Related to the titration of 30.00 mL of a 0.0700 M acetic acid solution with 0.0900 M KOH: What is the initial pH of the analyte solution? What volume of KOH is required to reach the equivalence point of the titration (in mL)? How many mmol of the salt are present at the equivalence point? (ANALYTICAL AMOUNT, NOT EQUILIBRIUM AMOUNT) What is the volume of the solution at the equivalence point (in mL)? What is the molar concentration of the salt at the equivalence point? (ANALYTICAL CONCENTRATION, NOT EQUILIBRIUM CONCENTRATION) What is the pOH at the equivalence point? How many mL of KOH have been added at the half-equivalence point? What is the pH at the half-equivalence point?

in an acidbase titration, 10.0 mL (VB)of NH3 (Ka(NH+) = 5.8*10^ - 19) 0.18 M (CB) are titrated at the equivalence point (EP) with 10.0 ml (VA) of HCI 0.18 M (CA). Calculate (to two decimal places) the pH of the solution at the equivalence point.

For a buffer initially containing .08 mol of benzoic acid (HC7H5O2) and .12 mol of C7H5O2 in 1.0 L, what is the pH after .07 mol of OH is added to the buffer? .07 mol OH- .08 mol HC,H,O2 .12 mol C,H¿0; O 4.57 O 5.47 O 2.91 O 4.37 O 3.71

A solution of a weak acid is titrated with a standard solution of a strong base. The progress of the titration is followed with a pH meter. Which of the following observations best describes what would occur? Initially the pH of the solution increases slowly, and then it increases much more rapidly, before increasing slowly again At the equivalence point, the pH is 7 The pH of the solution gradually decreases throughout the experiment After the equivalence point, the pH becomes constant because this is the buffer

When a 20.1 mL sample of a 0.367 M aqueous hydrocyanic acid solution is titrated with a 0.492 M aqueous barium hydroxide solution, (1) What is the pH at the midpoint in the titration? (2) What is the pH at the equivalence point of the titration? (3) What is the pH after 11.2 mL of barium hydroxide have been added?

A solution of an unknown weak base (0.495 g in 100 mL of water) was prepared and titrated with standardized 0.113 M HCÌi and the pH of the solution was plotted as a function of titrant added (shown below). Titration of a Weak Base With 0.113 M HCI 12 10 10 20 30 40 50 60 70 80 90 Volume of HCl added (ml) Possible identities for the three liquid bases are shown in the table below. Base pyrole pyrimidine pyridine triethylamine 2.51 x 10-14 1.25 x 10-13 1.70 x 10-9 5.30 x 104 Density (g/mL) 0.967 1.02 0.982 0.762 Based on the data above, identify the weak base and explain your selection. The best explanations will account for all relevant experimental data. Additionally, suggest an indicator to use for this titration if it were to be done without a pH meter. Hd

-2 A chemistry graduate student is given 100. mL of a 0.80M chlorous acid (HCIO,) solution. Chlorous acid is a weak acid with K,=1.1 × 10 ´. What mass of KCIO, should the student dissolve in the HCIO, solution to turn it into a buffer with pH = 1.37? You may assume that the volume of the solution doesn't change when the KC10, is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. x10

(Oxalic, Sulfurous, Citric, Hydrofluoric, Formic, Benzoic, Acetic, Hypochlorous, Hydrocyanic, Phenol, Nitrous) Of the acids listed above, which is most suitable to make a buffer with pH = 7.0?  What should be added to this acid to create a buffer (give a chemical formula).

Predict the equivalence point (volume of NaOH in mL) of acid-base titration: 0.300M NaOH in 25.00mL 0.300M HCl 0.1104M NaOH in 15.00mL of 0.1033M HCl

A certain indicator, HA, has a K value of 2.0 x 10. The protonated form of the indicator is blue and the ionized form is red. What is the pK, of the indicator? pK = What is the color of this indicator in solution with pH = 3? about us careers privacy policy terms of use contact us help 949 PM XI 风下 3/10/202 edts f12 inse ho 立