9. 100 mL of 0.5M HNO2 (Ka = 4.5*10-4) is titrated with 0.5M KOH.
What is the pH after 100mL of 0.5M KOH is titrated into the acid?
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9. 100 mL of 0.5M HNO2 (Ka = 4.5*10-4) is titrated with 0.5M KOH. What is...
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.
A 42.0 mL sample of 0.120 M HNO2 is titrated with 0.214 M KOH. (Ka for HNO2 is 4.57×10−4.) Determine the pH at the equivalence point for the titration of HNO2 and KOH.
A 41.0 mL sample of 0.174 M HNO2 is titrated with 0.264 M KOH. (Ka for HNO2 is 4.57×10−4.) Determine the pH at the equivalence point for the titration of HNO2 and KOH.
A 40.0 mL sample of 0.150 M HNO2 (Ka = 4.60 x 10-4) is titrated with 0.200 M KOH. Calculate: a. the pH after adding 10.00 mL of KOH b. the pH at one-half the equivalence point c. the pH after adding 20.00 mL of KOH d. the volume required to reach the equivalence point e. the pH at the equivalence point f. the pH after adding 45.00 mL of KOH
50.0 mL of 0.090 M nitrous acid (HNO2, Ka = 7.1 x 10-4), is titrated with 0.100 M NaOH, requiring 45.0 mL of strong base to reach the equivalence point. (a) What will be the pH after 35.0 mL of NaOH have been added? (b) What will be the pH at the equivalence point? (c) What will be the pH after 60.0 mL of NaOH have been added?
a solution of nitrous acid (HNO2 , Ka=4.5*10^-4) has a pH OF 1.85. How many grams of nitrous acid are there in 100 ml of the solution?
A 15.0 mL sample of 0.21 M nitrous acid (HNO2), Ka = 4.6x10-4) is titrated with 0.15 M NaOH. Calculate the pH after the addition of the following volumes of base: a. 0.00 mL b. 10.00 mL c. 21.00 mL d. 25.00 mL
A 15 mL sample of hydrofluoric acid, Ka=6.8x10^-4 was titrated with .475 M KOH. The equivalence point was reached after addition of 19.35 mL of base. Determine the molar concentration of the original hydrofluoric acid solution, and find the pH of the solution.
Nitrous acid, HNO2(aq), has a Ka of 4.5 x 10-4 at 25 °C. What is the pH of a solution that contains 1.0 M KNO2(aq) and 0.50 M HNO2(aq).
What is the pH of aqueous 0.10 M HNO2? Ka(HNO2) = 4.5 x 10-4 a. 1.67 b. 3.35 c 1.00 d. 4.35 e. 2.17