How much 0.939 M LiOH will be needed to raise the pH of 0.381 L of 4.51 M ascorbic acid (H2C6H6O6) to a pH of 10.89?
How much 0.939 M LiOH will be needed to raise the pH of 0.381 L of...
How many liters of 0.951 M LiOH will be needed to raise the pH of 0.263 L of 4.55 M carbonic acid (H2CO3) to a pH of 9.904?
How many liters of 0.669 M KOH will be needed to raise the pH of 0.339 L of 4.01 M carbonic acid (H2CO3) to a pH of 9.727? Ka=5.6×10–11
How much LiOH (in grams) is needed to prepare 475 mL of solution with a pH of 11.2 ?
How many liters of 0.547 M koh will be needed to raise the ph of 0.223L of 4.77 M absorbic acid to a ph of 11.11?
What is the pH of a solution that consists of 0.50 M H2C6H6O6 (ascorbic acid) and 0.75 M NaHC6H6O6 (sodium ascorbate)? What is the pH if 20.0 mL of a 0.280 M perchloric acid is added to 200.mL of the ascorbic acid sodium ascorbate solution? What is the pH if 30.0 mL of a 0.125 M sodium hydroxide is added to 200.mL of the ascorbic acid sodium ascorbate solution? The ionization constant for ascorbic acid is 6.8 x 10–5
please help with this one What will the pH of a solution be when 0.3678 L of 2.657 M KOH is added to 0.231 L of 1.77 M ascorbic acid (H2C6H6O6)? Enter your answer to 4 significant figures. (click here to open a table of Ka and Kb values in a new window) pH of solution Tries 0/2 Submit Answer
Calculate the pH of a 0.05 M solution of ascorbic acid ( H2C6H6O6 = H2ASC) Ka1 = 1 x 10-5 Ka2= 5 x 10-12 H2ASC (aq) + H2O (l) <=> H3O+ (aq) + HASC- (aq)
Calculate the pH and the concentrations of all species present in 0.11 M ascorbic acid (H2C6H6O6) solution. (Ka1=8.0×10−5), (Ka2=1.6×10−12) Part A: Calculate the pHpH of a 0.11 MM solution of ascorbic acid. Part B: Calculate the concentration of H2C6H6O6 in a 0.11 MM solution of ascorbic acid. Part C: Calculate the concentration of HC6H6O6−HC6H6O6− in a 0.11 MM solution of ascorbic acid. Part D: Calculate the concentration of C6H6O62−C6H6O62− in a 0.11 MM solution of ascorbic acid Part E: Calculate...
Find the pH of a 0.225 M ascorbic acid (H2C6H6O6) solution. Find the equilibrium concentration of C6H6O6 -2. Ka1 = 8.01 x 10-5 Ka2 = 1.59 x 10-12
An aqueous solution contains 0.381 M ammonia (NH3). How many mL of 0.215 M hydrochloric acid would have to be added to 250 mL of this solution in order to prepare a buffer with a pH of 9.090?