The following graph shows the pH curve for the titration of 25 mL of a 0.1 M monoprotic acid solution with a 0.1 M solution of a monoprotic base. 14_PH 12 10 8 6 4 2 0 05 10 15 20 25 30 35 40 45 50 mL of 0.1 M base added (1) The pH curve represents the titration of a e acid with a (2) Choose a suitable indicator for the endpoint of the titration from the following pulldown list. 8 Malachite green Thymol blue Methyl orange Bromocresol green Methyl red Bromothymol blue Cresol red Phenolphthalein Thymolphthalein Alizarin yellow 0.2 pH 0 1 2 3 4 5 6 8 10,0 104 10.1 12.0 9 10 11 12 13 14 e base.

Consider the titration of 50.00 mL of 0.100 M CH3CO2H with 0.200 M KOH, calculate the pH after adding 30.00 mL of KOH. Ka for CH3CO2H = 1.8 x 10-5. Group of answer choices 12.10 1.90 11.50 7.00

You are titrating 30 mL of 0.100M H3PO4 with 0.200 M KOH. For H3PO4: Ka1=1.1X 10-2, Ka2 = 7.5 X 10-8, and Ka3 = 4.8 X 10-¹3. What is the pH after you add 15.00 mL of KOH?

Consider the titration of 50.00 mL of 0.100 M CH3CO2H with 0.200 M KOH, calculate the pH after adding 30.00 mL of KOH. Ka for CH3CO2H = 1.8 x 10-5. Group of answer choices 12.10 1.90 11.50 7.00

Titus titrates 60 mL of 0.700 M lactic acid (HC,H,O,, Ka = 1.5 × 10-4) using 0.750 M NaOH. Calculate the pH of the resulting solution at each of the following points in the titration. After adding 42 mL of the NaOH solution: At the equivalence point: After adding 75.9 mL of the NaOH solution:

An indicator (ka 1.7X10-6) is red but changes to blue when ionized. The indicator was used in the titration of 10 mL of 0.2 M HCI with 15 mL of 0.2 M of NaOH. At what pH you would expect the indicator to change color?   9.11-11.11   6.85-8.85   5.32-7.32   3.98-5.98   4.77-6.77

The following graph shows the pH curve for the titration of 25 mL of a 0.1 M monoprotic acid solution with a 0.1 M solution of a monoprotic base. 14 - pH 12 10 8 6 4 2 10 15 20 25 30 35 40 45 50 mL of 0.1 M base added (1) The pH curve represents the titration of a v acid with a v base. (2) Choose a suitable indicator for the endpoint of the titration from the following pulldown list. Malachite green 0.2 1.8 Thymol blue 1.2 2.8 8.0 9.6 Methyl orange 3.2 4.4 Bromocresol green 3.8 5.4 Methyl red 4.8 6.0 Bromothymol blue 6.0 7.6 Cresol red 7.0 8.8 Phenolphthalein 8.2 10.0 Thymolphthalein 9.4 10.6 Alizarin yellow 10.1 12.0 pH 0 1 2 3 4 6. 8 10 11 12 13 14

when a weak base ammonia is titrated with HCl at equivalence point, its pH = 7.00 true or false?

When titrating ammonia with a hydrochloric acid at 25°c, the O pH will be less than 7 at the equivalence point. O pH will be 7 at the equivalence point. O titration will require more moles of acid than base to reach the equivalence point. O titration will require more moles of the base than acid to reach the equivalence point. O pH will be greater than 7 at the equivalence point.

Calculating the pH of a weak base titrated with a strong acid 0/5 Izabella An analytical chemist is titrating 165.0 mL of a 0.7400M solution of methylamine (CH3NH2) with a 0.4100M solution of HNO3. The pK of methylamine is 3.36. Calculate the pH of the base solution after the chemist has added 318.6 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places. pH = ☐ ☑ ك Ar B•