Part 1 - Determining Kp by lon Concentration9.924.039.3325 x 10pH of solution:pOH = 14-pH:[OH] = 10:Complete the following ICE table (using x):Kup TableMg(OH); (s):Molarity: initialconcentration1ChangeEquilibriumconcentration|-X0.15589 MB (OH)2Complete the following ICE table (now using actual concentrations):Mg(OH), (8)K, TableMolarity: initialconcentrationChangeEquilibriumconcentrationKip [Mg][OH]:Mg (aq)4XX+ 2 OH(aq)02xMg² (aq) +2xTo find K, use the above ICE table to find the concentration of Mg" (you found the concentration ofOH above using the pOH). Because there is a 1:2 stoichiometric ratio between Mg" and OH, [Mg] =[OH 1/2. Plug the values of [Mg] and [OH-] into the K, expression below:2OH(aq)

Ksp is the equilibrium constant when a solid is dissolved in liquid.For a reaction,The Ksp can be…

Part 1 - Determining K, by lon Concentration 9.97 4.03 9.3325 x 10 pH of solution: pOH = 14-pH: JOH] = 100 Complete the following ICE table (using x): Kup Table Mg(OH) (s) Molarity: initial concentration 1 Change Equilibrium concentration Kup Table Molarity: initial concentration Change (-X 0.15580 MB (OH)2 My Complete the following ICE table (now using actual concentrations): Mg(OH), (8) Equilibrium concentration -5 11 Kip [Mg][OH]: Mg (aq) X X + 2 OH(aq) 0 2x 2x Mg (ag) + 2 OH (aq) To find K, use the above ICE table to find the concentration of Mg (you found the concentration of OH above using the pOH). Because there is a 1:2 stoichiometric ratio between Mg" and OH, [Mg] = [OH 1/2. Plug the values of [Mg] and [OH] into the K, expression below: ys 4

Part 1 - Determining K, by lon Concentration 9.97 4.03 9.3325 x 10 pH of solution: pOH = 14-pH: JOH] = 100 Complete the following ICE table (using x): Kup Table Mg(OH) (s) Molarity: initial concentration 1 Change Equilibrium concentration Kup Table Molarity: initial concentration Change (-X 0.15580 MB (OH)2 My Complete the following ICE table (now using actual concentrations): Mg(OH), (8) Equilibrium concentration -5 11 Kip [Mg][OH]: Mg (aq) X X + 2 OH(aq) 0 2x 2x Mg (ag) + 2 OH (aq) To find K, use the above ICE table to find the concentration of Mg (you found the concentration of OH above using the pOH). Because there is a 1:2 stoichiometric ratio between Mg" and OH, [Mg] = [OH 1/2. Plug the values of [Mg] and [OH] into the K, expression below: ys 4

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

Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H) and the amine group (NHR) are protonated. However, as the pH of the solution increases (say, by adding base), the carboxylic acid proton is removed, usually at a pH between 2 and 3. In a middle range of pHs, therefore, the amine group is protonated, but the carboxylic acid group has lost the proton. (This is called a zwitterion.) At more basic pH values, the amine proton is dissociated. What is the pH of a 0.20 M solution of alanine hydrochloride, [NH3CHCH3CO2H]Cl?
If the pH of a 0.200 M solution of the CICH2O¯ ion is 12.05, then what is the value for the basicity constant, Kp, of CICH20-? You do not need to make a simplifying assumption CICH,0-(aq) + H2O(1) СICH-OОH(aq) + ОН (аq) K½ = ?
Consider the weak bases below and their Kp values: NH3 Ky = 1.8 x 10-5 C2H5NH2 Kp = 5.6 x 10-4 C5H5N Kp = 1.7 x 10-9 Arrange the conjugate acids of these weak bases in order of increasing acid strength. O CsH;NH< NH,*< C2H5NH3* C2H5NH;*= NH,= C5H5NH* C2H5NH3*< NH4*< C5H5NH* O NH,*< C,H5NH;*
A 400 mL sample of 0.4375 M ethyl amine C2H;NH2 (K, = 4.5m10-4) reacted with 2.50L of HCN ((K, = 6.2m10-10) at 298 K and 1.2 atm. Assuming the volume of the solution remains constant. calculate concentrations of all species present and pH at equilibrium.
What is the pH at 25 °C of water saturated with CO2 at apartial pressure of 1.10 atm? The Henry’s law constant forCO2 at 25 °C is 3.1 x 10-2 mol/L-atm.
and Obedi X 101 Chem101 14.4 Hydrolysis of Salt X Microsoft PowerPoint X M Inbox (570)-mirandae X app.101edu.co Question 26 of 66 The following acid-base reaction occurs spontaneously in the gas phase at 25.0°C: NH3(g) + HCI(g) NH,CI(s) Calculate the equilibrium constant for this reaction at 298.15 K. Substance (jou/r) -17 (6) HN -95 (6) ICH -203 (s) 1ɔ*HN esc
The lactate ion, C, H,O, (aq), reacts with water to form lactic acid and hydroxide ion. C;H,05 (aq) + H, O(1) = HC,H;O;(aq) + OH (aq) In a 0.378 M solution of sodium lactate, the [OH¯] = 5.2 × 10-6 M. Use the ICE table to determine the concentrations of OH¯ and HC, H,O,. You will use these values to calculate the Kp for HC,H,O3. C;H;O5 (aq) + H,O(1) = HC,H;O,(aq) + ОН (аq) initial 0.378 change +x +x equilibrium 0.378 – x What is the value for x in these expressions? Hint: you are given this value in the problem. x = M
Consider the dissociation of hydrocyanic acid in aqueous solution HCN - CN + H* for which K, is 4.9 x 101°. (i) Find the pH of a solution initially 102 M in HCN, and the degree of dissociation of the HCN, a. (ii) To this solution is added more CN' until [CN'] = (0.1 M. What is the new pH of the solution? (ii) Without making a new numerical cakculation, explain qualitatively how the degree of dissociation would change if the solution is diluted.
The acid dissociation constants for sulfurous acid are: Ka = 1.2 x 10-2 and Kaz = 6.6 x 10-8. (i) Calculate the pH of a solution of 0.100 M H2SO3. (ii) Calculate the pH of a solution of 0.100M NazSO.. (iii) Calculate the pH of a solution resulting when equal volumes of the solutions described in parts (i) and (ii) are mixed.
2. Determine [H3O+] and [OH] concentrations (in M to two decimal places) for each: (a) Pure water at 10 °C (K = 0.293 x 10-14) W (b) An aqueous solution with a pH of 3.23 A: 5.41x108; 5.41×10-8 A: 5.89x104; 1.70×10-11
NH3 is a weak base. It ionizes in water to produce NH4+ and OH-. Its Kb = 1.8  10-5 and Kw = 1  10-14 at 25oC. Please complete following tasks for a solution of 0.0500 M NH3 (aq) at 25oC. (a) ionization % of NH3, (b) pH of this solution, (c) concentration of OH- ; and (d) concentration of NH4+
A solution is prepared at 25 °C that is initially 0.15M in acetic acid (HCH,CO,), a weak acid with K,=1.8 × 10 and 0.40M in potassium acetate (KCH,CO,). cCalculate the pH of the solution. Round your answer to 2 decimal places. pH = 0