50. ml of a 1.0 M solution of hydrochloric acid, HCl, is titrated with a 1.0 M solution of sodium hydroxide. What is the pH after 51 mL of NaOH has been added? Assume that the volumes are additive.
As the NaOH solution is added to the HCl solution, H+(aq) reacts with OH–(aq) to form H2O.
Both Na+ and Cl– are spectator ions, having negligible effect on the pH.
In order to determine the pH of the solution, we must first determine how many moles of H+ were originally present and how many moles of OH– were added. We can then calculate how many moles of each ion remain after the neutralization reaction.
In order to calculate [H+], and hence pH, we must also remember that the volume of the solution increases as we add titrant to the solution, thus diluting the concentration of all solutes present.
The number of moles of H+ in the original HCl solution = molarity * volume = 1.0 mol/litre * 0.050 litre = 0.05 moles
The number of moles of OH– in 51.00 mL of 1 M NaOH = 1 * 0.051 = 0.051 moles
here we have crossed the equivalence point and the solution have more OH- ions than H+ ions.
so here H+ is the limiting ion
=> 0.05 moles of H+ will react with 0.05 moles of OH– ions
so the remaining moles of OH– = 0.051 - 0.05 = 0.001 moles
During the course of the titration the volume of the reaction mixture increases as the NaOH solution is added to the HCl solution.
total volume of the solution = 50 + 51 = 101 ml = 0.101 L
hence the concentration of OH– = moles / volume = 0.001 / 0.101 = 9.9*10-3 moles / L
pOH of the solution = - log (concentration of OH– ) = - log ( 9.9*10-3 ) = 2.004 = 2
pH = 14 - pOH = 14 - 2 = 12
50. ml of a 1.0 M solution of hydrochloric acid, HCl, is titrated with a 1.0...
If 32.12 mL of 3.77 M hydrochloric acid solution, HCl, are titrated with 51.5 mL of sodium hydroxide solution, NaOH, according to HCl(aq) + NaOH(aq) - NaCl(aq) + H2O(1) what is the concentration of the sodium hydroxide solution? (Enter your
5.00 mL of 0.250 M ammonia (NH3) is titrated with 0.100 M hydrochloric acid (HCl). The Kb for ammonia is 1.75 x 10-5 What is the pH of the ammonia solution prior to the addition of any HCl? What is the pH of the solution after 5.00 mL of HCl has been added?
1) When a 21.5 mL sample of a 0.337 M aqueous nitrous acid solution is titrated with a 0.373 M aqueous sodium hydroxide solution, what is the pH after 29.1 mL of sodium hydroxide have been added 2) A 28.6 mL sample of 0.226 M methylamine, CH3NH2, is titrated with 0.221 M nitric acid. After adding 11.5 mL of nitric acid, the pH is 3) A 24.0 mL sample of 0.372 M methylamine, CH3NH2, is titrated with 0.381 M hydrochloric...
A) A 21.5 mL sample of a 0.452 M aqueous nitrous acid solution is titrated with a 0.356 M aqueous sodium hydroxide solution. What is the pH at the start of the titration, before any sodium hydroxide has been added? pH = B) A 42.1 mL sample of a 0.399 M aqueous acetic acid solution is titrated with a 0.219 M aqueous sodium hydroxide solution. What is the pH after 51.8 mL of base have been added? pH = C)...
When a 26.7 ml sample of a 0.361 M aqueous nitrous acid solution is titrated with a 0.346 M aqueous sodium hydroxide solution, what is the pH after 41.8 mL of sodium hydroxide have been added? pH- A 47.8 ml sample of a 0.422 M aqueous nitrous acid solution is titrated with a 0.473 M aqueous sodium hydroxide solution. What is the pH after 17.2 mL of base have been added? pH-
(1) A 31.4 mL sample of a 0.531 M aqueous nitrous acid solution is titrated with a 0.305 M aqueous barium hydroxide solution. What is the pH after 10.4 mL of base have been added? (2) When a 28.7 mL sample of a 0.424 M aqueous hydrofluoric acid solution is titrated with a 0.352 M aqueous sodium hydroxide solution, what is the pH after 51.9 mL of sodium hydroxide have been added?
A 75 mL solution of .400 M chlorous acid is titrated with a .125 M solution of sodium hydroxide. What is the pH of the solution after 380 mL of the sodium hydroxide solution has been added? Ka for chlorous acid is 1.1 x 10-2. (hint: your answer should contain four significant figures)
A 200. mL solution of 0.25 M ammonia is titrated with 1.0 M HCl. Calculate the pH after 60 mL of HCl have been added.
25. A 50.0 mL sample of 0.150 M weak acid was titrated with a 0,150 M NaOH solution. What is the pH after 30.0 mL of the sodium hydroxide solution is added? The Ka of the acid is 1.9x10(3 points) D) 4.78 E) None of these C) 3.03 (A) 4.90 B) 1.34 26. A 25.0 mL sample of 0.25 M hydrofluoric acid (HF) is titrated with a 0.25 M NaOH solution. What is the pH after 38.0 mL of base...
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 =