Which of the following aqueous solutions are good buffer systems ? . 0.26 M hydrochloric acid + 0.24 M potassium chloride . 0.14 M acetic acid + 0.20 M potassium acetate . 0.16 M potassium hypochlorite + 0.23 M hypochlorous

29,310 results
  1. 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

  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

    Aqueous sulfurous acid H2SO3 and aqueous sodium chloride are formed by the reaction of aqueous sodium sulfite Na2SO3 and aqueous hydrochloric acid HCl . Write a balanced chemical equation for this reaction.

  4. 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

  5. Chemistry

    Write a balanced equation: Aluminum reacts with aqueous hydrochloric acid to form hydrogen gas and aqueous aluminum chloride. I think: Al+HCl(aq)-->H(g)AlCl(aq) But I don't really know if I am doing it right or not

  6. chem

    Aqueous sodium chloride and aqueous sulfurous acid are formed by the reaction of aqueous sodium sulfite and aqueous hydrochloric acid . write the balanced equation?

  7. chem

    What mass of hydrochloric acid (in grams) can be neutralized by 2.3g of sodium bicarbonate? (: Begin by writing a balanced equation for the reaction between aqueous sodium bicarbonate and aqueous hydrochloric acid.)

  8. chem

    Which of the following could be added to a solution of sodium acetate to produce a buffer? ? A) acetic acid only B) acetic acid or hydrochloric acid C) potassium acetate only D) sodium chloride or potassium acetate E) hydrochloric acid only i knowt he

  9. Chem--buffers

    Explain why a mixture formed by mixing 100 mL of 0.100M CH3COOH and 50 mL of 0.100M NaOH will act as a buffer? in adittion to this, how do you identify if a an aqueous solution is a buffer solution, such as a solution with an acid and a base, but no common

  10. CHEM

    Which reactants could be used safely to prepare potassium chloride? 1. aqueous potassium hydroxide and dilute hydrochloric acid 2. aqueous potassium sulphate and aqueous sodium chloride 3. potassium and aqueous sodium chloride The answer is 1, but i don't

  11. Chemistry - pH

    Calculate the pH of each of the following solutions: a) .35 M hydrochloric acid, HCl b) .35 M acetic acid, HC2H3O2 c) .35 M sodium hydroxide, NaOH Can someone please explain to me how to calculate the pH in a way that is easy to understand? I am confused.

  12. Chemistry

    1.06g of sodium trioxocarbonate(iv) reacted with excess dilute 0.1M hydrochloric acid, after the reaction, the unreacted acid required 24cm3 of 0.1M sodium hydroxide for its complete neutralization. Calculate the original volume of the hydrochloric acid

  13. Chemistry

    Which of the following aqueous solutions are good buffer systems ? . 0.26 M hydrochloric acid + 0.24 M potassium chloride . 0.14 M acetic acid + 0.20 M potassium acetate . 0.16 M potassium hypochlorite + 0.23 M hypochlorous acid . 0.31 M hydrocyanic acid +

  14. 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

  15. chemistry (buffers)

    How can weak acid nitrous acid HNO2 form a buffer solution with equal concentrations and volumes with weak base NH3? I thought that buffer solutions only occured between weak acids and strong bases or vice versa. The example above as two weak soltuions.

  16. Chemistry 12

    15. The concentration of hydroxide ions in a solution of nitric acid 0.2 M is: a. 2 x 10-14 M b. 5 x 10-14 M c. 5 x 10-7 M d. 2 x 10-1 M 16. Aqueous solutions of strong acids and strong bases: a. are good electricity conductors b. make litmus paper become

  17. College Algebra

    How many liters of 80% hydrochloric acid must be mixed with 40% hydrochloric acid to get 15 liters of 65% hydrochloric acid? Write your answer rounded to three decimals. Show all work.

  18. 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

  19. 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? =\

  20. Chemistry

    Please help me Sketch a separation scheme showing how you would separate the following two component mixture: m-nitroaniline and hexanol. All the substances are soluble in ether. You can use any of the following solutions in your separation: aqueous

  21. 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

  22. chemistry

    An aqueous solution is 40.0% by mass hydrochloric acid, HCl, and has a density of 1.20 g/mL. The molality of hydrochloric acid in the solution is m.

  23. Chemistry

    Which one of the following pairs of 0.100 mol L-1 solutions, when mixed, will produce a buffer solution? A. 50. mL of aqueous CH3COOH and 25. mL of aqueous CH3COONa B. 50. mL of aqueous CH3COOH and 25. mL of aqueous HCl C. 50. mL of aqueous NaOH and 25. mL

  24. chemistry

    If you need to prepare 250.0 mL of a pH 5.00 buffer tha t has a total buffer concentration of acetic acid + sodium acetate of 0.050 M, how many moles of each will you need to prepare the solution? Given solutions of acetic acid and sodium acetate with

  25. chemistry

    When aqueous solutions of potassium hypochlorite and nitric acid are mixed, an aqueous solution of potassium nitrate and hypochlorous acid results. Write the net ionic equation for the reaction. Use H+ for the hydronium ion.

  26. Chemistry

    I have a 1L solution of 0.02M sodium acetate and 0.02M acetic acid. What is the pH after the addition of 0.05 moles of hydrochloric acid? I know this is a buffer question but I have no idea how I am supposed to go about getting the answer... I know Ka

  27. 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

  28. calculus

    Solve the system by the method of your choice. Identify systems with no solutions and systems with infinitely many solutions, using set notation to express their solutions: x + y = 3 -2 + y = -3 (0 ,-5) (0 , 0) (-2 ,-1) (-2,-3)

  29. Chemistry

    Addition of which of the following substances will increase the solubility of CuCO3 (s) in water ? CuCO3 ---- Cu^2+ (aq) +2 CO3^2- (aq) 1. Aqueous hydrochloric acid 2. Aqueous sodium carbonate 3. Solid copper (II) carbonate a) 1 only b) 2 only c) 3 only d)

  30. Chemistry

    1. Calculate the pH of a buffer solution that contains 0.32 M benzoic acid (C6H5CO2H) and 0.17 M sodium benzoate (C6H5COONa). [Ka = 6.5 × 10-5 for benzoic acid] Round your answer to two places past the decimal. 2. A solution is prepared by mixing 470 mL

  31. Chemistry

    250-mL volumetric flask, 125 mL of a 6.0 M hydrochloric acid was added. This was then diluted with more water to reach the 250-mL mark. What is the molarity of the acid at this time? Initial: M1 = 6.0 M hydrochloric acid V1 = 125 mL = 0.125 L Diluted: M2 =

  32. 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]

  33. Chemistry

    What mass of hydrochloric acid (in grams) can be neutralized by 2.3g of sodium bicarbonate(Hint: Begin by writing a balanced equation for the reaction between aqueous sodium bicarbonate and aqueous hydrochloric acid.)

  34. 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?

  35. MATH

    Jenny is running an experiment for organic chemistry class. She needs exactly 100 ml of 70% hydrochloric acid, but the lab only has 90% and 40% solutions. How much of each solutions does she need to mix in order to obtain 100 ml of 70% hydrochloric acid

  36. Chemistry

    A buffer solution is made as followed: i)adding 13.50mL of 0.200mol/L sodium hydroxide to 50.00mL of 0.100mol/L propanoic acid. ii)diluting the resulted buffer into a total volume of 100.00mL Using IRE-C tables (if possible) calculate: a)The pH of the

  37. 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 ?

  38. chemistry

    acetic acid: 0.1 M 30ml hydrochloric acid 0.1 M 5 ml sodium hydroxide 0.1 M 15 ml Buffer + 5ml of: 1.91 ph ph (measured): 4:52 ph HOW DO I CALCULATE PH(CALCULATED)? AND ALSO IT SAYS SHOW YOUR CALCULATION FOR THE PH OF THE BUFFER BEFIRE AND AFTER THE

  39. Chemistry

    Predict whether the Ph endpoint is =7 >7, or

  40. chemistry

    An aqueous solution contains 0.445 M ethylamine (C2H5NH2). How many mL of 0.226 M hydrochloric acid would have to be added to 150 mL of this solution in order to prepare a buffer with a pH of 10.200

  41. CHEMISTRY

    In a study of the reaction of magnesium with hydrochloric acid, two experiments were carried out. Each uses 1 g of magnesium ribbon, and 50 mL of hydrochloric acid was added to each reaction flask. One of the hydrochloric acid solutions added was more

  42. Chemistry 101

    Write the molecular, total ionic, and net ionic, for the reaction. 1). Aqueous sodium carbonate is reacted with aqueous nickle (11) chloride. 2). Aqueous potassium hydroxide is mixed with aqueous hydrochloric acid.

  43. Chemistry- HW Check

    I have seven homework problems. I did them but I wasn't sure if I did them correctly. Did I do them correct? Thank you! Give the reaction that describes how the hydrazine, N2H4(aq), / hydrazinium ion, N2H51+(aq), buffer reacts with a strong base such as

  44. chemistry

    #1)hydrochloric acid is a relatively strong acid . imagine that HCl is added to a buffer solution containing the weak acid phosphoric acid and a salt a)will HCl react with weak acid (H3PO4), or will it react with the salt (Na2HPO4)? b)one product of this

  45. Chemistry Help

    You are required to make 500 mL of a buffer solution with pH = 5.0 and a total acetate concentration of 0.1000 M. You are supplied with solid sodium actetate (CH3COONa) and 2.00 M hydrochloric acid. What mass of sodium acetate and what volume of

  46. Chemistry

    Rank the following solutions in order of increasing acidity. 1 M phenol 1 M boric acid 1 M cyanic acid 1 M formic acid 1 M hydrochloric acid 2. Rank the following solutions in order of increasing basicity. 1 M C3H5O3Na 1 M KF 1 M KOCN 1 M KOCl All I know

  47. chemistry

    Solutions of acetic acid and hydrochloric acid of the same concentration are not equally acidic. Which of the two solutions has a lower pH? Why?

  48. Chemistry

    Determine the pH of the following solutions: a) A 250.0 mL solution that contains 0.125 M benzoic acid and 0.147 M sodium benzoate. b) The solution in part (a) after 30.0 mL of 0.510 M hydrochloric acid has been added. a. Ka = 6.3 x 10^-5 pKa = 4.20 pH =

  49. stomach

    Under certain abnormal conditions, the stomach does not secrete hydrochloric acid. Identify three functions that hydrochloric acid has in the digestive process and describe how the failure to secrete hydrochloric acid will affect these processes.

  50. 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

  51. Chemistry

    14.6 mL of hydrochloric acid is completely neutralized by 25.0 mL of 1.40 M sodium hydroxide, what was the hydrochloric acid mass percent (m/m) before the titration? (Density of hydrochloric acid is 1.02 g/cm3)

  52. Chemistry

    Which of the following is an example of a physical change ? A) Zinc metal is added to hydrochloric acid and a gas is released. B) Concentrated hydrochloric acid is diluted with water. C) Acid rain causes the decomposition of a marble statue. D)

  53. Chemistry

    A buffer was prepared by dissolving 22.61g of NaCLO2 into 0.100L of 4.00M aqueous HCLO2. Calculate the pH of the original Chlorous acid/chlorite ion buffer. Ka= 1.1 x 10^-2.

  54. Chem

    If you need to prepare 250.0 mL of a pH 5.00 buffer tha t has a total buffer concentration of acetic acid + sodium acetate of 0.050 M, how many moles of each will you need to prepare the solution? Given solutions of acetic acid and sodium acetate with

  55. Chemistry 122

    A solution is prepared to be 0.10 M acetic acid, HC2H3O2, and 0.20 M sodium acetate, NaC2H3O2. What is the pH of this buffer? Ka for acetic acid is 1.7 x 10^-5. What is the pH after 9.5 mL of 0.10 M hydrochloric acid is added?

  56. 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

  57. chem

    If 0.752 g of pure sodium carbonate was dissolved in water and the solution titrated with 25.90 mL of hydrochloric acid to a methyl orange end point, calculate the molarity of the hydrochloric acid solution. (Hint: This process takes the carbonate ion to

  58. chemistry

    what will be the pH of a 100mL buffer solution containing 0.064 M of acetic acid and 0.036M f sodium acetate, after addition of 1 millimole of the hydrochloric acid? pka=4.75

  59. chemistry

    Propionic acid has a ka of 1.3x10^(-5), 50.0ml of a buffer solution having a pH of 4.65 is to be prepared using a 0.20 M solutions of propionic acid and sodium propionate. How many ml of each of these solutions must be mixed? Thanks in Advanced !

  60. Chemistry

    If you need to prepare 250.0 mL of a pH 5.00 buffer that has a total buffer concentration of acetic acid + sodium acetate of 0.050M, how many moles of each will you need to prepare the solution? Given solutions of acetic acid and sodium acetate with

  61. Chemistry

    What volume of 0.200M of aqueous solution of formic acid, a weak monoprotic acid (KA = 1.78x10-4) and 0.200M aqueous solution of NaOH would you mix to prepare a 500mL of a buffer solution of pH = 4.0.

  62. Chem Lab Help

    You are provided with 5 M solutions of sodium hydroxide and hydrochloric acid for use in this experiment (Separation). How you would have prepared these solutions. Thanks!

  63. Chem Help Please!

    You are provided with 5 M solutions of sodium hydroxide and hydrochloric acid for use in this experiment (Separation). How you would have prepared these solutions. Thanks!

  64. Chemistry

    Assignment  Calculate the pH, pOH, [H+], and [OH] for each of the following solutions. Show all work. (10 Points) Solution Composition of Starting Materials 1 0.10 M acetic acid 2. 5 mL 0.10 M acetic acid + 5 mL wa 3 1 mL 0.10 M acetic acid + 99 mL

  65. chemistry

    I have many questions. I have a test tuesday and need to get these problems done and understand them today because i am currently studying. I am in college and my professor has not emailed me back regarding solutions for the review problems she posted. Is

  66. Chemistry

    How many moles of hydrochloric acid (pKa of HF=3.14) must be added to 500.0 mL of 0.30M sodium fluoride (NaF) to give a buffer of pH 3.50? Ignore the volume change due to the addition of hdrofluoric acid

  67. analytical chemistry

    a buffer solution is 0.2M in acetic acid and in sodium acetate. Calculate the change in pH upon adding 1.0ml of 0.1M hydrochloric acid to 10ml of this solution.(Given pKA of acetic acid is 4.76)

  68. Biology

    What is the biological importance of what you observed? I observed different solutions pH levels (like water, skim milk, phosphate buffer, etc) before and after adding acid. I also observed different antacid solutions (alka-seltzer, tums, etc) to see how

  69. Chemistry

    What volume of 0.200M of aqueous solution of formic acid, a weak monoprotic acid (KA = 1.78x10-4) and 0.200M aqueous solution of NaOH would you mix to prepare a 500mL of a buffer solution of pH = 4.0. I know I need to use the H-H equation, I'm just not

  70. calculus

    Solve the system by the method of your choice. Identify systems with no solutions and systems with infinitely many solutions, using set notation to express their solutions: (0 ,-5) (0 , 0) (-2 ,-1) (-2,-3)

  71. chemistry

    I need 1L of a pH 4 buffer with a total molarity of 1. Propose a buffer system and a recipe to achieve this goal. (acetic acid/acetate would probably be a good choice.) help please!

  72. chemistry

    I need 1L of a pH 4 buffer with a total molarity of 1. Propose a buffer system and a recipe to achieve this goal. (acetic acid/acetate would probably be a good choice.) help please!

  73. chemistry

    I need 1L of a pH 4 buffer with a total molarity of 1. Propose a buffer system and a recipe to achieve this goal. (acetic acid/acetate would probably be a good choice.) help please!

  74. Chemistry

    IN the polystyrene beaker, mix 20mL of 0.1 M Acetic acid and 25mL of 0.1M Sodium Acetate and immediately measure the pH. Remove the electrode and add 5ml of 0.1 M HCl to this buffer. Stir the solution and measure the pH. _______________ INFO: concentration

  75. 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?

  76. Chemistry

    An aqueous solution contains 0.196 M hydrosulfuric acid and 0.190 M hydrochloric acid. Calculate the sulfide ion concentration in this solution. [S2-] = _________mol/L.

  77. Chemistry

    1. Calculate the pH of a buffer solution that contains 0.32 M benzoic acid (C6H5CO2H) and 0.17 M sodium benzoate (C6H5COONa). [Ka = 6.5 × 10-5 for benzoic acid] Round your answer to two places past the decimal. 2. A solution is prepared by mixing 470 mL

  78. chemistry

    Calculate the pH of a [Acid] M aqueous solution of each of the hydrochloric and acetic acids: Acid [Acid] pH HCl 0.10 HC2H3O2 0.10 I know that HCl is just -log(0.10) which is 1, but can't get the pH of HC2H3O2.

  79. Chemistry

    If you had one gallon of concentrated hydrochloric acid (12 N) and added water to make dilute hydrochloric acid (6 N), how much dilute hydrochloric acid would you have?

  80. Pharmacy Math

    A prescription calls for 250ml of a 0.1N hydrochloric acid HCL solution. How many ml of concentrated hydrochloric acid are needed to make this solution? The specific gravity hydrochloric acid is 1.18 the molecular weight is 36.46 and the concentration is

  81. chemistry

    Write a balanced chemical equation for the neutralization reaction between aqueous hydrochloric acid and aqueous calcium hydroxide. Be sure the formulas are written correctly before balancing, and include phases. HCl+H2CaO2 im not sure that's written

  82. chemisty

    When magnesium metal and an aqueous solution of hydrochloric acid combine, they produce an aqueous solution of magnesium chloride and hydrogen gas. Using the equation, Mg (s) + 2HCl (aq) MgCl2 (aq) + H2 (g), if 24.3 g of Mg and 75.0 g of HCl are allowed to

  83. chemistry

    When magnesium metal and an aqueous solution of hydrochloric acid combine, they produce an aqueous solution of magnesium chloride and hydrogen gas. Using the equation, Mg (s) + 2HCl (aq) → MgCl2 (aq) + H2 (g), if 48.6 g of Mg and 150.0 g of HCl are

  84. chem 2

    which one of the following pairs of 0.100 mol L-1 solutions, when mixed will produce a buffer solution? a 50. mL of aquesous CH3COOH and 25.mL of aquesous HCI b 50. mL of quesous CH3COOH and 100. mL of aqueous NaOH c 50. mL of aquesous NaOH and 25. mL of

  85. Chemistry

    1.)An ammonia/ammonium buffer solution contains 0.35 M NH3 and 0.72 M NH4+. The Kb value of ammonia is 1.8×10−5. Calculate the pH of this buffer. 2.) Nitrous acid has a Ka of 4.5×10−4. What is the pH of a buffer solution containing 0.15 M HNO2 and

  86. 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

  87. Chemistry

    I'm not sure how to do these...I keep getting the wrong answers... Please help someone... Mg(s) + 2 HCl(aq)= MgCl2 (aq) + H2(g) a. What volume of 15.7 M hydrochloric acid will react with 2.1 grams of Mg? b. What mass of magnesium will react with 8.5 liters

  88. chem

    A sewage cleanser contains concentrated hydrochloric acid (HCl) as the active ingredient. A titration experiment was carried out to determine the concentration of hydrochloric acid in the domestic cleanser. 25.0 mL of the cleanser were diluted to 250.0 mL

  89. Chemistry

    I did an experiment on Buffers: In a polystyrene beaker, mix 20 ml of 0.1M Acetic acid ad 25 ml of 0.1 M sodium acetate and immediately measure the pH. Remove the electrode and add 5 ml of 0.1 M HCL to this buffer. Stir the solution and measure the pH.

  90. 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

  91. 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

  92. chemistry

    what makes a good buffer? is it that it has a strong base and a strong acid? and why is blood a good buffer? is that because the oxygen it carries acts as a strong base?

  93. chemistry

    Hydrochloric acid solution reacts with zinc according to the following equation: 2H3O + Zn -> Zn^2+ + H2 +2H2O 100ml of hydrochloric acid solution Ca=0.5mol/l must be prepared from C=5mol/l hydrochloric solution. 1) Specify the glassware needed for this

  94. BioChem

    1.Suppose you had a buffer containing 0.5 moles of sodium monobasic phosphate and 0.5 moles of sodium dibasic phosphate. How many moles of hydrochloric acid would this phosphate buffer be able to accept before the pH of the solution began to change

  95. CHEMISTRY

    USING EQUATION SHOW HOW AQUEOUS SOLUTION OF HYDROCHLORIC ACID CONTAINING HYDROXONIUM ION NEUTRALISED POTASSIUM HYDROXIDE

  96. Chemistry

    The pH of a buffer can be predicted using the Hendersen-Hasselbach equation: pH=pKa+ log([conjugate base][conjugate acid]) The choice of the conjugate acid-base pair (as you did in the previous questions) determines the pKa value to be used in the H-H

  97. science

    write word equations and balanced chemical equations for each of the following reactions: a)calcium bicarbonate reacts with hydrochloric acid. b)magnesium hydroxide reacts with hydrochloric acid. c)Aluminum hydroxide reacts with hydrochloric acid.

  98. Chemistry

    An aqueous solution contains 0.216 M ascorbic acid (H2C6H6O6) and 0.131 M hydrochloric acid. Calculate the ascorbate (C6H6O62-) ion concentration in this solution. [C6H6O62-] =______________ mol/L.

  99. Chemitry

    Consider the neutralization reaction that takes place when hydrochloric acid reacts with aqueous calcium hydroxide Write a conversion factor that relates moles of hydrochloric to moles of calcium hydroxide for this reaction

  100. chemistry

    A student mixes four reagents together, thinking that the solutions will neutralize each other. The solutions mixed together are 50.0 mL of 0.100 M hydrochloric acid, 100.0 mL of 0.200 M of nintric acid,500. mL of 0.0100 M calcium hydroxide, and 200.0 mL

Pages

  1. 1
  2. 2
  3. 3
  4. 4
  5. 5
  6. 6
  7. 7
  8. 8
  9. 9
  10. 10
  11. 11
  12. 12
  13. 13
  14. 14
  15. 15
  16. 16
  17. 17
  18. 18
  19. 19
  20. 20