Which of the following statements is true of weak acids dissolved in water:
They are completely ionized in water
They are totally unionized in water
They are partially ionized in water
The dissociation constant is a function of pH
QUESTION 13
Which of the following is a hydroxide ion?
H3O+
OH-
HOOH
CH3OH2+
QUESTION 14
The following molecule is an example of which class of compounds? CH3CH2CH2COOH
Hydrocarbon
Acid
Alcohol
Aldehyde
QUESTION 15
Which of the following would not form a suitable buffer?
Acetic acid/ acetate (pKa 4.76)
Carbonic acid/ bicarbonate (pKa 3.6)
Bicarbonate/ carbonate (pKa 10.3)
Hydrochloric acid/ chloride (pKa -6.3)
1 points
QUESTION 16
How many grams of NaCl in 10 liter to make a 0.834 M solution (NaCl MW = 58.44 g / mol)?
487
QUESTION 17
The pH of a solution that is 0.25 molar in acetic acid and 0.1 molar in sodium acetate is 4.36. What is the pKa of acetic acid?
4.36
4.76
7.76
3.76
QUESTION 18
Malate dehydrogenase converts Malate to oxaloacetate in the citric acid cycle. If the ratio of products/reactants was 1/1,000,000 in this reaction in a cell, and the standard free energy change (ΔG°’) for the reaction is 29.7 kJ mole-1, what is the ΔG?
-5.6 kJ mole-1
5.6 kJ mole-1
-4.8 kJ mole-1
4.8 kJ mole-1
None of the above
QUESTION 19
What is the pH of a solution where the concentration of hydrogen ions is 2 x 10-5 molar?
5
2.5
4.7
9
QUESTION 20
Bromine is one of the few elements that exists as a liquid at room temperature. At what temperature (in K) would this reaction Br2 (l) à Br2 (g) be at equilibrium. Given that at room temperature (298 K), DH = 30.91 kJ/mol, DG = 3.13 kJ/mol and DS = 0.0932 mol.K
298 K
364 K
253 K
331 K
Which of the following statements is true of weak acids dissolved in water: They...
What concentrations of acetic acid (pKa=4.76)(pKa=4.76) and acetate would be required to prepare a 0.10 M0.10 M buffer solution at pH 4.6pH 4.6? Note that the concentration, pH value, or both may differ from that in the first question. Strategy Rearrange the Henderson–Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid), [A−]/[HA][A−]/[HA] . Use the mole fraction of acetate to calculate the concentration of acetate. Calculate the concentration of acetic acid. Step 1: The ratio...
What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.10 M buffer solution at pH 4.9? Note that the concentration and/or pH value may differ from that in the first question. 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid), [A^-]/[HA]. 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate the concentration of acetic acid. That is, there are...
What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.20 M buffer solution at pH 5.0? Note that the concentration, pH value, or both may differ from that in the first question. Strategy 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid). [A-V[HA). 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate the concentration of acetic acid. Step 1:...
Given 1 M solutions of acetic acid and sodium acetate, and distilled water, describe the preparation of 1 L of 0.1 M acetate buffer at pH = 5.4. The relevant pKa is 4.76.
500 mg of sodium acetate is dissolved in 500.0 mL of de-ionized water. Calculate the pH of this solution. MM(sodium acetate) = 82.0324 g/mol, Ka(acetic acid) = 1.75 x 10-5
what concentration of acetic acid (pka=4.76) and acetate would be required to prepare a .15 M buffer solution at pH 5.0? What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.15 M buffer solution at pH 5.07 Note that the concentration, the pH, or both values may differ from that in the first question. Strategy 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid). (AVHA)....
when a 7.00 g sample of KSCN is dissolved in water in a calorimeter that has a total he capacity of 4.36 kJ. K^-1, the temperature decreases by .400 K. calculate the molar heat of solution of KSCN. Resources Give Up?9 When a 7.00 g sample of KSCN is dissolved in water in a calorimeter that has a total heat capacity of 4.36 kJ .K-, the decreases by 0.400 K. Calculate the molar heat of solution of KSCN kJ/mol TOOLS...
What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.15 M buffer solution at pH 4.9? Note that the concentration and/or pH value may differ from that m the first question. STRATEGY 1. Rearrange the Hendereon-Hasselbalch equation to solve for thfe rabo of base (acetate) to aad (acetic add).[A^-]/[HA]. 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate the concentration ot acetic acid.
4. What molar ratio of HPO4 2-to H2PO4-in solution would produce a pH of 7.0? Phosphoric acid (H3PO4), a triprotic acid, has 3 pKa values: 2.14, 6.86, and 12.4. Hint: Only one of the pKa values is relevant here. 5. For a weak acid with a pKaof 6.0, calculate the ratio of conjugate base to acid at a pH of 5.0. 6. Which of these compounds would be the best buffer at pH 5.0: formic acid (pKa 3.8), acetic acid...
4. A solution is made by dissolving 15.00 grams of acetic acid and 3.25 grams of sodium acetate in 500.00 mL of water. What is the pH of the solution? The K, of acetic acid is 1.8 x 10. (Hints: First convert grams to mol and then determine the molarity of acetic acid and sodium acetate, ...) 5. What is the pH of a 2.50 molar solution of NHCl(aq)? The Ko for NH, is 1.8 x 105. 6. A certain...