47. Calculate [OH-] in each aqueous solution at 25 °C, and classify the solution as acidic or basic. MISSED THIS? Read Section 17.5 a. [H3O+] = 1.2 × 10-8 M c. [H3O+] = 3.5 x 10-2 M b. [H3O+] = 8.5 x 10-5 M
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![47. Calculate [OH-] in each aqueous solution at 25 °C, and classify
the solution as acidic or basic.
MISSED THIS? Read Section 17.5
a. [H3O+] = 1.2 ×
10-8 M
c. [H3O+] = 3.5 x
10-2 M
b. [H3O+] = 8.5 x 10-5 M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F765b863c-0883-4071-8f0f-832646f981bf%2F364124da-a2e1-4157-b89e-a8574b3959a2%2Faelyur_processed.jpeg&w=3840&q=75)
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- Tomato juice has a OH- concentration equal to 1 X 10 -10, what is the pH of this solution?Calculate the concentration of Y4-ion in 0.0100 M EDTA solution at pH 6. α4 = 2.2 x 10-5 for pH 6.You need a buff er at pH 7.5 for use in purifying a protein at 4°C. You have chosen Tris, pK 8.08, ΔH° = 50 kJ · mol−1. You carefully make up 0.01 M Tris buffer, pH 7.5 at 25°C, and store it in the cold to equilibrate it to the temperature of the purifi cation. When you measure the pH of the temperature-equilibrated buff er it has increased to 8.1. What is the explanation for this increase? How can you avoid this problem?
- Draw the titration curve for an 800 mL 0.25 M solution of Arginine. (Graph pH vs. mole OH-.) Where onthe curve is the charge on Arginine +1.5? Identify it on the graph.Quinine ( C20 H24 N2 O2) is the most important alkaloid derived from cinchona bark. It is used as an antimalarial drug. For quinine, pK, = 5.1 and pK, = 9.7 ( pKp = – log Kp). Only 1 g quinine will dissolve in 1920.0 mL of solution. Calculate the pH of a saturated aqueous solution of quinine. Consider only the reaction | Q+ H2O= QH+ + OH- described by pK, where Q = quinine. pH =Calculate the concentration of Y4-ion in 0.0100 M EDTA solution at pH 6. for pH 6, α4 = 2,2 x 10-5
- Refer to the following titration curve below: 13 12 11 10 9 7 6 5 4 3 4 6 8 10 12 14 16 18 20 22 24 26 28 30 Volume of Titrant / mL - Unknown Acid 0.10 mol/L - titrant = NaOH 0.1 mol/L At ph 10.0, which form of histidine is most abundant? His2+ His- His° His+An enzyme (molecular weight= 24 kDa, pI= 5.5) is contaminated with two other proteins, one witha similar molecular mass and a pI of 7.0 while the other has a molecular mass of 100 kDa and a pIof 5.4. Suggest how the contaminated enzyme can be purified.The pH of a 0.0082 M solution of HNO₃ is
- The pks of the amino acid Cys are 1.92, 10.70 and 8.37. If Cys was used as a buffer, what would be the ratio of conjugate base to weak acid in a pH 7.00 Cys buffer? Choose the one closest answer. Be sure to show your work on your scratclr paper. You cannot receive credit without showing your work. 0.0000083 to 1 0.000199 to 1 O 0.043 to 1 O 23.4 to 1What 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 stepThe PI of protein P is 7.3. One can purify protein P by: Anion-exchange chromatography at pH 2.0 Anion-exchange chromatography at pH 7.3 Anion-exchange chromatography at pH 9.0 Anion-exchange chromatography at pH 4.3