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Calculate the pH of a buffer solution of a .050M nitrous acid (HNO2, Ka = 4.5x10-4) and .1M KNO2.
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Can anyone help me with this question? Calculate the pH of a buffer solution of a...
What would be the pH of a buffer that contains 0.987 grams of Nitrous acid (HNO2) and 1.242 grams of sodium Nitrite (NaNO2), in 250ml of solution?(Ka of Nitrous acid = 4.5X10-4)
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Close Problens Calculate the pH of a weak acid solution (IHAb 100.Ka). Calculate the pH of a 0.406 M aqueous solution of nitrous acid (HNO,, K-4.5x10) and the equilibrium concentrations of the weak acid and its conjugate base. pHH [HNO2 lequilibrium NO2 lequilbrium Show Approach
Question 5 5 pts Calculate the pH of a solution that contains 0.191 M HNO2 and 0.336 M KNO2. The K, for nitrous acid (HNO2) is 4.5*10-4 3.59
A chemistry graduate student is given 450. mL of a 0.90 M nitrous acid (HNO2) solution. Nitrous acid is a weak acid with K-4.5x10 . What mass o KNO2 should the student dissolve in the HNO2 solution to turn it into a buffer with pH-3.20? You may assume that the volume of the solution doesn't change when the KNO2 is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.
12. Calculating pH of a buffer. a) A solution is prepared that is initially 0.44M in HNO2 and 0.093M in KNO2. Ka=4.5*10-4. Calculate pH. b) A solution is prepared that is initially 0.49M in CH3NH2 and 0.33 in CH3NH3CI. Kb=4.4*10-4. Calculate pH.
Find the pH of a 0.246 M KNO2 solution. (The Ka of nitrous acid, HNO2, is 4.6×10−4.)
Question 2: A) Calculate the pH of the buffer that results from mixing 56.1 mL of a 0.406 M solution of HCHO2 and 11.9 mL of a 0.606 M solution of NaCHO2. The Ka value for HCHO2 is 1.8×10−4 B) Calculate the initial pH and the final pH after adding 0.010 mol of NaOH. 300.0 mL of a buffer solution that is 0.225 M in HCHO2 and 0.280 M in KCHO2 C) Calculate the initial pH and the final pH...
7. (a) Define pH (b) Calculate the pH of 0.030 M Ba(OH)2 solution (c) Calculate the pH of a solution containing 0.085 M nitrous acid alone and a solution containing 0.085 M nitrous acid and 0.10 M potassium nitrite (KNO2). K, for HNO2 = 4.5 x 10-
Now calculate the [H+] and pH of a 0.00725
M solution of nitrous acid.
Nitrous acid (HNO2) is a weak acid that partially dissociates as follows, with a Ka = 0.0004266: HNO2 + H20 + H30+ + NO2 a) Calculate the [h+] and pH of a 1.73 M solution of nitrous acid. [H+]=49) 0.0270 b) pH = 49 1.57 c) Now calculate the [H+] and pH of a 0.00725 M solution of nitrous acid. 49) 0.0016 d) 49 1.7
13. Calculating the composition of a buffer of a given pH. a) Kb=5.4*10-4 125mL of 0.90M (CH3)2NH Calculate the mass of (CH3)2NH2Br should the student dissolve in the (CH3)2NH solution to turn into a buffer with pH=10.70. MW-125.9956g/mol b) Ka=4.5*10-4 125mL of 1.40M HNO2 solution Calculate the mass of KNO2 should the student dissolve in the HNO2 solution to turn into a buffer with pH=3.30