Please click on an indicator which would be appropriate for the titration illustrated in the plot on the right Crystal violet Cresol red Thymol blue Erytvosin B Titration Curve (oxalic acid/NaOH) 2,4-Dinrophenol 14 Bromphenol blue Mety orange 12 Bromcresol green 10 Mety red Eriochrome BlackT 8 Bromcresol purple 6. Alzan Bronthymal blue 4. Phenol red Nophenol 2. Cresolphthalein 0. 5 10 15 20 25 30 35 40 45 Volume of NaOH added (ml) Phenophthalein Thymolphealen Azan yelow R Tadera Ce Ge 6. 10 11 12 13 Hd

Describe the shape of the titration curve shown, describe why it has this shape.

The following plot shows a titration curve for the titration of 1.00L of 1.00M diprotic acid H2A with NaOH. 14 12 10 0.50 1.50 1.00 2.00 250 3.00 Moles of OH added Which point or points are within any buffer region? O points a and c O point a O point b O points b and d Hd

Consider the titration of a 25.0mL sample of 0.195M acetic acid (CH3COOH) with 0.300M NaOH. How many mL of NaOH is required to reach the equivalence point? The Ka of acetic acid is 1.8x10-5.

make a recipe with full written out steps for 100mL of the TES buffer 30 mM TES has pH of 7.2 and the pKa=7.55   4 mM MgCl2 4 mM NaCl 40 mM 2-mercaptoethanol   acid and base stocks are 2 M MgCl2 and NaCl stocks are 0.5 M 2-mercaptoethanol stock is 1.4 M

Calculate the volume of acetic acid (CH3CO₂H) and the mass of sodium acetate (CH₂CO₂Na) needed in order to prepare 1.0 L of a 200 millimoles acetate buffer at pH 4.5. The original concentration of acetic acid is coming from a pure acetic acid (called "glacial") is a liquid at room temperature, with a density of 1.049 g/mL and a formula weight of 60.05 g/mol. Sodium acetate is a solid, with a formula weight of 82.03 g/mol.

For each scenario below, select the color of the solution using the indicator thymol blue during the titration. When you first add indicator to your Na2CO3 solution, the solution is basic (pH ~10), and the color is [Select] At the equivalence point for the titration, the moles of added HCI are equal to the moles of Na2CO3. One drop (or less!) past this is called the endpoint. The added HCI begins to titrate the thymol blue indicator itself. At the endpoint, the indicator color is [Select] When you weren't paying attention and added too much HCI (~12 mL extra), the color is [Select] When you really weren't paying attention and reached the second equivalence point of Na2CO3, the color is ✓ [Select] blue yellow red orange green Question 9

1) a)Interpret and explain each region that appears in the titration graph. b)Indicate the color changes and the range in which each indicator is changing the color

Please answer; they were all the same choices.

From the standard properties of plotted titration curves, which one best represents the titration of a weak acid with a strong base? The curve is with a semi S orientation with the midpoint of the steep part at pH 7 The curve is with a semi Z orientation with the midpoint of the steep part at pH 7 The curve is with an "S' orientation with the midpoint of the steep part at pH > 7 The curve is with a "Z" orientation with the midpoint of the steep part at pH <7 Representative curve cannot be predicted