If 100ml of a 0.134 M solution of HNO2 and 0.056 LiNO2 is reacted with 50ml of a 0.100 M of KOH what is the resulting pH of the solution? Ka=4.6 x 10^-4
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If 100ml of a 0.134 M solution of HNO2 and 0.056 LiNO2 is reacted with 50ml...
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1.A 25.00 ml smaple of 0.523 M nitrous acid, HNO2, solution is titrated with a 0.213 M NaOH. For HNO2, Ka = 4.0 X 10^-4 a) What is the pH before any NaOH is added? b) Write the reaction that takes place as KOH solution is added to the HNO2 solution. c) write the reaction that determines the pH at the equivialnce point. -What is the pH at the equivilance point -what is the pH at the 1/2 equivilance point...
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a) A 41.0 mL sample of 0.194 M HNO2 is titrated with 0.220 M KOH. (Ka for HNO2 is 4.57×10−4.) Determine the pH at the equivalence point for the titration of HNO2 and KOH. b) A 50.0-mL sample of 0.200 M sodium hydroxide is titrated with 0.200 M nitric acid. Calculate the pH of the solution, after you add a total of 56.7 mL 0.200 M HNO3.
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Part A What is pH of 1.2 M solution of HNO2. Ka 4.6*104 SubmitF Request Answer
6. Calculate the pH of 0.010 M HNO2 solution. The K, for HNO2 is 4.6 x 104 Answer: pH = 2.72