During the titration of 25 mL of 0.1 M maleic acid with 0.1M NAOH. We have studied the plot of alpha values as a function of volume and the plot of pH as a function of volume. Beyond the first equivalence point: O a0 is negligeable, a1 decreases and a2 increases O a0 decreases, a1 is negligeable and a2 increases O a0 is negligeable, a1 increases and a2 decreases a0 is negligeable, a1 increases and a2 increases

A 75.0-mL volume of 0.200 mol L-1 NH3 (Kp = 1.8 × 10-5) is titrated with 0.500 mol L' HNO3. Calculate the pH after the addition of 13.0 mL of HNO3. Express your answer numerically. • View Available Hint(s) να ΑΣΦ pH

Propanoic acid has a Ka=1.3x10-5. The titration starts with 40.00 mL of 0.1000 M propanoic acid (HPr), and we slowly add 0.1000 M NaOH. What is the pH at 40.00 mL and 50.00 mL?

What is the pH in the titration of 10 mL of 0.20 M carbonic acid by 0.10 M NaOH after adding 40 mL NaOH Ka1= 4.4 x 10-7Ka2= 4.7 x 10-11

A The graph shows the titration curves of a strong acid and a weak acid. Estimate the pk, of the weak acid from its titration curve V 14 12 10 pH 12086420 Volume of strong base (ml) 1st attempt Write the estimated pK, to one decimal place 1 OF 8 QUESTIONS COMPLETED 82 W S # 3 Z X E 80 FI D $ 4 C R F K5 V 4 FS T G A 6 B S Y 27 & H 8 U N 8 00 DHI 14 M 9 K TV O hi See Periodic Table O L SUBMIT ANSWER P ** FIL

Calculate the pH for the complete titration of 100.0 mL of 0.122 M hydrazine, H2NNH2, with 0.200 M nitric acid.  The Kb for hydrazine is 3.00x10-6. 9.39 3.32 4.80 9.60 4.70 3.22

This graph shows the titration of 35.0 mL of methylamine solution with 0.0986 M HCI. Determine the molarity of the methylamine solution. concentration: M 12- 11- 10- er Titration of methylamine with HCI 900BD14 15 16 17 18 19 20 21 HCT ond)

Determine the pH during the titration of 60.4 mL of 0.442 M formic acid (Ka = 1.8×10-4) by 0.442 M KOH at the following points.   At the equivalence point (e) After the addition of 90.6 mL of KOH

Consider the titration of 50.0 mL of 0.1000 M diprotic acid H2A (Ka1 = 1.63 × 10-5, Ka2 = 6.09 × 10-10) titrated with 0.2000 M NaOH.  Determine the pH of the solution after the addition of 50.00 mL of KOH.