You have 1.25 L of a 2.00 M solution of Hypochlorous acid, HClO to which you will add 1.5 M NaOH to adjust the pH.
a) what is the pH of hte solution when 0.500 L of NaOH is added?
b) How many mL of soldium hydroxide should be added to prepare the 7.00 pH buffer solution?
c) If 75.0 mL of 1.5 M Ba(OH)2 is added to the buffer in part 'b' when it is starting at pH 7.00 before adding Ba(OH)2, what is the new pH? Ba(OH)2 is a strong dihydroxic base.
You have 1.25 L of a 2.00 M solution of Hypochlorous acid, HClO to which you...
A buffer solution is made by adding 1.00 M weak acid (pKa = 4.45) to 1.25 M solution of its conjugate base to make 100 mL of buffer solution. Calculate the pH after 75.0 mL of 0.725 M strong acid has been added.
A 50 mL sample of 0.150 M hypochlorous acid (one of weak acids) is titrated with a 0.150 M NaOH (one of strong bases) solution. The acid-base equation is as follows: HClO (aq) + OH-(aq) → H2O(l) + ClO-(aq) What is the pH after 25 mL of base is added?
Ka for hypochlorous acid, HClO, is 3.0 x 10^-8. Calculate the pH after 10.0, 20.0, 30.0, and 40.0 ml of 0.100M NaOH have been added to 40.0ml of 0.100M HClO. Expert Answer GoldenApple6699 GoldenApple6699 answered this Was this answer helpful? 8 0 766 answers At any point between 0 and 40 mL of NaOH added, you will have a solution containing both HClO and ClO- ... that's a buffer system (a weak acid and its conjugate base) and the pH...
Calculate the pH of a solution produced by adding 0.50 L of 1.00 M HCl to 0.50 L of 2.00 M NaClO. Ka(HClO) = 2.9x10-8 Calculate the pH of a solution produced by adding 0.50 L of 1.00 M NaOH to 0.50 L of 2.00 M HClO. Ka(HClO) = 2.9x10-8 It is desired to have a buffer with a pH = 5.000 using acetic acid. If [HAc] + [Ac─ ] = 0.500 M, what is the required [HAc] and [Ac─...
1) When a 18.9 mL sample of a 0.401 M aqueous hypochlorous acid solution is titrated with a 0.426 M aqueous sodium hydroxide solution, what is the pH after 26.7 mL of sodium hydroxide have been added? 2) A buffer solution contains 0.381 M NaHSO3 and 0.281 M K2SO3. Determine the pH change when 0.083 mol HCl is added to 1.00 L of the buffer. pH change =
15.1 A 39.8 mL sample of a 0.448 M aqueous hypochlorous acid solution is titrated with a 0.234 M aqueous potassium hydroxide solution. What is the pH after 50.5 mL of base have been added? 15.2 What is the pH at the equivalence point in the titration of a 24.9 mL sample of a 0.313 M aqueous hypochlorous acid solution with a 0.479 M aqueous barium hydroxide solution? 12.1 How many grams of solid ammonium bromide should be added to...
1.) Calculate the pH of 1.0 L of the buffer 2.00 M CH3COONa/2.00 M CH2COOH before and after the addition of 0.090 mol NaOH. The Ka of CH2COOH is 1.8 x 10% 2.) A 0.4277 g sample of a monoprotic acid neutralizes 244 ml of 0.1381 M KOH solution. Calculate the molar mass of the acid. 3.) In a titration experiment, 27.4 ml of 0.613 M HCOOH neutralize 21.5 ml of Ba(OH)2. What is the concentration of the Ba(OH)2 solution?
Answer the following questions for titration of 10.00 mL of a hypochlorous acid solution with a 0.09975 M sodium hydroxide. 1. If 20.05 mL of the sodium hydroxide solution were required to reach the endpoint in the titration, what was the original concentration of the hypochlorous acid solution? 2. What was the initial pH of the hypochlorous acid solution (before any sodium hydroxide was added)? 3. What was the pH in the titration after addition of 4.01 mL of NaOH?...
An aqueous solution contains 0.475 M hypochlorous acid. How many mL of 0.277 M potassium hydroxide would have to be added to 225 mL of this solution in order to prepare a buffer with a pH of 7.450 ml
A buffer solution contains 0.355 M hypochlorous acid and 0.347 M sodium hypochlorite. If 0.0243 moles of hydrochloric acid are added to 125 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume does not change upon adding hydrochloric acid) pH=?