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(a)
Interpretation:
The picture that represents weak diprotic acid should be identified.
Concept Introduction:
Diprotic Acids: The acids that has 2 protons for donation are termed as diprotic acids.
(b)
Interpretation:
The box that contains impossible situation should be determined.
Concept Introduction:
Diprotic Acids: The acids that has 2 protons for donation are termed as diprotic acids.
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Chapter 10 Solutions
Fundamentals of General, Organic, and Biological Chemistry, Books a la Carte Edition; Modified Mastering Chemistry with Pearson eText -- ValuePack ... and Biological Chemistry (4th Edition)
- Give the equation for the complete titration of aspartic acid with a base, NaOH. At what pH, can you use aspartate solution a buffer?arrow_forwardWhat is the pH of a buffer of a buffer system that contains a weak acid of .19 M and conjugate base of .12 M ? The Ka of the acid is 5.6x 10 -6 pH= pKa + log ( [A- ]/[HA]) please show me step by steparrow_forwardthe pH of a solution is decreased from 9 to 8, it means that the A) concentration of H+ has decreased to one-tenth (1/10) what it was at pH 9. B) concentration of H+ has increased 10-fold (10X) compared to what it was at C) concentration of OH- has increased 10-fold (10X) compared to what it was at D) concentration of OH- has decreased to one-tenth (1/10) what it was at pH 9. E) Both B and D are correct. parrow_forward
- 4.2 (b) Using the equation below, explain what happens to maintain the pH of the solution: A (aq) H(aq) HA (aq) (i) when an acid is added (ii) when a base is added (iii) Give one example each of a buffer in both living and non-living systems +arrow_forwardFor each of the following chemicals, name the general class they belong to, discuss their solubility in water and explain why they are/are not soluble in water (note the numbers are all subscripts): a) CH3(CH2)26COOH b) KCl c) CH3OHarrow_forwardA buffer solution contains an equal concentration of weak acid HX and its conjugate base ion X™. The ionization constant Ka of HX is 2.2 x 10-8. What is the pH of the buffer?arrow_forward
- Buffers are aqueous solutions that tend to resist changes in pH when small amounts of strong acid (H+) or base (OH-) are added. Compare the changes in the pH of the resulting solution when you add 0.1 M NaOH in (a) distilled water and (b) bicarbonate solution. A) (a) and (b) solutions will have the same pH. B) pH change in (b) will be higher than in (a). C) No changes in pH of both solutions. D) pH change in (a) will be higher than in (b).arrow_forwardCalculate the pH of a dilute solution that contains a molar ratio of potassium acetate to acetic acid (pKa 5 4.76) of (a) 2:1; (b) 1:3.arrow_forwardWhat is the pH of a buffer that contains 0.9 M ammonia and 0.3 M ammonium ion? (Ka for ammonium ion = 5.8 x 10-10arrow_forward
- Mixtures of amino acids can be analyzed by first separating the mixture into its components through ion‑exchange chromatography. Amino acids placed on a cation‑exchange resin containing sulfonate (−SO−3)(−SO3−) groups flow down the column at different rates because of two factors that influence their movement: (1) ionic attraction between the sulfonate residues on the column and positively charged functional groups on the amino acids, and (2) aggregation of nonpolar amino acid side chains with the hydrophobic backbone of the polystyrene resin. Note that the ionic attraction is more important than hydrophobicity for this column media. For each pair of amino acids, identify which will be eluted first from a cation‑exchange column using a pH 7.0pH 7.0 buffer.arrow_forwardAre there any H3O+ ions present in pure water at neutral pH (i.e., at pH = 7.0)? If so, how are they formed?arrow_forwardThe ionization of p-nitrophenol is shown below (pKa = 7.0): a. Identify the weak acid and conjugate base. b. At pH 7, what are the relative concentrations of ionized and un-ionized p-nitrophenol? c. If enough concentrated hydrochloric acid is added to a solution of p-nitrophenol to lower the pH from 7 to 5, what will happen to the relative concentrations of the ionized and un-ionized forms? d. Ionized p-nitrophenol has a yellow color, while the un-ionized form is colorless. The yellow color can be measured using a spectrophotometer at 400nm. In order to determine the total amount of p-nitrophenol in a solution, would you perform the spectrophotometer reading at an acidic or basic pH? Clearly explain why? e. A solution of p-nitrophenol at pH 7.95 was found to have an A400 of 0.255 . What is the total concentration (in µM) of p-nitrophenol (ionized plus un-ionized) in the solution? The molar extinction coefficient of p-nitrophenol is 18,500 M-1cm-1 and the pKa is 7.arrow_forward