A 1.39 L buffer solution consists of 0.144 M butanoic acid and 0.328 M sodium butanoate. Calculate the pH of the solution following the addition of 0.067 moles of NaOH. Assume that any contribution of the NaOH to the volume of the solution is negligible. The K, of butanoic acid is 1.52 x 10-s. pH 5.29 %3D Incorrect

A 1.39 L buffer solution consists of 0.144 M butanoic acid and 0.328 M sodium butanoate. Calculate the pH of the solution following the addition of 0.067 moles of NaOH. Assume that any contribution of the NaOH to the volume of the solution is negligible. The K, of butanoic acid is 1.52 x 10-s. pH 5.29 %3D Incorrect

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter10: Potentiometry And Redox Titrations

Section: Chapter Questions

Problem 7P

See similar textbooks

Similar questions

What is the pH of a solution which is equimolar with respect to both ethanoic acid and sodium ethanoate? (Ka for ethanoic acid is 1.8 x 10-5 moldm-3) What special property does this solution have?
When a drop (taken to be 0.20 cm3) of 1.0 M HCI(aq) is added to 25 cm3 of pure water, the resulting hydroniumion concentration rises to 0.0080 mol dm- 3 and so the pH changes from 7.0 t o 2.1, a big change. Now suppose the drop is added to 25 cm3 of an ethanoate buffer solution that is 0.040 MNaCH3CO2(aq) and 0.080 M CH3COOH(aq). What will be the change in pH?
How many grams of potassium napthenate (KC11H7O2; MW=210.27 g/mole; Kb=85x10-10) must be added to 50.0 ml of 0.4 M Naphthenic acid (HC11H7O2; Ka=5.4x10-5) to obtain a buffer with pH 5.0?
I was just wondering how you got the 4.0 x 10-4 for the acidionzation constant.
3. Calculate the (a) pH (b) pOH (c) percent ionizaton of 0.100 M ammonia. NH3 kb = 1.8x10^-5 4. Give five (5) techniques on how to produce an ideal precipitate in the analysis of sodium fluoride, NaF with silver nitrate, AgNO3 as precipitant using precipitation gravimetry. please answer all questions. I don't have questions left so i cannot repost the other question
a) At temperature 25°C, 0.02 M hydrazine, N2H4 solution is 0.69% ionised. Calculate the i. Concentration of OH- ion ii. ionisation constant, Kb b) Calculate the mass of sodium benzoate, C6H5COONa that should be added to 500 mL of 0.2M aqueous benzoic acid, C6H5COOH solution to produce a buffer with pH 3.50?[ Ka for C6H5COOH = 6.3 x10-5] c) When a 1 x 10-3 moldm-3 solution of CaCl2 is mixed with an equal volume of a 1 x 10-3 moldm-3 solution of Na2SO4, will precipitate form? (Ksp CaSO4= 2 x 10-5) Do you mean that pH? That was all the given information the question gave.. I don't understand how to use the ionised part the most
Kb for methylamine at 25°C is 4.4 x 10-4 what is its pH if 0.10M solution is used.
v. What is pH? Calculate the pH for 0.0001N NH4OH solution of 100mL volume. The pKb value for NH4OH at 25oC is 1.76 x 10-5.
The experimental Ksp of calcium hydroxide is _________ x 10-6 if 23.09mL of the sat. calcium hydroxide solution was titrated with 12.53mL of 0.049M HCl(aq), considering 4 as an exact value for the calculation?
A hypothetical weak acid, HA, was combined with NaOH in the followingproportions: 0,20 mol HA, 0,08 mol NaOH. The mixture was diluted to a totalvolume of 1,0 L and the pH was found to be 4,80. a). What is the pKa of the acid?
Why do you have to titrate until or above pH = 12.5 ± 0.2 to properly identify the unknown acid solution?
Full acid, HOOC = CH-COOH is a biphatic acid and we will label it as H2M. Acid constant data for the two protonation phases of the acid: K H.M+H2O = H, 0++HM- HM +H2O = H, 0++M2– a1 = 1.3x10-2 K.2 = 5.9 x 10-7 Measure 0.1 ml of 0.100 M of malic acid with 0.100M NaOH and measure the H variability as a function of the added base volume. A. Calculate the PH value at the beginning of the titration. B. Calculate the pH value at the first equivalent point. C. Calculate the pH value at the second equivalent point. D. Draw the titration curve in the graph. Indicate in the graph titles and units for the axes.