You have to calculate the pH of 0.020 M NH3 (Kb = 1.75 x 10-5). a- Write the four equations to solve this problem. b- Simplify the algebra by making two reasonable assumptions and calculate the pH. c- Verify if both assumptions are accepted when the error introduced by each assumption is less than 5%.

You have to calculate the pH of 0.020 M NH3 (Kb = 1.75 x 10-5). a- Write the four equations to solve this problem. b- Simplify the algebra by making two reasonable assumptions and calculate the pH. c- Verify if both assumptions are accepted when the error introduced by each assumption is less than 5%.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter21: Potentiometry

Section: Chapter Questions

Problem 21.22QAP

See similar textbooks

Similar questions

You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.
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?
You mix 50.0 mL of 0.250 M CH3COOH with 1.00 mL of 0.500 M NaOH. Calculate the pH of the mixture. The total volume is 51.0 mL. Use two stages method to solve this problem (I. stoichiometric reaction between acid and base, II. Acid-Base Equilibrium, ICE). Ka of CH3COOH = 1.8 x 10-5.
a) Why can you not prepare a solution of pH = 8 by diluting sufficiently a 0.01 M solution of HCl with water? b) You could determine Ka for benzoic acid by measuring the pH of a 0.010 M solution of benzoic acid. Why is the graphical method used in this experiment a better way of determining Ka? c) List the measurements along with their uncertainties made in the determination of the molar mass of benzoic acid. Calculate the uncertainty in the mola r mass of benzoic acid determined by the titration.
250 mL pure water at 25C is added with 0.105x10-6 L H2SO4 Solution which contains 98.0 wt % sulfuric acid and has a density of 1.84 g/mL. what is the pH of the water after the sulfuric soultion is added?
Calculate the pH of a mixture containing 0.23 M HONH2 and 0.44 M HONH3Cl. (Kb = 1.1 × 10–8) What information do we need to calculate the pH? (Choose all letters that apply.) a. 0.23 M HONH2b. 0.44 M HONH3Clc. the major species in the solutiond. pOH = –log[OH–] and 14.00 = pOH + pHe. Kb = 1.1 × 10–8
Determine the base ionization constant (in x 10-5) of a 0.0925 g sample of a weak base (molar mass = 17.03 g/mol), B, that is dissolved in water to produce 100 mL of a solution with a pH of 11.00.
At 25oC, a 100mL solution is found to contain 20% by mass acetic acid (CH3COOH). The density of the solution is 1.05g/cm3. If this solution is diluted further to form 700mL, what will be the A) [OH-], B) pH and C) % dissociation of the resulting acetic acid solution? CH3COOH -> H+ + CH3COO- (Kb = 5.56x10-10)
Determine the OH- and H+ concentration and calculate the pH, pOH of a solution that is 0.70 M NH3 solution. USE THE ICE method NH3 + H2O <--> NH4 + + OH- Kb = 1.8 x 10-5
Calculate the pH of a solution made by dissolving 1.87g of sodium caproate (NaC6H11O2) in water and diluting it toa total volume of 500mL. For the caproate ion, Kb=7.58 x 10^-10
A solution is made by mixing 0.400M in formic acid, HCOOH, and 1.00M in sodium formate, HCOONa? Ka=1.80x10-4. The total volume is 1.00L. What is the pH of this solution upon the addition of 0.075moles of HCl?
Find the pH of the following solutions 0.6g phenol C6H5OH in 500 mL H2O, Ka = 1 x 10-10