5. What is the pH of a 0.056 M HNO3 solution? A. 0.056 B. 1.25 C. 12.75 D. 2.88 E. 11.11
A 0.056 M solution of diethylamine has a pH of 11.90. What is the value of for this weak base?
Calculate the pH at the equivalence point in titrating 0.056 M solutions of each of the following with 0.013 M NaOH. (a) nitric acid (HNO3) pH = (b) arsenous acid (H3AsO3), Ka = 5.1e-10 pH = (c) ascorbic acid (HC6H7O6), Ka = 8e-05 pH =
A solution of HNO3 has a concentration of 1.75x10-4 M. a. What is the pH of the solution? ( write answer to the hundredths place) b. What is the pOH of the solution? ( write answer to the hundredths place) c. Is the solution acidic, basic or neutral?
Calculate the pH of a 1.260 M solution of HNO3.
A solution of HNO3 has a concentration of 1.75x10^-4 M. a. What is the pH of the solution? ( write answer to the hundredths place) b. What is the pOH of the solution? ( write answer to the hundredths place) c. Is the solution acidic, basic or neutral? please help
A) calculate the ph of a 0.028 M HNO3 solution B) Calculate the pH of a 0.028 M solution of benzoic acid (Ka=6.5x10^-5)
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
a) Determine the pH of a 2.3x10^−3 M solution of HNO3
What is the pH of a .75 M HNO3 solution? a. .12 b. .29 c. .63 d. .82 e >1.0