1. The following bases and their conjugate acids (as the chloride salt) are available in the...
1. The following bases and their conjugate acids (as the chloride salt) are available in the lab: ammonia (NH3); pyridine (C5H5N); ethylamine (CH3CH2NH2). You need to make a buffer with a pH of 9 with a total concentration of buffering agents is to be 0.5M. Considering this,
a) Choose the best acid/base pair
b) Give the recipe for preparing 1 L of the solution
c) Calculate the pH after adding 0.02 moles of NaOH to 1L of the solution
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1. The following bases and their conjugate acids (as the
chloride salt) are available in the...
Lab 5 Buffers 1. Dissolved ions in salt solutions can act as acids or bases and...
Lab 5 Buffers 1. Dissolved ions in salt solutions can act as acids or bases and react with water to produce hydronium ions or hydroxide ions that contribute to the pH of the salt solution. Since strong acids and strong bases completely ionize in solution, the reverse reaction essentially does not occur, meaning that the resulting conjugate base of a strong acid or conjugate acid of a strong base do NOT act as acids or bases. Ions that are conjugate...
1. Label the acids, bases, conjugate acids, and conjugate bases in the reactions below: a. Na2CO3(aq)...
1. Label the acids, bases, conjugate acids, and conjugate bases in the reactions below: a. Na2CO3(aq) + 2 HCl (aq) H2CO, (aq) + 2 NaCl (aq) b. NH” (aq) + CN + NH3 (aq) + HCN (aq) c. Na2HPO4 (aq) + NaOH(aq) - Na PO. (aq) + H20 (1) d. H2O(l) + NaH (s) H2(g) + NaOH(aq) 2. Calculate the pH of the following solutions: a. [H,O') = 4.5 x 10° b. 12 M HCl C. 0.13 M NaOH d....
The following shows a list of weak acids and bases with their Ka and Kb values....
The following shows a list of weak acids and bases with their Ka and Kb values. Substances Ka Substances Kb Cyanic acid (HCN) 4.9 x 10-10 Ammonia (NH3) 1.8 x 10-5 Nitrous acid (HNO2) 4.5 x 10-4 Aniline (C6H5NH2) 4.3 x 10-10 Hydrofluoric acid (HF) 6.8 x 10-4 Pyridine (C5H5N) 1.7 x 10-9 Acetic acid (CH3COOH) 1.8 x 10-5 Methylamine (CH3NH2) 4.4 x 10-4 If you want to make a pH 8.0 buffer solution, which of the following acids or...
Lab 8: Acids and Bases: Fill in these tables Acid Base Conjugate Acid HNO2 H2O HF...
Lab 8: Acids and Bases: Fill in these tables Acid Base Conjugate Acid HNO2 H2O HF H₂O HO" Conjugate Base Balanced Reaction HNO3 + H2O → NO,' + H2O F NH3 + HCN » NH+ CNC HCI NaOH H, O CIO, Which of the above could you make a buffer with? (using the Kor Na salt of the conjugate base of course) | (ОН) pH [H30] 2.5 x 100M Acidic, Basic or Neutral? 3.6 x 10M
Consider the following table: Name Formula Conjugate Acid Ammonia NH3 ΝΗ, Methylamine CH3NH2 CH, NH3 +...
Consider the following table: Name Formula Conjugate Acid Ammonia NH3 ΝΗ, Methylamine CH3NH2 CH, NH3 + Ethylamine C2H5NH2 C,HNH3 Aniline CH NH2 CH3NH, Pyridinem CH N CH NH Kb 1.8 x 10-5 4.38 x 10-4 5.6 x 10-4 3.8 x 10-10 1.7 x 10-9 Which base would be the best choice for preparing a pH = 9.50 buffer? methylamine pyridine ethylamine aniline ammonia
Preparing Buffer Solutions: Calculating the Volume of Weak Base Needed Use the table of K values ...
Preparing Buffer Solutions: Calculating the Volume of Weak Base Needed Use the table of K values given with this problem to choose the best weak base to start from for making a buffer that holds the pH of the solution at 5.00. Make your selection so that you maximize the capacity of the buffer. Assume that you want to make 700 mL of a buffer and you have already added enough of the conjugate acid salt to make the final...
Consider the following data on some weak acids and weak bases: acid Ka name formula hypochlorous...
Consider the following data on some weak acids and weak bases: acid Ka name formula hypochlorous acid HClO ×3.010−8 hydrofluoric acid HF ×6.810−4 base Kb name formula pyridine C5H5N ×1.710−9 ammonia NH3 ×1.810−5 Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. solution Ph...
Buffers are solutions designed to resist changes in pH from the addition of small amounts of acids or bases
Buffers are solutions designed to resist changes in pH from the addition of small amounts of acids or bases. Buffers are comprised of a solution of a weak acid with its conjugate base. When an outside base is added to the buffer, the weak acid in the buffer neutralizes the hydroxide ion of the base, thus retarding its ability to raise the solution's pH. When an outside acid is added to the buffer, the conjugate base of the buffer neutralizes...
Determining Ionic StrengthUnlike strong acids and bases that ionize completely in solution, weak acids...
Determining Ionic StrengthUnlike strong acids and bases that ionize completely in solution, weak acids or bases partially ionize. The tendency to ionize (i.e., the ionic strength) of a weak acid or base can be quantified in several ways includingKa or Kb,pKa or pKb,and percent ionization.Part APyridine is a weak base that is used in the manufacture of pesticides and plastic resins. It is also a component of cigarette smoke. Pyridine ionizes in water as follows:C5H5N+H2O?C5H5NH++OH?The pKb of pyridine is 8.75....
A buffer solution contains 0.229 M ammonium chloride and 0.457 M ammonia. If 0.0568 moles of...
A buffer solution contains 0.229 M ammonium chloride and 0.457 M ammonia. If 0.0568 moles of hydroiodic acid are added to 250 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume does not change upon adding hydroiodic acid) pH = Submit Answer Retry Entire Group 9 more group attempts remaining A buffer solution contains 0.443 M ammonium chloride and 0.314 M ammonia. If 0.0313 moles of potassium hydroxide are added to 225...
1. Label the acids, bases, conjugate acids, and conjugate bases in the reactions below: a. Na2CO3(aq) + 2 HCl (aq) H2CO, (aq) + 2 NaCl (aq) b. NH” (aq) + CN + NH3 (aq) + HCN (aq) c. Na2HPO4 (aq) + NaOH(aq) - Na PO. (aq) + H20 (1) d. H2O(l) + NaH (s) H2(g) + NaOH(aq) 2. Calculate the pH of the following solutions: a. [H,O') = 4.5 x 10° b. 12 M HCl C. 0.13 M NaOH d....
Lab 8: Acids and Bases: Fill in these tables Acid Base Conjugate Acid HNO2 H2O HF H₂O HO" Conjugate Base Balanced Reaction HNO3 + H2O → NO,' + H2O F NH3 + HCN » NH+ CNC HCI NaOH H, O CIO, Which of the above could you make a buffer with? (using the Kor Na salt of the conjugate base of course) | (ОН) pH [H30] 2.5 x 100M Acidic, Basic or Neutral? 3.6 x 10M
Consider the following table: Name Formula Conjugate Acid Ammonia NH3 ΝΗ, Methylamine CH3NH2 CH, NH3 + Ethylamine C2H5NH2 C,HNH3 Aniline CH NH2 CH3NH, Pyridinem CH N CH NH Kb 1.8 x 10-5 4.38 x 10-4 5.6 x 10-4 3.8 x 10-10 1.7 x 10-9 Which base would be the best choice for preparing a pH = 9.50 buffer? methylamine pyridine ethylamine aniline ammonia
Preparing Buffer Solutions: Calculating the Volume of Weak Base Needed Use the table of K values given with this problem to choose the best weak base to start from for making a buffer that holds the pH of the solution at 5.00. Make your selection so that you maximize the capacity of the buffer. Assume that you want to make 700 mL of a buffer and you have already added enough of the conjugate acid salt to make the final...
A buffer solution contains 0.229 M ammonium chloride and 0.457 M ammonia. If 0.0568 moles of hydroiodic acid are added to 250 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume does not change upon adding hydroiodic acid) pH = Submit Answer Retry Entire Group 9 more group attempts remaining A buffer solution contains 0.443 M ammonium chloride and 0.314 M ammonia. If 0.0313 moles of potassium hydroxide are added to 225...
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