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12. Determine the pH of a 3.0 M solution of a weak base at 25.0°C if AH° is -17.5 kJ/mol and AS° is -110.5 J/mol-K.
In aqueous solution, the azide ion, N3−, is a weak base that accepts a proton from water to form the hydroxide ion, OH −, and hydrazoic acid, HN3, according to the following equation. N3−(aq) + H2O(l) equilibrium reaction arrow OH −(aq) + HN3(aq) The base-dissociation constant (Kb) for this base is 4.04 ✕ 10−10. If a 0.082 M solution of azide ions is prepared, what is the final pH of the solution? (Assume that the temperature is 25°C.)
Model 2: A weak base increases the hydroxide concentration of a solution, but the amount of reaction is small. Na OH 圖B molecule ON BH+ ion H20 molecules are not shown H20 molecules are not shown A solution of a strong base, NaOH A solution of a weak base, B Critical Thinking Questions 7. How was the species BH produced in Model 2? 8. Complete and balance the following reaction equation for the weak base pyridine: CsH5N(aq) + H20(I) =...
The degree to which a weak base dissociates is given by the base-ionization constant, Kb. For the generic weak base, B B(aq)+H2O(l)⇌BH+(aq)+OH−(aq) this constant is given by Kb=[BH+][OH−][B] Strong bases will have a higher Kb value. Similarly, strong bases will have a higher percent ionization value. Percent ionization=[OH−] equilibrium[B] initial×100% Strong bases, for which Kb is very large, ionize completely (100%). For weak bases, the percent ionization changes with concentration. The more dilute the solution, the greater the percent ionization....
For a weak base (B), a 0.0100 M and a 0.100 M solution was made. Students obtained the following pH value for the solution. Fill in the table. Report all answers (except pH or pOH values) in scientific notation. 0.0100 M B 0.100 M B pOH 4.32 3.48 [OH-] [BH+] [B] (at equilibrium) Kb For the same solution fill out the following information: 0.0100 M B 0.100 M B pH (Do not...
what is the pH of a buffer solution containing 0.23 M HNO2 and 0.15 M NO2 Nitrous acid has a Ke of 4.5 x 10-4. Part A What is the pH of a buffer solution containing 0.23 M HNO2 and 0.15 M NO? Express your answer using two decimal places. 19 AEO ? pH = Submit Request Answer Provide Feedback Google Drive @ Quinet C Chego Coinmame R PL Access SIUE CHW11 Chapter 11 Homework Problem 25 25 of 25...
percent ionization of a weak base pH and Percent lonization of a Weak Base Ammonia, NH, is a weak base with a Ky, value of 1.8 x 105 The degree to which a weak base dissociates is given by the base ionization content K) For the generic weak base, B B(aq) + H2O(1) BH(aq) + OH (!) this constant is given by Pan A KDO What is the pH of a 0.165 Mammonia solution? Express your answer numerically to two...
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)...
(Set 2) Practice Problems in Equilibrium All weak acids use this generic equation: HA(aq)+ H2O() A (aq) + H30*(aq) And all weak bases use this one: B(aq)+ H2O(I) = BH*(aq)+ OH'(aq) Part A: Finding K, or Kb 3.012? What is the value of Ka for a weak acid if a 1.44 M solution has a pH 1. 2. A weak acid is 0.00987 M, but is found to be 25.5 % ionized. What is the pH? 3. The pH for...
1 . If a buffer solution is 0.260 M in a weak acid (?a=8.3×10−5)and 0.480 M in its conjugate base, what is the pH? pH= 2. If a buffer solution is 0.200 M in a weak base (?b=5.0×10−5) and 0.530 M in its conjugate acid, what is the ph 3. Phosphoric acid is a triprotic acid (?a1=6.9×10−3, ?a2=6.2×10−8 , and ?a3=4.8×10−13 To find the pH of a buffer composed of H2PO4 - (aq) ) and HPO4 2− (aq) , which...