What is the pH of 0.15 M aqueous nitrite ion? (Kb of NO2– = 1.7 × 10–11) NO2–(aq) + H2O(l) HNO2(aq) + OH-(aq)
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Homework Answers
Answer:-
This question is solved by using simple concept of hydrolysis of salt of weak acid and then determination of pH.
The answer is given in the image,
![Answer: CNO2-J = 0.15 Kb = lo 7x10-11 Nog Cont 490 LUSZ HNO2009) + Onions Kb = CHNO3) (04-) [Mon] 107x10-11 = 2. 10.15 x2 = 2](http://img.homeworklib.com/questions/2f8394c0-d5f1-11eb-96fa-b1240d18c349.png?x-oss-process=image/resize,w_560)
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What is the pH of 0.15 M aqueous nitrite ion? (Kb of NO2– = 1.7
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Question 14
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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...
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Question 14
QUESTION 13 What is the final pH if 36.0 mL of 0.15 M of NaOH is added to 90.0 mL of 0.80 M acetic acid? Ky for acetic acid is 1.8 x 10-5, CH3COOH(aq) + OH(aq) + H2O(l) + CH3COO (aq) Note: No quadratic. Need ICE table QUESTION 14 The Ksp for Mg(OH)2 is 1.8 x 10-11. What is the concentration, in M, of OH ions in a saturated solution of Mg(OH)2? 52x104 1.7×104 3.3 x 10-4 26x104
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