Indicator pH range Methyl orange 3.1 - 4.4 Methyl red 4.4 - 6.2 Bromthymol blue 6.2 – 7.6 Phenolphthalein 8.0 - 10.0 to the table According above, which pH indicator would be the best choice when titrating acetic acid, CH;COOH, with sodium hydroxide, NaOH?. A- methyl orange B- methyl red C- bromthymol blue D- phenolphthalein Page 27 28

1) Determine the pH during the titration of 74.5 mL of 0.348 M nitrous acid (Ka = 4.5×10-4) by 0.348 M NaOH at the following points.   (a) Before the addition of any NaOH ?   (b) After the addition of 18.0 mL of NaOH ?   (c) At the half-equivalence point (the titration midpoint) ?   (d) At the equivalence point ?   (e) After the addition of 112 mL of NaOH ?

Give typed full explanation not a single word hand written otherwise leave it

If a 0.552M HCl caq) solution is used by a scientist to titrate 10.00mL of a weak base, based curve (shown below), what base? write your the titration the concentration of the auswer with 4 decitual places. pH Curve OM is 12 10 8 6 4 2 0 5:0 2 1.5 n 3 3.5 A Volume of Titrant / mL 7.5 8 8.5

Calculate change in pH of a buffer solution

There are 50.00 mL of a hydrazine solution (H2NNH2, Kb = 1.3 x 10-6) 0.1000 mol L-1. Calculate the pH by adding the following volumes in mL of 0.1000 mol L-1 HCl:a) 0.00 b) 25.00 c) 49.00 d) 50.00 e) 60.00Generate the titration curve and choose the best indicator for this procedure.Below are the answers, however, show the calculations:a) 10.56 b) 8.11 c) 6.42 d) 4.71 e) 2.04 Don't forget the titration curve!

Assuming equal concentrations of conjugate base and acid, which one of the following mixtures is best suited for preparing a buffer solution with pH of 4.74?   Question 2 options:   NH3 / NH4Cl  (Ka = 5.6 × 10–10)   NaNO2 / HNO2  (Ka = 4.5 × 10–4)   CH3COONa / CH3COOH  (Ka = 1.8 × 10–5)   NaCl / HCl   NaOCl / HOCl  (Ka = 3.2 × 10–8)

A triprotic acid is titrated with KOH. What species are NOT in solution to any large extent between the 1st and 2nd equivalence points? Select all that apply. O H3A O HA? O A³- K+ O OH H2A

pH calculation after the first equivalence point:   Calculate the pH of 50.0 mL of 0.250 M oxalic acid (HOOCCOOH) upon addition of 31.9 mL of 0.500 M NaOH. Round your calculated value for pH to two figures to the right of the decimal point. Significant constants: Ka1 of oxalic acid = 5.60 x 10-2 and Ka2 of oxalic acid = 5.42 x 10-5

100. mL of 0.200 M HC1 is titrated with 0.250 M NaOH.