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![ой - Initial c Change В но o - ca t ca o +Ca. c- initial conc of base = 0.15m & degree of dissociation Kb. Lent] [ои-1 [61 Kb](http://img.homeworklib.com/questions/7cd7b780-0b91-11ec-a7b9-dd5aa34f2ac6.png?x-oss-process=image/resize,w_560)
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A hypothetical weak base has Kg = 5.0 x 108. Calculate the equilibrium concentrations of the...
Calculate the solubility (in moles per liter) of Al(OH)3 (Ksp = 2 x 10-2) in each...
Calculate the solubility (in moles per liter) of Al(OH)3 (Ksp = 2 x 10-2) in each of the following. a. water Solubility = mol/L b. a solution buffered at pH = 5.0 Solubility = mol/L c. a solution buffered at pH = 10.0 Solubility = moll Submit Answer Try Another Version 6 item attempts remaining
[References) A 0.079 M solution of diethylamine has a pH of 12.00. What is the value...
[References) A 0.079 M solution of diethylamine has a pH of 12.00. What is the value of Ky for this weak base? (C2H6)2NH(aq) + H2O(l) = (C2H6)2NH2+ (aq) + OH(aq) K- Submit Answer Try Another Version 10 item attempts remaining
The pH of an aqueous solution of 0.544 M quinoline (a weak base with the formula...
The pH of an aqueous solution of 0.544 M quinoline (a weak base with the formula C H2N) is Submit Answer Try Another Version 1 item attempt remaining
The Kp for lead iodide (Pbl) is 1.4 x 108. Calculate the solubility of lead iodide...
The Kp for lead iodide (Pbl) is 1.4 x 108. Calculate the solubility of lead iodide in each of the following a. water Solubility = mol/L b. 0.22 M Pb(NO3)2 Solubility mol/L c. 0.022 M Nal Solubility = mol/L Submit Answer Try Another Version 6 item attempts remaining
Consider a weak acid HX. If a 0.10-M solution of has a pH of 4.83 at...
Consider a weak acid HX. If a 0.10-M solution of has a pH of 4.83 at 25°C, what is △Go for the acid's dissociation reaction at 25°C? kJ/mol Submit Answer Try Another Version 9 item attempts remaining
A stock solution of K S is available to prepare solutions that are more dilute. Calculate...
A stock solution of K S is available to prepare solutions that are more dilute. Calculate the volume, in ml., of a 2.0-M solution of KS required to prepare exactly 100 ml of a 0.130-M solution of Kys ml Submit Show Approach Show Tutor Steps Submit Answer Try Another Version 10 item attempts remaining Click to try another version of this item. "Note that your response(s) and the points you have earned on this item will be cleared. Previous News)...
Calculate pH of a weak base solution. Please box answers! Thank you! Tutored Practice Problem 16.4.5...
Calculate pH of a weak base solution. Please box answers!
Thank you!
Tutored Practice Problem 16.4.5 G S GRASS Calculate the pH of a weak base solution ([B]o > 100Ko). Close Problem Calculate the pH of a 0.286 M aqueous solution of hydroxylamine (NH,OH, Kb - 9.1x10') and the equilibrium concentrations of the weak base and its conjugate acid. PH (NH3OH)equilibrium [NH3OH lequilibrium - Check & Submit Answer Show Approach
UTOR Calculate K from Equilibrium Concentrations Some HI is placed in a sealed flask and heated...
UTOR Calculate K from Equilibrium Concentrations Some HI is placed in a sealed flask and heated to 775 K. When equilibrium is reached the flask is found to contain HII (0.137 M), H, (3.28X10M), and (23X10M) What is the value of the equilibrium constant for this reaction at 775 K? 2HI(g) H +1 K-L Submit Show Approach Show.tor Steps Try Another Version 9 item attempts Submit Answer
TUTOR STEP The equilibrium concentrations can then be calculated from the value of x. Enter them...
TUTOR STEP The equilibrium concentrations can then be calculated from the value of x. Enter them here. H2O(l) HB+ (aq) + 0.15 0 B(aq) + Initial (mol/L) Change (mol/L) -8.7 x 10-5 Equilibrium (mol/L) 0.15 – 8.7 x 10-5 OH(aq) 0 +8.7 x 10-5 8.7 x 10-5 +8.7 x 10-5 8.7 x 10-5 pOH = -log[OH ]. Use this to calculate pH using pH = 14.00 - POH. [B] = 0.149 mol/L [HB]= mol/LX [OH'] = mol/L X pH =...
help please Pyridine is a weak organic base, and readily forms a salt with hydrochloric acid....
help please
Pyridine is a weak organic base, and readily forms a salt with hydrochloric acid. CsH; N(aq) + HCl(aq) = CsH NH+ (aq) + CI(aq) CI", if K, for pyridine is 1.5 x What is the pH of a 0.018 M solution of pyridinium hydrochloride, C, H, NH pH = Submit Answer Try Another Version 2 item attempts remaining
Calculate the solubility (in moles per liter) of Al(OH)3 (Ksp = 2 x 10-2) in each of the following. a. water Solubility = mol/L b. a solution buffered at pH = 5.0 Solubility = mol/L c. a solution buffered at pH = 10.0 Solubility = moll Submit Answer Try Another Version 6 item attempts remaining
[References) A 0.079 M solution of diethylamine has a pH of 12.00. What is the value of Ky for this weak base? (C2H6)2NH(aq) + H2O(l) = (C2H6)2NH2+ (aq) + OH(aq) K- Submit Answer Try Another Version 10 item attempts remaining
The pH of an aqueous solution of 0.544 M quinoline (a weak base with the formula C H2N) is Submit Answer Try Another Version 1 item attempt remaining
The Kp for lead iodide (Pbl) is 1.4 x 108. Calculate the solubility of lead iodide in each of the following a. water Solubility = mol/L b. 0.22 M Pb(NO3)2 Solubility mol/L c. 0.022 M Nal Solubility = mol/L Submit Answer Try Another Version 6 item attempts remaining
Consider a weak acid HX. If a 0.10-M solution of has a pH of 4.83 at 25°C, what is △Go for the acid's dissociation reaction at 25°C? kJ/mol Submit Answer Try Another Version 9 item attempts remaining
A stock solution of K S is available to prepare solutions that are more dilute. Calculate the volume, in ml., of a 2.0-M solution of KS required to prepare exactly 100 ml of a 0.130-M solution of Kys ml Submit Show Approach Show Tutor Steps Submit Answer Try Another Version 10 item attempts remaining Click to try another version of this item. "Note that your response(s) and the points you have earned on this item will be cleared. Previous News)...
Calculate pH of a weak base solution. Please box answers!
Thank you!
Tutored Practice Problem 16.4.5 G S GRASS Calculate the pH of a weak base solution ([B]o > 100Ko). Close Problem Calculate the pH of a 0.286 M aqueous solution of hydroxylamine (NH,OH, Kb - 9.1x10') and the equilibrium concentrations of the weak base and its conjugate acid. PH (NH3OH)equilibrium [NH3OH lequilibrium - Check & Submit Answer Show Approach
UTOR Calculate K from Equilibrium Concentrations Some HI is placed in a sealed flask and heated to 775 K. When equilibrium is reached the flask is found to contain HII (0.137 M), H, (3.28X10M), and (23X10M) What is the value of the equilibrium constant for this reaction at 775 K? 2HI(g) H +1 K-L Submit Show Approach Show.tor Steps Try Another Version 9 item attempts Submit Answer
TUTOR STEP The equilibrium concentrations can then be calculated from the value of x. Enter them here. H2O(l) HB+ (aq) + 0.15 0 B(aq) + Initial (mol/L) Change (mol/L) -8.7 x 10-5 Equilibrium (mol/L) 0.15 – 8.7 x 10-5 OH(aq) 0 +8.7 x 10-5 8.7 x 10-5 +8.7 x 10-5 8.7 x 10-5 pOH = -log[OH ]. Use this to calculate pH using pH = 14.00 - POH. [B] = 0.149 mol/L [HB]= mol/LX [OH'] = mol/L X pH =...
help please
Pyridine is a weak organic base, and readily forms a salt with hydrochloric acid. CsH; N(aq) + HCl(aq) = CsH NH+ (aq) + CI(aq) CI", if K, for pyridine is 1.5 x What is the pH of a 0.018 M solution of pyridinium hydrochloride, C, H, NH pH = Submit Answer Try Another Version 2 item attempts remaining
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