A buffer solution is made by dissolving 0.230 moles of sodium hypochlorite in 1.00 L of...

A buffer solution is made by dissolving 0.230 moles of sodium hypochlorite in 1.00 L of 0.220 M hypochlorous acid (HClO). What is the pH of the solution after 0.0100 moles of sodium hydroxide is added? (The Ka of HClO is 2.9

Solutions

Expert Solution

Moles of HClO = M * V = 0.220 M * 1 L = 0.220 mol

Moles of NaClO = 0.230 mol

HClO + NaOH ------------> NaClO + H2O

0.220 0.01 0.230 ( Initial)

- 0.01 - 0.01 + 0.01 (change)

0.21 0 0.24 (Final)

Now,

pH before addition of NaOH is

pH = pKa + log( [ NaClO] / [HClO] )

pH = - log( 2.9 x 10^-8) + log(0.230 / 0.220)

pH = 7.537 + 0.02 = 7.56

pH after addition of NaOH is

pH = 7.56 + log[ ( NaClO)_left / (HClO)_left ]

pH = 7.56 + log( 0.24 / 0.21)

pH = 7.56 + 0.058 = 7.618 = 7.62

queen_honey_blossom answered 2 hours ago

Next > < Previous

Related Solutions

What is the pH of a buffer solution made by dissolving 10 g of sodium acetate...

What is the pH of a buffer solution made by dissolving 10 g of sodium acetate in 200 ml of 1M acetic acid? The Ka for acetic acid id 1.7*10-5. B. Calculate the pH of the solution if 10 ml of 0.100M HCl is added to the solution. C. What will the pH be if 5.00 ml of 0.150M NaOH was added to solution in B? D. Write the equation when an acid and a base are added to the...

A 300.0 mL buffer solution is 0.230 M in acetic acid and 0.230 M in sodium...

A 300.0 mL buffer solution is 0.230 M in acetic acid and 0.230 M in sodium acetate. Part A: What is the initial pH of this solution? Part B: What is the pH after addition of 0.0050 mol of HCl? Part C: What is the pH after addition of 0.0050 mol of NaOH?

A solution is made by a dissolving 16.8 g of sodium fluoride , NaF , in...

A solution is made by a dissolving 16.8 g of sodium fluoride , NaF , in enough water to make exactly 500.ml of solution . Calculate the molarity of each species: NaF, Na+ and F-.

A buffer is made by dissolving 4.800 g of sodium formate (NaCHO2) in 100.00 mL of...

A buffer is made by dissolving 4.800 g of sodium formate (NaCHO2) in 100.00 mL of a 0.30 M solution of formic acid (HCHO2). The Ka of formic acid is 1.8 x 10-4. a) What is the pH of this buffer? b) Write two chemical equations showing how this buffer neutralizes added acid and added base. c) What mass of solid NaOH can be added to the solution before the pH rises above 4.60?

A buffer is made by dissolving 4.900 g of sodium formate (NaCHO2) in 100.00 mL of...

A buffer is made by dissolving 4.900 g of sodium formate (NaCHO2) in 100.00 mL of a 0.31 M solution of formic acid (HCHO2). The Ka of formic acid is 1.8 x 10-4. a) What is the pH of this buffer? b) Write two chemical equations showing how this buffer neutralizes added acid and added base. c) What mass of solid NaOH can be added to the solution before the pH rises above 4.60?

A 1.00 liter solution contains 0.42 moles nitrous acid and 0.32 moles sodium nitrite . If...

A 1.00 liter solution contains 0.42 moles nitrous acid and 0.32 moles sodium nitrite . If 0.16 moles of nitric acid are added to this system, indicate whether the following statements are True or False. (Please Explain Your Answers!) (Assume that the volume does not change upon the addition of nitric acid.) A. The number of moles of HNO2 will decrease. B. The number of moles of NO2- will remain the same. C. The equilibrium concentration of H3O+ will increase....

A solution is made by dissolving 0.0100 mol of HF in 1.00 kg of water. The...

A solution is made by dissolving 0.0100 mol of HF in 1.00 kg of water. The solution was found to freeze at –0.0236 °C. Calculate the value of i and estimate the percent ionization of HF in this solution. i =____ so HF is ______

A solution is made by dissolving 0.0100 mol of HF in 1.00 kg of water. The...

A buffer solution is prepared by dissolving 0.250 mol of solid methylamine hydrochloride (CH3NH3Cl) in 1.00...

A buffer solution is prepared by dissolving 0.250 mol of solid methylamine hydrochloride (CH3NH3Cl) in 1.00 L of 1.10 M methylamine (CH3NH2). The Kb for methylamine is 4.40x10-4. (Assume the final volume of the solution is 1.00 L). A) Write a balanced molecular, total ionic, and net ionic equation for the completion reaction that occurs when NaOH is added to this buffer. B) What is the pH of the solution when 100.0 mL of 1.15 M NaOH is added? (show...

A 1.00 liter solution contains 0.24 M hypochlorous acid and 0.31 M sodium hypochlorite. If 0.160...

A 1.00 liter solution contains 0.24 M hypochlorous acid and 0.31 M sodium hypochlorite. If 0.160 moles of potassium hydroxide are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of potassium hydroxide.) A. The number of moles of HClO will decrease. B. The number of moles of ClO- will increase. C. The equilibrium concentration of H3O+ will remain the same. D. The pH will decrease....

Subjects