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![Qu. consider an acid HA HA ? Ht + Á Ka= [H+] [A-] LHA) The younla you calculating the pH of a weak acid is pH = -dog (CHA] x](http://img.homeworklib.com/questions/e683bab0-6ea0-11ea-8181-c1dab32f1e9b.png?x-oss-process=image/resize,w_560)
need question 6 5. What is the pH for a base if the concentration is 0.0045 M and Kb = 2.3 * 10-7? 6. What is the...
need question 6
5. What is the pH for a base if the concentration is 0.0045 M and Kb = 2.3 * 10-7? 6. What is the pH of 0.59 M NaNO2 if the K, for HNO2 is 7.1*10-47 Dan D . .
need question 5 5. What is the pH for a base if the concentration is 0.0045...
need question 5
5. What is the pH for a base if the concentration is 0.0045 M and Kb = 2.3 * 10-7? 6. What is the pH of 0.59 M NaNO2 if the K, for HNO2 is 7.1*10-47 Dan D . .
(Set 2) Practice Problems in Equilibrium All weak acids use this generic equation: HA(aq)+ H2O() A (aq) + H30*(aq) And...
(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) Determine the pH of a 0.0785 M unknown weak base solution. Kb of the unknown...
1) Determine the pH of a 0.0785 M unknown weak base solution. Kb of the unknown weak base is 4.7 x 10−6. 2) An unknown weak acid solution with a concentration of 0.0850 M has a pH of 4.35. What is the Ka for this weak acid? 3) What is the pH of a 0.0380 M solution of HNO2? (Use your workbook to find Ka) 4) An unknown weak base solution with a concentration of 0.187 M has a pH...
1. What is the Kb for B-, if the Ka for the acid (HB) is 2.5...
1. What is the Kb for B-, if the Ka for the acid (HB) is 2.5 x 10-8? 2. What is the hydronium ion concentration of a 3.50 x 10-2 M solution of the monoprotic acid, HBrC6H4COO, for which Ka = 1.00 x 10-4? 3. What is the Ka value for HB, if a solution that is 0.25 M B- and 0.55 M HB produces a pH of 4.95? 4. Calculate the pH of a solution containing .225 moles of...
What is the pH of a solution prepared to 0.040 M NaNO2. Ka HNO2 = 7.1...
What is the pH of a solution prepared to 0.040 M NaNO2. Ka HNO2 = 7.1 x 10-4
A) Calculate the pH of a 0.0116 M aqueous solution of methylamine (CH3NH2, Kb = 4.2×10-4)...
A) Calculate the pH of a 0.0116 M aqueous solution of methylamine (CH3NH2, Kb = 4.2×10-4) and the equilibrium concentrations of the weak base and its conjugate acid. pH = ? [CH3NH2]equilibrium = ? M [CH3NH3+ ]equilibrium = ? M B)Calculate the pH of a 0.0115 M aqueous solution of nitrous acid (HNO2, Ka= 4.6×10-4) and the equilibrium concentrations of the weak acid and its conjugate base. pH = ? [HNO2]equilibrium = ? M [NO2- ]equilibrium = ? M C)...
Post-Lab Assignment: pH and Buffers 1. A buffer is prepared from a weak acid with a...
Post-Lab Assignment: pH and Buffers 1. A buffer is prepared from a weak acid with a Ka - 7.1 x 104 and its conjugate base. a. What pH would provide maximum buffer capacity? b. What would be the buffer range for this acid? (Your answer should show the lowest and the highest pH that would provide a reasonably effective buffer.) 2. If you were provided with a 0.1 M solution of an unknown weak acid and a 0.1 M solution...
Which of the following combinations would make a buffer with pH close to 3.0? HClO2 Ka...
Which of the following combinations would make a buffer with pH close to 3.0? HClO2 Ka = 1.1 × 10-2 NH3 Kb = 1.8 × 10-5 HNO2 Ka = 7.2 × 10-4 C5H5N Kb = 1.5 × 10-9 Equal volumes of 0.10 M NH4Cl and 0.10 M NH3 Equal volumes of 0.10 M HClO2 and 0.10 M NaClO2 Equal volumes of 0.10 M HNO2 and 0.10 M NaNO2 Equal volumes of 0.10 M HCl and 0.10 M NaCl Equal volumes...
You have nitrous acid, HNO2, Ka=4.0 x 10-4 Calculate the pH of the solution and calculate...
You have nitrous acid, HNO2, Ka=4.0 x 10-4 Calculate the pH of the solution and calculate the concentration of HNO2 and its conjugate base in a 0.025 M HNO2 Solution. Please please show all work!
need question 6
5. What is the pH for a base if the concentration is 0.0045 M and Kb = 2.3 * 10-7? 6. What is the pH of 0.59 M NaNO2 if the K, for HNO2 is 7.1*10-47 Dan D . .
need question 5
5. What is the pH for a base if the concentration is 0.0045 M and Kb = 2.3 * 10-7? 6. What is the pH of 0.59 M NaNO2 if the K, for HNO2 is 7.1*10-47 Dan D . .
(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...
Post-Lab Assignment: pH and Buffers 1. A buffer is prepared from a weak acid with a Ka - 7.1 x 104 and its conjugate base. a. What pH would provide maximum buffer capacity? b. What would be the buffer range for this acid? (Your answer should show the lowest and the highest pH that would provide a reasonably effective buffer.) 2. If you were provided with a 0.1 M solution of an unknown weak acid and a 0.1 M solution...
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