The amino acid proline has ionization constants Ka1 = 1.12 x 10 ^-2 AND kA2 = 2.29 X 10 ^-11, which correspond to the carboxylic acid group and the amino group respectively. Calculate the pH of a 0.154 M proline (HP) solution.
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The amino acid proline has ionization constants Ka1 = 1.12 x 10 ^-2 AND kA2 = 2.29 X 10 ^-11, which correspond to the
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- The amino acid asparagine has ionization constants Kal = 6.92 x 10-3 and K ₁2 = 6.92 x 10-3 and K₁2 = 1.86 x 10-9, which correspond to the carboxylic acid group and the amino group respectively. Calculate the pH of a 0.170 M asparagine (HN) solution. pH =Sodium hydroxide is a strong electrolyte and hydrates in water according to the following equation: NaOH (s) → Na* (aq) + OH (aq) The concentration of NaOH is 6.66 x 103, Calculate the pH of the solution.Determine the pH of a 1.497 M solution of potassium cyanide (KCN) in water. Ka for HCN is 6.17 × 10–10. Enter your response in pH units to the nearest 0.01.
- The barium oxide is a strong electrolye: BaO(s) + H2O(l) → Ba2+(aq) + 2 OH−(aq). What is the pH of a solution prepared by dissolving 0.175 g of solid BaO in enough water to make 1.00 L of aqueous solution (at 25°C)? Enter your answer in decimal format with two decimal places (value ± 0.02). The answer is 11.36 would like an explanation to this problem please.Give the definitions of pH and pKa. What are the differences between these two terms? Calculate the pH of salicylic acid solution when the solution is titrated to contain only 1.0% of salicylates. Use the fact, pKa (salicylic acid) = 2.97, in your calculation.The equilibrium expression for any weak acid can be written as HA (aq) + H20 (1) = A- (aq) + H;O+ (aq) 1. Write the K value expression based on the equation above (remember that pure liquids are not included in the K expression). This is given the special symbol Ka. 2. In this experiment, you will be using pH to find [H3O+]. The relationship is [H3O*] = 10-PH . For a pH of 7.4, find the [H3O+].
- The amino acid isoleucine has ionization constants Kal = 4.81 x 10-3 and K₁2 = 1.75 x 10-¹0, which correspond to the carboxylic acid group and the amino group respectively. Calculate the pH of a 0.279 M isoleucine (HI) solution. pH =pH = −log[H+] where [H+] is the hydrogen ion concentration, measured in moles per liter. Solutions with a pH-value of less than 7 are acidic; solutions with a pH-value of greater than 7 are basic; solutions with a pH-value of 7 (such as pure water) are neutral. Black coffee has a pH of 5 and pure water has a pH of 7. Compare the pH of each and determine how much more acidic black coffee is than pure water.Calculate pH of 2.5 x 10-3 M HCl(aq). HCl(aq) is strong base.
- Calculate the pH and pOH of the following solutions (see Appendix 11 of your textbook for pKa values): 1. 0.01 M HBr 2. 0.00005 M HBr 3. 0.00002 МКОН 4. 0.01 M CH,COOH 5. 0.00001 M CH,COOH 6. 0.01 M HIO, 7. 0.01 M pyridine Calculate the pH of the following solutions: 1. 0.01 M NAHS 2. 0.005 M NaН.РО, 3. 0.005 M Na,HPO, 4. 0.005 M Na PO, 5. 0.1 ΜΝΗ,CN Calculate the pH of the following buffer solutions: 1. 1.7 g/L of NH, and 5.35 g/L of NH,Cl. 2. 50 mL of 1 M CH,COONA and 1 L 0.1 M CH,COOH. 3. 50 mL of 1 M NaOH and 1 L 0.1 M CH,COOH. 4. 10 mL 0.1 H,PO, + 25 mL 0.1 NaOH 5. 10 mL 0.1 H,PO, + 25 mL 0.1 Na,PO, 6. A buffer solution pH=5.00 contains 0.01 M CH,COOH. Calculate the concentration of sodium acetate it contains. 7. What weight of NH,Cl should be added to 1 L of 0.1 M NH, solution to get pH=9.00?Calculate the pH of 0.10 M (COOH)2 (aq), oxalic acid. Ka1 = 5.9 × 10–2 ; Ka2 = 6.4 × 10–5.The ionization constant, Ka, for dichloroacetic acid, HC2HO2Cl2 , is 5.0 × 10‑2. What is the pH of a 0.15 molar solution of this acid?
