Question

In: Chemistry

A buffer solution is formed by mixing 50mL of 0.30M HClO with 300mL of 0.20M NaClo....

A buffer solution is formed by mixing 50mL of 0.30M HClO with 300mL of 0.20M NaClo. The ka for HClO is 2.9 x 10^-8.

1. Write the buffer reaction including states and excluding spectator ions.

2. Calculate the initial concentration of each buffer component.

3. Calculate the pH of the buffer - be sure to include validation if approximations are used.

Solutions

Expert Solution

1. HClO + NaClO

weak acid and its salt with strong base is called acid buffer solution.

HClO                                           NaClO

M1 = 0.3                     M2 =                                                       M1 = 0.2M                              M2=

V1   = 50ml                  V2 = 50+300 = 350ml                           V1   = 3000ml                        V2 = 300+50= 350ml

M1V1   = M2V2                                                                                 M1V1   = M2V2          

   M2   = M1V1/V2    = 0.3*50/300 = 0.05M                                   M2   = M1V1/V2   = 0.2*300/350 = 0.1714M

            Ka = 2.9*10^-8

           PKa = -logKa

                     = -log2.9*10^-8   = 7.5376

         PH = PKa + log[NaClO]/[HClO]

                = 7.5376 + log0.1714/0.05

                = 7.5376 + 0.5354   = 8.073 >>>>answer


Related Solutions

A buffer solution is made that is 0.363 M in HClO and 0.363 M in NaClO...
A buffer solution is made that is 0.363 M in HClO and 0.363 M in NaClO . (1) If Ka for HClO is 3.50×10-8 , what is the pH of the buffer solution?   (2) Write the net ionic equation for the reaction that occurs when 0.082 mol HCl is added to 1.00 L of the buffer solution. Use H3O+ instead of H+ . A buffer solution is made that is 0.388 M in HCN and 0.388 M in NaCN. (1)...
A 200 ml buffer solution is made up of 0.20 M HClO and 0.15 M NaClO....
A 200 ml buffer solution is made up of 0.20 M HClO and 0.15 M NaClO. What is the pH after 1.71 grams of barium hydroxide is added to solution? (assume no volume change with addition)? HINTS: Ka of HClO is 2.9x108 and barium hydroxide has a molar mass of 171.35 g/mole.
Part A: What is the pH of solution made by mixing 300ml of 0.120M H2SO4 with...
Part A: What is the pH of solution made by mixing 300ml of 0.120M H2SO4 with 185ml of 0.150M Sr(OH)2? Part B: 250ml of 0.150M nitric acid is added to 300ml of 0.200M Sulfuric (H2SO4) and then diluted up to 1.000L, what is the resulting pH? Part C: How much 0.440M solution of Nitric Acid is needed to bring 22.1ml of 0.300M NaOH to neutrality?
What is the pH of a solution prepared by mixing 60.0 mL of 0.20M potassium carbonate...
What is the pH of a solution prepared by mixing 60.0 mL of 0.20M potassium carbonate (K2CO3) with 140.0 mL of 0.1M potassium bicarbonate (KHCO3)? a. 6.43 b. 6.30 c. 6.67 d. 10.32 e. 10.18
50 mL of 2.0 M NaOH is added to a 1.0L buffer solution that is 0.20M...
50 mL of 2.0 M NaOH is added to a 1.0L buffer solution that is 0.20M in HF and 0.20M in KF. The ka for HF is 3.5 x 10^-4. 1. Write the reaction or the buffer only including states and excluding spectator ions. 2. Write the neutralization reaction that occurs after the addition of LiOH including states and excluding spectator ions. 3. Calculate the amount of moles remaining and the final concentration for each component of the solution after...
1. For a buffer solution that is made of 200.0 mL of 0.300 M HCLO with...
1. For a buffer solution that is made of 200.0 mL of 0.300 M HCLO with 100.0 mL of 0.200 M KCLO. The Ka for HCLO is 2.9*10^8. What is the PH of the buffer? 2. Consider the same solution. To this solution, if 10.00 mL of 0.100 M HCl is added, what is the new pH? *both answers to 2 decimal places*
Just answers. A. A buffer solution that is 0.431 M in HClO and 0.431 M in...
Just answers. A. A buffer solution that is 0.431 M in HClO and 0.431 M in NaClO has a pH of 7.46. (1) The addition of 0.01 mol of H3O+ to 1.0 L of this buffer would cause the pH to _________(increase slightly, increase by 2 units,decrease slightly,decrease by 2 units,not change.) (2) The capacity of this buffer for added OH- could be increased by the addition of 0.147 mol  _________(of the weak acid,of the salt.) B. How many grams of...
Calculate the pH of a solution prepared by mixing 300mL of 0.250 m aqueous HF (dens=1.10g/mL)...
Calculate the pH of a solution prepared by mixing 300mL of 0.250 m aqueous HF (dens=1.10g/mL) with 43.6g of an aqueous solution that is 3.6% NaOH by mass. (dens=1.02g/mL).
A buffer solution is PARTIALLY neutralizing hypochlorous acid with sodium hydroxide; the Ka of HClO is...
A buffer solution is PARTIALLY neutralizing hypochlorous acid with sodium hydroxide; the Ka of HClO is 3.5 x 10-8 . Use the Henderson-Hasselbalch equation. a) If 50.0 mL of 1.00M HClO is used to make the buffer, what volume of 0.500M NaOH is needed for the final pH of the buffer to be equal to the pKa of the acid? b) Assuming no density change upon mixing, what are the concentrations of the wek acid (HClO) and its conjugate base...
A buffer solution was prepared by mixing 300.0 mL of a 0.200 M solution of hydroxylamine...
A buffer solution was prepared by mixing 300.0 mL of a 0.200 M solution of hydroxylamine (OHNH2, Kb = 1.1 × 10-8) and 250.0 mL of a 0.300 M solution of its hydrochloride salt (OHNH3+ Cl- ). Calculate the pH of the solution after the addition of 1.08 g of solid NaOH (molar mass = 40.00 g/mol). Assume that there is no volume change upon the addition of solid.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT