M Cl and 0.015 M CrO4^2?

  45. George School

    Ag2CrO4(s) + 2e- 2Ag(s) + CrO42-(aq) A chemist wishes to determine the concentration of CrO42- electrochemically. A cell is constructed consisting of a saturated calomel electrode (SCE; which has a reduction potential of 0.242 V relative to the SHE) and a

  46. Electrochemistry

    Ag2CrO4(s) + 2e- 2Ag(s) + CrO42-(aq) A chemist wishes to determine the concentration of CrO42- electrochemically. A cell is constructed consisting of a saturated calomel electrode (SCE; which has a reduction potential of 0.242 V relative to the SHE) and a

  47. Chemistry

    What is the molar concentration of silver ion in a solution containing 1.3 × 10–4 M CrO42–, saturated with Ag2CrO4? The Solubility Product Constant, Ksp for Ag2CrO4 is 9 × 10–12 (A) 1.3 × 10–16 (B) 7 × 10–16 (C) 9 × 10–12 (D) 2.6 × 10–4

  48. Chemistry

    Electrochemisry. Candy Chemist wishes to determine the concentration of CrO4^2- by electrochemical means in solution, and subsequently the Ksp of Ag2CrO4. She sets up one half-cell comprised of the Ag+|Ag couple (E=+0.799V) and a second half-cell in which

  49. electrochemistry

    What is the anode and cathode of this problem? A chemist wishes to determine the concentration of CrO4-2 ions electrochemically. A cell is constructed consisting of saturated calomel electrode (SCE) and a silver wire coated with Ag2CrO4. The SCE is

  50. chemistry

    Determine if the following reaction is spontaneous under standard conditions. Zn(s) + 4 CN¡V(aq) + Ag2CrO4(s) „³ Zn(CN)42¡V(aq) + 2 Ag(s) + CrO42¡V(aq)

  51. Chemistry

    A chemist wishes to determine the concentration of CrO4-2 ions electrochemically. A cell is constructed consisting of saturated calomel electrode (SCE) and a silver wire coated with Ag2CrO4. The SCE is composed of mercury in contact with a saturated

  52. chemistry

    A chemist wishes to determine the concentration of CrO4-2 ions electrochemically. A cell is constructed consisting of saturated calomel electrode (SCE) and a silver wire coated with Ag2CrO4. The SCE is composed of mercury in contact with a saturated

  53. chemistry

    A sample of silver chromate (Ag2CrO4) has a mass of 29.0 g. How many CrO42- ions are present?

  54. Chemistry

    at 23C the reaction CaCrO4 -> Ca2+ + CrO42- has an equilibrium constant of 7.1 x 10-4. what are the equilibrium concentrations of Ca2+ and CrO42- in a saturated solution?

  55. Chem- Please check :)

    The solubility of silver chromate is 500 ml of water at 25 degrees celsius is 0.0129g. Calculate its solubility product constant. n = m/M = 0.0129g/331.73g/mol = 3.888 x 10^-5mol concentration (ag2crO4)=n/V =3.888x10^-5/0.5L = 7.777 x 10^-5 ag2crO4 2ag+ +

  56. CHEMISTRY

    Balance the following equation. (for a balanced eq. aA + bB → cC + dD, enter your answer as the integer abcd) CrO42−(aq) + H2O(l) + HSnO2− → CrO2−(aq) + OH−(aq) + HSnO3−(aq)

  57. Chemistry

    Assign oxidation numbers to all species in the redox reactions below. Identify the oxidizing and reducing agents. 1. Fe(OH)2 (s) + CrO42- (aq) → Fe2O3(s) + Cr(OH)4-(aq) (basic)

  58. Chemistry

    Choose the two half-reactions from a table of standard reduction potentials that most closely approximate the reaction that occur within the battery (Pacemaker). What is the standard voltage generated by a cell operating with these half-reactions? (i got

  59. chemistry

    Calculate the molarity (mol/L) of Ba2+ when BaCrO4 is placed in a 0.0457 M K2CrO4 solution. The equation represents the solubility process. K(sp)=1.2x10^-10 BaCrO4 (s) Ba2+ (aq) + CrO42- (aq)

  60. Chemistry

    Solutions of silver nitrate and sodium chromate are mixed. What is the net ionic equation? I got: 2Ag(aq) + CrO4-2(aq) -> Ag2CrO4(s) is that right?

  61. Chemistry- Le chatelier's Principle

    HOw would you predict the colour change or changes in number of states for the following: To a solution of 5 drops of 0.3 M K2CrO4 ans 2 drops of 0.3M NaOH add a drop at a time 0.1 M Ba(NO3)2 until a change is noticed. Given: BaCrO4(s) ---> Ba2+ + CrO42-

  62. Chem

    Calculate the Keq of the reversible reactions Cr2O7 + 2OH -> CrO4 + H2O and 2CrO42->Cr2O72 , given the following data: HCrO4 -> H + CrO42 K = 3.2 x 10^-7 2HCrO4 -> Cr2O72 + H2O K = 34 H2O -> H+ + OH- K = 1 x 10^-14 HCL and NaOH = 1M KCrO4 and KCr2O7 = 0.1M

  63. Chemistry

    For the following reactions, determine the equilibrium constant equation. 1) CO2(g) + H2(g) CO(g) + H2O(g) 2) 2NO(g) + 2H2(g) N2(g) + 2H2O(g) 3) Cu(s) + 2Ag+(g) Cu2+(g) + 2Ag(s) 4) H2(g) + I2(g) 2HI(g)

  64. chemistry 2

    The voltaic cell reaction NiO2(s)+4H^+(aq)+ 2Ag(s)-->Ni^2+(aq)+2H20(l)+ 2Ag^+ has a E cell= +2.48V. What will the cell potential be at a pH of 5.00 when the concentration of NiO^2+ and Ag^+??? I need to know how to set this type of problem up to solve it

  65. Chemisty

    if the chemist mistakenly makes 275 ml of solution instead of the 200ml, what molar concentration of sodium nitrate will the chemist have actually prepared

  66. Chemistry

    Quantitative anaylsis of cl- ion is often performed by a titration with silver nitrate, using sodium chromate as an indicator. As standardized AgNo3 is addded, both white AgCl and red Ag2CrO4 precipitate, but so long as some cl- remains, the Ag2CrO4

  67. Chemistry

    A solution of barium chromate is prepared by dissolving 6.3 x 10-3 g of this yellow solid in 1.00 L of hot water. Will solid barium chromate precipitate upon cooling to 25°C? Proof? You want to compare Qsp to Ksp (at 25o C.) Ag2CrO4(s) ==>2Ag^+ + CrO4^=

  68. Chemistry

    For the following balanced equation: 2 Ag+ (aq) + Cu(s) ---> Cu2+ (aq) + 2 Ag(s) Which letter corresponds to the correct cell notation at standard state conditions? A. Cu2+(aq)/ Cu(s) // Ag(s) / Ag+(aq) B. 2Ag+(aq)/ Cu2+(aq)// 2Ag(s)/ Cu(s) C. Ag+(aq) /

  69. UCI Chemistry Webworks

    For the following balanced equation: 2 Ag+ (aq) + Cu(s) Cu2+ (aq) + 2 Ag(s) Which letter corresponds to the correct cell notation at standard state conditions? A. 2Ag+(aq) | Cu2+(aq) || 2Ag(s) | Cu(s) B. Cu(s)| Cu2+(aq) || Ag+(aq) | Ag(s) C. Ag+(aq) |

  70. Chemistry

    For the following balanced equation: 2 Ag+ (aq) + Cu(s) Cu2+ (aq) + 2 Ag(s) Which letter corresponds to the correct cell notation at standard state conditions? A. 2Ag+(aq) Cu2+(aq) 2Ag(s) Cu(s) B. Cu(s) Cu2+(aq) Ag+(aq) Ag(s) C. Ag+(aq) Cu2+(aq) Cu(s)

  71. Chemistry

    A chemist wants to make a solution of 3.4 M HCl. There are two solutions of HCL that he can find on the shelf. One has a concentration of 6.0 M, while the other has a concentration of 2.0 M. Which solution can the chemist use to make the desired acid?

  72. Algebra

    A chemist made 50 ounces of an acidic solution by mixing two different concentrations of the solution. He mixed x ounces of acidic solution with an 80% concentration and an acidic solution with 90% concentration. Which equation can be used to determine the

  73. Chemistry

    Using the total volume at endpoint (51.98mL) and the fact that the concentration of CrO4 ^2- due to Mohr's indicator is 0.26 M, find the actual concentration of CrO4^ 2- at the endpoint (or at the instant just before Ag2CrO4 begins to form). Any help I am

  74. Chem

    Can somebody check this for me?? Ksp AgCl 1.8x10^-10 Ag2CrO4 1.0x10^-12 AgI 1.0x10^-16 Ag3Po4 1.0x10^-16 1. calc the [Ag+] and [Cl-] at equivalence point. I got 1.3x10^-5 2. Calc. the [CrO4-2] required to precipitate AgCr04 if the [Ag+] equals the conc.

  75. Chemistry

    Choose the two half-reactions from a table of standard reduction potentials that most closely approximate the reaction that occur within the battery. What is the standard voltage generated by a cell operating with these half-reactions? 2Li(s) + Ag2CrO4(s)

  76. Chemistry

    Claculate the voltage of the following cell at 25 Degress Celcius. 2Ag (aq) (0.010M) + Cu(s) -> Cu^2(aq)(0.1M) +2Ag(s)

  77. Chemistry

    predict if precipitation will occur when 36ml of 0.0039M Na2CrO4 is mixed with 18ml of 0.00033M AgNO3. M.W of Ag2CrO4 :331.73g/mol Kspof ag2cro4 1.1x10^-12

  78. Chemistry

    split the following redox equation to oxidation and reduction 1 Fe 2Ag -> Fe2 2Ag 2 Cl2 I -> 2Cl- I2?

  79. chemistry

    How many grams of Cu (s) are needed to form 6.00g Ag from a solution of AgNO3? The reaction is Cu (s)+2Ag^+(ag)--> Cu^2+(aq)+2Ag (s) the molar masses are: Ag=107.868 and Cu=63.546g

  80. science

    CH3CH2CHO + 2Ag(NH3)2OH = CH3CH2COONH4+2Ag+H20+3NH3 yield of Ag obtained = 75% calculate minimum mass of propanal that must have been used to form 5g of silver

  81. science

    Which of the following reactions can occur or not.explain Zn + 2H -> Zn + H2 Fe + 2Ag -> Fe + 2Ag Cu + Pb -> Cu + Pb

  82. College Chemistry

    For my homework I got this problem that my professor never went over in class how to do it and I don't know how to interpret it. A chemist runs a second order reaction of A->B starting at 10mili moles/L concentration of A (and no B). After one hour the

  83. College Chemistry

    For my homework I got this problem that my professor never went over in class how to do it and I don't know how to interpret it. A chemist runs a second order reaction of A->B starting at 10mili moles/L concentration of A (and no B). After one hour the

  84. College Chemistry

    For my homework I got this problem that my professor never went over in class how to do it and I don't know how to interpret it. A chemist runs a second order reaction of A->B starting at 10mili moles/L concentration of A (and no B). After one hour the

  85. Chemistry

    In a titration for the determination of the chloride ion, a solution of 0.1M agno3 is used against a solution, the volume of which is 100ml. At the completion of the titration, the residual concentrations of silver and chloride ions are equal and the total

  86. College Chemistry

    For my homework I got this problem that my professor never went over in class how to do it and I don't know how to interpret it. A chemist runs a second order reaction of A->B starting at 10mili moles/L concentration of A (and no B). After one hour the

  87. Chemistry

    In a titration for the determination of the chloride ion, a solution of 0.1M agno3 is used against a solution, the volume of which is 100ml. At the completion of the titration, the residual concentrations of silver and chloride ions are equal and the total

  88. Chemistry

    1)Write the general equation used to determine the volume of stock required to make a given concentration of standard? Define any terms you used. ----use the 100ml flasks to create four serial dilutions of the stock 10,000uM nitrate solution that has been

  89. chemistry

    A chemist performed an experiment in which silver nitrate was used to precipitate all of the chromate ion as silver chromate, Ag2CrO4 from 200 mL of a solution of potassium chromate, K2CrO4. This process required 120 mL of 0.200 M AgNO3. Write the balanced

  90. Chemistry

    What property of the following reaction might be qualitatively measured to follow the rate of reaction? A) C(s) + H20(g) > H2(g) + CO(g) B) Cu(s) + 2Ag+(aq) > Cu2+(aq) + 2Ag(s)

  91. Chemistry

    What property of the following reaction might be qualitatively measured to follow the rate of reaction? A) C(s) + H20(g) > H2(g) + CO(g) B) Cu(s) + 2Ag+(aq) > Cu2+(aq) + 2Ag(s)

  92. Chemistry

    calculate the minimum concentration of ag+ ion that must be added to (or built up in) a 0.140 m Na2CrO4 solution in order to initiate a precipitation of silver chromate. The ksp of ag2cro4 is 1.2 × 10^-12.

  93. Chemistry

    0.10 M potassium chromate is slowly added to a solution containing 0.50 M AgNO3 and 0.50 M Ba(NO3)2. What is the Ag+ concentration when BaCrO4 just starts to precipitate? The Ksp for Ag2CrO4 and BaCrO4 are 1.1 x 10-12 and respectively.

  94. chemistry- electrochem

    Given a cell based on the spontaneous reaction 2AgCl(s) + Zn(s) ® 2Ag(s) + 2Cl– + Zn2+ If the zinc ion concentration is kept constant at 1 M, and the chlorine ion concentration is decreased from 1 M to 0.001 M, the cell voltage should increase by 0.06 V

  95. CHEMISTRY

    Given a cell based on the spontaneous reaction 2AgCl(s) + Zn(s) ® 2Ag(s) + 2Cl– + Zn2+ If the zinc ion concentration is kept constant at 1 M, and the chlorine ion concentration is decreased from 1 M to 0.001 M, the cell voltage should increase by 0.06 V

  96. chemistry

    a chemist puts 6 moles of nitrogen gas and 7 moles hydrogen gas into an evacuated 1 liter container. The system reaches equilibrium at a certain temperature according to the process outlined above. when the system is at equilibrium the chemist determines

  97. chemistry

    A chemist added 3.15 grams of HNO3 to a solution of the same acid with concentration of 9 mol/L. dilutes the resulting solution up to the 100ml volume. The resulting solution will have what concentration?

  98. Chemistry

    Consider a solution containing 4.35 mM of an analyte, X, and 1.09 mM of a standard, S. Upon chromatographic separation of the solution peak areas for X and S are 3251 and 10075, respectively. Determine the response factor for X relative to S. F=? To

  99. chemistry 101

    We add excess Na2CrO4 solution to 42.0 mL of a solution of silver nitrate (AgNO3) to form insoluble solid Ag2CrO4. When it has been dried and weighed, the mass of Ag2CrO4 is found to be 0.590 grams. What is the molarity of the AgNO3 solution? Answer in

  100. chem 101

    We add excess Na2CrO4 solution to 42.0 mL of a solution of silver nitrate (AgNO3) to form insoluble solid Ag2CrO4. When it has been dried and weighed, the mass of Ag2CrO4 is found to be 0.590 grams. What is the molarity of the AgNO3 solution? Answer in

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