Homework Answers
ADDITION OF NH3 IN WATER PRODUCES WEAK BASE NH4OH .
THUS THE pH > 7 FOR AQUEOUS SOLUTION OF AMMONIA
ON ADDITION OF NH4NO3 IT IS A SALT HAVING COMMON ION NH4+ THUS WILL EXERT COMMON ION EFFECT ON DISSOCIATION OF NH4OH CAUSING THE EQUILLIBRIUM TO SHIFT BACKWARDS THEREBY DECREASING THE CONCENTRATION OF BOTH NH4+ IONS AND OH- IONS
THUS IT WILL ALSO DECREASE THE pH OF THE SOLUTION
IT WILL SHIFT THE
NH3 + H2O = NH4OH
EQUILLIBIRUM TOWARDS AMMONIA THAT IS IT SHIFTS THE REACTION BACKWARDS THUS
REACTION SHIFTS TOWARDS LEFT
HENCE A AND B ARE THE CORRECT OPTIONS
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You have an aqueous solution of the weak base NH, and you measure the pH. If...
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Predicting pH Imagine you have a 0.125 M aqueous solution of aspirin, an acid drug with...
Predicting pH
Imagine you have a 0.125 M aqueous solution of aspirin, an acid drug with pKa = 3.5, in equilibrium. a) Estimate the pH of the solution Hint: Determine if it is an acid or base solution, weak or strong If weak acid/base, first try (H+) = /K,C, or [OH-] = K,C, b) Predict what would happen to the pH when you add more H2 Hint: First figure out what happens to the concentrations HA(aq) + H2O(0) A (aq)...
Calculate the pH of a Weak Base Question The weak base dimethylamine, NH(CHs)2, has a molar...
Calculate the pH of a Weak Base Question The weak base dimethylamine, NH(CHs)2, has a molar mass of 45.09 g/mol and a base-dissociation constant K, 5.4 x 10. What is the pH of an aqueous solution of dimethylamine that contains 2.04 g of dimethylamine in 0.100 L of solution? Use pK 14.0 for the ion-product of water. Round your answer to one decimal place. Provide your answer below pi-14.0 FEEDBACK MORE INSTRUCTION Content attribution
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
is a solution that resists changes in pH when a small amount of acid or base...
is a solution that resists changes in pH when a small amount of acid or base is added to best buffer solutions are prepared from weak acids and their conjugate base added as a sodium of potassium salt. Most biological systems must maintain a very narrow range of pH; therefore, buffers allow the biological solution to function correctly. Blood is a good example of a biological system that must maintain a pH in a very narrow range from 7.3 to...
A)Calculate the pH of a weak base solution ([B]0 > 100 • Kb). Close Problem Calculate the pH o...
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Calculate the pH of a 0.0198 M aqueous solution of dimethylamine ((CH),NH, Kn=5.9x104) and the equilibrium concentratio...
Calculate the pH of a 0.0198 M aqueous solution of dimethylamine ((CH),NH, Kn=5.9x104) and the equilibrium concentrations of the weak base and its conjugate acid. PH M [(CH3)2NH)equilibrium [(CH3)2NH2 Lequilibrium = C =
a OH Old Exam Question Example #2 Imagine you have a 0.125 M aqueous solution of...
a OH Old Exam Question Example #2 Imagine you have a 0.125 M aqueous solution of aspirin, an acid drug with pk, = 3.5, in equilibrium. a) Estimate the pH of the solution Hint: Determine if it is an acid or base solution, weak or strong If weak acid/base, first try (H*] = KC, or [OH-] = K,C, b) Predict what would happen to the pH when you add more H20 Hint: First figure out what happens to the concentrations...
9.34 correct 1/1 2. The pH of a 1.66 M solution of a weak base B...
9.34 correct 1/1 2. The pH of a 1.66 M solution of a weak base B is measured to be 10.51 Determine Kb of the base no answer given 0/1 Determine K, of the weak bases's conjugate acid, HB no answer given 0/1 Determine [H*] in a 2.00 M solution of the chloride salt, HBCI M no answer given 0/1 Determine the pH of a 2.00 M solution of the chloride salt, HBCI no answer given 0/1 Your grade will...
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The pH of an aqueous solution of 0.328 M trimethylamine (a weak base with the formula (CHN) is The hydronium ion concentration of an aqueous solution of 0.493 M hydroxylamine (a weak base with the formula NH,OH) is ... [H,0") - M The pOH of an aqueous solution of 0.445 M trimethylamine (a weak base with the formula (CH),N) is
Predicting pH
Imagine you have a 0.125 M aqueous solution of aspirin, an acid drug with pKa = 3.5, in equilibrium. a) Estimate the pH of the solution Hint: Determine if it is an acid or base solution, weak or strong If weak acid/base, first try (H+) = /K,C, or [OH-] = K,C, b) Predict what would happen to the pH when you add more H2 Hint: First figure out what happens to the concentrations HA(aq) + H2O(0) A (aq)...
Calculate the pH of a Weak Base Question The weak base dimethylamine, NH(CHs)2, has a molar mass of 45.09 g/mol and a base-dissociation constant K, 5.4 x 10. What is the pH of an aqueous solution of dimethylamine that contains 2.04 g of dimethylamine in 0.100 L of solution? Use pK 14.0 for the ion-product of water. Round your answer to one decimal place. Provide your answer below pi-14.0 FEEDBACK MORE INSTRUCTION Content attribution
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
is a solution that resists changes in pH when a small amount of acid or base is added to best buffer solutions are prepared from weak acids and their conjugate base added as a sodium of potassium salt. Most biological systems must maintain a very narrow range of pH; therefore, buffers allow the biological solution to function correctly. Blood is a good example of a biological system that must maintain a pH in a very narrow range from 7.3 to...
Calculate the pH of a 0.0198 M aqueous solution of dimethylamine ((CH),NH, Kn=5.9x104) and the equilibrium concentrations of the weak base and its conjugate acid. PH M [(CH3)2NH)equilibrium [(CH3)2NH2 Lequilibrium = C =
a OH Old Exam Question Example #2 Imagine you have a 0.125 M aqueous solution of aspirin, an acid drug with pk, = 3.5, in equilibrium. a) Estimate the pH of the solution Hint: Determine if it is an acid or base solution, weak or strong If weak acid/base, first try (H*] = KC, or [OH-] = K,C, b) Predict what would happen to the pH when you add more H20 Hint: First figure out what happens to the concentrations...
9.34 correct 1/1 2. The pH of a 1.66 M solution of a weak base B is measured to be 10.51 Determine Kb of the base no answer given 0/1 Determine K, of the weak bases's conjugate acid, HB no answer given 0/1 Determine [H*] in a 2.00 M solution of the chloride salt, HBCI M no answer given 0/1 Determine the pH of a 2.00 M solution of the chloride salt, HBCI no answer given 0/1 Your grade will...
Salt of a Weak Base and a Strong Acid. pH of Solution. Calculate the pH of a 1.19 M aqueous solution of triethylamine hydrochloride ((C2H5)3NHCI) (For triethylamine, (C2H5)3N, Kb = 4.00x 10-4.) Give two decimal places in your answer.
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