how can you tell if two reactants will make a buffer?

30,550 results
  1. Chemistry

    Select the statements that correctly describe buffers.? 1) The pH of a buffer solution does not change significantly when any amount of a strong acid is added. 2) The Ka of a buffer does not change when any amount of an acid is added to the buffer

  2. Chemistry

    Which of the following pairs would make a good buffer solution in an aqueous solution? A) H2SO4 and NaHSO4 B) Ca(NO3)2 and HNO3 C) HCl and NaCl D) HF and NaOH E) none of them I know the answer is D but I don't understand why. I would think it would be C

  3. chemistry

    A reaction with an equilibrium constant Kc = 1.5 x 1021 would consist of which of the following at equilibrium: A) approximately equal reactants and products B) some reactants and products with reactants slightly favored C) some reactants and products with

  4. chemistry

    A reaction with an equilibrium constant Kc = 1.5 x 10-25 would consist of which of the following at equilibrium: A. some reactants and products with products slightly favored B. essentially all products C. some reactants and products with reactants

  5. Science HELP

    Sodium is a metal and chlorine is a poisonous gas. Neither is safe to eat. However, when sodium and chlorine combine, it produces edible table salt. What can be concluded? A. Table salt has similar physical properties of both reactants. B. Table salt is a

  6. chemistry

    What is ΔH in the equation ΔG = ΔH - TΔS? A. The change in specific heat between the products and the reactants B. The change in enthalpy between products and reactants in a reaction C. The change in entropy between products and reactants in a reaction

  7. Chemistry

    A buffer consisting of H2PO4- and HPO42-, helps control the pH of physiological fluids. Many carbonated soft drinks also use this buffer system. You were asked to prepare this buffer from K2HPO4 and KH2PO4. Identify the week acid and base components of

  8. school

    What is the pH of 0.1 M formic acid solution? Ka=1.7„e10-4? What is the pH value of buffer prepared by adding 60 ml of 0.1 M CH3COOH to 40 ml of a solution of 0.1 M CH3COONa? What is the pH value of an acetate buffer (pK=4.76) prepared by adding 20 ml of

  9. general science

    which of the following accurately shows the correct terms for the two sides of a chemical equation, correctly placed to the left or to the right where they belong and also shows the correct symbol that is written between them? reactants --> products

  10. biochemistry with more info that was needed

    Calculate the weight of the buffers you will use to make the buffers for Part A for all the buffer possibilities listed under procedures in Part A, step 1. In other words, how many grams do you need to make 100 mL of a 0.1 M buffer? Buffer pKa1 pKa2 pKa3

  11. Chemistry

    Based on the chemical reaction: N2(g) + 3H2(g) → 2NH3(g), which statement is TRUE regarding the mass of the reactants compared to the mass of the products? a) There is not enough information given to answer this question. b) The mass of the reactants is

  12. Chemistry

    Buffer capacity is a measure of a buffer solution\'s resistance to changes in pH as strong acid or base is added. Suppose that you have 165 mL of a buffer that is 0.360 M in both benzoic acid (C6H5COOH) and its conjugate base (C6H5COO–). Calculate the

  13. chemistry

    a buffer composed of 0.50mol acetic acid and 0.50mol sodium acetate is diluted to a volume of 1.0L. The pH of the buffer is 4.74. How many moles of NaOH must be added to the buffer solution to increase its pH to 5.74?

  14. AP CHEMISTRY

    A buffer, consisting of H2PO4− and HPO42−, helps control the pH of physiological fluids. Many carbonated soft drinks also use this buffer system. What is the pH of a soft drink in which the major buffer ingredients are 7.20 g of NaH2PO4 and 4.90 g of

  15. Chemistry university

    what is the ph of 50ml buffer solution which is 2M in CH3COOH and 2M in CH3CooNa? 1 Initial PH before the addition of acids and base? 2 What is the new PH after 2ml of 6.00M HCl is added to this buffer? 3 what is the new PH after 2.00ml of 6.00M NaoH is

  16. Chemistry(Please check, thank you)

    For an experiment on the effect of a buffer solution, I need to calculate the expected pH of the buffer. I know that I have to make an amounts table and use the Hasselbalch equation to find the pH. For the first part, 0.10M HCl was added to a buffer. The

  17. chemistry

    Which of the following accurately shows the correct terms for the two sides of a chemical equation, correctly placed to the left or to the right where they belong, and also shows the correct symbol that is written between them? Choose a,b,c, or d. the

  18. Chemistry

    Calculate the pH of the 0.20 M NH3/0.20 M NH4Cl buffer. What is the pH of the buffer after the addition of 10.0 mL of 0.10 M HCl to 65.0 mL of the buffer?

  19. Chemistry

    Which statement describes a chemical reaction at equilibrium? Reactant molecules and product molecules have the same velocity. Molecules of reactants and products collide with the same frequency. The concentrations of reactants and products are equimolar.

  20. chemistry

    If you add 5.0 mL of 0.50 M NaOH solution to 20.0 mL to Buffer C, what is the change in pH of the buffer? (where buffer C is 8.203 g sodium acetate with 100.0 mL of 1.0 M acetic acid) I have calculated the pH of buffer C to be 4.74. Now what? =\

  21. Chemistry

    Calculate the pH of the 0.20 M NH3/0.25 M NH4Cl buffer. I calculated the pH to be 9.15 What is the pH of the buffer after the addition of 10.0 mL of 0.10 M HCl to 72.5 mL of the buffer?

  22. CHEMISTRY

    A buffer that is 0.271 M in acid, HA, and 0.150 M in the potassium salt of its conjugate base, KA, has a pH of 2.85. What is the pH of the buffer after 130. mL of 0.155 M LiOH is added to 0.650 L of this buffer? Assume that the volumes are additive.

  23. chemistry

    To create a 0.1 M carbonate buffer pH = 10.2. You choose to use a combination of HCO3- / CO32-. This buffer system has pKa = 9.9. a) Calculate how much you need to weigh in each of the sodium salts, NaHCO3 and Na2CO3, to create 1.0 L carbonate (with total

  24. Chemistry--need help!

    1. To make a buffer using NH4OH, you must add a. a neutal salt b. you can't use it to make a buffer c. nothing d. its salt 2. Acidosis is a condition where the body fluids are too acidic. If someone with acidosis uses a lot of salt on their food, a. the

  25. Chemistry

    You need to prepare 1.0 L of a buffer with a pH of 9.15. The concentration of the acid in the buffer needs to be 0.100 M. You have available to you a 1.00 M NH4Cl solution, a 6.00 M NaOH solution, and a 6.00 M HCl solution. Determine how to make this

  26. Chemistry

    Describe how a buffer behaves. Your description should include an explanation of why the addition of NaOH to the HAc solution formed a buffer. What happens to the pH when a small quantity of a strong acid or base is added to a buffer solution? What happens

  27. chemistry

    How do you calculate the pH when the following substances are added to a buffer.(all of the solutions are at .10M conc.) The buffer: 50mL NH3 + 50mL NH4NO3 1) 10mL buffer + 6mL water 2)10mL buffer + 5mL water +1mL HCl 3)10mL buffer + 6mL HCl 4)10mL buffer

  28. Chemistry

    c) Now make up 500 mL of a 0.025M phosphate buffer using the 0.1M phosphate buffer. Show all your workings. The 0.1M is made of 120.1ml conjugate base and 379.9ml acid.

  29. Chemistry

    Which of the following accurately shows the correct terms for the two sides of a chemical equation, correctly placed to the left or to the right where they belong, and also shows the correct symbol that is written between them? Choose a,b,c, or d. ** I

  30. chemistry

    wich of the following shows the correct terms for the two sides of a chemical equation correctly placed to the left or right where thay belong an also shows the correct symbol reactants---products products=reactants reactants=sum or sum----reactants please

  31. chemistry

    In protein precipitation, two liters of 5mM buffer solution with pH 5.2 is needed in the isolation of albumin. Which among the buffer solutions is best fitted for the said purpose?justify your answer. a. acetate buffer with pka=4.73? b. tris-aminomethane

  32. chemistry

    Choices: True,False. Select all that are True. The pH at the equivalence point of a weak base with a strong acid is expected to be less than 7 because of the presentce of the conjugated acid in the water. One cannot prepare a buffer from a strong acid and

  33. AP Chemistry

    A buffer, consisting of H2PO4− and HPO42−, helps control the pH of physiological fluids. Many carbonated soft drinks also use this buffer system. What is the pH of a soft drink in which the major buffer ingredients are 7.20 g of NaH2PO4 and 4.90 g of

  34. chem

    how can you tell if two reactants will make a buffer?

  35. chemistry AP

    You have to design a buffer based on one of the systems below System 1: HA1 and A1-1 K= 4 E-3 System 2: HA2 and A2-1 K= 5 E-4 System 3: HA3 and A3-1 K= 6 E-5 For the following parts assume that the buffer above in system2 has been constructed with [HA] =1M

  36. Chemistry

    Find the reactants for the following products: Reactants: Products: NH3(g) + CO2(g) + H2O(l) Reactants: Products: ZnSO4(aq) + Cu(s) Reactants: Products: CuO(s) Reactants: Products: Na+1(aq) + CO3-2(aq) Reactants: Products: SrCO3(s) + NaNO3(aq)

  37. Chemistry

    Consider the following buffer equilibrium: HF (high concentration) + H2O H3O+ (low concentration) + F- ( high concentration) Using Le Chatelier's Principle, explain what happens to the pH of the buffer solution when a small amount of NaOH is added.

  38. Chemistry

    Given the reaction A(g) + B(g) 2AB(g) 1. What does equilibrium mean? -equal mols or pressure between reactants and products? Is there more reactants or products? 2. Will the equilibrium be the same if i started with the reactants only vs if i started with

  39. CHEMISTRY HELP!

    a. According to the Henderson-Hasselbalch equation, how many grams of sodium acetate will you need to add to 125 mL of 0.100 M acetic acid to make a pH=4.74 buffer? (I found this to be 1.025g) I need help with the rest b. What is the actual pH of the

  40. college chem

    a. According to the Henderson-Hasselbalch equation, how many grams of sodium acetate will you need to add to 125 mL of 0.100 M acetic acid to make a pH=4.74 buffer? b. What is the actual pH of the resulting buffer when you add that many grams of sodium

  41. chemistry

    200X buffer is given in class.How much of stock sol and how much distilled water is used to make? a)50 ml of a 1X buffer solution? b)100 ml of a 20X buffer solution? c)10 ml of a 400X solution

  42. Chemistry

    H3PO4 Ka1= 7.5x10^-3 Ka2= 6.2x10^-8 Ka3=4.2x10-^13 Explain how you will make a buffer with a pH of 11.80 using solid Na2HPO4 and either 2.00 M NaOH or 2.00 M HCL. The most concentrated component should have a concentration of 0.50 M, and you need to make

  43. chemistry

    During lab, you are provided with a stock antibody solution (Ab) that has a concentration of 400 μg/μl. For lab, it is necessary make the following dilutions (Fill in the blanks): 5μL of Stock Ab + 195μL of buffer to make a 1:____ dilution at

  44. CHEMISTRY

    I have trouble how to resist pH in buffer solutions ( in acidic buffer , and in basic buffer ) when we add an acid , and a base ! how the reactions in buffer follow Le chatlier's principle ?

  45. chemistry

    Select only the True statements about buffer systems. Select all that are True. 1. Starting with NH3(aq) and adding a small amount of HCl(aq) will make a buffered solution. 2. The blood buffer, among other things, is supported by carbonic acid and its

  46. chemistry

    A buffer is made by combining 3.50 L of 0.200M butylamine, C4H9NH2 with 7.50L of 0.100M butylammonium chloride, C4H9NH3Cl. Assuming that volumes are additive, calculate the following. A) the pH of the buffer. B) the pH of the buffer after the addition of

  47. chemistry

    A buffer is made by combining 3.50 L of 0.200M butylamine, C4H9NH2 with 7.50L of 0.100M butylammonium chloride, C4H9NH3Cl. Assuming that volumes are additive, calculate the following. A) the pH of the buffer. B) the pH of the buffer after the addition of

  48. Biochemistry

    A buffer solution is prepared by mixing 2.50 mL of 2.00M sodium acetate with 3.30mL of 0.500M HCl and diluting the buffer with water to a final volume of 500.0mL. pK acetic acid: 4.76 what is ph of buffer? what is final concentration of buffer?

  49. Chemistry

    500 ml of a buffer solution with ph=2.10 must be prepared using .4 M HNO2 and solid KNO2. The ka value of HNO2 is 4e-3. a.) What mass of KNO2 should be added to 3 L of the HNO2 to make the buffer? b.) What is the buffer's pH after 150 ml of .5 M HNO3 is

  50. college chemistry

    How do you calculate the pH difference when the following substances are added to a buffer.(all of the solutions are at .10M conc.) The buffer: 50mL NH3 + 50mL NH4NO3 1) 10mL buffer + 6mL water 2)10mL buffer + 5mL water +1mL HCl 3)10mL buffer + 6mL HCl

  51. college chemistry

    How do you calculate the pH when the following substances are added to a buffer.(all of the solutions are at .10M conc.) The buffer: 50mL NH3 + 50mL NH4NO3 1) 10mL buffer + 6mL water 2)10mL buffer + 5mL water +1mL HCl 3)10mL buffer + 6mL HCl 4)10mL buffer

  52. Chemistry

    You want to make 1000 ml of an 0.1 M HA buffer so that the pH=pKa of HA. To make this buffer you need to add ____ HA and ____ mL of 1M NaOH and then add enough water to give 1000 mL. HA is a weak acid.

  53. Chemistry

    c) Now make up 500 mL of a 0.025M phosphate buffer using the 0.1M phosphate buffer. Show all your workings. The 0.1M is made of 120.1ml conjugate base and 379.9ml acid.

  54. Chemistry

    Take into account correction factors for phosphate buffers, predict the pH when 0.50ml of 1M HCl is added to 40mL of .10M buffer at expected pH 6 and pH 6.5. The buffer was made with Na2HPO4 and NaH2PO4. pKa is 7.2. When I did this before, I got a lower pH

  55. Chemistry

    What is the Henderson-Hasselbach equation? Use the equation to determine the ratio of [A-] to [HA] necessary to create an ammonium chloride/ammonia buffer with a pH of 8.50. Describe how to make this buffer given a solution of 0.1 M NH3 (aq) and a bottle

  56. biochem

    I need to create a 100ml buffer with a pH of 4.00 using 0.100M Benzoic acid (pKa = 4.20)and 0.180M sodium benzoate. What volume of each material do I need to make this buffer? I think I need to use pH=pKa + log(A/HA)but am not sure if that is correct. Any

  57. chemistry

    If you add 5.0 mL of 0.50 M HCl solution to 20.0 mL to Buffer C, what is the pH of the buffer? (where buffer C is 8.203 g sodium acetate with 100.0 mL of 1.0 M acetic acid)

  58. Biochemistry

    A buffer is made at pH 7.3. 0.15 M using imidazole And 1 M hydrochloric acid to form the buffer. Can you show calculations for the formation of 500 mls of this buffer?

  59. Chemistry

    The pH of a 25.0 mL sample of a buffer changed by one unit when 4.19 mL of 0.24 M HCl was added to it. What is the acid buffer capacity of this buffer?

  60. Chemistry

    You are given an assignment to make 250ml buffer solution having 0.25M weak acid and 0.2M of its conjugate base. You have stock solutions 1.5M acid and 0.5M of the conjugate base. Clearly explain how you are going to make this buffer solution. Can anyone

  61. chemistry

    sorry i will improve my english which is correct of this equation reactants---products products=reactants reactants=sum or sum----reactants i just do not get this

  62. Science

    Sodium is a medal and chlorine is a poisonous gas. Neither is safe to eat. However, when sodium and chlorine is combine, it produces edible table salt. What can be concluded? 1) Table salt has similar physical properties of both reactants. 2)Table salt is

  63. Science~!

    Sodium is a metal and chlorine is a poisonous gas. Neither is safe to eat. However, when sodium and chlorine combine, it produces edible table salt. What can be concluded? (1 point) Table salt has similar physical properties of both reactants.*** Table

  64. science help

    Sodium is a metal and chlorine is a poisonous gas. Neither is safe to eat. However, when sodium and chlorine combine, it produces edible table salt. What can be concluded? A. Table salt has similar physical properties of both reactants. B. Table salt is a

  65. Chemistry

    A pH = 7.6 buffer is needed in the lab. This buffer is made by first dissolving 17.42 g K2HPO4 in 600 mL of water. What is the pH of this salt solution? This solution of course will be too basic becuase we only have the base of the buffer present. What

  66. AP Chemistry

    We're doing a lab in my class and we're supposed to make a buffer at a certain pH. I have decided to make a buffer with a pH of 5.0 using glacial acetic acid (pure CH3COOH) and sodium acetate. I found that the ratio of acid to base is 1.41 M: 1.0 M and now

  67. Chemistry

    The acetate buffer were prepared by mixing 0.1 M ch3cooh with 0.1M ch3cooNa in the ratio 8:2 and 2:8. Calculate the resulting ph after the addition of 2mL of 0.1 M HCl to 10 ml of buffer 8:2 and 4ml of 0.1 M NaOH to 10 ml of buffer 8:2.

  68. chemistry

    pls help i need to do this in less than 2 hours :(( A buffer is made up of 250 mL each of 0.43 M KH2PO4 and 0.27 M K2HPO4.(Ka=6.2 x 10-8) Assuming that volumes are additive, calculate the pH of the buffer after addition of 100 mL of 0.8 M NaOH to the

  69. CHEMISTRY

    A buffer that is 0.271 M in acid, HA, and 0.150 M in the potassium salt of its conjugate base, KA, has a pH of 2.85. What is the pH of the buffer after 130. mL of 0.155 M LiOH is added to 0.650 L of this buffer? Assume that the volumes are additive.

  70. chemistry

    prepare a phosphate buffer with pH= 7 from solid NaH2PO4 (pKa =7.21) and Na2HPO4. 1) calculate the ratio of [CB]/[acid] I got the ratio as 0.62 2) calculate the mass of each component required to make 1L of a .1 M buffer solution 3) if the pH is 7.10, how

  71. Chemistry

    How many grams of Na-benzoate (powder) do I need to prepare a buffer with pH = 4.2? How many grams of salt (NaCl) do I need to add to this buffer to make it a saturated solution of the salt? Thanks

  72. chemistry

    is there any way to know if its products or reactants..? The equilibrium constant for the gas phase reaction N2 (g) + 3H2 (g) (2 arrows: one to right, one to left.) 2NH3 (g) is Keq = 4.34 × 10^-3 at 300°C. At equilibrium, __________. A) reactants

  73. chemistry 2

    You are instructed to create 800. mL of a 0.69 M phosphate buffer with a pH of 7.6. You have phosphoric acid and the sodium salts NaH2PO4, Na2HPO4, and Na3PO4 available. what is the molarity needed for the acid component of the buffer?What is the molarity

  74. chemistry

    A reaction with an equilibrium constant Kc = 1.5 x 1021 would consist of which of the following at equilibrium: A. some reactants and products with reactants slightly favored B. essentially all products C. essentially all reactants D. approximately equal

  75. science

    How do i prepare 0.1 ml KH2PO4-KOH buffer, PH 7.4 (20mM)? Deoxyribose (2.8mM) - EDTA (0.1 mM) - H2O2 (1mM) - vaniline10 mM - phosphate buffer pH 6.9 - Phosphate buffer, 20mM - Phosphate buffer 0.1 M (pH 7.4) - Ascorbate (0.1mM). ( please i want the amount

  76. chemistry

    Acetic acid (CH3COOH) has a Ka of 1.8x10^-5. a buffer is to be prepared with a pH of 5.00 from solutions of CH3COOH and sodium acetate (NaCH3COO) of the same concentration. How many mLs of NaCH3COO would have been added to 100 mL of CH3COOH to make the

  77. Chemistry

    You have 800 mL of a 0.050M phosphate buffer, pH 6.5. You need to increase the pH of this buffer to 7.5 by using 6.00M NaOH. Determine the volume of NaOH needed. What will be the final concentration of the buffer?

  78. chemistry

    1L of a buffer composed of acetic acid and sodium acetate has a pH of 4.3. Adding 10mL of 2M sodium hydroxide solution to 100mL of this buffer causes the pH to rise to 4.87. what is the total molarity of the original buffer?

  79. chemistry

    a 2.00l buffer contains 1.00 mol HNO3 mixed with 1.00mol NaNO2 a. write the relevant ionization equation for this buffer. b. determine its pH c. determine the new pH if 1.00g of NaOH is added to the buffer.

  80. chemistry

    a 2.00l buffer contains 1.00 mol HNO3 mixed with 1.00mol NaNO2 a. write the relevant ionization equation for this buffer. b. determine its pH c. determine the new pH if 1.00g of NaOH is added to the buffer

  81. Chemistry

    Buffer capacity is a measure of a buffer solution\'s resistance to changes in pH as strong acid or base is added. Suppose that you have 165 mL of a buffer that is 0.360 M in both benzoic acid (C6H5COOH) and its conjugate base (C6H5COO–). Calculate the

  82. chemistry

    A buffer consists of 0.14 M KHCO3 and 0.61 M K2CO3. Carbonic acid is a dirpotic acid with Ka1= 4.5*10^-7 and Ka2= 4.7*10^-11. a) which Ka value is more important to this buffer b) what is the buffer pH?

  83. Biochemistry

    You wish to make 3 reactions (1 ml each) with the specified amounts of protein. The remainder of each reaction consists entirely of buffer. The source of your protein is a stock solution that has a concentration of 0.5 mg/ml. What is the volume of stock

  84. Chemistry

    Assume you have prepared 100.0 mL of a buffer solution using 0.400 mol of acetic acid (pKa = 4.74) and 0.400 mol of sodium acetate. The pH of this buffer solution is initially 4.74. After preparing this buffer solution, you added 55.0 mL of a 1.10 M NaOH

  85. Chemistry

    Your laboratory supervisor directs you to prepare 500.0 mL of a buffer with a pH of 9.40. You have available all the weak acids and bases listed in your textbook's appendix and the salts of those weak acids and bases. Describe how you could make this

  86. chem

    a buffer is made by adding 150 ml of .595M BaF2 and 0f .500M of HF solution. calculate the pH of this buffer system calculate the pH of this buffer after adding .100 mol Hcl calculate the pH of this buffer after adding .0750 mol Ca(OH)2 ka(HF)= 6.9x10^-4

  87. BIOLOGY

    A reference calls for the use of "one litre of 0.1 molar acetate buffer pH 5.2” Calculate the amounts of sodium acetate and acetic acid required to make up this buffer, given that for acetic acid Ka = 1.8 x 10-5

  88. biology

    You are preparing 500 mL of Denaturation Buffer containing 1.5 M NaCl and 0.5 M NaOH. Your stock solutions are 5 M NaCl and 6 M NaOH. How would you prepare the Denaturation Buffer? Include all of the solutions needed to make the buffer. For Nacl, C1V1=C2V2

  89. Chemistry

    Your laboratory supervisor directs you to prepare 500.0 mL of a buffer with a pH of 9.40. You have available all the weak acids and bases and the salts of those weak acids and bases. Describe how you could make this buffer.

  90. Chemistry

    I'm reviewing for a test and I'm on Le Chatelier's principle. Decreasing the temperature of an exothermic reaction shifts the equilibrium to the right? I understood this weeks ago but now I can't remember. Wouldn't decreasing the temperature cause there to

  91. Chemistry

    Q1: You wish to prepare a buffer solution with pH = 11.10. What volume of 6.0 M HCl would you add to 500 mL of 0.10 M (C2H5)2NH to prepare the buffer? You may assume that the solution’s volume remains constant. Q2: What is the resulting pH when 20 mL of

  92. Chemistry

    Q1: You wish to prepare a buffer solution with pH = 11.10. What volume of 6.0 M HCl would you add to 500 mL of 0.10 M (C2H5)2NH to prepare the buffer? You may assume that the solution’s volume remains constant. Q2: What is the resulting pH when 20 mL of

  93. chemistry

    A buffer is made by adding 0.300 mol HC2H3O2 and 0.300 mol NaC2H3O2 to enough water to make 1.00 L of solution. The pH of the buffer is 4.74 . Calculate the pH of this solution after 0.020 mol of NaOH is added.

  94. Chemistry

    How many moles of conjugate base (Na2HPO4) are present in 40mL of .010M buffer at pH 7.5 vs at pH 6? Buffer was made up of Na2HPO4 and NaH2PO4. pH=pKa +log[A/HA]; pKa=7.2.... When I did the calculations I got the same amount as if it were in a 0.1M buffer

  95. Chemistry

    A buffer is prepared by mixing 0.30 mole of formic acid (HCNO2) and 0.20 mole of sodium formate (NaCHO2) in enough water to make 0.50 liter of solution. Ka of formic acid is 1.7 x 10-4. Calculate the pH of the resulting buffer solution.

  96. Chemistry

    TRUE OR FALSE? 1) A solution that is made out of 1.00mol/L ammonia and 0.50mol/L of ammonium chloride is a basic buffer. 2) The pH at the equivalence point of a weak base with a strong acid is expected to be less than 7 because the acid that is added is

  97. chemistry AP

    You have to design a buffer based on one of the systems below System 1: HA1 and A1-1 K= 4 E-3 System 2: HA2 and A2-1 K= 5 E-4 System 3: HA3 and A3-1 K= 6 E-5 For the following parts assume that the buffer above in system2 has been constructed with [HA] =1M

  98. Chemistry

    A buffer contains the weak acid HA abd its conjugated base A-. The weak acid has a Ka of 1.51 x10^-5 and the buffer has a pH of 4.25. Which statement is true about the relative concentrations of HA and A- in the buffer? A) [HA]>[A-] B) [HA]

  99. AP Chem (Conceptual Questions)

    Hey guys! If you could just please, look over a few of these conceptual problems because I'm pretty confused? (I put what I think is the answer below each question). Thank you for any help in advance!!!! A.Which statement *does not* apply to a

  100. chemistry

    Write down a balanced acid-base reaction given the following reactants Reactants: NaOH(aq) + HCl(aq)

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