Which of the following oxoacids has the smallest value for Ka,1 ? H2TeO3 H2SO3 H2TeO4 H2SeO4...
Which of the following oxoacids has the smallest value for Ka,1 ?
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H2TeO3 |
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H2SO3 |
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H2TeO4 |
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H2SeO4 |
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H2SeO3 |
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H2SO4 |
Which of the following choices is appropriate if you have made an HBrO/NaBrO buffer and the pH is 8.0, and you want to have the buffer with equal amounts of conjugate components. Choose all that apply.
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Add some strong base |
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Add some strong acid |
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Add some weak base |
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Add some weak acid |
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Add some water |
Homework Answers
Add Answer to:
Which of the following oxoacids has the smallest value for
Ka,1 ?
H2TeO3
H2SO3
H2TeO4
H2SeO4...
You work in a chemistry lab, and are asked to prepare 500 mL of a buffer solution with pH-3.20, T...
You work in a chemistry lab, and are asked to prepare 500 mL of a buffer solution with pH-3.20, The weak acid solution concentration in this buffer should be 0.250 M and salt is a solid. The following steps walk you through a step by step process of this preparation. a. Choose the proper weak acids for the buffer solution Table 1. Ionization constant Ka for some weak acids Name Hydrofluoric acid Nitrous acid Fulminic acid Acetic acid Hypochlorous acid...
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...
help with 5 and 6 please 5. Choose the effective pH range of a HF/Naf buffer. For HF, Ka = 3.5 x 10-4 6. If a small...
help with 5 and 6 please
5. Choose the effective pH range of a HF/Naf buffer. For HF, Ka = 3.5 x 10-4 6. If a small amount of a strong acid is added to buffer made up of a weak acid, HA, and the sodium salt of its conjugate base, NaA, the pH of the buffer solution does not change appreciably because a) the Ka of HA is changed. b) the strong acid reacts with Ato give HA, which...
Which of the following statements is NOT true? Select all that apply. Group of answer choices...
Which of the following statements is NOT true? Select all that apply. Group of answer choices a. The concentration of H+ can be determined from the concentration of OH- and the Kw. b. An acid and its conjugate base differ only by one hydroxide ion c. An acid with a Ka > 1 is considered a weak acid d. The conjugate base of a strong acid will be a strong base e. Strong acids are expected to completely ionize in...
Which of the following mixtures does not result in a buffer? A. 25 mL of 0.1M...
Which of the following mixtures does not result
in a buffer?
A. 25 mL of 0.1M NaBrO with 40 mL of 0.2M HBrO
B. 25 mL of 0.1M NaOH with 40 mL of 0.2M HBrO
C. 100 mL of 0.1M HCl with 100 mL of 0.3M NH3
D. 50 mL of 2M NH4Cl with 75 mL of 3M
NH3
E. 25 mL of 0.1M NaOH with 40 mL of 0.2M NH3 (correct
answer)
^ This is how I worked it...
1. What is the pH of a hypoiodous acid/sodium hypoiodite buffer in which the concentration of...
1. What is the pH of a hypoiodous acid/sodium hypoiodite buffer in which the concentration of the weak acid component is 0.129 M and the concentration of the conjugate base is 0.102 M?Ka=2.3E-11. 2. The pH of a hypoiodous acid/sodium hypoiodite buffer in which the concentration of the weak acid component is 0.140 M and the concentration of the conjugate base is 0.070 M is 10.34. Suppose 0.128 g of solid NaOH are added to 100 mL of this buffer...
What is the net ionic equation for the neutralization reaction between a HI with NH3? HI...
What is the net ionic equation for the neutralization reaction between a HI with NH3? HI (aq) + NH3 (aq) ⇌ NH4I (aq), HI (aq) + OH- (aq) ⇌ H2O (l) + I- (aq), H3O+ (aq) + OH- (aq) ⇌ 2 H2O (l) H3O+ (aq) = NH3 (aq) = NH4+ (aq) + H2O (l) Which statement about buffers is NOT true? A buffer can be made by neutralizing some of the weak base in solution by adding a strong acid,...
The acid form of the indicator bromocresol green has ka = 2.0 * 10-5. For which...
The acid form of the indicator bromocresol green has ka = 2.0 * 10-5. For which one of the following types of titrations would bromocresol green be the appropriate indicator? Multiple Choice O strong acid/weak base strong acid/strong base O weak acid/strong base O weak acid/weak base O O None of these choices are correct.
Preparing Buffer Solutions: Calculating the Number of Grams of Conjugate Base Needed Use the table of K values give...
Preparing Buffer Solutions: Calculating the Number of Grams of Conjugate Base Needed Use the table of K values given with this problem to choose the best weak acid to start from for making a buffer that holds the pH of the solution at 8.50. Make your selection so that you maximize the capacity of the buffer. Weak Acid K 1.8 X 10-5 6.5 X 10-5 1.5 X 10-5 You select a 800.0 ml volumetric flask to which you add 8.00...
1. What is the pH of a solution which is 0.025 M in weak base and...
1. What is the pH of a solution which is 0.025 M in weak base and 0.039M in the conjugate weak acid (Ka = 7.1 × 10-6)? 2. A buffer solution is made using a weak acid, HA , that has a pKa of 5 . If the pH of the buffer is 8 , what is the ratio of [A−] to [HA] ? 3.A buffer solution is made using a weak acid, HA . If the pH of the...
You work in a chemistry lab, and are asked to prepare 500 mL of a buffer solution with pH-3.20, The weak acid solution concentration in this buffer should be 0.250 M and salt is a solid. The following steps walk you through a step by step process of this preparation. a. Choose the proper weak acids for the buffer solution Table 1. Ionization constant Ka for some weak acids Name Hydrofluoric acid Nitrous acid Fulminic acid Acetic acid Hypochlorous acid...
help with 5 and 6 please
5. Choose the effective pH range of a HF/Naf buffer. For HF, Ka = 3.5 x 10-4 6. If a small amount of a strong acid is added to buffer made up of a weak acid, HA, and the sodium salt of its conjugate base, NaA, the pH of the buffer solution does not change appreciably because a) the Ka of HA is changed. b) the strong acid reacts with Ato give HA, which...
Which of the following mixtures does not result
in a buffer?
A. 25 mL of 0.1M NaBrO with 40 mL of 0.2M HBrO
B. 25 mL of 0.1M NaOH with 40 mL of 0.2M HBrO
C. 100 mL of 0.1M HCl with 100 mL of 0.3M NH3
D. 50 mL of 2M NH4Cl with 75 mL of 3M
NH3
E. 25 mL of 0.1M NaOH with 40 mL of 0.2M NH3 (correct
answer)
^ This is how I worked it...
The acid form of the indicator bromocresol green has ka = 2.0 * 10-5. For which one of the following types of titrations would bromocresol green be the appropriate indicator? Multiple Choice O strong acid/weak base strong acid/strong base O weak acid/strong base O weak acid/weak base O O None of these choices are correct.
Preparing Buffer Solutions: Calculating the Number of Grams of Conjugate Base Needed Use the table of K values given with this problem to choose the best weak acid to start from for making a buffer that holds the pH of the solution at 8.50. Make your selection so that you maximize the capacity of the buffer. Weak Acid K 1.8 X 10-5 6.5 X 10-5 1.5 X 10-5 You select a 800.0 ml volumetric flask to which you add 8.00...
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